Final Exam Review 2014Ch.3 Scientific Measurement: pg. 96 (74, 79)74. Make the following conversions:

A. 157 cs to secondsB. 42.7 L to milliliters C. 261 nm to millimetersD. 0.065 km to decimeters E. 642 cg to kilogramsF. 8.25 x 102 cg to nanograms

79. Rank these numbers from smallest to largest:A. 5.3 x 104

B. 5.7 x 103

C. 4.9 x 10-2

D. 0.0057E. 5.1 x 10-3

F. 0.0072 x 102

Ch.17 Thermochemistry: pg. 586 (61, 74)61. Explain why ice melts in at 0 ͒C without an increase of temperature, even though heat flows from the surroundings to the system (the ice).

74. A 1.55-g piece of stainless steel absorbs 141 J of heat when its temperature increase by 178 ͒C. What is the specific heat of the stainless steel?

Ch.4 Atomic Structure: pg. 115 #21, pg. 119 #34, pg. 122 #5121. Three Chromium isotopes are Chromium-50, Chromium-52, and Chromium-53. How many neutrons are in each isotope, given that Chromium has an atomic number of 24?

34. List the number of protons, neutrons, and electrons in each pair of isotopes.

A. 63 Li, 7

3 Li B. 42

20Ca, 4410Ca

C. 7834 Se, 80

34Se

51. Complete the following table:

Atomic #Mass ## of Protons# of Electrons

9A.______ B.______ 10

C.____D.______ 14 15

E.____ 47F.______ 25

G.____ 55 25H.______

Ch.5 Electrons in Atoms: pg. 153 #59, pg. 157 #1-1459. An atom of an element has two electrons in the first energy level and five electrons in the second energy level. Write the electron configuration for this atom and and name the element. How many unpaired electrons does an atom of this element have?

1. Select the correct electron configuration for silicon, atomic number 14.A. 1s2 2s2 2p2 3s2 3p2 3d2 4s2

B. 1s2 2s2 2p4 3s2 3p4

C. 1s2 2s6 2p6

D. 1s2 2s2 2p6 3s2 3p2

2. Which two orbitals have the same shape? A. 2s and 2pB. 2s and 3sC. 3p and 3dD. more than one is correct.

3. Which of these statements characterize the nucleus of every atom?I. It has a positive charge.II. It is very dense.III. It is composed of protons, electrons, and neutrons.

A. I and II onlyB. II and III onlyC. I and III onlyD. I, II, and III

4. As the wavelength of light increases...A. the frequency increasesB. the speed of light increases

C. the energy decreasesD. the intensity increases

5. In the third energy level of an atom...A. there are two energy sublevelsB. the f sublevel has 7 orbitalsC. there are 3 s orbitalsD. a maximum of 18 electrons are allowed

Letter choices for 6-10A. s2 p6

B. s2 p2

C. s2

D. s4 p1

E. s2 p4

Which configuration is the configuration of the highestoccupied energy level for each of these elements?

6. sulfur7. germanium8. beryllium9. krypton10. strontium

Use the drawings to answer 11-14; each representsan electromagnetic wave.

A.

B.

C.

11. Which wave has the longest wavelength?12. which wave has the highest energy?13. which wave has the lowest frequency?14. which wave has the highest amplitude?

Ch.6 Organizing the Elements: pg. 187 #30,31,51, pg. 190 #8830. Identify each property below as more characteristic of a metal or a nonmetal.

A. a gas at room temperatureB. brittleC. malleableD. poor conductor of electric currentE. shiny

31. In general, how are metalloids different from metals and nonmetals?

51. In which pair of elements are the chemical properties of the elements most similar? Explain your reasoning.

A. sodium and chlorineB. nitrogen and phosphorousC. boron and oxygen

88. The volume of a liquid in a graduated cylinder is reported as 31.8 mL.A. How many significant figures are there in this measurement?B. In which digit is there uncertainty?

Ch.7 Ionic and Metallic Bonding: pg.214 #28,32,6728. To which group on the periodic table does each of the following elements belong? How many valence electrons do atoms of each element have?

A. nitrogenB. lithiumC. phosphorousD. barium E. bromineF. carbon

32. write the symbol for the ion formed when each of the following elements loses its valence electrons.

A. aluminumB. lithiumC. bariumD. potassium E. calciumF. strontium

67. Which of the following compounds are most likely not ionic?A. H2OB. Na2OC. CO2

D. CaSE. SO2

F. NH3

Ch.8 Covalent Bonding: pg. 256 #39,43,77,110, pg.261 #639. The melting point of a compound is 1240 ͒C. Is this compound most likely an ionic compound or a molecular compound?

43. Identify the phrases that generally apply to molecular compounds:A. contain metals and nonmetalsB. are often gases or liquidsC. have low melting pointsD. contain ionic bondsE. use covalent bonding

77. What is the geometry around the central atom in each of these simple molecules?

A.

