Test Unit 3 CA STDS Test STILL NEEDS 7a CA STD & Check everything ok & correlates to following standards:

1a, b, d, g, j

2a, b, d, e, f, g, h

3a

6f

7a-d

8c, d

10a, b, d, e, f

True/FalseIndicate whether the statement is true or false.

____ 1. Crystallization is a separation technique used to produce rock candy from a sugar solution.

____ 2. The periodic table organizes elements into a grid of vertical columns known as periods.

____ 3. Mendeleev’s original table could accommodate elements that did not even exist.

____ 4. The emission of photons from the surface of a metal depends on the frequency of incident light, not on the intensity of light.

____ 5. A chemical bond results from the interaction between two nuclei.

____ 6. The element, neon, with the electron configuration 1s 2s 2p , will not form a chemical bond with another element, oxygen.

____ 7. A sodium ion is more stable than a sodium atom.

____ 8. The more negative the lattice energy of an ionic compound, the weaker the force of attraction.

____ 9. An oxygen atom, having electron configuration 1s 2s 2p , forms a single bond with another oxygen atom.

____ 10. A sigma bond is formed between two atoms when the valence atomic orbital of one atom overlaps end-to-end with that of the other atom.

____ 11. The bond angle for a molecule with sp hybridized atom is always 109.5°.

____ 12. Word equations use words to indicate reactants and products of chemical reactions.

____ 13. The kinetic-molecular theory assumes that the distance between the particles of a gas is so large that there are no significant attractive or repulsive forces.

____ 14. When the molecules of gases are heated, the average kinetic energy of the molecules increases.

____ 15. The amount of energy required to change the phase of a molecular substance such as sucrose is greater than an ionic substance such as table salt.

____ 16. At 50°C temperature and 1.15 atm pressure, water exists in the vapor phase.

____ 17. Carbon dioxide cannot be liquefied above the critical temperature, even when high pressure is applied.

____ 18. According to the phase diagram of carbon dioxide, it is liquefied at critical temperature and pressure.

____ 19. A piece of paper burns faster than pieces of shredded paper.

____ 20. In an esterification reaction, , sulfuric acid acts as a homogeneous catalyst.

____ 21. The potential energy of an activated complex is maximum.

____ 22. The minimum amount of energy needed by the reactant to form the activated complex and lead to a reaction is known as the activation energy.

____ 23. If the potential energy of the product is less than that of the reactants, the energy released when an activated complex forms a product will be more than the activation energy. The reaction will be endothermic.

____ 24. If the temperature of the reactants is increased, the rate of the reaction will decrease.

____ 25. The isobutane given below is an example of a branched-chain hydrocarbon.

____ 26. The IUPAC name of is 2-ethyl butane.

____ 27. Cyclohexane is a cyclic hydrocarbon having six carbon atoms in a straight chain.

____ 28. Sunflower oil is a vegetable oil that reacts with bromine. Therefore, it contains unsaturated hydrocarbons.

____ 29. The IUPAC name of is 3-methyl-3-hexene.

____ 30. D-glucose and L-glucose are optical isomers.

____ 31. The two dipeptides, Glycylphenylalanine (Gly-Phe) and Phenylalanylglycine (Phe-Gly), differ in their properties.

____ 32. In a nucleotide, the nitrogen base is the same, but the sugar and phosphate groups vary.

CompletionComplete each statement.

33. The minimum amount of energy that can be gained or lost by an atom is known as a ____________________.

34. The group 2A elements are known as ____________________ metals.

35. Elements that have physical and chemical properties of both metals and nonmetals are known as ____________________.

36. Chemical bond formation may take place due to the interaction between a(n) ____________________ and an anion.

37. An ionic bond results due to the ____________________ attraction between two oppositely charged ions.

38. When a cellulose paper is dipped in water, the force existing between the particles of the cellulose paper and the water particles is a(n) ____________________ force.

39. A human body controls its temperature by the method of ____________________.

40. At boiling point, the ____________________ pressure over a liquid equals the atmospheric pressure.

41. During the deposition process by which atmospheric carbon dioxide undergoes a phase change to form solid carbon dioxide, energy is ____________________.

42. The ____________________ is defined as the system along with the surroundings.

43. The molar enthalpies of condensation and vaporization have the ____________________ numerical value.

44. If the temperature at which a reaction occurs increases, the number of collisions ____________________.

45. The IUPAC name of a compound represented by the line structure is ____________________.

46. The IUPAC name of is ____________________.

47. The number of different groups attached to an asymmetric carbon atom is ____________________.

48. In aromatic compounds, the position of the double bond is ____________________.

49. The IUPAC name of is ____________________.

50. The molecular formula of octane is ____________________.

51. The correct structure of 4-methyl-2-pentanol is ____________________.

52. In a condensation reaction, two amino acids combine to form an amide, and release ____________________ in the process.

53. When an egg is boiled, the protein rich egg white solidifies due to the ____________________ of its protein.

54. Blood sugar and fruit sugar are ____________________ with respect to the arrangement of their atoms.

55. The three-dimensional shape of protein structure is determined by the interactions among the ____________________.

Multiple ChoiceIdentify the choice that best completes the statement or answers the question.

____ 56. Which of the following elements is a metal?a. Boron c. Magnesiumb. Nitrogen d. Carbon

____ 57. According to ____ periodic table, the physical and chemical properties of elements are periodic functions of their atomic weights.a. Dmitri Mendeleev’s c. Henry Moseley’sb. John Newlands’ d. Lothar Meyer’s

____ 58. A compound BeCl uses sp hybrid orbitals of Be atom. Which of the following is the correct bond angle in the compound?a. 104.5° c. 120°b. 109.5° d. 180°

____ 59. A gas particle of mass 5.31 10 kg has a velocity of 1.00 102 m/s. What is the kinetic energy of the molecule?a. 5.31 10 kg m2/s2 c. 2.65 10 kg m2/s2

b. 5.31 10 kg m2/s2 d. 10.6 10 kg m2/s2

____ 60. Which of the following about an ice cube floating in a glass of water is correct?a. The temperature of the ice cube increases.b. The temperature of the ice cube decreases.c. The temperature of the ice cube remains constant.d. The temperature of the ice cube will fluctuate.

____ 61. Which of the following factors does not affect the rate of reaction?a. The physical state of the reactants.b. The amount of the reactants.c. The size of the container used.d. The temperature at which the reaction is carried out.

____ 62. Which of the following statements about a catalyst is true?a. A catalyst can initiate a reaction.b. A catalyst can accelerate the rate of a reaction.c. A catalyst can be consumed during a reaction.d. A catalyst can be changed chemically during a reaction.

____ 63. The correct IUPAC name of the compound is ____.a. 3,4-dimethylpentane c. 2,3-dimethylpentaneb. 2,3-dimethylbutane d. 2,2,3-dimethylbutane

____ 64. Name the cycloalkane given below.

a. 1,2,4-trimethylcyclohexane c. 1,2,4-trimethylcyclopentaneb. 1,2,4-dimethylcyclopentane d. 1,3,5-trimethylcyclopentane

____ 65. Which is NOT an isomer of hexane?a. 2-methylpentane c. 2,3-dimethylbutaneb. 2,2-dimethylbutane d. 2-methyl-2-ethylbutane

____ 66. How are 3-methylheptane,3,3-dimethylhexane and 2-ethyl-4-methylpentane related to each other?a. They are geometric isomers. c. They are structural isomers.b. They are homologous. d. They are optical isomers.

____ 67. Which compound has a hydroxyl group?a. c.

b. d.

____ 68. Which technique uses a porous barrier to separate a solid from a liquid?a. Chromatography c. Distillationb. Crystallization d. Filtration

____ 69. What is the frequency range for X rays?a. 106 Hz c. 1014 Hzb. 108 Hz d. 1018 Hz

____ 70. How many valence electrons are present in silicon?a. One c. Fourb. Two d. Six

____ 71. The electron configuration of Na is [Ne]3s1 and that of Cl is [Ne]3s23p5. What is the formula of the compound when these elements react?a. Na Cl c. NaClb. NaCl d. Na Cl

____ 72. Fluorine belongs to group 7A. How many covalent bonds are formed between two fluorine atoms? a. 1 c. 3b. 2 d. 4

____ 73. How many bond pairs of electrons exist in a molecule of ammonia?a. 1 c. 8b. 4 d. 10

____ 74. If the electronegativity of H is 2.20 and of Cl is 3.55, which type of bond is formed between H and Cl, when they form hydrogen chloride?a. Ionic c. Covalentb. Polar ionic d. Polar covalent

Short Answer

75. Define a photon. What is the formula used to calculate the energy of a photon?

76. Why does a piece of iron appear red when heated sufficiently and blue at a higher temperature?

77. How is light produced in neon signs?

78. State the drawbacks of Rutherford’s nuclear atomic model.

79. List and define the characteristics of a wave.

80. What is the ground state electron configuration of chlorine and the number of valence electrons in it?

81. How many valence electrons are present in cesium? Write the electron configuration of cesium if the atomic number is 55.

82. What is meant by continuous electromagnetic spectra?

83. Write the noble gas form of the electron configuration and the electron dot structure of sodium and oxygen.

84. What is meant by atomic emission spectra?

85. State the importance of atomic emission spectra.

86. Write the noble gas form of the electron configuration and the electron dot structure of selenium and phosphorus.

87. State the periodic law.

88. Identify the representative elements from the list given below.

Na, Ca, Sc, Co, Ni, Si, N, Se, Cl, Ge

89. Why is argon placed before potassium in the modern periodic table?

90. Why do elements in the same group have similar properties?

91. The second ionization energy of sodium is very high as compared to the first ionization energy. Explain this trend of sodium.

92. Why is the size of a sodium ion (Na+) less than that of a sodium atom (Na)?

93. What are phosphors? Give examples from the periodic table.

94. List the general electron configuration and location of the s, p, d, and f-block elements in the periodic table.

95. Use the periodic table to write the names of the third alkali metal and the first transition metal.

96. Two hydrogen atoms combine to form a hydrogen molecule. How many bonds can a hydrogen atom form with another hydrogen atom and what is the outer electronic configuration of hydrogen?

97. Ammonia is formed with one nitrogen and three hydrogen atoms. What is the electron configuration of nitrogen? How many lone pairs of electrons are present in nitrogen in an ammonia molecule?

98. There exists a direct relationship between the energy needed to break a bond and the bond length. The bond dissociation energy of fluorine is 159 kJ/mol, oxygen is 498 kJ/mol, and nitrogen is 945 kJ/mol. Which molecule has the strongest covalent bond and the shortest bond length?

99. The melting point of sugar is lower than that of common salt. What type of bonding can you predict for each compound? What type of force acts among the ions or molecules in the two compounds?

100. Define reactants in a chemical reaction.

101. Define products in a chemical reaction.

102. Define a skeleton equation.

103. What is stoichiometry?

104. What is a mole ratio?

105. Balance the following equation and determine the possible mole ratios.

106. Describe the basic assumptions of the kinetic molecular theory of gases that confirm the ideal behavior of gases.

107. Explain why the molecules of cooking oil are not held together as tightly as the molecules of table salt.

108. During both evaporation and boiling, a liquid changes to a gas. How is the boiling of liquid related to the evaporation process?

