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CNS: GEAS 4

CHEMISTRY

1.What was the first major demonstration of a chemical reaction that producedheat?

A.mold C. iceB.fire * D. earthquake

2.During the Dark Ages, alchemistsA.promised to turn lead into goldB.were the first true experimenting chemistsC.discovered crystallization and distillation proceduresD.all of these *

3.A hypothesis isA.container or performing experimentsB.way to describe heat transfer between mineralsC.sterile medical deviceD.statement or idea that describes or attempts to explain observable

information*

4.Which early scientist accurately described the configuration of the Sun, Moonand planets in relationship to each other?

A.Linus Pauling C. Nicolas Copernicus *B.Claudius Ptolemy D. Leonardo da Vinci

5.An experiment isA.controlled testing of the properties of a substance or system through

carefully recorded measurements *

B.an uncontrolled testing of the properties of a substance or system throughcarefully recorded measurements

C.a one-time reporting of a few observable characteristicsD.a bad choice brought on by peer pressure

6.Who is said to be the founder of the scientific method?A.Alexander Fleming C. Galileo Galilei *B.Joseph Priestly D. Antone Lavoisier

7.A theoryA.accounted for a rulers need to produce gold from zincB.is the result of sudden aspiration during a lightning stormC.predicts the outcome of new testing based on past experimental data*D.is a type of atomic particle

8.John Dalton proposed the first theory onA.the rotation of the satellite around SaturnB.the characteristics of individual atoms and particles*C.the complex interaction of solids when meltedD.the neutralization pfpH

9.A scientific law is baseddescribed asA.a series of rules made by the representatives of the governmentB.a good idea that many people agree voluntarilyC.the transmutation of lead into goldD.a hypothesis or theory that is tested repeatedly with the same results and

thought to be without exception*

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10. The law of partial pressures can be best described by the followingequation:

A.Ptotal= P1 + P2 + P3*B.Ptotal= (P1 + P2)/ P3C.Ptotal= (P1 + P2 ) D.Ptotal= 2(P1 + P2 + P3)

11. Chemistry is known asA.an attraction between two peopleB.an exact scienceC.an experimental science *D.a method to describe units of heat

12. In 1670, Gabriel Mouton suggestedA.a law of partial pressuresB.the boiling point of alcoholC.The Sun as the center of the universeD.a decimal system of measurement *

13. The International System of Units (SI) ha how many base units?A.4 B. 6 C. 7 * D. 9

14. Exponential or scientific notation isA.method where numbers are written in powers of 10 *B.a shorthand method of number accountingC.a way to write very large and very small numbersD.all of these

15. The number of digits recorded in a measurement isA.always whole numbersB.significant digits or figures *C.a way to count on your fingersD.the method of including all zeros

16. Precision is described asA.more accurate than excisionB.less accurate than two significant digitsC.the closeness of two sets of measured groups of values *D.the equal spacing of numbers around a common number

17. Accuracy isA.more precise than two significant digitsB.the closeness pf two sets of measured groups of valuesC.only applicable to experimental measurementD.the closeness of a single measurement to its true value *

18. Rounding is used primarily toA.sum up significant figuresB.drop non-significant digits in calculation *C.drop digits greater than 5D.increase all numbers to the most certain number

19. Conversion factors make use ofA.relationship between two units or quantities in fractional form *B.the fact that units are always written as whole numbersC.numbers which cannot be divided into smaller unitsD.a direct connection between weight and volume

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20. Which of the units blow is an example of SI derived units?A.cm/m C. m/kg2B.m/s2 D. m/ft2

Properties of Matter

21. Matter isA.a legal termB.something found in the lower atmosphereC.anything that has mass and occupies space *D.anything that can be seen

22. AtomsA.are found only in solid materialsB.were thought to next to the smallest particlesC.were first found in antsD.contain particles such as protons and neutrons *

