Advanced Chemistry Name ________________________________________

Final Review (2012/2013)

Chapters 1-2: Introduction to chemistry/Matter and Change

1) The study of the composition and structure of matter is the domain of which field of science?

a) geology

b) biology

c) physics

d) chemistry

2) What is the second step in the scientific method?

a) law

b) conclusion

c) hypothesis

d) experiment

e) test

3) Matter is defined as anything that _____.

a) can be weighed on a balance

b) has a definite volume

c) has a fixed volume and weight

d) has mass and takes up space

4) In the following list, only __________ is not an example of matter.

a) planets

b) light

c) dust

d) elemental phosphorus

e) table salt

5) Which state of matter takes both the shape and volume of its container?

a) solid

b) liquid

c) gas

d) both B. and C.

6) A combination of sand, salt, and water is an example of a __________.

a) homogeneous mixture

b) heterogeneous mixture

c) compound

d) pure substance

e) solid

7) Which of the above diagrams could be molecules of an element?

8) Which of the above diagrams could be molecules of a compound?

9) For which of the following can the composition vary?

a) pure substance

b) element

c) both homogeneous and heterogeneous mixtures

d) homogeneous mixture

e) heterogeneous mixture

10) The apparatus pictured at right would be appropriate for separation of

a) carbon dioxide and water

b) alcohol and water

c) copper sulfate (aq)and water

d) silver chloride (ppt)and water

11) If matter is uniform throughout, cannot be separated into other substances by physical processes,

and cannot be decomposed into other substances by chemical processes, it is _______.

a) an element

b) a compound

c) a homogeneous mixture

d) a heterogeneous mixture

e) a mixutre of compounds

12) If matter is uniform throughout and cannot be separated into other substances by physical means, it is _______.

a) a compound

b) either an element or a compound

c) a homogeneous mixture

d) a heterogeneous mixture

e) an element

13) Of the following, only __________ is a chemical reaction.

a) melting of lead

b) dissolving sugar in water

c) tarnishing of silver

d) crushing of stone

e) dropping a penny into a glass of water

14) What happens to the individual atoms in a chemical reaction?

a) Some are destroyed and some are created.

b) Some are destroyed.

c) They are rearranged

d) Some are created.

15) Which of the following is a chemical property?

a) freezing point

b) density

c) reactivity with oxygen

d) color

Chapter 3: Scientific Measurement

16) What length should be recorded for the object at right?

a) 1.6 cm

b) 1.65 cm

c) 1.650 cm

d) 1.7 cm

17) What volume should be recorded for the liquid at right?

a) 8.2 mL

b) 8.20 mL

c) 8.04 mL

d) 8.40 mL

18) The prefix milli means

a) 1/1000

b) 1/100

c) 1/10

d) 1000

19) A kilogram is the same as

a) 1/1000 g

b) 1/100 g

c) 1/10 g

d) 1000 g

20) Precision refers to _______.

a) how close a measured number is to other measured numbers

b) how close a measured number is to the true value

c) how close a measured number is to the calculated value

d) how close a measured number is to zero

e) how close a measured number is to infinity

21) Accuracy refers to _______.

a) how close a measured number is to zero

b) how close a measured number is to the calculated value

c) how close a measured number is to other measured numbers

d) how close a measured number is to the true value

e) how close a measured number is to infinity

22) Which of the following has the same number of significant figures as the number 1.00310?

a) 1 x 106

b) 199.791

c) 8.66

d) 5.119

e) 100

23) How many significant figures are there in the number 0.00230?

a) 2

b) 3

c) 5

d) 6

e) 4

24) How many significant figures should there be in the answer to the following?

23.1 + 0.11 + 140.3 + 52.07 = _____

a) 5

b) 1

c) 2

d) 3

e) 4

25) How many significant figures should there be in the answer to the following?