109. Explain the reason behind the formation of dew on grass.

110. Draw the structures of 2,2,3-pentanetriamine and 1,3,5-cyclohexanetriol.

111. Use the structural formula to write the equation for the following reaction:1-pentanol 1-pentene + water

112. Write the name and structure of the monomers that react to form the polymers given below:a. PVCb. Teflon

113. Give the name and structure of the simplest possible amino acid.

114. Proteins are found to exist mainly in two shapes in a three-dimensional structure. What are the two shapes and what is the main binding force holding these shapes?

Problem

115. A part of visible light has frequency 7.90 1016 s–1. Calculate its wavelength if the velocity of light is 3.00 108 m/s.

116. A radiostation broadcasts a program at 122.9 MHz. Calculate the wavelength of the radiowave at this frequency.

117. Calculate the wavelength of light in nm that has a the frequency of 1.24 1015 s–1. The velocity of light is 3.00 108 m/s.

118. Calculate the energies of two radiations. The first radiation is of wavelength 419 nm and the second is of wavelength 614 nm. The value of Planck’s constant is 6.626 10–34 J s.

119. Tiny water droplets in the air disperse the white light of the sun into a rainbow. What is the energy of a photon from the red portion of the rainbow if it has a frequency of 4.57 1014s–1?

120. Write the ground state electron configuration of sulfur and draw its electron-dot structure.

121. Two elements A and B have atomic numbers 8 and 17 respectively. Identify their groups in the periodic table.

122. An element has similar chemical properties as oxygen and selenium. It has an atomic number greater than krypton but less than iodine. Use the periodic table to identify the element.

123. Predict the position of an element with electron configuration (n–1)d1, ns2, where n 4.

124. Identify the element having the largest size and the element having the highest electronegativity from the list of electron configurations given below:a. [Ne] 3s23p3

b. [Ne] 3s23p4

c. [Ne] 3s23p5

d. [Ne] 3s23p34s23d3

125. Arrange the elements given below in the increasing order of their atomic size.Element A 1s22s22p6

Element B 1s22s2

Element C 1s22s22p63s1

Element D 1s22s22p3

126. Write the electron dot structure of the element of 7A group and third period.

127. The electron configuration of an element is 1s 2s 2p . It forms a compound having two bonds with hydrogen atoms. Determine the number of lone pairs of electrons and the number of electrons that are involved in the process of bonding with the hydrogen atoms?

128. Hydrogen selenide has selenium and hydrogen atoms. How many pairs of electrons are needed to form bonds in the compound? How many lone pairs of electrons does the central element possess?

129. Stibine is formed with antimony sulfide and hydrogen atoms. How many lone pairs of electrons does the central element possess? Does the central element fulfill its octet?

130. The molar mass of a gas X is 30.0 g/mol. If the velocity of its molecules at a temperature is 157 m/s, what is the kinetic energy of the gas molecules?

131. When a 50.0-g nugget of pure gold is heated from 35.0°C to 50.0°C, it absorbed 5200.0 J of energy. Find the specific heat of gold.

132. An unknown substance weighing 42.0 g was heated from 36.0°C to 65.0°C. In this process, the substance absorbed 5895 J of energy. What is the specific heat of the substance?

133. How much heat is absorbed by 15.5 g of water when its temperature is increased from 20.0°C to 50.0°C? The specific heat of water is 4.184 J/(g °C).

134. A metal weighing 50.0 g absorbs 220.0 J of heat when its temperature increases by 120.0°C. What is the specific heat of the metal?

135. A 23.0-g sample of water is put into a calorimeter and heated until its temperature increases from 31.0°C to 68.0°C. If the specific heat of water is 4.18 J/(g °C), calculate the heat absorbed by water.

136. Calculate the heat gained by 125.0 g of water when it is put into a calorimeter and its temperature is increased by 90.00°C. The specific heat of water is 0.4184 J/(g °C).

137. Calculate the heat required to melt 64.0 g of solid methanol, given that the molar enthalpy of fusion is 3.22 kJ/mol and the molar mass of methanol is 32.0 g.

138. Write the IUPAC name of the following structure:

139. How many electrons are shared between the carbon atoms in ethene and ethyne? Draw their Lewis structures and calculate.

140. Write the IUPAC name of the following compound:

141. Determine the IUPAC name of the following structure:

142. Identify the functional group present in the compounds:a. CH3-O-CH2CH3

b.

143. Draw the structures of the following compounds and name the functional group of each.a. Methanamideb. Ethyl ethanoatec. Butanoic acidd. 3-hexanone

144. Name the functional group present in the following compound.

OH

145. Complete the IUPAC name of the following ester:

Essay

146. You are provided a 20-mL solution of methanol and water.a. Name the technique that you would use to separate and identify the components of the solution.

b. Provide specific details of the method used.c. State the advantage of the method you choose.

147. The electron configuration of zinc is 1s 2s 2p 3s 3p 4s 3d .a. How many electrons are there in the outermost level?b. Which electrons are lost when zinc forms a bond?c. What is the charge on zinc when it loses electrons in forming a bond?

148. Lithium is a reactive metal that reacts with oxygen to form an oxide.a. How many valence electrons does lithium have?b. How many electrons does lithium lose or gain to achieve a stable octet configuration?c. What is the formula of lithium oxide?

149. Represent the reaction between nitrogen and hydrogen in terms of:a. Particlesb. Molesc. Mass

150. Represent the reaction between zinc and nitric acid in terms of:a. Particlesb. Molesc. Mass

151. In the equation for the combustion of butane, show that the law of conservation of mass is observed. Interpret the equation for the combustion of butane in terms of:a. Representative particlesb. Molesc. Mass

152. Alkanes are compounds of carbon and hydrogen.a Write the molecular formula of an alkane having five carbon atoms.b Write the condensed structural formula of an alkane having five carbon atoms.c Write all of the structural formulas of branched-chain alkane with the molecular formula from part a.

153. Phenylalanine is among the 20 amino acids identified so far.a. Give the structure of phenylalanine.b. Give the structural representation of condensation reaction of two amino acids. You may use R , R for

the side chains of the above amino acids in the equation.c. What causes denaturation of proteins?

154. A disaccharide on hydrolysis gives two monosaccharides. Identify the following compounds A, B, X, and Y, and complete the equations with the correct names of all the compounds.

a. A + H O X + Fruit sugar

b. B + H O X + X

c. Milk sugar + H O X + Y

155. A polysaccharide is a polymer of simple sugars with the same type of bonding that joins two monosaccharides in a disaccharide.a. What is the minimum monomer unit required for a complex carbohydrate?b. What type of bond joins different monosaccharides to form polysaccharides?c. Give the cyclic structural representation of the condensation reaction in the formation of sucrose.

Test Unit 3 CA STDSAnswer Section

TRUE/FALSE

1. ANS: TThe crystallization technique results in the formation of pure solid particles of a substance from a solution containing a dissolved substance. As water evaporates from the sugar-water solution, sugar is left behind as a solid crystal on a string.

PTS: 1 DIF: 1 REF: Page 69OBJ: 3.3.3 List and describe several techniques used to separate mixtures.NAT: B.2 STA: 6fTOP: List and describe several techniques used to separate mixtures.KEY: Crystallization MSC: 1NOT: Correct! Crystallization produces highly pure solids.

2. ANS: FThe periodic table organizes elements into a grid of vertical columns known as groups or families.

PTS: 1 DIF: 1 REF: Page 70OBJ: 3.4.2 Describe the organization of elements in the periodic table.NAT: UCP.1 | B.2 STA: 1aTOP: Describe the organization of elements in the periodic table.KEY: Periodic table MSC: 1NOT: The periodic table organizes elements into a grid of horizontal rows known as periods. The grid of vertical columns is known as groups or families.

3. ANS: TMendeleev was able to predict the properties of elements that were not yet discovered.

PTS: 1 DIF: 1 REF: Page 70OBJ: 3.4.2 Describe the organization of elements in the periodic table.NAT: UCP.1 | B.2 STA: 1aTOP: Describe the organization of elements in the periodic table.KEY: Periodic table MSC: 2NOT: Mendeleev left blank spots in his table. By analyzing the similarities among the elements and their repetition pattern, he was able to predict the properties of undiscovered elements.

4. ANS: TA metal does not eject photoelectrons below a specific frequency of incident light even if the intensity of light increases.

PTS: 1 DIF: 1 REF: Page 123OBJ: 5.1.2 Define a quantum of energy and explain how it is related to an energy change of matter.NAT: B.6 STA: 1j | 1hTOP: Define a quantum of energy and explain how it is related to an energy change of matter.KEY: The photoelectric effect MSC: 1NOT: In the photoelectric effect, photons are emitted from the surface of a metal when light of a certain frequency shines on the surface.

5. ANS: F

Chemical bonds are formed by the attraction between a positive nucleus and the negative electrons or the attraction between a positive ion and a negative ion.

PTS: 1 DIF: 1 REF: Page 211 OBJ: 8.1.1 Define chemical bond.NAT: B.1 STA: 2a TOP: Define chemical bond.KEY: Chemical bond MSC: 1NOT: Nucleus of an atom is positively charged, and the interaction between two nuclei will be repulsive in nature.

6. ANS: TThe presence of eight electrons in the outermost energy level of neon provides a stable electron configuration, called an octet.

PTS: 1 DIF: 2 REF: Page 212OBJ: 8.1.2 Relate chemical bond formation to electron configuration.NAT: B.1 STA: 2a | 1g TOP: Relate chemical bond formation to electron configuration.KEY: Chemical bond | Electron configuration MSC: 2NOT: Noble gases have high ionization energies and low electron affinities. They show a general lack of chemical reactivity. Neon is a noble gas and, therefore, it will not form a chemical bond with another element.

7. ANS: TA sodium ion is formed by the loss of an electron from a sodium atom. It has a stable octet configuration.

PTS: 1 DIF: 1 REF: Page 212 | Page 213OBJ: 8.1.3 Describe the formation of positive and negative ions.NAT: B.1 STA: 1c | 2a TOP: Describe the formation of positive and negative ions.KEY: Cation MSC: 2NOT: Sodium atom has one 3s valence electron. When sodium loses this outer valence electron, the resulting electron configuration will be identical to that of the noble gas, neon.

8. ANS: FLattice energy is the energy required to separate one mole of the ions of an ionic compound. The higher its value, the stronger is the force.

PTS: 1 DIF: 1 REF: Page 219OBJ: 8.2.3 Discuss the energy involved in the formation of an ionic bond.NAT: B.3 | B.4 | B.6 STA: 2gTOP: Discuss the energy involved in the formation of an ionic bond.KEY: Lattice energy MSC: 2NOT: Lattice energy denotes the force of attraction among the constituent ions.

9. ANS: FTo fulfill its octet, each oxygen atom shares two electrons with another oxygen atom, forming a double covalent bond between them.

PTS: 1 DIF: 2 REF: Page 245OBJ: 9.1.2 Describe the formation of single, double, and triple covalent bonds.NAT: B.1 STA: 2a | 2b | 2eTOP: Describe the formation of single, double, and triple covalent bonds.KEY: Double covalent bond MSC: 2NOT: Oxygen is two electrons short from fulfilling its octet.

10. ANS: TThe end-to-end overlap of two valence atomic orbitals from two atoms results into concentrating electron density in the bonding orbital between the two atoms.