23. Physical properties of matterA.contain all heat-bearing compoundsB.include color, form, density, and boiling point *C.are only visible under ultraviolet lightD.are directly related to muscle mass

24. Pure substancesA.are homogenous and have unchanging chemical composition *B.are heterogeneous and have unchanging chemical compositionsC.seldom exist in natureD.are found in cubic form only

25. Antoine LavoisierA.is called the father of modern chemistryB.

identified 33 elements

C.should have stayed away from government taxationD.all of these *

26. SolidsA.have measurable volume and can change shapeB.are always heavy to transportC.are fixed and rigid with a measurable volume *D.change shape with little effort

27. Chemical propertiesA.describe a materials behaviour when acted on by something else *B.are those things that can be seenC.are associated with waters freezing pointD.are defined as solids, liquids, and gases

28. An elementA.is an animal, vegetable, or mineralB.is made up of pure chemical and not divided into simpler parts *C.can be separated into neutrons and protonsD.is a six-sided solid

29. PercentA.comes from the Latin word machine

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B.can be calculated for diamond facetsC.is the number of parts of one material found in another *D.is an ancient form of Greek counting

30. Barium isA.green in color and melts at 627CB.never used in medicineC.a different compound completely when meltedD.silvery white and found in the solid state *

Elements, Symbols, and the Periodic Table

31. When John Newlands made a list of the elements in the 1860s, heA.noticed the list seemed far longer than he rememberedB.wrapped the list around his favourite mineral sampleC.saw that the elements lined up and repeated in groups of eight *D.sae similarities between elements and called it Newlands rule

32. Who published Die Modernen Theorien der Chemie in 1864?A.Johnnes KeplerB.Lothar Meyer *C.Antonie Baguyer de ChancourtoisD.Dimitri Mendeleyv

33. Currently, the modern Periodic Table contains how many elements?A.57B.88C.109D.between 112 and 118 depending which research papers you read *

34. Which of the following is not an elemental family group?A.halogen C. alkali metalB.rare Earth D. alloy *

35. The following are all names for the element sulphur, exceptA.schwefel C. selenur *B.svavel D. azufre

36. Over 100 years ago, the Periodic table contained gaps becauseA.experimental data hinted at elements in between known elements *B.researchers couldnt agree on which elements to includeC.experimental equipment wasnt accurate enough to find elementsD.scientists didnt transcribe earlier Periodic Tables correctly

37. The formula (C6H4Cl)2CHCCl3is shorthand for what compound?A.acetyl chlorideB.dichlorodiphenyltrichloroethane*C.polypropylene dichlorideD.chlorofluorocarbon

38. The standardized system of naming chemical compounds is calledA.the Bernouli rule C. chemical nomenclature *B.the Periodic Table D. the Octave rule

39. All the metals listed below are solid at room temperature exceptA.mercury * C. molybdenumB.tin D. iron

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40. The 28 elements potassium(K) through krypton (Kr) are found inA.group 7 of the Periodic TableB.period 6 of the Periodic TableC.goupr 5 of the Periodic TableD.period 4 of the Periodic Table *

Atoms, Elements, and Compounds

41. Electrons areA.sub-atomic particles with a +1 chargeB.equal to the number of protons in a nucleus *C.said to be charmedD.sub-atomic particles with a +2 charge

42. The plum pudding model of an atom was replaced bu theA.orbital theory of protons and neutrons *B.plum pudding model with currantsC.Meyer model of electronsD.Octave rule

43. The modern concept of the atom was developed byA.E. W. Muller C. Lothar MeyerB.J.J. Thomson D. Ernest Rutherford

44. Protons share the dense nucleus withA.neutrons * C. quarksB.molecules D. atoms

45. The arrangement of atoms in a molecule canA.cause explosive reactionsB.affect the reactivity of a moleculeC.mean the difference between hadronsD.