(3.15 x 1.06) + (21 x 1.773) = _____

a) 1

b) 2

c) 3

d) 4

e) 5

Chapter 5: Atomic Structure and the Periodic Table

26) Who was the first person to suggest the idea of atoms, in the fourth centrury B.C.

a) Dalton

b) Thomson

c) Democritus

d) Galileo

e) Atomos

27) The gold foil experiment performed in Rutherford's lab __________.

a) confirmed the plum-pudding model of the atom

b) led to the discovery of the atomic nucleus

c) was the basis for Thompson's model of the atom

d) utilized the deflection of marbles by gold foil

e) proved the law of multiple proportions

28) Rutherford's gold foil experiment showed that _______.

a) the "plum-pudding" model of the atom was incorrect

b) most of the mass of an atom is concentrated in a tiny portion of its total volume

c) the positively charged particles within an atom are concentrated in a tiny portion of its volume

d) α-particles(the radiation emitted from uranium) are less massive than gold nuclei

e) all of these are correct

29) There are _____ electrons, _____ protons, and _____ neutrons in an atom of

a) 132, 132, 54

b) 54, 54, 132

c) 78, 78, 54

d) 54, 54, 78

e) 78, 78, 132

30) All atoms of a particular element contain the same number of _______.

a) neutrons

b) protons

c) protons and neutrons

d) protons, neutrons, and electrons

e) subatomic particles

31) Different isotopes of a particular element contain different numbers of _______.

a) protons

b) neutrons

c) protons and neutrons

d) protons, neutrons, and electrons

e) none of these is correct

32) Which one of the following is a nonmetal?

a) W

b) Sr

c) Os

d) Ir

e) Br

33) Of the following, only _________ is not a metalloid.

a) B

b) Al

c) Si

d) Ge

e) As

34) Which pair of elements below should be the most similar in chemical properties?

a) N and O

b) P and S

c) K and Ca

d) K and Mg

e) Sr and Ba

35) Horizontal rows of the periodic table are known as _______.

a) periods

b) groups

c) metalloids

d) metals

e) nonmetals

36) Vertical columns of the periodic table are known as _______.

a) metals

b) periods

c) nonmetals

d) groups

e) metalloids

37) Lithium is a _____ and magnesium is a _____.

a) nonmetal, metal

b) nonmetal, nonmetal

c) metal, metal

d) metal, metalloid

e) metalloid, metalloid

38) Oxygen is a _____ and nitrogen is a _____.

a) metal, metalloid

b) nonmetal, metal

c) metalloid, metalloid

d) nonmetal, nonmetal

e) nonmetal, metalloid

39) __________ are found uncombined, as monatomic species in nature.

a) Noble gases

b) Chalcogens

c) Alkali metals

d) Alkaline earth metals

e) Halogens

40) The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms

is __________.

a) C12H14O6

b) CHO

c) CH2O

d) C6H7O3

e) C2H4O

Chapter 6: Chemical Names and Formulas

41) Of the choices below, which one is not an ionic compound?

a) PCl5

b) MoCl6

c) RbCl

d) PbCl2

e) NaCl

42) The number of oxygen atoms in Ca(NO3)2 is:

a) 6

b) 5

c) 3

d) 2

43) The molecular formula of a compound is always _____ the empirical formula.

a) more complex than

b) different from

c) an integral multiple of

d) the same as

e) simpler than

44) Of the following, _________ contains the greatest number of electrons.

a) P3+

b) P

c) P2-

d) P3-

e) P2+

45) Which one of the following is most likely to lose electrons when forming an ion?

a) F

b) P

c) Rh

d) S

e) N

46) There are _____ protons, _____ neutrons, and _____ electrons in 131I-.

a) 131, 53, and 54

b) 131, 53, and 52

c) 53, 78, and 54

d) 53, 131, and 52

e) 78, 53, and 72

47) Which species has 16 protons?

a) 31P

b) 34S2-

c) 36Cl

d) 80Br-

e) 32S

48) The charge on the manganese in the salt MnF3 is __________.

a) +1

b) -1

c) +2

d) -2

e) +3

49) Aluminum reacts with a certain nonmetallic element to form a compound with the general formula AlX. Element X is a

diatomic gas at room temperature. Element X must be __________.

a) oxygen

b) fluorine

c) chlorine

d) nitrogen

e) sulfur

50) Sodium forms an ion with a charge of _______.

a) +1

b) -1

c) +2

d) -2

e) 0

51) Calcium forms an ion with a charge of _______.

a) -1

b) -2

c) +1

d) +2

e) 0

52) Iodine forms an ion with a charge of _______.