PTS: 1 DIF: 1 REF: Page 245OBJ: 9.1.2 Describe the formation of single, double, and triple covalent bonds.NAT: B.1 STA: 2a | 2b | 2eTOP: Describe the formation of single, double, and triple covalent bonds.KEY: Sigma bond MSC: 1NOT: A sigma bond occurs when the electron pair is shared in an area centered between the two atoms.

11. ANS: FThe angle is 109.5° when there are no lone pairs of electrons on the central atom.

PTS: 1 DIF: 1 REF: Page 259OBJ: 9.4.2 Predict the shape of and the bond angles in a molecule.NAT: B.1 | B.4 STA: 2f TOP: Predict the shape of and the bond angles in a molecule.KEY: Molecular shape MSC: 1NOT: If there are no lone pairs of electrons, then for a sp3 hybridized atom, the bond angle is 109.5°.

12. ANS: TWord equations use words or statements to indicate reactants and products.

PTS: 1 DIF: 1 REF: Page 279OBJ: 10.1.2 Represent chemical reactions with equations. NAT: UCP.1 | UCP.2 | B.3STA: 3a TOP: Represent chemical reactions with equations.KEY: Word equations MSC: 1NOT: Skeleton equations use chemical formulas to indicate reactants and products.

13. ANS: TDue to the lack of any significant attractive or repulsive forces between the particles of the gas, gas particles are separated by empty space in the container in which the gas is kept.

PTS: 1 DIF: 1 REF: Page 385 | Page 386OBJ: 13.1.1 Use the kinetic-molecular theory to explain the behavior of gases.NAT: UCP.2 | B.2 | B.4 STA: 4g | 2dTOP: Use the kinetic-molecular theory to explain the behavior of gases.KEY: Kinetic-molecular theory MSC: 1NOT: Most of the space in the container in which a gas is contained remains empty.

14. ANS: TOn heating, the temperature of a gas rises. Heat energy supplied increases the speed of the molecules and thereby increase the average kinetic energy.

PTS: 1 DIF: 2 REF: Page 386OBJ: 13.1.1 Use the kinetic-molecular theory to explain the behavior of gases.NAT: UCP.2 | B.2 | B.4 STA: 4g | 2dTOP: Use the kinetic-molecular theory to explain the behavior of gases.KEY: Kinetic-molecular theory MSC: 2NOT: According to the kinetic molecular theory of gases, the average kinetic energy of a molecule is directly proportional to the absolute temperature.

15. ANS: FThe amount of energy required to change the phase of a molecular substance such as sucrose is less than an ionic substance such as table salt.

PTS: 1 DIF: 1 REF: Page 404OBJ: 13.4.1 Explain how the addition and removal of energy can cause a phase change.

NAT: UCP.3 | B.2 | B.4 | B.6 STA: 7cTOP: Explain how the addition and removal of energy can cause a phase change.KEY: Phase change MSC: 2NOT: The amount of energy required to change the phase of a substance depends on the strength of the force that keeps the particles together in the previous phase. In sucrose, the forces are weaker than the table salt.

16. ANS: FAccording to the phase diagram, water exists in the liquid phase at the given temperature and pressure.

PTS: 1 DIF: 2 REF: Page 408 OBJ: 13.4.2 Interpret a phase diagram.NAT: UCP.3 STA: 7c TOP: Interpret a phase diagram.KEY: Phase diagram MSC: 2NOT: At 50°C, water can exist in the vapor phase at a very low pressure.

17. ANS: TA critical temperature of a gas may be defined as that temperature above which it cannot be liquefied, no matter how great the pressure applied.

PTS: 1 DIF: 2 REF: Page 409 OBJ: 13.4.2 Interpret a phase diagram.NAT: UCP.3 STA: 7c TOP: Interpret a phase diagram.KEY: Phase diagram MSC: 2NOT: Carbon dioxide cannot exist in liquid phase above the critical temperature, 31°C.

18. ANS: TCritical point indicates the critical temperature and critical pressure at which a gas is liquefied.

PTS: 1 DIF: 2 REF: Page 409 OBJ: 13.4.2 Interpret a phase diagram.NAT: UCP.3 STA: 7c TOP: Interpret a phase diagram.KEY: Critical point MSC: 2NOT: Carbon dioxide is liquefied at critical temperature, 31°C and critical pressure, 72.9 atm.

19. ANS: FLarger the surface area, faster is the rate of reaction. The surface area of a piece of paper is less than pieces of shredded paper of the same mass.

PTS: 1 DIF: 1 REF: Page 537OBJ: 17.2.1 Identify factors that affect the rates of chemical reactions.NAT: B.3 STA: 8b | 8c TOP: Identify factors that affect the rates of chemical reactions.KEY: Rate of reaction | Surface area MSC: 1NOT: Pieces of shredded paper burn faster than a piece of paper of the same mass.

20. ANS: TIn an esterification reaction, the reactants (RCOOH, ROH) and the catalyst (H2SO4) are in the same physical state (liquid).

PTS: 1 DIF: 1 REF: Page 541 OBJ: 17.2.2 Explain the role of a catalyst.NAT: UCP.2 | B.3 STA: 8c TOP: Explain the role of a catalyst.KEY: Homogeneous catalyst MSC: 1NOT: The reactant and the catalyst are in the same physical state (liquid). Therefore, sulfuric acid acts as a homogeneous catalyst.

21. ANS: TSince an activated complex is a temporary, unstable species, it possesses maximum potential energy.

PTS: 1 DIF: 1 REF: Page 532OBJ: 17.1.2 Relate rates of chemical reactions to collisions between reacting particles.

NAT: B.3 | B.4 STA: 8a | 8dTOP: Relate rates of chemical reactions to collisions between reacting particles.KEY: Activated complex MSC: 2NOT: Due to maximum potential energy, an activated complex or transition state decomposes to form product or may break apart to re-form the reactant.

22. ANS: TActivation energy has a direct influence on the rate of a reaction.

PTS: 1 DIF: 1 REF: Page 533 | Page 534OBJ: 17.1.2 Relate rates of chemical reactions to collisions between reacting particles.NAT: B.3 | B.4 STA: 8a | 8dTOP: Relate rates of chemical reactions to collisions between reacting particles.KEY: Activation energy MSC: 1NOT: The difference in the potential energy between the reactant and the activated complex is the activation energy.

23. ANS: FIf the potential energy of the product is less than that of reactants, the energy released, when an activated complex forms a product, will be more than the activation energy. The reaction will be exothermic.

PTS: 1 DIF: 2 REF: Page 534OBJ: 17.1.2 Relate rates of chemical reactions to collisions between reacting particles.NAT: B.3 | B.4 STA: 8a | 8dTOP: Relate rates of chemical reactions to collisions between reacting particles.KEY: Activation energy MSC: 2NOT: In an exothermic reaction, reactants possess enough energy to overcome the activation barrier from an activated complex. After releasing the energy, the activated complex breaks down to the product at a lower energy level.

24. ANS: FIf the temperature of the reactants is increased, the rate of the reaction will increase. Increasing the temperature increases the collisions between the reactants.

PTS: 1 DIF: 1 REF: Page 538OBJ: 17.2.1 Identify factors that affect the rates of chemical reactions.NAT: B.3 STA: 8b | 8c TOP: Identify factors that affect the rates of chemical reactions.KEY: Factors affecting the rate of a reaction MSC: 2NOT: he rate of a reaction is directly proportional to the kinetic energy of the reactants, which increases with increasing collision of reactants.

25. ANS: TA hydrocarbon that has at least one branch of carbon atom from the parent chain is called a branched-chain hydrocarbon. An istobutane has a branched carbon atom from the second carbon atom of the longest continuous chain.

PTS: 1 DIF: 3 REF: Page 701OBJ: 22.1.1 Describe the structures of alkanes. NAT: UCP.1 | B.2STA: 10b TOP: Describe the structures of alkanes. KEY: Branched-chain alkanesMSC: 2 NOT: An isobutane has a carbon-branch at the second position of its longest chain.

26. ANS: F

The ethyl group at the second position forms part of the parent chain and not a substituent alkyl group.

PTS: 1 DIF: 2 REF: Page 703OBJ: 22.1.2 Name an alkane by examining its structure. NAT: B.2STA: 10d TOP: Name an alkane by examining its structure.KEY: Nomenclature | Hydrocarbons MSC: 2NOT: The methyl group is not a part of the longest chain.

27. ANS: FThe prefix cyclo indicates the presence of a ring in the structure of a hydrocarbon.

PTS: 1 DIF: 1 REF: Page 706OBJ: 22.2.1 Name a cyclic alkane by examining its structure. NAT: UCP.3 | B.2STA: 10d TOP: Name a cyclic alkane by examining its structure.KEY: Cycloalkanes MSC: 1NOT: Straight-chain hydrocarbons do not have a prefix, cyclo, since all the carbon atoms are present in the form of a straight chain.

28. ANS: TOnly unsaturated hydrocarbons react with bromine due to the presence of at least one double or triple bond between the carbon atoms.

PTS: 1 DIF: 2 REF: Page 710OBJ: 22.2.4 Distinguish between saturated and unsaturated hydrocarbons.NAT: B.2 STA: 10dTOP: Distinguish between saturated and unsaturated hydrocarbons.KEY: Unsaturated hydrocarbons MSC: 2NOT: Saturated hydrocarbons do not react with bromine.

29. ANS: FThe correct IUPAC name of the given compound is 3-methyl-2-hexene.

PTS: 1 DIF: 1 REF: Page 712OBJ: 22.3.3 Name an alkene or alkyne by examining its structure.NAT: B.2 STA: 10d TOP: Name an alkene or alkyne by examining its structure.KEY: Nomenclature of alkenes MSC: 2NOT: The IUPAC name depends on the position of the double bond in a compound. Bonds are numbered in a way that gives the lowest set of numbers.

30. ANS: TD-glucose and L-glucose have the same molecular formula but the arrangement of atoms is different.

PTS: 1 DIF: 1 REF: Page 719OBJ: 22.4.3 Recognize different structural isomers given a structural formula.NAT: UCP.2 | B.2 STA: 10dTOP: Recognize different structural isomers given a structural formula.KEY: Optical isomers MSC: 1NOT: The molecular formula of optical isomers are the same. D and L represent the different arrangement of atoms.

31. ANS: T

The amino acids that determine the properties, are linked in different order in the dipeptides, Glycylphenylalanine (Gly-Phe) and Phenylalanylglycine (Phe-Gly). Hence, the two dipeptides differ in their properties.

PTS: 1 DIF: 1 REF: Page 777OBJ: 24.1.1 Describe the structures of amino acids and proteins.NAT: B.2 | C.5 STA: 10a | 10c | 10fTOP: Describe the structures of amino acids and proteins. KEY: PeptideMSC: 1NOT: In (Gly-Phe), the ring structure is attached to the carbon atom adjacent to the nitrogen atom linking the amino acids, where as in (Phe-Gly), it is attached to the second carbon atom.

32. ANS: FIn a nucleotide, the phosphate group is the same but the sugar and nitrogen base vary.

PTS: 1 DIF: 1 REF: Page 788OBJ: 24.4.1 Identify the structural components of nucleic acids.NAT: B.2 STA: 10a TOP: Identify the structural components of nucleic acids.KEY: Nucleotide MSC: 1NOT: Sugar and nitrogen base can be different in a nucleotide, but the phosphate group remains the same.