predict when it will be discovered *

46. The force that binds two or more atoms together is known asA.chemical bond * C. joulesB.valence D. electromagnetism

47. A structural formula showsA.the calculated distance between atomsB.the molecular weight of a moleculeC.the valency of oxygenD.how an element is connected to others in a molecule *

48. An atomA.is 10-8Angstroms in diameterB.is composed of different sub-particles *C.has only two electrons in each orbital shellD.is classified as strange and charmed

49. A molecular formulaA.gives the total number of moles in a compoundB.is used only in derived chemical compoundsC.gives the number of each elemental atom in a molecule *D.is handy to have, but doesnt include all the elements

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50. The neutron is a sub-atomic particleA.with no electric charge *B.with a -1 electric chargeC.smaller than an electronD.with n counterpart within the atom

Electron Configuration

51. The Aufbau principleA.defines the undefined particles of the nucleusB.is a method used to describe an atoms ground state *C.provides radioactive levels of elementsD.lists the negative and positive spin of atoms

52. Electrons haveA.a positive chargeB.are unreactive in the metal groupC.serve as the glue between nuclei of atoms *D.have only two outermost orbits

53. Ionization energy of an elementA.is the amount of thrust needed to fly at mach speedB.is the energy a neutron generatesC.cannot be calculated or observedD.is the energy needed to detach an electron from an elemental atom *

54. Noble gasesA.are highly reactive with heliumB.are highly reactive with strontiumC.are unreactive under normal conditions *D.are not related to nobility

55. A bond between atoms in a molecule isA.

made up of a shared electron pair *

B.stronger than static electricityC.always located in the 3s orbitalD.only a double bond

56. Elements in column IV of the Periodic Table haveA.three electrons with which to create bondsB.four electrons with which to create bonds *C.five electrons with which to create bondsD.unreactive bonding electrons for other elements

57. The electron configuration of an atomA.is determined by the amount of kinetic energy presentB.is found by calculating atomic massC.is written as s, p, d, and f subshellsD.described the specific distribution of electrons in a subshell *

58. Freidrich Hund worked onA.calculating the energy signature of calciumB.the nature of electron spinC.the lowest energy arrangements of subshells electrons *D.his familys tulip farm until he was twelve

59. The number of bonds an atom can form with other atoms

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A.depends on its overall sizeB.is calculated using orbital theoryC.depends on the specific gravity of the atomD.depends on the number of electrons it can share *

60. The Pauli exclusion principle states thatA.any atoms with a free s orbital can form bondsB.no two can occupy the same orbital unless their spins are different *C.two atoms sharing an orbital are matched exactlyD.atoms of the same configuration do not change

Concentration and Molarity

61. ConcentrationA.is most important to understand chemistryB.is the volume per velocity of molecular movementC.can mean the difference between life and death *D.is found by mixing a weak acid and strong acid

62. Percent mass of solutionA.is used to find the amount of solute in solvent *B.is used to weigh grams onto a scientific balanceC.never uses the total mass of the soluteD.can be achieved without knowing the atomic weight of the chemicals involve

63. Chemical concentrations are most often expressed asA.ppc (parts per centimeters)B.ppb (parts per billion)C.pgs (parts per gram solvent)D.ppm (Parts per million) *

64. MolarityA.equals massB.

is used to find general amounts

C.equals concentration *D.has the opposite function of polarity

65. A moleA.has 102atoms in a sampleB.has the same number of atoms in a sample as 12 grams of 12C *C.is a small, black, furry rodent that lives undergroundD.is seldom used in modern chemical calculations

66. Avogadros numberA.is equal to 6.02 x 1023atoms or molecules *B.is equal to 4.02 x 1023atoms or moleculesC.is equal to 2.60 x 1023atoms or moleculesD.is equal to 23.02 x 106atoms or molecules

67. Avogadros numberA.was first suggested by Anastasia AvogadroB.has never been proven decisivelyC.is used to calculate the number of electrons in a sampleD.is equal to one mole *