B.

C.

D.

110. Which of these statements about the periodic table is correct?I. Elements are arranged in order of increasing massII. A period is a horizontal rowIII. Nonmetals are located on the right side of the table

A. I onlyB. I and II onlyC. I, II, and IIID. I and III onlyE. II and III only

6. Draw the electron dot structure for each example molecule.

bonding pairsnon-bonding pairsarrangement of electron pairs

molecular shapeexample

40tetrahedraltetrahedralCH4

31tetrahedralpyramidalNCl3

22tetrahedralbentH2S

13tetrahedrallinearHF

Ch.9 Chemical Names and Formulas: pg. 299 #80,8180. Write formulas for these compounds:

A. potassium permanganateB. calcium hydrogen carbonateC. dichlorine heptoxideD. trisilicon tetranitrideE. sodium dihydrogen phosphateF. phosphorus pentabromide

81. Write formulas for these compounds:A. magnesium sulfideB. sodium phosphite C. barium hydroxideD. copper (II) nitriteE. potassium sulfiteF. calcium carbonateG. sodium bromide H. ferric sulfate

Ch.10 Chemical Quantities: pg. 327 #35, pg. 338 #54, 65,111,116,122,pg. 343 #2,35. calculate the percent by mass of nitrogen in these fertilizers:

A. NH3

B. NH4NO3

54. find the number of moles in each substance:A. 2.41 x 1024 formula units of NAClB. 9.03 x 1024 formula units of HgC. 4.65 x 1024 molecules of NO2

65. how many moles is each of the following:A. 15.5 g SiO2

B. 0.0688 g AgClC. 79.3 g Cl2

D. 5.96 g KOHE. 937 g Ca( C2H3O2)2

F. 0.800 g Ca

111. classify each of the following as a physical change or a chemical change:A. an aspirin tablet is crushed to a powderB. a red rose turns brownC. grape juice turns to wineD. fingernail polish remover evaporatesE. a bean seed sproutsF. a piece of copper is beaten into a thin sheet

116. how many protons, electrons, and neutrons are in each isotope?A. zirconium-90B. palladium-108C. bromine-81D. antimony-123

122. draw electron dot structures and predict the shapes of the following molecules:A. PH3

B. COC. CS2

D. CF4

2. calculate the molar mass of ammonium phosphate, (NH4)3 PO4

A. 113.0 g/molB. 121.0 g/molC. 149.0 g/molD. 242.0 g/mol

Ch.11 Chemical Reactions: pg. 377#41,43, pg.380 #7541. write a balanced equation for each of the following double- replacement reactions:

A. H2C2O4(aq) + KOH (aq) →B. CdBr2(aq) + Na2S(aq) →

43. balance each equation and identify its type:A. Hf(s) + N2(g) → Hf3N4(s)B. Mg(s) + H2SO4(aq) → MgSo4(aq) + H2(g)C. C2H6(g) + O2(g) → CO2(g) + H2O(g)D. Pb(NO3)2(aq) + NaI(aq) → PbI2(s) + NaNO3(aq)

75. calculate the number of moles in each substance:A. 54.0 L of nitrogen dioxide (at STP)

B. 1.68 g of magnesium ionsC. 69.6 g of sodium hypochloriteD. 4.27 x 1024 molecules of carbon monoxide

Ch. 12 Stoichiometry: pg. 411 #47c. pg. 416 #102, pg. 417 #147c. How many grams of N2F4 can be produced from 225 g F2?

102. how many moles is each of the following:A. 47.8 g KNO3

B. 2.22 L SO2 (at STP)C. 2.25 x 1022 molecules PCL3

1. nitric acid is formed by the reaction of nitrogen dioxide with water.3NO2(g) + H2O(l) → NO(g) + 2HNO3(aq)

How many moles of water are needed to react with 8.4 mol NO2

A. 2.8 molB. 3.0 molC. 8.4 molD. 25 mol

Ch. 14 The Behavior of Gases: pg.480 #49, pg.484 #12349. describe what happens to the volume of a balloon when it is taken outside on a cold winter day. explain why the observed change happens

123. use the drawings to explain how gas pressure is produced.

Ch. 19 Acids, Bases, and Salts: pg.652 #6, pg. 662 #18,19, pg.675 #39,426. how are the properties of acids and bases similar? how are they different?

18. how are the concentrations of hydrogen ions and hydroxide ions related in an aqueous solution?

19. what is the range of pH values in the following solutions:

A. basicB. acidicC. neutral

39. what are the products of a reaction between an acid and a base?

42. write balanced equations for the following acid-base reactions:A. H2SO4 (aq) + KOH (aq) →B. H3PO4 (aq) + Ca(OH)2 (aq) →C. HNO3 (aq) + Mg(OH)2 (aq) →