COMPLETION

33. ANS: quantum

PTS: 1 DIF: 1 REF: Page 122OBJ: 5.1.2 Define a quantum of energy and explain how it is related to an energy change of matter.NAT: B.6 STA: 1j | 1hTOP: Define a quantum of energy and explain how it is related to an energy change of matter.KEY: Quantum MSC: 1

34. ANS: alkaline earth

PTS: 1 DIF: 1 REF: Page 155OBJ: 6.1.1 Trace the development and identify key features of the periodic table.NAT: G.3 | B.1 | UCP.1 STA: 1a | 1b | 1c | 1fTOP: Trace the development and identify key features of the periodic table.KEY: Alkaline earth metals MSC: 1

35. ANS: metalloids

PTS: 1 DIF: 1 REF: Page 158OBJ: 6.1.1 Trace the development and identify key features of the periodic table.NAT: G.3 | B.1 | UCP.1 STA: 1a | 1b | 1c | 1fTOP: Trace the development and identify key features of the periodic table.KEY: Metalloids MSC: 1

36. ANS: cation

PTS: 1 DIF: 1 REF: Page 211 OBJ: 8.1.1 Define chemical bond.NAT: B.1 STA: 2a TOP: Define chemical bond.KEY: Chemical bond MSC: 1

37. ANS: electrostatic

PTS: 1 DIF: 1 REF: Page 215OBJ: 8.2.1 Describe the formation of ionic bonds. NAT: B.1 | B.4STA: 2a TOP: Describe the formation of ionic bonds.KEY: Ionic bond MSC: 1

38. ANS: intermolecular

PTS: 1 DIF: 1 REF: Page 393OBJ: 13.2.1 Describe and compare intramolecular and intermolecular forces.NAT: B.2 | B.4 STA: 2dTOP: Describe and compare intramolecular and intermolecular forces.KEY: Intermolecular forces | Intramolecular force MSC: 1

39. ANS: evaporation

PTS: 1 DIF: 1 REF: Page 405OBJ: 13.4.1 Explain how the addition and removal of energy can cause a phase change.NAT: UCP.3 | B.2 | B.4 | B.6 STA: 7cTOP: Explain how the addition and removal of energy can cause a phase change.KEY: Evaporation MSC: 1

40. ANS: vapor

PTS: 1 DIF: 1 REF: Page 406OBJ: 13.4.1 Explain how the addition and removal of energy can cause a phase change.NAT: UCP.3 | B.2 | B.4 | B.6 STA: 7cTOP: Explain how the addition and removal of energy can cause a phase change.KEY: Vapor pressure MSC: 1

41. ANS: released

PTS: 1 DIF: 1 REF: Page 407OBJ: 13.4.1 Explain how the addition and removal of energy can cause a phase change.NAT: UCP.3 | B.2 | B.4 | B.6 STA: 7cTOP: Explain how the addition and removal of energy can cause a phase change.KEY: Condensation MSC: 2

42. ANS: universe

PTS: 1 DIF: 1 REF: Page 498OBJ: 16.2.1 Describe how a calorimeter is used to measure energy absorbed or released.NAT: B.5 | B.6 STA: 7dTOP: Describe how a calorimeter is used to measure energy absorbed or released.KEY: System | Surroundings MSC: 1

43. ANS: same

PTS: 1 DIF: 1 REF: Page 502OBJ: 16.3.2 Describe how energy is lost or gained during changes of state.NAT: B.3 | B.5 | B.6 STA: 7cTOP: Describe how energy is lost or gained during changes of state.KEY: Molar enthalpy of condensation and vaporization MSC: 1

44. ANS: increases

PTS: 1 DIF: 1 REF: Page 538OBJ: 17.2.1 Identify factors that affect the rates of chemical reactions.

NAT: B.3 STA: 8b | 8c TOP: Identify factors that affect the rates of chemical reactions.KEY: Rate of reaction | Temperature MSC: 1

45. ANS: cyclopropane

PTS: 1 DIF: 1 REF: Page 706OBJ: 22.2.1 Name a cyclic alkane by examining its structure. NAT: UCP.3 | B.2STA: 10d TOP: Name a cyclic alkane by examining its structure.KEY: Cycloalkanes MSC: 1

46. ANS: 2-hexyne

PTS: 1 DIF: 1 REF: Page 715OBJ: 22.3.3 Name an alkene or alkyne by examining its structure.NAT: B.2 STA: 10d TOP: Name an alkene or alkyne by examining its structure.KEY: Nomenclature of alkynes MSC: 2

47. ANS:four4

PTS: 1 DIF: 1 REF: Page 719OBJ: 22.4.3 Recognize different structural isomers given a structural formula.NAT: UCP.2 | B.2 STA: 10dTOP: Recognize different structural isomers given a structural formula.KEY: Asymmetric carbon MSC: 1

48. ANS:delocalizednot fixed

PTS: 1 DIF: 1 REF: Page 722 | Page 723OBJ: 22.5.1 Compare and contrast the properties of aromatic and aliphatic hydrocarbons.NAT: B.2 STA: 10dTOP: Compare and contrast the properties of aromatic and aliphatic hydrocarbons.KEY: Aromatic compounds MSC: 2

49. ANS: 1-ethyl-2,3-dimethylbenzene

PTS: 1 DIF: 1 REF: Page 724OBJ: 22.5.1 Compare and contrast the properties of aromatic and aliphatic hydrocarbons.NAT: B.2 STA: 10dTOP: Compare and contrast the properties of aromatic and aliphatic hydrocarbons.KEY: Nomenclature of aromatic compound MSC: 2

50. ANS:

PTS: 1 DIF: 3 REF: Page 701OBJ: 22.1.1 Describe the structures of alkanes. NAT: UCP.1 | B.2STA: 10b TOP: Describe the structures of alkanes. KEY: Molecular formulaMSC: 2

51. ANS:

PTS: 1 DIF: 1 REF: Page 744OBJ: 23.2.2 Draw the structure of alcohols, ethers, and amines.NAT: B.2 STA: 10e TOP: Draw the structure of alcohols, ethers, and amines.KEY: Structure of alcohols MSC: 2

52. ANS: water

PTS: 1 DIF: 1 REF: Page 777OBJ: 24.1.1 Describe the structures of amino acids and proteins.NAT: B.2 | C.5 STA: 10a | 10c | 10fTOP: Describe the structures of amino acids and proteins. KEY: PeptideMSC: 1

53. ANS: denaturation

PTS: 1 DIF: 1 REF: Page 778OBJ: 24.1.1 Describe the structures of amino acids and proteins.NAT: B.2 | C.5 STA: 10a | 10c | 10fTOP: Describe the structures of amino acids and proteins. KEY: DenaturationMSC: 1

54. ANS: structural isomers

PTS: 1 DIF: 1 REF: Page 781OBJ: 24.2.1 Describe the structures of monosaccharides, disaccharides, and polysaccharides.NAT: B.2 STA: 10aTOP: Describe the structures of monosaccharides, disaccharides, and polysaccharides.KEY: Monosaccharides | Disaccharides | Polysaccharides MSC: 1

55. ANS: amino acids

PTS: 1 DIF: 1 REF: Page 778OBJ: 24.1.1 Describe the structures of amino acids and proteins.NAT: B.2 | C.5 STA: 10a | 10c | 10fTOP: Describe the structures of amino acids and proteins. KEY: Amino acidsMSC: 1

MULTIPLE CHOICE

56. ANS: CMetals are elements that are generally shiny when smooth and clean, solid at room temperature, and good conductors of heat and electricity.

FeedbackA Boron is a nonmetal and a poor conductor of electricity.B Nitrogen is a nonmetal and gas at room temperature.

C Correct! d/ Carbon is a nonmetal and a dull-looking solid.D

PTS: 1 DIF: 1 REF: Page 155 | Page 156 | Page 158OBJ: 6.1.1 Trace the development and identify key features of the periodic table.NAT: G.3 | B.1 | UCP.1 STA: 1a | 1b | 1c | 1fTOP: Trace the development and identify key features of the periodic table.KEY: Metals MSC: 1

57. ANS: AMendeleev noticed that when elements are ordered by their increasing atomic mass, there was a repetition, or periodic pattern, in their properties.

FeedbackA Correct!B John Newlands discovered the law of octaves.C Henry Moseley discovered the modern periodic table.D Lothar Meyer discovered the connection between atomic mass and elemental properties.

PTS: 1 DIF: 1 REF: Page 152OBJ: 6.1.1 Trace the development and identify key features of the periodic table.NAT: G.3 | B.1 | UCP.1 STA: 1a | 1b | 1c | 1fTOP: Trace the development and identify key features of the periodic table.KEY: Periodic properties MSC: 1

58. ANS: DThere is maximum repulsion between two lone pairs when they are diametrically opposite to each other.

FeedbackA The bond angle is 104.5°, when the hybridization is sp3, and there are two lone pairs of

electrons.B The bond angle is 109.5°, when there are no lone pairs of electrons in the sp3 hybridized

central atom.C The bond angle is 120° for the sp2 hybridized atom.D Correct!

PTS: 1 DIF: 1 REF: Page 259OBJ: 9.4.2 Predict the shape of and the bond angles in a molecule.NAT: B.1 | B.4 STA: 2f TOP: Predict the shape of and the bond angles in a molecule.KEY: Molecular shape MSC: 1

59. ANS: C

The kinetic energy of a particle is .

FeedbackA Instead of multiplying the mass and velocity, multiply the square of velocity by the

mass.B Divide the product of multiplication of mass and the square of velocity by 2.C Correct!D Instead of multiplying the product of mass and the square of velocity by 2, divide the

product of multiplication of mass and square of velocity by 2.

PTS: 1 DIF: 1 REF: Page 386OBJ: 13.1.1 Use the kinetic-molecular theory to explain the behavior of gases.NAT: UCP.2 | B.2 | B.4 STA: 4g | 2dTOP: Use the kinetic-molecular theory to explain the behavior of gases.KEY: Particle energy MSC: 3

60. ANS: CThe heat flow from water to ice is used to break the hydrogen bonds of the ice crystal.

FeedbackA Ice remains at the same temperature.B The temperature of water decreases as heat flows from water to ice.C Correct!D The temperature of ice does not depend on the temperature of water.

PTS: 1 DIF: 1 REF: Page 404OBJ: 13.4.1 Explain how the addition and removal of energy can cause a phase change.NAT: UCP.3 | B.2 | B.4 | B.6 STA: 7cTOP: Explain how the addition and removal of energy can cause a phase change.KEY: Phase change MSC: 1

61. ANS: CThe rate of a reaction is not affected by the size of the container.

FeedbackA The rate of a reaction is affected by the physical state of the reactants.B The amount of a substance affects the rate of a reaction.C Correct!D The rate of a reaction is affected by the temperature at which the reaction is carried out.

PTS: 1 DIF: 1 REF: Page 537 | Page 538OBJ: 17.2.1 Identify factors that affect the rates of chemical reactions.NAT: B.3 STA: 8b | 8c TOP: Identify factors that affect the rates of chemical reactions.KEY: Factors affecting the rate of a reaction MSC: 1

62. ANS: BA catalyst accelerates the rate of a reaction by bringing down the energy of activation.

FeedbackA A catalyst cannot initiate a reaction.B Correct!C A catalyst cannot be consumed during a reaction.D A catalyst does not participate in the reaction.