68. Empirical formulasA.show the elements proportions in a compound

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B.indicate probable ideal gas combinationsC.are always the same as the molecular formulaD.give the whole number ration of elements in a compound *

69. Molar mass (MM) is measured inA.moles/solute C. grams/mole *B.grams/liter D. moles/solvent

70. In order to convert mass to moles, you needA.a calculatorB.a list of atomic masses *C.the boiling point of the solventD.a very sensitive scale

The Hydrogen Atom

71. Hydrogen is key toA.the making of candle waxB.bonding with carbon in organic molecules *C.radioactive reactionsD.the formation of ozone

72. The atomic number of hydrogen isA.1 * C. 3B.2 D. 4

73. In water molecules, how many oxygen atoms) combine with hydrogen atoms?A.1 C. 3B.2 * D. 4

74. Reduction if the process ofA.calculating the oxidation number of oxygenB.increasing the oxidation number of hydrogenC.

losing hydrogen or electrons in a reaction

D.gaining hydrogen or electrons in a reaction *75. Hydrogen makes up roughly what % of the universes visible mass?

A.33% C. 70%B.50% D. 90% *

76. Oxidation isA.a (-) loss in oxidation number*B.a (+) gain in oxidation numberC.only possible with oxygenD.a new form of acne medication

77. When hydrogen sulphide burns in oxygen, the productsA.are oxygen and sulphurB.are water and sulphur oxide *C.smell like tea tree oilD.smell like almonds

78. The number used to track electrons in a reaction is theA.atomic number C. ionization numberB.reactant number D. oxidation number *

79. What are the parts of the opposite theory?

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A.organic and inorganic elementsB.crystallizations and condensationC.oxidation and reduction *D.metals and non-metals

80. When one element causes he oxidation of another element, it isA.oxidized C. reduced *B.an acid D. a base

Atomic Numbers and Ions

81. Monatomic ionsA.are pretty boring C. have only one atom *B.have less than one oxygen D. contain actinium

82. 82. The chemical prefix bu meansA.two atomsB.double the number of atomsC.containing hydrogen *D.containing oxygen

83. Polyatomic ionsA.have more than one atom *B.less than one ion of oxygenC.have only one type of atomD.contain polonium

84. The chemical prefix hypo meansA.less than one nitrogen atomB.triple the number of hydrogen atomsC.contains sulphurD.contains one less oxygen atom *

85.

Gaps were included in the first Periodic TableA.because they didnt understand the octet ruleB.to allow for undiscovered elements *C.to make it easier to write on one pageD.to eliminate arguments about placement

86. Polyatomic ionsA.have no charge C. have ionic bondsB.have an overall charge * D. contain only oxygen

87. 87. Iron can form how many ions?A.4 C. 2 *B.3 D. 1

88. Germanium wasA.discovered by a Swiss chemistB.named from the Greek word for geraniumC.discovered in 1862D.slid into an open gap in the first Period Table *

89. Mendelevium with an atomic number 101A.has 101 protons *B.was named after the scientist Gregor MendelC.was discovered in 1855

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D.has no isotopes90. In chemistry, the lowest common multiple is

A.a negative factor used in general mathematicsB.easiest to use when the charge from one ion is used as the multiplier for

the other ion *

C.was first used by Albert EinsteinD.is only used in group IIA of the Periodic Table

Organic Chemistry and Functional Groups

91. Organic chemistry is based onA.nitrogen compoundB.protein polymerizationC.carbon-based compounds *D.the theory of particle-wave chemistry

92. Which of the following does not contain carbon?A.carbohydrates C. synthetic fibersB.jet fuel D. table salt *

93. The simplest hydrocarbon molecule isA.methane * C. propaneB.ethane D. butane

94. The bond between the carbons in the ethane isA.single bond C. double bond *B.triple bond D. quadruple bond

95. Tetrahedral bonding angles of carbon are aboutA.20 degrees C. 90 degreesB.45 degrees D. 109 degrees *

96.