a) -7

b) +1

c) -2

d) +2

e) -1

53) Which pair of elements is most apt to form an ionic compound?

a) barium, bromine

b) calcium, sodium

c) oxygen, fluorine

d) sulfur, fluorine

e) nitrogen, hydrogen

54) Predict the empirical formula of the ionic compound that forms from sodium and fluorine.

a) NaF

b) Na2F

c) NaF2

d) Na2F3

e) Na3F2

55) The correct name for SrO is _______.

a) strontium oxide

b) strontium hydroxide

c) strontium peroxide

d) strontium monoxide

e) strontium dioxide

56) The correct name for CaH2 is _______.

a) hydrocalcium

b) calcium dihydride

c) calcium hydroxide

d) calcium dihydroxide

e) calcium hydride

57) The correct name for SO is _______.

a) sulfur oxide

b) sulfur monoxide

c) sulfoxide

d) sulfate

e) sulfite

58) The correct name for N2O5 is _______.

a) nitrous oxide

b) nitrogen pentoxide

c) dinitrogen pentoxide

d) nitric oxide

e) nitrogen oxide

59) The correct name for HClO3 is _______.

a) hydrochloric acid

b) perchloric acid

c) chloric acid

d) chlorous acid

e) hydrochlorous acid

60) The correct formula of iron(III) bromide is __________.

a) FeBr2

b) FeBr3

c) FeBr

d) Fe3Br3

e) Fe3Br

61) The formula of ammonium carbonate is __________.

a) (NH4)2CO3

b) NH4CO2

c) (NH3)2CO4

d) (NH3)2CO3

e) N2(CO3)3

62) The formula of the chromate ion is __________.

a) CrO42-

b) CrO23-

c) CrO1-

d) CrO32-

e) CrO2-

63) Which one of the following is the correct name for Mg(ClO3)2?

a) magnesium chlorate

b) manganese chlorate

c) magnesium chloroxide

d) magnesium perchlorate

e) manganese perchlorate

64) The formula for aluminum hydroxide is __________.

a) AlOH

b) Al3OH

c) Al2(OH)3

d) Al(OH)3

e) Al2O3

65) The name of the ionic compound (NH4)3PO4 is ___________.

a) ammonium phosphate

b) nitrogen hydrogen phosphate

c) tetrammonium phosphate

d) ammonia phosphide

e) triammonium phosphate

66) SO42- is the

a) sulfate ion

b) sulfide ion

c) cyanide ion

d) carbonate ion

e) sulfite ion

Chapter 8: Chemical Reactions

67) The equation that correctly describes the reaction above is

a) Al2 + 3 Cl2 --> Al2Cl6

b) 2 Al + 3 Cl --> 2 AlCl3

c) 2 Al + Cl2 --> 2 AlCl

d) 2 Al + 3 Cl2 --> 2 AlCl3

68) What is the whole number that appears in front of a formula in a chemical equation?

a) a subscript

b) a superscript

c) a ratio

d) a coefficient

69) In every balanced chemical equation, each side of the equation has the same number

of _____.

a) coefficients

b) atoms

c) subscripts

d) molecules

e) moles

70) The equation AX + BY → AY + BX is the general equation for a

a) synthesis reaction.

b) single-replacement reaction.

c) decomposition reaction.

d) double-replacement reaction.

71) The reaction Mg + 2HCl → H2 + MgCl2 is a

a) composition reaction.

b) single-replacement reaction.

c) reaction.

d) double-replacement reaction.

72) What is the balanced equation when aluminum reacts with copper(II) sulfate?

a) Al + Cu2S → Al2S + Cu

b) Al + CuSO4 → AlSO4 + Cu

c) 2Al + 3CuSO4 → Al2(SO4)3 + 3Cu

d) 2Al + Cu2SO4 → Al2SO4 + 2Cu

Cl

Cl

Al

Al

Al

Al

Cl

Cl

Cl

Cl

Cl

Cl

Cl

Cl

Cl

Cl

73) Of the reactions below, which one is not a synthesis (combination) reaction?

a) C + O2 CO2

b) 2Mg + O2 2MgO

c) 2N2 + 3H2 2NH3

d) CaO + H2O Ca(OH)2

e) Cd(NO3) + Na2S CdS + 2NaNO3

74) Which of the following are decomposition reactions?