PTS: 1 DIF: 1 REF: Page 539 OBJ: 17.2.2 Explain the role of a catalyst.NAT: UCP.2 | B.3 STA: 8c TOP: Explain the role of a catalyst.KEY: Catalyst MSC: 1

63. ANS: CThe longest chain has five carbon atoms. The numbering of the chain is done such that all the alkyl groups get the lowest possible position number. The names selected for the alkyl groups and the parent chain are according to the IUPAC rules.

FeedbackA The numbering of the chain is incorrect.B The carbon atoms in the longest chain are not counted correctly.C Correct!D The selection of the longest chain is incorrect.

PTS: 1 DIF: 2 REF: Page 703OBJ: 22.1.2 Name an alkane by examining its structure. NAT: B.2STA: 10d TOP: Name an alkane by examining its structure.KEY: Naming | Branched-chain hydrocarbon MSC: 2

64. ANS: CThe compound is a cyclic hydrocarbon having a five-member carbon ring and a methyl group as a substituent at 1, 2, and 4 positions. The numbering of the cyclic ring is chosen such that the lowest possible numbers are given to the methyl groups.

FeedbackA The use of the word cyclohexane is wrong as it indicates the presence of six carbon

atoms in the ring.B The use of the word di is wrong as it indicates the presence of two substituents (methyl

group) of the same type.C Correct!D The order of numbering a cyclic ring is incorrect.

PTS: 1 DIF: 1 REF: Page 707OBJ: 22.2.1 Name a cyclic alkane by examining its structure. NAT: UCP.3 | B.2STA: 10d TOP: Name a cyclic alkane by examining its structure.KEY: Nomenclature | Cycloalkanes MSC: 2

65. ANS: DThe total number of carbon atoms in 2-methyl-2-ethylbutane is seven.

FeedbackA The molecular formula is the same as hexane, but the molecular structure is different.B The molecular formula is the same as hexane, but the molecular structure is different.C The molecular formula is the same as hexane, but the molecular structure is different.D Correct!

PTS: 1 DIF: 3 REF: Page 717OBJ: 22.4.1 Distinguish between the two main categories of isomers, structural isomers, and stereo isomers.NAT: B.2 STA: 10dTOP: Distinguish between the two main categories of isomers, structural isomers, and stereo isomers.KEY: Structural isomerism MSC: 2

66. ANS: CStructural isomers have the same molecular formula, but the atoms are bonded in a different order.

FeedbackA Geometric isomers must have a double bond.B Homologs have different molecular formulas.C Correct!D Optical isomers have at least one chiral carbon atom.

PTS: 1 DIF: 3 REF: Page 717 | Page 718 | Page 719OBJ: 22.4.1 Distinguish between the two main categories of isomers, structural isomers, and stereo isomers.NAT: B.2 STA: 10dTOP: Distinguish between the two main categories of isomers, structural isomers, and stereo isomers.KEY: Structural isomerism | Sterioisomerism MSC: 2

67. ANS: AAlcohols have a hydroxyl (OH) functional group.

FeedbackA Correct!B The compound has a ketone group as the functional group.C The compound has an ester group as the functional group.D The compound has an ether group as the functional group.

PTS: 1 DIF: 2 REF: Page 738OBJ: 23.1.1 Describe a functional group and give examples. NAT: B.2STA: 10e TOP: Describe a functional group and give examples.KEY: Functional groups MSC: 2

68. ANS: DIn the filtration technique, the mixture is poured through filter paper (porous barrier) that is folded into a cone shape. The liquid passes through the cone, leaving behind the solid particles trapped in the filter paper.

FeedbackA Chromatography is a technique that separates the components of a mixture on the basis

of the tendency of each to travel or be drawn across the surface of another material.B Crystallization is a separation technique that results in the formation of pure solid

particles of a substance from a solution containing the dissolved substance.C Distillation is a separation technique that is based on differences in the boiling points of

the substances involved in the separation process.D Correct!

PTS: 1 DIF: 1 REF: Page 68OBJ: 3.3.3 List and describe several techniques used to separate mixtures.NAT: B.2 STA: 6fTOP: List and describe several techniques used to separate mixtures.KEY: Filtration MSC: 1

69. ANS: DFrequency is the number of waves that pass a given point per second.

FeedbackA The AM frequency in radiowaves is 10^6 Hz.B The FM frequency in radiowaves is 10^8 Hz.C Infrared rays have a frequency of 10^14 Hz.D Correct!

PTS: 1 DIF: 2 REF: Page 120OBJ: 5.1.1 Compare the wave and particle models of light. NAT: B.1STA: 1j TOP: Compare the wave and particle models of light.KEY: Frequency MSC: 1

70. ANS: CThe electron configuration of silicon is 1s22s22p63s23p2

.

FeedbackA Silicon is a group 4A element.B Silicon is a group 4A element.C Correct!D Silicon is a group 4A element.

PTS: 1 DIF: 2 REF: Page 140OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence electrons. NAT: B.1 | B.6 STA: 2eTOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.KEY: Valence electrons MSC: 2

71. ANS: CTo acquire a stable electron configuration, Na loses one electron, thereby forming Na . Cl gains the electron, making Cl–. There is transfer of only one electron in the entire process.

FeedbackA The metal loses only one electron from its outer orbital.B The halogen gains only one electron in the process.C Correct!D The formula should state the simplest ratio of ions.

PTS: 1 DIF: 2 REF: Page 216OBJ: 8.2.1 Describe the formation of ionic bonds. NAT: B.1 | B.4STA: 2a TOP: Describe the formation of ionic bonds.KEY: Ionic bond MSC: 2

72. ANS: AFluorine can acquire the configuration of a stable octet by sharing one electron with another fluorine atom, forming only one covalent bond.

FeedbackA Correct!B There are seven valence electrons in fluorine. Each fluorine atom requires one more

electron to fulfill the octet.C To form three covalent bonds with another fluorine atom, each atom needs three

unpaired electrons.D To form four covalent bonds with another fluorine atom, each atom needs four unpaired

electrons which it does not have.

PTS: 1 DIF: 2 REF: Page 243OBJ: 9.1.2 Describe the formation of single, double, and triple covalent bonds.NAT: B.1 STA: 2a | 2b | 2eTOP: Describe the formation of single, double, and triple covalent bonds.KEY: Covalent bond MSC: 2

73. ANS: BThe total number of bond pairs is the number of bonding electrons divided by two.

FeedbackA There is one lone pair of electrons on a nitrogen atom.B Correct!C The total number of bonding electrons is 8.D The total number of electrons in a molecule of ammonia is 10.

PTS: 1 DIF: 1 REF: Page 252OBJ: 9.3.1 List five basic steps used in drawing Lewis structures.NAT: B.1 STA: 2e TOP: List five basic steps used in drawing Lewis structures.KEY: Structural formula MSC: 2

74. ANS: DSince the electronegativities between the two atoms are different, the atom with higher electronegativity will have a greater tendency to share the electrons. This results in a polar covalent bond.

FeedbackA The bond formed between H and Cl is by sharing electron.B In case of ionic bond, the electron is completely transferred from one atom to another.C The difference in the electronegativities between the two atoms is such that Cl has a

higher share of electrons.D Correct!

PTS: 1 DIF: 1 REF: Page 263OBJ: 9.5.1 Describe how electronegativity is used to determine bond type.NAT: B.1 | B.4 STA: 2gTOP: Describe how electronegativity is used to determine bond type.KEY: Electronegativity MSC: 2

SHORT ANSWER

75. ANS:A photon is a particle of electromagnetic radiation that has no mass and carries a quantum of energy. The energy of a photon can be calculated using the formula Equantum h , where E is energy of the photon, h is Planck’s constant, and is frequency of the photon.

PTS: 1 DIF: 1 REF: Page 123OBJ: 5.1.1 Compare the wave and particle models of light. NAT: B.1STA: 1j TOP: Compare the wave and particle models of light.KEY: Photon | Energy levels MSC: 1

76. ANS:A piece of iron appears red when heated sufficiently and blue at a higher temperature, because the kinetic energy of iron increases when it is heated. With an increase in the amount of energy, different colors of light are emitted. These colors correspond to different frequencies and wavelengths.

PTS: 1 DIF: 1 REF: Page 122OBJ: 5.1.2 Define a quantum of energy and explain how it is related to an energy change of matter.NAT: B.6 STA: 1j | 1hTOP: Define a quantum of energy and explain how it is related to an energy change of matter.KEY: Quantum MSC: 2

77. ANS:

Light is produced in neon signs by passing electricity through a tube filled with neon gas. Neon atoms in the tube absorb energy and become excited. These excited and unstable atoms then release energy by emitting light.

PTS: 1 DIF: 1 REF: Page 125OBJ: 5.1.3 Contrast continuous electromagnetic spectra and atomic emission spectra.NAT: B.6 STA: 1jTOP: Contrast continuous electromagnetic spectra and atomic emission spectra.KEY: Atomic emission spectrum MSC: 1

78. ANS:The drawbacks of Rutherford’s nuclear atomic model are:a. It lacks details about how electrons are arranged around the nucleus.b. It does not explain why certain elements are more reactive than other elements.c. It does not explain why the negatively charged electrons in an atom are not pulled into the atom’s

positively charged nucleus.d. It does not account for the differences in chemical behavior among the various elements.

PTS: 1 DIF: 2 REF: Page 117OBJ: 5.1.1 Compare the wave and particle models of light. NAT: B.1STA: 1j TOP: Compare the wave and particle models of light.KEY: Atomic emission spectrum MSC: 2

79. ANS:The characteristics of a wave are:a. Wavelength - It is the shortest distance between equivalent points on a continuous wave.b. Frequency - It is the number of waves that pass through a given point per second.c. Amplitude - It is the height of a wave from the origin to a crest or from the origin to a trough.d. Speed - All electromagnetic waves, including visible light, travel at a speed of 3.00 108 m/s in

vacuum. The speed of light is the product of its wavelength and frequency.

PTS: 1 DIF: 1 REF: Page 118 | Page 119OBJ: 5.1.1 Compare the wave and particle models of light. NAT: B.1STA: 1j TOP: Compare the wave and particle models of light.KEY: Frequency | Wavelength | Amplitude MSC: 2

80. ANS:The ground state electron configuration of chlorine is 1s22s22p63s23p5. It has 7 valence electrons.

PTS: 1 DIF: 1 REF: Page 138OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence electrons. NAT: B.1 | B.6 STA: 2eTOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.KEY: Valence electrons | Electron configuration MSC: 2

81. ANS:There is only one valence electron in cesium. The electron configuration of cesium with atomic number 55 is [Xe]6s1.

PTS: 1 DIF: 1 REF: Page 140OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence electrons. NAT: B.1 | B.6 STA: 2eTOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.KEY: Valence electrons | Electron configuration MSC: 1

82. ANS:A spectrum is formed due to the dispersion of light when it is passed through a prism. It is called continuous if the dispersion of light is without any discontinuity in wavelength.