96. Alkanes areA.formed from NH2 groupsB.an example of homologous series *C.composed of many different element groups.D.only found in organic compound reactions

97. Since ethyne is a linear molecule, the two carbons form a triple bond ofA.180 degree angles * C. 120 degree anglesB.45 degree angles D. 109 degree angles

98. Bond polarityA.occurs in the northern hemisphere of the globeB.occurs when electron pairs are unequally shared between atoms *C.was discovered in 1862D.is best seen in group VIII of the Periodic Table

99. Saturated hydrocarbon compoundsA.contain many double bonds in long chainsB.contain triple bonds to oxygen moleculesC.are open to hydrogen bondingD.contain only single bonds *

100. Carbon isA.the element that bonds with sulphur to from cyanide

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B.unable to from triple bonds with nitrogenC.found in greater than 95% of all known chemicals *D.number 8 in the Periodic Table and has an atomic weight of 16

Radiochemistry

101. Radioactivity is best described asA.a radio signal accompany by energy flowB.violent reaction with waterC.extremely low levels of visible energy releaseD.spontaneous disintegration of isotopes and radiation emission *

102. Frederick Soddy named isotopes from the Greek word iso meaningi)A. glowing C. easily seenii) B. same place * D. brittle

103. Elements with the same number of protons, but a different number of neutroare called

i)A. alkali metals C. isotopes *ii) B. electron receptors D. covalent bonds

104. Beta () particles areA.ions of neutral chargeB.negatively (-) charged particles *C.positively (+) charged particlesD.non-existent in universe

105. Tritium hasA.1 electron and 1 protonB.1 electron and 1 neutronC.2 protons and 2 electronsD.1 proton and 2 neutrons *

106.What is heavy water?

A.water with mercuryB.water made mostly from deuterium and oxygen *C.water made from 2 molecules of hydrogenD.an unreactive, neutral form of distilled water

107. What is the atomic number of 24Mg?A.8 C. 22B.12 * D. 37

108. Radioactive decay generallyA.occurs within secondsB.gives off a great amount of heatC.takes place as a transforming process over yearsD.all of these *

109. Which of the following are all magic numbers?A.2, 8, 20, 28, 50, 82, 114 *B.2, 8, 20, 26, 82C.2, 8, 12, 22, 50, 82, 114D.2, 8, 18, 24, 48, 60, 82

110. Transmutation occurs when theA.electrons are thrown off in a reaction

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B.low-speed interaction occurs between metalsC.neutrons have the same magic number as electronsD.nucleus of an element is hit by particles of another element *

Metals

111. Which of the following element groups are most widely known?A.halogens C. transition metals *B.metalloids D. lanthanides

112. Which element is the best conductor of electricity?A.gold C. copperB.silver * D. aluminium

113. Most metals are naturally fondA.as pure metalsB.in limestone rockC.in steam bedsD.combined with other elements in ores *

114. Gold isA.the most malleable and ductile metal *B.not used in jewelryC.not an obsession for alchemistsD.always used to fill cavities in teeth

115. How do electrons behave in metal elements?A.they are highly reactiveB.they form long, linear moleculesC.they float around in metal ions like broth *D.they react in ion pairs

116. What is re benefit of electron sharing?A.

the bonds are easily broken

B.softer, more ductile alloys are formedC.inner shell electrons can be usedD.it is a much more efficient use of energy *

117. Which metal wins the friendliest award?A.sodium B. nickel C. mercury D. iron *

118. Which two metals combine to give galvanized metal?A.lead and iron C. silver and aluminumB.zinc and iron * D. lead and silver

119. Which of the following elements are stored in oil to prevent explosions?A.lithium * C. ytterbiumB.actinium D. strontium

120. When naming compoundsA.metals come after metal saltsB.two non-metals are named alphabeticallyC.metal come before hydrogenD.metals come before non-metals *