1) CH4(g) + O2(g) CO2(g) + H2O(l)

2) CaO(s) + CO2(g) CaCO3(s)

3) Mg(s) + O2(g) MgO(s)

4) PbCO3(s) PbO(s) + CO2(g)

a) 1, 2, and 3

b) 4 only

c) 1, 2, 3, and 4

d) 2 and 3

e) 2, 3, and 4

75) When the reaction below is balanced, the coefficients are __________.

NH3 + O2 NO2 + H2O

a) 1,1,1,1

b) 4,7,4,6

c) 2,3,2,3

d) 1,3,1,2

e) none of these

76) What is the coefficient of FeCl3 when the following equation is balanced?

FeCl3 + Na2CO3 Fe2(CO3)3 + NaCl

a) 1

b) 2

c) 3

d) 5

e) 4

77) What is the coefficient of O2 when the following equation is balanced?

C4H8O2 + O2 __________

a) 2

b) 3

c) 5

d) 6

e) 1

Chapter 7: Chemical quantities

The formula weight (amu) of potassium phosphate is __________.

a) 173.17

b) 251.37

c) 212.27

d) 196.27

e) 86.07

78) The mass % of C in CH4 is __________.

a) 25.13

b) 133.6

c) 74.87

d) 92.26

e) 7.743

79) A sample of CH4O with a mass of 32.0 g contains __________ molecules of CH4O.

a) 5.32 × 10-23

b) 1.00

c) 1.88 × 1022

d) 6.02 × 1023

e) 32.0

80) How many hydrogen atoms are there in 25 molecules of C4H4S2?

a) 25

b) 3.8 x 1024

c) 6.0 x 1025

d) 100

e) 1.5 x 1025

81) The molar mass of H2O is 18.015 g/mol. How many grams of H2O are present in 0.20 mol?

a) 0.2 g

b) 3.6 g

c) 35.9 g

d) 89.9 g

82) How many oxygen atoms are there in 52.06 g of carbon dioxide?

a) 1.424 x 1024

b) 6.022 x 1023

c) 1.204 x 1024

d) 5.088 x 1023

e) 1.018 x 1024

83) What is the empirical formula for a compound that contains 29% Na, 41% S, and 30% O by mass?

a) Na2S2O3

b) NaSO2

c) NaSO

d) NaSO3

e) Na2S2O6

84) A compound's empirical formula is C2H5. If the formula mass is 58 amu, what is the molecular formula?

a) C3H6

b) C4H10

c) C5H8

d) C5H15

Chapter 9: Stoichiometry

85) The coefficients in a chemical equation represent the

a) masses, in grams, of all reactants and products.

b) relative numbers of moles of reactants and products.

c) number of atoms in each compound in a reaction.

d) number of valence electrons involved in the reaction.

86) Which reactant controls the amount of product formed in a chemical reaction?

a) excess reactant

b) composition reactant

c) mole ratio

d) limiting reactant

87) What is the maximum possible amount of product obtained in a chemical reaction?

a) theoretical yield

b) percent yield

c) mole ratio

d) actual yield

88)

a) 1:1

b) 1:3

c) 1:2

d) 2:3

89) In the reaction 2Al2O3 → 4Al + 3O2, what is the mole ratio of aluminum to oxygen?

a) 10:6

b) 3:4

c) 2:3

d) 4:3

90)

a) 9.0 mol

b) 27 mol

c) 18 mol

d) 36 mol

91) A sample of nitrogen (9.27 g) reacts completely with magnesium, according to the equation:

3 Mg + N2 Mg3N2

The mass of Mg consumed is _____ g.

a) 8.04

b) 24.1

c) 16.1

d) 0.92

e) 13.9

92) Silver nitrate and aluminum chloride react with each other by exchanging anions:

AgNO3 + AlCl3 Al(NO3)3 + AgCl

What mass (g) of AgCl is produced when 4.22 g of AgNO3 react with 7.73 g of AlCl3. The reaction must be balanced.

a) 17.6

b) 4.22

c) 24.9

d) 3.56

e) 11.9

93) Determine the mass (g) of SO3 that is produced by the reaction of 1.0 g of S with 1.0 g of O2 according to the equation:

2S(s) + 3O2(g) 2SO3(g)

a) 0.27

b) 1.7

c) 2.5

d) 3.8

e) 2.0

94) The reaction of 1.0 g of sulfur with 1.0 g of oxygen according to the reaction below produced 0.80 g of sulfur trioxide. The

yield of sulfur trioxide was _____%.