PTS: 1 DIF: 1 REF: Page 125OBJ: 5.1.3 Contrast continuous electromagnetic spectra and atomic emission spectra.NAT: B.6 STA: 1jTOP: Contrast continuous electromagnetic spectra and atomic emission spectra.KEY: Continuous electromagnetic spectrum MSC: 1

83. ANS:

a. The noble gas form of the electron configuration of sodium is [Ne]3s1. Its electron dot structure is b. The noble gas form of electron configuration of oxygen is [He]2s22p4. Its electron dot structure is

PTS: 1 DIF: 2 REF: Page 138 | Page 140OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence electrons. NAT: B.1 | B.6 STA: 2eTOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.KEY: Electron configuration | Electron-dot structure MSC: 2

84. ANS:An atomic emission spectrum of an element is the set of the frequencies of the electromagnetic waves emitted by the atoms of the element upon excitation.

PTS: 1 DIF: 1 REF: Page 125 | Page 126OBJ: 5.1.3 Contrast continuous electromagnetic spectra and atomic emission spectra.NAT: B.6 STA: 1jTOP: Contrast continuous electromagnetic spectra and atomic emission spectra.KEY: Atomic emission spectrum MSC: 1

85. ANS:The atomic emission spectrum of an element consists of a number of bright lines separated by dark lines. These lines in the atomic emission spectrum are characteristic of the atoms of an element, and, therefore, the atomic emission spectra of the elements can be used to identify them.

PTS: 1 DIF: 2 REF: Page 125 | Page 126OBJ: 5.1.3 Contrast continuous electromagnetic spectra and atomic emission spectra.NAT: B.6 STA: 1jTOP: Contrast continuous electromagnetic spectra and atomic emission spectra.KEY: Atomic emission spectrum MSC: 2

86. ANS:a. The noble gas form of the electron configuration of selenium is [Ar]4s24p4. Its electron-dot structure is

b. The noble gas form of the electron configuration of phosphorus is [Ne]3s23p5. Its electron-dot structure

is .

PTS: 1 DIF: 2 REF: Page 138OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence

electrons. NAT: B.1 | B.6 STA: 2eTOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.KEY: Electron configuration | Electron-dot structure MSC: 2

87. ANS:The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic numbers.

PTS: 1 DIF: 1 REF: Page 153OBJ: 6.1.1 Trace the development and identify key features of the periodic table.NAT: G.3 | B.1 | UCP.1 STA: 1a | 1b | 1c | 1fTOP: Trace the development and identify key features of the periodic table.KEY: Periodic table MSC: 1

88. ANS:Na, Ca, N, Si, Se, Cl, Ge

PTS: 1 DIF: 1 REF: Page 154OBJ: 6.1.1 Trace the development and identify key features of the periodic table.NAT: G.3 | B.1 | UCP.1 STA: 1a | 1b | 1c | 1fTOP: Trace the development and identify key features of the periodic table.KEY: Metals MSC: 2

89. ANS:In the modern periodic table, the elements are placed in the order of their increasing atomic numbers. The atomic number of argon is 18 while the atomic number of potassium is 19. Therefore, argon is placed before potassium in the modern periodic table.

PTS: 1 DIF: 1 REF: Page 153OBJ: 6.1.1 Trace the development and identify key features of the periodic table.NAT: G.3 | B.1 | UCP.1 STA: 1a | 1b | 1c | 1fTOP: Trace the development and identify key features of the periodic table.KEY: Atomic number MSC: 2

90. ANS:Elements in the same group have the same electron configuration and number of valence electrons. Valence electrons determine the properties of elements. Therefore, properties of elements in the same group are similar.

PTS: 1 DIF: 1 REF: Page 159OBJ: 6.2.1 Explain why elements in the same group have similar properties.NAT: UCP.1 | B.1 | B.2 STA: 1d | 1gTOP: Explain why elements in the same group have similar properties.KEY: Groups | Electron configuration MSC: 2

91. ANS:Ionization is related to the number of valence electrons in an atom. Sodium has one valence electron. It forms a common sodium 1+ ion, but is unlikely to form a sodium 2+ ion. The jump in ionization energy shows that atoms hold onto their inner core electrons more strongly than they hold onto their valence electrons.

PTS: 1 DIF: 1 REF: Page 167 | Page 168OBJ: 6.3.2 Relate period and group trends in atomic radii to electron configuration.NAT: UCP.1 | B.1 | B.2 STA: 1c | 2gTOP: Relate period and group trends in atomic radii to electron configuration.KEY: Ionization energy MSC: 2

92. ANS:The loss of an electron from a sodium atom results in a smaller radius. The electrostatic repulsion between the remaining number of electrons decreases thus allowing them to be pulled closer to the nucleus. Therefore, the size of a sodium ion (Na+) is less than that of a sodium atom (Na).

PTS: 1 DIF: 2 REF: Page 165OBJ: 6.3.2 Relate period and group trends in atomic radii to electron configuration.NAT: UCP.1 | B.1 | B.2 STA: 1c | 2gTOP: Relate period and group trends in atomic radii to electron configuration.KEY: Atomic size | Ionic radius MSC: 2

93. ANS:Phosphors are substances that emit light when struck by electrons. Elements from the lanthanides series are used as phosphors.

PTS: 1 DIF: 1 REF: Page 158OBJ: 6.1.1 Trace the development and identify key features of the periodic table.NAT: G.3 | B.1 | UCP.1 STA: 1a | 1b | 1c | 1fTOP: Trace the development and identify key features of the periodic table.KEY: Phosphors MSC: 1

94. ANS:The general electron configuration and locations of the block elements are:a. ns0-2 for s-block elements in groups 1 and 2.b. ns0-2 and np0-6 for p-block elements in groups 13, 14, 15, 16, 17, and 18.c. (n–1)d0-10 and ns0-2 for d-block elements in groups 3, 4, 5, 6, 7, 8, 9, 10, 11, and 12.d. (n–2)f0-14, (n–1)d0-10, np0-6, and ns0-2 for f-block elements in lanthanide and actinide groups.

PTS: 1 DIF: 2 REF: Page 161OBJ: 6.2.2 Identify the four blocks of the periodic table based on electron configuration.NAT: UCP.1 | B.1 STA: 1d | 1g | 2eTOP: Identify the four blocks of the periodic table based on electron configuration.KEY: Electron configuration MSC: 1

95. ANS:Potassium is the third alkali metal and scandium is the first transition metal in the periodic table.

PTS: 1 DIF: 1 REF: Page 156OBJ: 6.1.1 Trace the development and identify key features of the periodic table.NAT: G.3 | B.1 | UCP.1 STA: 1a | 1b | 1c | 1fTOP: Trace the development and identify key features of the periodic table.KEY: Alkali metals | Transition metals MSC: 1

96. ANS:A hydrogen atom can form only one bond with another hydrogen atom. The outer electronic configuration of hydrogen 1s .

PTS: 1 DIF: 2 REF: Page 242OBJ: 9.1.2 Describe the formation of single, double, and triple covalent bonds.NAT: B.1 STA: 2a | 2b | 2eTOP: Describe the formation of single, double, and triple covalent bonds.KEY: Covalent bond MSC: 2

97. ANS:

The electron configuration of nitrogen is 1s 2s 2p . There is only one lone pair of electrons in nitrogen in an ammonia molecule.

PTS: 1 DIF: 2 REF: Page 243OBJ: 9.1.2 Describe the formation of single, double, and triple covalent bonds.NAT: B.1 STA: 2a | 2b | 2eTOP: Describe the formation of single, double, and triple covalent bonds.KEY: Lone pair MSC: 2

98. ANS:The nitrogen molecule has the strongest covalent bond and the shortest bond length.

PTS: 1 DIF: 2 REF: Page 246OBJ: 9.1.4 Relate the strength of covalent bonds to bond length and bond dissociation energy.NAT: B.1 | B.5 STA: 7bTOP: Relate the strength of covalent bonds to bond length and bond dissociation energy.KEY: Covalent bond MSC: 2

99. ANS:Sugar forms a covalent bond, whereas, common salt forms an ionic bond. Sugar has van der Walls forces, whereas, the force in common salt is ionic in nature.

PTS: 1 DIF: 2 REF: Page 266OBJ: 9.5.3 Describe the characteristic of compounds that are covalently bonded.NAT: B.1 | B.4 STA: 2hTOP: Describe the characteristic of compounds that are covalently bonded.KEY: Properties of covalent compounds MSC: 2

100. ANS:The starting substances of a chemical reaction are called reactants.

PTS: 1 DIF: 1 REF: Page 278OBJ: 10.1.2 Represent chemical reactions with equations. NAT: UCP.1 | UCP.2 | B.3STA: 3a TOP: Represent chemical reactions with equations.KEY: Chemical reactions MSC: 1

101. ANS:The substances formed in a chemical reaction are called products.

PTS: 1 DIF: 1 REF: Page 278OBJ: 10.1.2 Represent chemical reactions with equations. NAT: UCP.1 | UCP.2 | B.3STA: 3a TOP: Represent chemical reactions with equations.KEY: Chemical reactions MSC: 1

102. ANS:The equation that uses chemical formulas to identify the reactants and the products is called a skeleton equation.

PTS: 1 DIF: 1 REF: Page 279OBJ: 10.1.2 Represent chemical reactions with equations. NAT: UCP.1 | UCP.2 | B.3STA: 3a TOP: Represent chemical reactions with equations.KEY: Skeleton equation MSC: 1

103. ANS:Stoichiometry is a study of quantitative relationships between the amounts of reactants used and the products formed by a chemical reaction.

PTS: 1 DIF: 1 REF: Page 354OBJ: 12.1.1 Identify the quantitative relationships in a balanced chemical equation.NAT: UCP.3 | B.3 STA: 3a | 3dTOP: Identify the quantitative relationships in a balanced chemical equation.KEY: Stoichiometry MSC: 1

104. ANS:A mole ratio is the ratio between the numbers of moles of any two substances in a balanced chemical equation.

PTS: 1 DIF: 1 REF: Page 356OBJ: 12.1.2 Determine the mole ratios from a balanced chemical equation.NAT: UCP.3 | B.3 STA: 3a | 3dTOP: Determine the mole ratios from a balanced chemical equation.KEY: Mole ratio MSC: 1

105. ANS:The balanced chemical equation is:

The possible mole ratios are:

PTS: 1 DIF: 2 REF: Page 356OBJ: 12.1.2 Determine the mole ratios from a balanced chemical equation.NAT: UCP.3 | B.3 STA: 3a | 3dTOP: Determine the mole ratios from a balanced chemical equation.KEY: Mole ratio MSC: 3

106. ANS:The basic assumptions of the kinetic molecular theory of gases that confirm the ideal behavior of gases are:a. The actual volume of molecules is negligible compared to the total volume of gas.b. The particles of gases are so spread out that there is no significant force among each other.c. Since all collisions of gases are perfectly elastic, there is no loss of kinetic energy of a gas molecule.

PTS: 1 DIF: 2 REF: Page 386OBJ: 13.1.1 Use the kinetic-molecular theory to explain the behavior of gases.NAT: UCP.2 | B.2 | B.4 STA: 4g | 2dTOP: Use the kinetic-molecular theory to explain the behavior of gases.KEY: Kinetic-molecular theory MSC: 1

107. ANS:

The molecules of cooking oil are nonpolar, and the electron clouds of nonpolar molecules repel each other forming a weaker attraction. Table salt molecules are polar, and the negative and positive regions of these molecules are strongly attracted to the oppositely charged regions of adjoining molecules forming strong dipole-dipole forces.