121. A chemical bond is aA.good interaction between friends

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B.poor possibility with alkali metalsC.relationship between atoms in a molecule *D.heat sensitive reaction inside the nucleus

122. Generally, ionic bonds form betweenA.two metals *B.a metal and oxygenC.a metal and a halogenD.two non-metals and two carbons

123. Ionic bond occursA.with only one type of anionB.in the presence of high temperatureC.when electrons are transferred from one element to another *D.in the presence of uranium

124. Electronegativity describes theA.bad attitudes of chemists when experiments dont worlB.inability to maintain chargeC.electron loss in a covalent bondD.ability of an atom in a covalent bond to pull electrons to itself *

125. The shared electron pair in a molecule is calledA.ionic bonding C. non-polar ionic bondingB.covalent bonding* D. isomer transfer

126. The ease with which electrons are lost in a covalent bond is though of asA.electropositivity* C. valence exchangeB.electronegativity D. electromagnetism

127. Which American chemist first described the electrical difference of bonds?A.Antoine Lavoisier C. Albert EinstienB.Stephen Hawking D. Linus PAuling *

128. Which of the following is the most electronegative element?A.gold C. bromineB.silver D. fluorine *

129. A dipole momentA.describes the diatomic formation of two elementsB.occurs when all electrons circle the nucleus equallyC.is a measurement of the charge separation in parts of a molecule *D.is composed of two polonium isotopes

130. When electrons are shared unequallyA.no reaction occursB.it is called polar covalent bonding *C.the electrical charge is always positiveD.only group IIA elements of the Periodic Table will react

Acids and Bases

131. Which of the following is not a property of an acid?A.has a pH > 7.0 *B.releases hydrogen (H+) ions when added to waterC.causes chemical burnsD.none of these

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132. A baseA.has a pH < 7.0B.does not cause chemical burnsC.does not ionize in waterD.is any solution that releases hydroxide (OH) ions in water *

133. The pH scale measuresA.the weight of a liquidB.the acidity of a liquid *C.the temperature of a liquidD.the density of a liquid

134. Which of the following is not a rule of thumb for deciding whether or noa solution is an acid?

A.in dilute solutions, acids taste bitter *B.litmus paper changes from blue to redC.acids react with metals like iron, magnesium, and zinc and release hydroge

gas

D.when combined with bases, the products are water and salt135. Which of the following is not a rule of thumb for deciding whether or noa solution is a base?

A.In dilute solutions, bases taste bitterB.litmus paper changes from red to blueC.bases react with acid to form water and saltD.bases feel sticky and tacky between the fingers on the skin *

136. 136. An acid is considered a strong acid whenA.combined with a base and gives off a very pungent odorB.it has a pH value > 9.0C.it completely ionizes in water and gives up a proton to water to from a

hydronium ion, H3O+*

D.it has strong conjugate base

137. A Bronsted-Lowry acidA.changes litmus paper from red to blueB.donates a proton in a reaction while a base is on the receiving end of the

proto transfer *

C.is a classification of a strong acidD.ionizes almost completely water

138. To be amphotericA.a stronger acid will be transformed into products that include a weaker acB.it is the element in the reaction that oxidizes another element while at t

same time being reduced itself

C.a stronger base ionizes almost completely in water, while weak bases do noD.an ion or more molecule an serve as either an acid or base in a reaction,

but has no protons (H+)

139. Oxidation isA.when a compound loses oxygen, gains hydrogen or gains electronsB.when a solution releases hydrogen (H+) ions when added to waterC.when a compound gains oxygen, loses hydrogen, or loses electrons *D.when acids and bases can accept protons in one reaction then turn around a

donate in a subsequent reaction

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140. Chemists Johannes Bronsted and Thomas LowryA.created litmus paperB.discovered buffers as sets of compounds that react with and occupy

hydrogen ions (H+) and hydroxide ions (OH-)

C.established the pH scaleD.described acids and bases while studying how proton transfer occurs *