2S + 3O2 2SO3

a) 30

b) 296

c) 21

d) 88

e) 48

Chapter 12: Properties of Gases

95) The standard molar volume of a gas at STP is

a) 22.4 L.

b) g-mol wt/22.4 L.

c) g/22.4 L.

d) 1 L.

96) Standard temperature and pressure (STP), in the context of gases, refers to __________.

a) 298 K and 1 atm

b) 298 K and 1 torr

c) 273 K and 1 atm

d) 273 K and 1 torr

e) 273 K and 1 pascal

97) If the volume of a container holding a gas is reduced, what will happen to the pressure within the container?

a) The pressure will decrease.

b) The pressure will increase.

c) The pressure will not change.

98) The volume of a gas is 93 mL when the temperature is 91ºC. If the temperature is reduced to 0ºC without changing the

pressure, what is the new volume of the gas?

a) 70 mL

b) 120 mL

c) 100 mL

d) 273 mL

99) A 150.0 L sample of gas is collected at 1.20 atm and 25ºC. What volume does the gas have at 1.50 atm and

20.0ºC?

a) 94 L

b) 143 L

c) 120 L

d) 183 L

100) A sample of gas initially at 6.00 atm was compressed from 8.00 L to 2.00 L at constant temperature. After the

compression, the gas pressure was __________ atm.

a) 12.0

b) 16.0

c) 18.0

d) 20.0

e) 24.0

101) Calculate the approximate volume of a 0.600 mol sample of gas at 15.0ºC and a pressure of

1.10 atm.

a) 12.9 L

b) 24.6 L

c) 22.4 L

d) 129 L

102) If five gases in a cylinder each exert 2 atm, what is the total pressure exerted by the

gases if mixed?

a) 0.2 atm

b) 10 atm

c) 0.5 atm

d) 5 atm

103) Arrange the following gases in order of increasing average molecular speed at 25 °C.

Cl2, O2, F2, N2

a) F2 < O2 < N2 < Cl2

b) Cl2 < F2 < O2 < N2

c) Cl2 < O2 < F2 < N2

d) N2 < F2 < Cl2 < O2

e) Cl2 < F2 < N2 < O2

Chapter 13: Electrons in Atoms

104) Which one of the following is correct?

a) ν + λ = c

b) ν ÷ λ = c

c) ν = cλ

d) λ = c ν

e) νλ = c

105) The energy of a photon of light is __________ proportional to its frequency and __________ proportional to its

wavelength.

a) directly, directly

b) inversely, inversely

c) inversely, directly

d) directly, inversely

e) indirectly, not

106) The wavelength of light that has a frequency of 1.66 × 109s-1 is __________ m.

a) 0.181

b) 5.53

c) 2.00 x 10-9

d) 5.53 x 108

e) none of the above

107) The energy of a photon that has a frequency of 8.21 × 1015 s-1 is __________ J.

a) 8.08 × 10-50

b) 1.99 × 10-25

c) 5.44 × 10-18

d) 1.24 × 1049

e) 1.26 × 10-19

108) What color of visible light has the longest wavelength?

a) blue

b) violet

c) red

d) yellow

e) green

109) Which of the following energy levels has the lowest energy?

a) 4f

b) 4s

c) 4p

d) 3d

110) An electron cannot have the quantum numbers n = __________, l = __________, ml = __________.

a) 2, 0, 0

b) 2, 1, -1

c) 3, 1, -1

d) 1, 1, 1

e) 3, 2, 1

111) At maximum, an f-subshell can hold __________ electrons, a d-subshell can hold __________ electrons, and a p-subshell

can hold __________ electrons.

a) 14, 10, 6

b) 2, 8, 18

c) 14, 8, 2

d) 2, 12, 21

e) 2, 6, 10

112) The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is

a) Mg (Z = 12).

b) S (Z = 16).

c) C (Z = 6).

d) Si (Z = 14).