PTS: 1 DIF: 2 REF: Page 393 | Page 394OBJ: 13.2.1 Describe and compare intramolecular and intermolecular forces.NAT: B.2 | B.4 STA: 2dTOP: Describe and compare intramolecular and intermolecular forces.KEY: Dipole-dipole force MSC: 3

108. ANS:During evaporation, the water molecules are present at the surface of the liquid in the form of vapor. Vapor exerts a pressure on the liquid known as vapor pressure. When a liquid is heated, the molecules tend to escape from the surface of the liquid. If the heating is continued, the process of evaporation takes place throughout the whole liquid. At this stage, the vapor pressure of a liquid equals the atmospheric pressure. This process is called the boiling of the liquid.

PTS: 1 DIF: 2 REF: Page 405 | Page 406OBJ: 13.4.1 Explain how the addition and removal of energy can cause a phase change.NAT: UCP.3 | B.2 | B.4 | B.6 STA: 7cTOP: Explain how the addition and removal of energy can cause a phase change.KEY: Evaporation | Boiling point elevation MSC: 2

109. ANS:Due to a decrease in the temperature at night, water vapor in the air loses energy. When low energy water vapor molecules collide with grass, they condense into drops of liquid water. These drops of liquid water are called as dew. The entire process is called condensation.

PTS: 1 DIF: 2 REF: Page 407 | Page 408OBJ: 13.4.1 Explain how the addition and removal of energy can cause a phase change.NAT: UCP.3 | B.2 | B.4 | B.6 STA: 7cTOP: Explain how the addition and removal of energy can cause a phase change.KEY: Condensation MSC: 2

110. ANS:

a. The structure of 2,2,3-pentanetriamine is .

b. The structure of 1,3,5-cyclohexanetriol is .

PTS: 1 DIF: 2 REF: Page 744 | Page 746OBJ: 23.2.2 Draw the structure of alcohols, ethers, and amines.NAT: B.2 STA: 10e TOP: Draw the structure of alcohols, ethers, and amines.

KEY: Structure of amine and alcohol MSC: 2111. ANS:

PTS: 1 DIF: 2 REF: Page 755OBJ: 23.4.2 Use structural formulas to write equations for reactions of organic compounds.NAT: B.2 | B.3 STA: 10eTOP: Use structural formulas to write equations for reactions of organic compounds.KEY: Dehydration reaction MSC: 2

112. ANS:

a. Vinyl chloride

b. Tetrafluoroethylene

PTS: 1 DIF: 2 REF: Page 763OBJ: 23.5.1 Describe the relationship between a polymer and the monomers from which it forms.NAT: B.2 | B.3 STA: 10bTOP: Describe the relationship between a polymer and the monomers from which it forms.KEY: PVC | Teflon MSC: 2

113. ANS:Glycine

PTS: 1 DIF: 2 REF: Page 776OBJ: 24.1.1 Describe the structures of amino acids and proteins.NAT: B.2 | C.5 STA: 10a | 10c | 10fTOP: Describe the structures of amino acids and proteins. KEY: Amino acidsMSC: 1

114. ANS:Three-dimensional protein structures exist in helix and pleated sheets shapes. Long chains of amino acids fold into these shapes due to the intermolecular attractions among them.

PTS: 1 DIF: 1 REF: Page 778OBJ: 24.1.1 Describe the structures of amino acids and proteins.NAT: B.2 | C.5 STA: 10a | 10c | 10fTOP: Describe the structures of amino acids and proteins. KEY: Amino acids | ProteinsMSC: 2

PROBLEM

115. ANS:3.80 10 9 m

PTS: 1 DIF: 1 REF: Page 119OBJ: 5.1.1 Compare the wave and particle models of light. NAT: B.1STA: 1j TOP: Compare the wave and particle models of light.KEY: Wavelength | Frequency MSC: 2 NOT: Wavelength = velocity/frequency.

116. ANS:2.441 m

PTS: 1 DIF: 2 REF: Page 121OBJ: 5.1.1 Compare the wave and particle models of light. NAT: B.1STA: 1j TOP: Compare the wave and particle models of light.KEY: Wavelength MSC: 3 NOT: Wavelength = velocity/frequency.

117. ANS:The wavelength is 242 nm.

PTS: 1 DIF: 2 REF: Page 120OBJ: 5.1.1 Compare the wave and particle models of light. NAT: B.1STA: 1j TOP: Compare the wave and particle models of light.KEY: Wavelength MSC: 3 NOT: Wavelength = velocity/frequency. 1m = 10^9 nm.

118. ANS:The first energy is 4.74 10–19 J.The second energy is 3.24 10–19 J.

PTS: 1 DIF: 3 REF: Page 124OBJ: 5.1.2 Define a quantum of energy and explain how it is related to an energy change of matter.NAT: B.6 STA: 1j | 1hTOP: Define quantum of energy and explain how it is related to an energy change of matter.KEY: Energy levels | Wavelength MSC: 3NOT: Energy = Planck's constant * frequency. Energy = Planck's constant * velocity/wavelength.

119. ANS:3.02 10–19 J

PTS: 1 DIF: 1 REF: Page 124OBJ: 5.1.2 Define a quantum of energy and explain how it is related to an energy change of matter.NAT: B.6 STA: 1j | 1hTOP: Define quantum of energy and explain how it is related to an energy change of matter.KEY: Energy levels MSC: 3NOT: Energy = Planck's constant * frequency.

120. ANS:

The ground state electron configuration of sulfur is [Ne]3s23p4. Its electron dot structure is

PTS: 1 DIF: 2 REF: Page 138OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence

electrons. NAT: B.1 | B.6 STA: 2eTOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.KEY: Electron-dot structure | Valence electrons MSC: 3

121. ANS:Element A belongs to group 6A and element B belongs to group 7A in the periodic table.

PTS: 1 DIF: 1 REF: Page 159OBJ: 6.2.1 Explain why elements in the same group have similar properties.NAT: UCP.1 | B.1 | B.2 STA: 1d | 1gTOP: Explain why elements in the same group have similar properties.KEY: Groups MSC: 1 NOT: Groups indicate the number of valence electrons.

122. ANS:Tellurium

PTS: 1 DIF: 1 REF: Page 157OBJ: 6.1.1 Trace the development and identify key features of the periodic table.NAT: G.3 | B.1 | UCP.1 STA: 1a | 1b | 1c | 1fTOP: Trace the development and identify key features of the periodic table.KEY: Periodic table MSC: 2NOT: Elements are arranged in the increasing order of their atomic numbers. Elements in groups have similar properties.

123. ANS:If n 4, the electron configuration of the element is 1s22s22p63s23p63d14s2. The element is scandium.

PTS: 1 DIF: 3 REF: Page 159OBJ: 6.2.2 Identify the four blocks of the periodic table based on electron configuration.NAT: UCP.1 | B.1 STA: 1d | 1g | 2eTOP: Identify the four blocks of the periodic table based on electron configuration.KEY: Electron configuration | Atomic number MSC: 2NOT: The total number of electrons is 21 with atomic number 21.

124. ANS:The element having the largest size has an electron configuration of [Ne] 3s23p34s23d3. The element having the highest electronegativity has an electron configuration of [Ne] 3s23p5.

PTS: 1 DIF: 2 REF: Page 163 | Page 168OBJ: 6.3.2 Relate period and group trends in atomic radii to electron configuration.NAT: UCP.1 | B.1 | B.2 STA: 1c | 2gTOP: Relate period and group trends in atomic radii to electron configuration.KEY: Electron configuration | Atomic size | Electronegativity MSC: 2NOT: The size of the atom depends on the number of shells in an atom. Electronegativity increases across a period.

125. ANS:The arrangement of elements in the increasing order of their atomic size is B < A < D < C. Element B is the smallest and Element C is the largest.

PTS: 1 DIF: 1 REF: Page 163OBJ: 6.3.2 Relate period and group trends in atomic radii to electron configuration.NAT: UCP.1 | B.1 | B.2 STA: 1c | 2gTOP: Relate period and group trends in atomic radii to electron configuration.KEY: Atomic size | Electron configuration MSC: 2

NOT: The size of an atom depends upon the number of shells in an atom. In the same period, the atomic size decreases from left to right.

126. ANS:

PTS: 1 DIF: 1 REF: Page 160OBJ: 6.2.2 Identify the four blocks of the periodic table based on electron configuration.NAT: UCP.1 | B.1 STA: 1d | 1g | 2eTOP: Identify the four blocks of the periodic table based on electron configuration.KEY: Electron-dot structure MSC: 1NOT: Groups indicate the number of valence electrons. Periods indicate the number of shells in an atom.

127. ANS:There are two lone pairs of electrons and there are four electrons involved in the process of bonding with the hydrogen atoms.

PTS: 1 DIF: 2 REF: Page 252OBJ: 9.3.1 List five basic steps used in drawing Lewis structures.NAT: B.1 STA: 2e TOP: List five basic steps used in drawing Lewis structures.KEY: Lone pair | Bond pair MSC: 2

128. ANS:Two pairs of electrons are needed to form bonds in the compound. The central element has two lone pairs of electrons.

PTS: 1 DIF: 2 REF: Page 252OBJ: 9.3.1 List five basic steps used in drawing Lewis structures.NAT: B.1 STA: 2e TOP: List five basic steps used in drawing Lewis structures.KEY: Lewis structure | Lone pair | Bond pair MSC: 2

129. ANS:The central element possesses three lone pairs of electrons and it fulfills its octet.

PTS: 1 DIF: 2 REF: Page 252OBJ: 9.3.1 List five basic steps used in drawing Lewis structures.NAT: B.1 STA: 2e TOP: List five basic steps used in drawing Lewis structures.KEY: Lewis structure | Lone pair | Bond pair MSC: 2

130. ANS:3.70 105 J/mol

PTS: 1 DIF: 1 REF: Page 387OBJ: 13.1.1 Use the kinetic-molecular theory to explain the behavior of gases.NAT: UCP.2 | B.2 | B.4 STA: 4g | 2dTOP: Use the kinetic-molecular theory to explain the behavior of gases.KEY: Kinetic-molecular theory MSC: 3NOT: The kinetic energy of a particle is 1/2 mv^2.

131. ANS:6.93 J/(g °C)

PTS: 1 DIF: 2 REF: Page 492OBJ: 16.1.3 Calculate the amount of heat absorbed or released by a substance as its temperature changes.NAT: UCP.3 | B.6 STA: 7c | 7dTOP: Calculate the amount of heat absorbed or released by a substance as its temperature changes.KEY: Specific heat MSC: 3NOT: Specific heat = absorbed heat/mass of gold * (final temperature - initial temperature)

132. ANS:4.07 103 J/(g °C)

PTS: 1 DIF: 2 REF: Page 492OBJ: 16.1.3 Calculate the amount of heat absorbed or released by a substance as its temperature changes.NAT: UCP.3 | B.6 STA: 7c | 7dTOP: Calculate the amount of heat absorbed or released by a substance as its temperature changes.KEY: Specific heat MSC: 3NOT: Specific heat of substance = absorbed energy/mass of substance * (final temperature - initial temperature)

133. ANS:1.94 103 J

PTS: 1 DIF: 2 REF: Page 493OBJ: 16.1.3 Calculate the amount of heat absorbed or released by a substance as its temperature changes.NAT: UCP.3 | B.6 STA: 7c | 7dTOP: Calculate the amount of heat absorbed or released by a substance as its temperature changes.KEY: Heat MSC: 3NOT: Absorbed heat = mass of water * specific heat of water * (final temperature - initial temperature).