Solids

141. Amorphous solidsA.are generally very denseB.have no specific form *C.become very rigid when heatedD.melt very fast when heated

142. Which of the following is not true of a crystalline solid?A.they are arranged into regular shapes based on a cube; simple, central, a

face centered

B.they can be predictably cut or broken along set linesC.they tend to be very unstable and can change state very easily *D. the atoms go together into specific crystal patterns of an ordered lattic

or framework

143. Which of the following is not a type of solid?A.anatomic* C. covalentB.metallic D. ionic

144. Stable molecules that give them flexibility and allow them to be formed insheets and strands without breaking is a property of what type of soloid?

A.anatomic C.covalentB.metallic * D. ionic

145. A solid that forms a lattice with the outside points made up of ions insteof large molecules is what type of solid?A.anatomic C. covalentB.molecular D. ionic *

146. Which is not a property of a covalent bond?A.The very stable bonding produces high melting and boiling pointsB.The contrasting forces give these solids high melting points *C.They are held together by single covalent bondsD.Nets, chains, and balls of carbon bonded into stable molecules make thes

solids hard and stable

147. The role of temperature in a solid isA.secondary to pressureB.only important to transition metalsC.a major player in what form an element takes at room temperature *D.insignificant

148. Metals found in the middle of the Periodic TableA.share a lot of the same characteristics *B.rarely react with other elementsC.have almost the same properties of goldD.are limited to reaction with oxygens

149. Gases are solids when

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A.there is an excess of oxygen in the reactionB.combined with lead or zincC.not in the liquid phaseD.the pressure is high and he temperature lowered to sub-zero levels *

150. Molecules in solidsA.are always shaped into a latticeB.have very little movement due to high density *C.bond easily to carbonD.are seldom organic in composition

Liquids

151. Density isA.determined by the boiling point of the liquidB.measured in grams per milliliter *C.the capability of the liquid to flow or not flow freelyD.the measurement of how much gas can be dissolved in the liquid

152. Relative density (specific gravity)A.is the ration of the density of a sample in liquid form divided by the

density of the sample in solid formB.is the ratio of the boiling point of liquid at atmospheric pressure divide

by the boiling point of a liquid at two atmospheres

C.measures volume of a sample when placed in waterD.is the ratio of the density of a sample at 20C divided byt eh density of

water at 4C. *

153. Viscosity is theA.temperature at which a liquid turns to a vapor (gas) at atmospheric pressuB.temperature at which a vapor condenses into a liquidC.capability of a liquid to flow or not flow freely at room temperature *D.ability of liquid molecules to turn to vapor

154. In the petroleum industry, the separation of different parts of naturallyoccurring crude oil and the collection of many products is an example of

A.vaporization C. condensationB.surface tension D. fractionation *

155. The stronger the molecular forces between molecules theA.lower the boiling point of a liquidB.more viscous a liquid *C.easier it is to condenseD.weaker the surface tension

156. Surface tensionA.is the force that pulls molecules down and to the sides *B.is tha capability of a liquid to flow or not flow freely at room temperatuC.measures evaporation rate of a liquidD.is the surfave of the liquid where evaporation takes place

157. VaporizationA.is when a vapor turns to a liquidB.is the capability of a liquid to flow or not flow freely at room temperatuC.is when a solid turns into a liquidD.is the way that molecules change from a solid or liquid to vapor *

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158. Boiling pointA.is the temperature at which the vapor pressure equals temperatureB.is the pressure at which mercury becomes a liquidC.is the temperature at which the vapor pressure equals atmospheric pressureD.is always longer when you are watching and waiting for it to boil

159. SolubilityA.takes place when one compound is dissolved into another *B.only happens with solutions containing acetoneC.of two or more mixing solutions cannot be performedD.is a reaction that takes place in the sun