113) The electron notation for aluminum (atomic number 13) is

a) 1s2 2s2 2p3 3s2 3p3 3d1.

b) 1s2 2s2 2p6 3s2 3p1.

c) 1s2 2s2 2p6 3s2 2d1.

d) 1s2 2s2 2p9.

114) The orbital notation depicted here is for the element:

a) Sulfur

b) Phosphorous

c) Nitrogen

d) Magnesium

115) The element that has a valence configuration of 4s1 is __________.

a) Li

b) Na

c) K

d) Rb

e) Cs

Chapter 14: Periodic Properties

116) In which set of elements would all members be expected to have very similar chemical properties?

a) O, S, Se

b) N, O, F

c) Na, Mg, K

d) S, Se, Si

e) Ne, Na, Mg

117) In which orbital does an electron in a lead atom experience the greatest effective nuclear charge?

a) 1s

b) 4p

c) 5s

d) 6s

e) 5d

118) Which one of the following is a metalloid?

a) Ge

b) S

c) Br

d) Pb

e) C

119) Which one of the following is a metal?

a) Ge

b) S

c) Br

d) Pb

e) C

120) The elements in groups 1A, 6A, and 7A are called, __________, respectively.

a) alkaline earth metals, halogens, and chalcogens

b) alkali metals, chalcogens, and halogens

c) alkali metals, halogens, and noble gases

d) alkaline earth metals, transition metals, and halogens

e) halogens, transition metals, and alkali metals

121) Atomic radius generally increases as we move __________.

a) down a group and from right to left across a period

b) up a group and from left to right across a period

c) down a group and from left to right across a period

d) up a group and from right to left across a period

e) down a group. The period position has no effect.

122) Which one of the following atoms has the largest radius?

a) N

b) F

c) Si

d) Cl

e) Ne

123) Ionization energy is the energy required to remove ____ from an atom of an element.

a) the electron cloud

b) an electron

c) the nucleus

d) an ion

124) Of the choices below, which gives the order for first ionization energies?

a) Cl > S > Al > Ar > Si

b) Ar > Cl > S > Si > Al

c) Al > Si > S > Cl > Ar

d) Cl > S > Al > Si > Ar

125) The most common nitrogen ion has a charge of __________.

a) -3

b) -1

c) +4

d) +6

e) sulfur does not form ions.

126) Which ion in the isoelectric series below has the smallest radius?

a) Al3+

b) Na+

c) O2-

d) F-

e) N3-

127) Of the atoms below, _____ is the most electronegative.

a) Br

b) O

c) Cl

d) N

e) F

128) Of the elements below, __________ is the most metallic.

a) sodium

b) barium

c) magnesium

d) calcium

e) cesium

Chapter 18: Properties of Solutions

129) The process of solute particles being surrounded by solvent particles is known as _________________.

a) salutation

b) agglomeration

c) solvation

d) agglutination

e) passivation

130) A supersaturated solution ____________.

a) is one with more than one solute

b) is one that has been heated

c) is one with a higher concentration than the solubility

d) must be in contact with undissolved solid

e) exists only in theory and cannot actually be prepared

131) Adding solute to a solution ____________ the freezing point and ______________ the boiling point of the solution.

a) decreases, decreases

b) increases, increases

c) raises, lowers

d) increases, increases

e) decreases, increases

132) Calculate the freezing point of a 0.05500 m aqueous solution of NaNO3.

a) 0.0286øC

b) -0.1023øC

c) 0.1023øC

d) -0.05627øC

e) -0.2046øC

133) How does solubility generally vary as the temperature increases?

a) solubility remains the same

b) solubility decreases

c) solubility increases

134) What is the molarity of a solution containing 9.0 moles of solute in 500.0 mL of solution?

a) 18M

b) 1.8M

c) 0.45M

d) 4.5M

e) 0.18M

135) What is the number of moles of solute in 250 mL of a 0.4M solution?

a) 0.62 mol

b) 0.1 mol

c) 1.0 mol

d) 1.6 mol

e) 0.16 mol

136) How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr?

a) 25 mL

b) 150 mL

c) 100 mL

d) 50 mL