134. ANS:0.367 J/(g °C)

PTS: 1 DIF: 1 REF: Page 497OBJ: 16.2.1 Describe how a calorimeter is used to measure energy absorbed or released.NAT: B.5 | B.6 STA: 7dTOP: Describe how a calorimeter is used to measure energy absorbed or released.KEY: Calorimeter MSC: 3NOT: Specific heat of metal = absorbed heat/mass of metal * change in temperature.

135. ANS:3.56 103 J

PTS: 1 DIF: 2 REF: Page 497OBJ: 16.2.1 Describe how a calorimeter is used to measure energy absorbed or released.NAT: B.5 | B.6 STA: 7dTOP: Describe how a calorimeter is used to measure energy absorbed or released.KEY: Calorimeter MSC: 3NOT: Absorbed heat = mass of substance * specific heat of substance * (final temperature - initial temperature).

136. ANS:4.70 104 J

PTS: 1 DIF: 1 REF: Page 496OBJ: 16.2.1 Describe how a calorimeter is used to measure energy absorbed or released.NAT: B.5 | B.6 STA: 7d

TOP: Describe how a calorimeter is used to measure energy absorbed or released.KEY: Calorimeter | Energy levels MSC: 3NOT: Heat = mass of water * specific heat of water * change in temperature.

137. ANS:6.44 kJ

PTS: 1 DIF: 2 REF: Page 504OBJ: 16.3.2 Describe how energy is lost or gained during changes of state.NAT: B.3 | B.5 | B.6 STA: 7cTOP: Describe how energy is lost or gained during changes of state.KEY: Molar enthalpy of fusion MSC: 3NOT: Convert grams of methanol to moles of methanol (64 g methanol * 1 mol methanol/32 g methanol). Calculate required heat by using the formula, required heat = 64 g methanol * 1 mol methanol/32 g methanol * 3.22 kJ/mol.

138. ANS:

5-ethyl-3,4,4-trimethyloctane

PTS: 1 DIF: 2 REF: Page 703OBJ: 22.1.2 Name an alkane by examining its structure. NAT: B.2STA: 10d TOP: Name an alkane by examining its structure.KEY: Nomenclature MSC: 2NOT: Select the longest chain and number it such that the lowest possible number positions are given to alkyl groups.

139. ANS:

a.

b.

In ethene, two electron pains are shared between the carbon atoms, and in ethyne, three electron pairs are shared between the carbon atoms.

PTS: 1 DIF: 2 REF: Page 710OBJ: 22.2.4 Distinguish between saturated and unsaturated hydrocarbons.NAT: B.2 STA: 10dTOP: Distinguish between saturated and unsaturated hydrocarbons.KEY: Structure | Unsaturated hydrocarbons MSC: 2NOT: Draw the structure of compounds on the basis of the four electrons present in the valence shell of carbon.

140. ANS:5-ethyl-4-methylnonane

PTS: 1 DIF: 3 REF: Page 703OBJ: 22.1.2 Name an alkane by examining its structure. NAT: B.2

STA: 10d TOP: Name an alkane by examining its structure.KEY: Nomenclature of alkane MSC: 2NOT: Identify the longest carbon atom chain. Number the chain such that the alkyl groups get the minimum value of numbers. Write the name of the alkyl groups in an alphabetic order.

141. ANS:

1-ethyl-4-propyl-1-cyclohexene

PTS: 1 DIF: 3 REF: Page 712OBJ: 22.3.3 Name an alkene or alkyne by examining its structure.NAT: B.2 STA: 10d TOP: Name an alkene or alkyne by examining its structure.KEY: Nomenclature MSC: 2NOT: The lowest possible numbers are given to substituents on the cyclic ring.

142. ANS:a. Etherb. Amine

PTS: 1 DIF: 1 REF: Page 745OBJ: 23.2.1 Identify the functional groups that characterize alcohols, ethers, and amines.NAT: B.2 STA: 10eTOP: Identify the functional groups that characterize alcohols, ethers, and amines.KEY: Functional groups MSC: 2NOT: a) Ethers contain an oxygen atom bonded to two carbon atoms. b) Amines contain a nitrogen atom bonded to a carbon atom in an aliphatic chain or aromatic ring.

143. ANS:

a. Amide

b. Ester

c. Carboxylic acid

d. Ketone

PTS: 1 DIF: 2 REF: Page 748 | Page 749 | Page 750 | Page 752OBJ: 23.3.1 Draw and identify the structures of carbonyl compounds including aldehydes, ketones, carboxylic acids, esters, and amides. NAT: B.2 STA: 10eTOP: Draw and identify the structures of carbonyl compounds including aldehydes, ketones, carboxylic acids, esters, and amides. KEY: Carbonyl compoundsMSC: 2NOT: a) Amides have CONH2 group. b) Esters have COOR group. c) Acids have COOH group. d) Ketones have RCOR group.

144. ANS:Hydroxyl

PTS: 1 DIF: 3 REF: Page 738OBJ: 23.1.1 Describe a functional group and give examples. NAT: B.2STA: 10e TOP: Describe a functional group and give examples.KEY: Functional groups MSC: 2NOT: A functional group in an organic molecule is an atom or group of atoms that always reacts in a certain way. The addition of a functional group to a hydrocarbon structure always produces a substance with physical and chemical properties that differ from those of the parent hydrocarbon.

145. ANS:Propyl butanoate

PTS: 1 DIF: 3 REF: Page 750OBJ: 23.3.1 Draw and identify the structures of carbonyl compounds including aldehydes, ketones, carboxylic acids, esters, and amides. NAT: B.2 STA: 10eTOP: Draw and identify the structures of carbonyl compounds including aldehydes, ketones, carboxylic acids, esters, and amides. KEY: Esters MSC: 2NOT: The name of an ester is formed by writing the name of the alkyl group followed by the name of the acid. The suffix -ic of the acid is replaced by -ate.

ESSAY

146. ANS:a. Use the distillation technique to separate and identify the components.b. Distillation is a separation technique that is based on the differences in the boiling points of the

substances involved. In the distillation of methanol and water, the mixture is heated until methanol boils to form vapor. The vapor is then condensed into a liquid and collected separately.

c. When precisely controlled, distillation can separate substances having boiling points that differ by only a few degrees.

PTS: 1 DIF: 2 REF: Page 69OBJ: 3.3.3 List and describe several techniques used to separate mixtures.NAT: B.2 STA: 6fTOP: List and describe several techniques used to separate mixtures.KEY: Distillation MSC: 3

147. ANS:a. 2b. 4sc. 2+

PTS: 1 DIF: 2 REF: Page 213OBJ: 8.1.3 Describe the formation of positive and negative ions.NAT: B.1 STA: 1c | 2a TOP: Describe the formation of positive and negative ions.KEY: Cation MSC: 2

148. ANS:a. Lithium has only 1 valence electron.b. Lithium loses its outermost lone electron from the 2s orbital to attain the stable configuration of helium.c. Li O

PTS: 1 DIF: 2 REF: Page 215OBJ: 8.2.1 Describe the formation of ionic bonds. NAT: B.1 | B.4STA: 2a TOP: Describe the formation of ionic bonds.KEY: Ionic bond MSC: 2

149. ANS:a. 1 molecule N2 + 3 molecules H2 2 molecules NH3

b. 1 mole N2 + 3 moles H2 2 moles NH3

c. 28.02 g N2 + 6.06 g H2 34.08 g NH3

PTS: 1 DIF: 2 REF: Page 355OBJ: 12.1.2 Determine the mole ratios from a balanced chemical equation.NAT: UCP.3 | B.3 STA: 3a | 3dTOP: Determine the mole ratios from a balanced chemical equation.KEY: Mole ratio MSC: 1

150. ANS:a. 4 atoms Zn + 10 molecules HNO3 4 formula units Zn(NO3)2 + 1 molecule N2O + 5 molecules H2Ob. 4 moles Zn + 10 moles HNO3 4 moles Zn(NO3)2 + 1 mole N2O + 5 moles H2Oc. 261.56 g Zn + 630.2 g HNO3 757.56 g Zn(NO3)2 + 44.02 g N2O + 90.10 g H2O

PTS: 1 DIF: 2 REF: Page 355OBJ: 12.1.2 Determine the mole ratios from a balanced chemical equation.NAT: UCP.3 | B.3 STA: 3a | 3dTOP: Determine the mole ratios from a balanced chemical equation.KEY: Mole ratio MSC: 1

151. ANS:The equation for the combustion of butane is .a. 2 molecules C4H10 + 13 molecules O2 8 molecules CO2 + 10 molecules H2O.b. 2 moles C4H10 + 13 moles O2 8 moles CO2 + 10 moles H2O.c. 116 g C4H10 + 416 g O2 352 g CO2 + 180 g H2O.Mass of reactants Mass of products 532 g.

PTS: 1 DIF: 2 REF: Page 355OBJ: 12.1.2 Determine the mole ratios from a balanced chemical equation.NAT: UCP.3 | B.3 STA: 3a | 3dTOP: Determine the mole ratios from a balanced chemical equation.KEY: Mole ratio MSC: 3

152. ANS:a.b.

c.

PTS: 1 DIF: 3 REF: Page 700OBJ: 22.1.1 Describe the structures of alkanes. NAT: UCP.1 | B.2STA: 10b TOP: Describe the structures of alkanes. KEY: Structure and formula of alkaneMSC: 2

153. ANS:

a.

b.c. Temperature variations, ionic strength, and pH are the main causes of denaturation in proteins.

PTS: 1 DIF: 2 REF: Page 776 | Page 778OBJ: 24.1.1 Describe the structures of amino acids and proteins.NAT: B.2 | C.5 STA: 10a | 10c | 10fTOP: Describe the structures of amino acids and proteins. KEY: Peptide | Amino acidsMSC: 2

154. ANS:

a. Sucrose + H O Glucose + Fructose

b. Maltose + H O Glucose + Glucose

c. Lactose + H O Glucose + Galactose

PTS: 1 DIF: 2 REF: Page 782OBJ: 24.2.1 Describe the structures of monosaccharides, disaccharides, and polysaccharides.NAT: B.2 STA: 10aTOP: Describe the structures of monosaccharides, disaccharides, and polysaccharides.KEY: Disaccharides MSC: 2

155. ANS:a. Twelve monomers are required to form a complex carbohydrate, which is also called a polysaccharide.b. The new type of bond formed between the monosaccharides is an ether functional group (C—O—C).

c.

PTS: 1 DIF: 2 REF: Page 782OBJ: 24.2.1 Describe the structures of monosaccharides, disaccharides, and polysaccharides.NAT: B.2 STA: 10aTOP: Describe the structures of monosaccharides, disaccharides, and polysaccharides.KEY: Polysaccharides | Monosaccharides | Disaccharides MSC: 2