160. Dynamic equilibriumA.occurs when both forward and reverse reactions happen at the same rate and

time *

B. is achieved only in open containersC.Occurs when a measuring cylinder is balanced two glass rodsD.Occurs when pressure and atmosphere are equal

161. Which of the following is not a true statement about gases?A.they are at least compacted form of matterB.they are more active than liquidC.they prefer to be as far as possible from each otherD.some gases take on very distinct shapes *

162. Which of the following is not true about kinetic energy?A.it is a type of energy a gas uses to stay in motionB.it is named after the scientist Sorensen Kinet *C.it can be very easily calculatedD.kinetic energy = mv2

163. Boyles laws describesA.the ideal gas lawB.

the relationship of atmospheric pressure and temperature

C.describes when temperature is held constant, a volume of gas is inverselyproportional to the pressure *

D.an idea that does not apply to ideal gas laws164. Charles law explains

A.how gases are always on the moveB.how equal volumes of gases at the same temperature and pressure have equal

number of molecules

C.the relationship of gas volume and gas pressureD.whe pressure is held constant, a volume of gas is directly proportional to

the Kelvin temperature *

165. Gay-Lussacs law explainsA.when volume is held constant, the pressure of a gas is directly proportion

to the Kelvin temperature *

B.when pressure is held constant, the volume of gas is directly proportionalto the Kelvin temperature

C.shen temperature is held constant, the volume of a gas is inverselyproportional to the pressure

D.the effect on changing temperature on gases166. Daltons law of partial pressures states that when

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A.temperature is constant and the gas volume expands, pressure equals aportion of the original

B.more than one gas mixes with one or more different gases, the pressure ofeach gas will add together to give the total pressure of the mixture *

C.more than one gas mixes with one or more different gases, the total pressuof the mixture will be the same as the heaviest gas

D.gases come together, only two will combine at any one time167. Which of the following is not true about atmospheric pressure?

A.it stays the same regardless of elevation *B.it is caused by the force of the air molecules that push against a unit arC.the standard unit of pressure is called torrD.1 atmosphere is found at sea level

168. When gases expand and mix with other gases to fill available space, it iscalled

A.vaporization C. solidificationB.evaporation D. diffusion*

169. In the equation PV = n RT, nis equal toA.pressure C. number of moles of gas *B.volume D. temperature

170. The pressure of a gas is directly proportional to the Kelvin temperate inA.Boyles law C. Boyds lawB.Gay-Lussacs law * D. Charles law

Biochemistry, Nanotechnology, and the Future

171. Single-celled organisms break down organic molecules throughA.vaporization C. metabolism *B.cell division D. evaporation

172.Organic protein molecules serve living systems in which of the following

ways?

A.strength C. messengersB.transport D. all of these *

173. Paul EhrlichA.received the Nobel Prize in 1948 for his treatment of mad cow diseaseB.is known as the father of chemotherapy *C.discovered chemical solutions that kill microorganism and patientsD.worked exclusively with chitin protein in crab shells

174. The core of hemoglobin molecule isA.iron * C. zincB.gold D. magnesium

175. Macromolecules areA.ionic compounds found in mineralsB.covalently bonded molecules of large size *C.about 2 millimeters longD.can be found in mercury solution

176. Amino acids areA.based on ethyl subgroupsB.bonded by (OH-)bonds

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C.available as supplement to improve eyesightD.bonded by peptide (C-N) bonds *

177. Ozone isA.made up of NH3moleculesB.increasing all the timeC.made up of O3molecules *D.located 250 miles up in the atmosphere

178. The three main types of radiation given off during decay areA.neutrino wavesB.alpha, beta, and gamma rays *C.tachyn emissionsD.alpha, beta, and zeta rays

179. Nanotechnology is the study of elementsA.at the single atom level 10-6 metersB.found outside a cell nucleusC.found only in platinum samples of high densityD.at the single atom level 10-9 meters *

180. When no molecules can be broken down, they areA.biodegradable * C. vaporizedB.catalytic D. saturated