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Chapter 8 Periodic Properties of the Elements
1) No two electrons can have the same four quantum numbers is known as (the)
A) Pauli exclusion principle.
C) Aufbau principle.
B) Hund's rule.
D) Heisenberg uncertainty principle.
Answer: A
2) Electrons filling up the orbitals from low to high is known as (the)
A) Pauli exclusion principle.
C) Aufbau principle.
B) Hund's rule.
D) Heisenberg uncertainty principle.
Answer: C
3) When filling degenerate orbitals, electrons fill them singly first, with parallel spins. This is
known as (the)
A) Pauli exclusion principle.
C) Aufbau principle.
B) Hund's rule.
D) Heisenberg uncertainty principle.
Answer: B
4) Which of the following statements is TRUE?
A) An orbital that penetrates into the region occupied by core electrons is less shielded from
nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
B) An orbital that penetrates into the region occupied by core electrons is more shielded from
nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
C) It is possible for two electrons in the same atom to have identical values for all four quantum
numbers.
D) Two electrons in the same orbital can have the same spin.
E) None of the above is true.
Answer: A
5) The element that corresponds to the electron configuration 1s22s22p63s23p64s13d5 is
A) titanium.
C) chromium.
E) iron.
B) vanadium.
D) manganese.
Answer: C
6) Give the ground state electron configuration for Se.
A) [Ar]4s23d104p4
C) [Ar]4s23d104p6
B) [Ar]4s24d104p4
D) [Ar]4s23d10
Answer: A
7) Give the ground state electron configuration for Sr.
A) [Kr]5s24d2
C) [Kr]5s2
B) [Kr]5s24d105p2
D) [Kr]5s25d105p2
Answer: C
E) [Ar]3d104p4
E) [Kr]5s24d10
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8) Give the ground state electron configuration for Pb.
A) [Xe]6s26p2
C) [Xe]6s25f146d106p2
B) [Xe]6s25d106p2
D) [Xe]6s24f145d106p2
Answer: D
9) How many valence electrons do the alkali metals possess?
A) 1
C) 7
B) 2
D) 6
Answer: A
10) How many valence electrons do the noble gases possess?
A) 1
C) 7
B) 2
D) 6
Answer: E
11) A cation of +2 indicates that an element has
A) lost two electrons.
C) lost two neutrons.
B) lost two protons.
D) gained two electrons.
Answer: A
12) Give the ground state electron configuration for F⁻.
A) 1s22s22p6
C) 1s22s22p4
B) 1s22s22p5
D) 1s22s22p3
Answer: A
13) Choose the ground state electron configuration for Zn2⁺.
A) [Ar]4s23d8
C) [Ar]4s23d6
D) [Ar]
B) [Ar]3d10
Answer: B
14) Choose the ground state electron configuration for Cr3⁺.
A) [Ar]4s13d2
C) [Ar]4s23d6
B) [Ar]
D) [Ar]3d3
Answer: D
E) [Xe]6s24f145d106s26p
E) 8
E) 8
E) gained two protons.
E) 1s22s22p2
E) [Ar]3d8
E) [Ar]4s23d1
15) Choose the valence orbital diagram that represents the ground state of Sr2⁺.
A)
B)
C)
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D)
E)
Answer: D
16) Identify the isoelectronic elements.
A) Cl-, F-, Br-, I-, AtB) N3-, S2-, Br-, Cs+, Sr2+
C) P3-, S2-, C1-, K+, Ca2+
Answer: C
D) Zn2+, Co2+, Cu2+, Cr2+, Cd2+
E) Ne, Ar, Kr, Xe, He
17) For a particular element, identify the species that has the smallest radius.
A) cation
C) neutral
E) They are all the same
B) anion
D) radical
size.
Answer: A
18) Identify the elements correctly shown by decreasing radii size.
A) N3- > N
C) N > N3B) K+ > K
D) Cu2+ > Cu+
Answer: A
E) S- > S2-
19) Choose the statement that is TRUE.
A) Outer electrons efficiently shield one another from nuclear charge.
B) Core electrons effectively shield outer electrons from nuclear charge.
C) Valence electrons are most difficult of all electrons to remove.
D) Core electrons are the easiest of all electrons to remove.
E) All of the above are true.
Answer: B
20) Which reaction below represents the electron affinity of Li?
A) Li(g) + e⁻ → Li⁻(g)
C) Li(g) + e⁻ → Li⁺(g)
B) Li(g) → Li⁺(g) + e⁻
D) Li⁺(g) → Li(g) + e⁻
Answer: A
21) Which reaction below represents the electron affinity of S?
A) S(g) + e⁻ → S⁻(g)
C) S(g) → S⁺(g) + e⁻
2
D) S⁻(g) → S(g) + e⁻
B) S⁻(g) + e⁻ → S ⁻(g)
E) Li⁺(g) + e⁻ → Li(g)
E) S2⁻(g) → S⁻(g) + e⁻
Answer: A
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22) Place the following in order of decreasing metallic character.
P
As
K
A) P > As > K
B) As > P > K
Answer: E
C) K > P > As
D) As > K > P
E) K > As > P
23) Place the following in order of increasing metallic character.
Rb
Cs
K
A) K < Cs < Na < Rb
B) Na < K < Rb < Cs
Answer: B
Na
C) Cs < Rb < K < Na
D) K < Cs < Rb < Na
24) Describe the reaction of the noble gases with metals.
A) inert
C) mild reaction
B) vigorous
D) forms water
Answer: A
25) Describe the reaction of the alkali metals with non-metals.
A) inert
C) mild reaction
B) vigorous
D) forms water
Answer: B
26) Identify the most reactive alkali metal with water.
A) Cs
C) K
B) Rb
D) Na
Answer: A
27) Identify a characteristic of halogens.
A) powerful reducing agents
B) forms water in reactions
C) powerful oxidizing agents
Answer: C
E) Na < Rb < Cs < K
E) dissolves
E) dissolves
E) Li
D) absorbs water in reactions
E) inert
28) How many valence electrons does an atom of Tl possess?
A) 3
C) 0
B) 5
D) 4
Answer: A
29) How many valence electrons does an atom of Ar possess?
A) 2
C) 7
B) 4
D) 0
Answer: E
E) 7
E) 8
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30) How many valence shell electrons does an atom of thallium have?
A) 1
C) 3
E) 7
B) 4
D) 81
Answer: C
31) An element that has the valence electron configuration 5s25p5 belongs to which period and
group?
A) period 5; group 5A
C) period 6; group 5A
B) period 5; group 7A
D) period 6; group 7A
Answer: B
32) Identify the noble gas that is used by researchers to cool down samples for analysis.
A) radon
C) helium
E) oxygen
B) neon
D) iodine
Answer: C
33) Give the number of core electrons for Te.
A) 2
C) 46
B) 6
D) 50
Answer: C
E) 11
34) How many unpaired electrons are present in the ground state N atom?
A) 0
C) 1
E) 4
B) 3
D) 2
Answer: B
35) How many unpaired electrons are present in the ground state Xe atom?
A) 2
C) 0
E) 8
B) 3
D) 5
Answer: C
36) Which atom in each group (I and II) has the smallest atomic radius?
(I) Ca, Ti, Br
(II) O, S, Se
A) Ca; O
B) Ca; Se
Answer: C
C) Br; O
D) Br; Se
37) Place the following elements in order of increasing atomic radius.
S
Te
A) Te < S < O
B) S < O < Te
Answer: C
O
C) O < S < Te
D) O < Te < S
E) Te < O < S
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38) Place the following in order of increasing atomic radius.
Sr
Li
A) Sr < Ca < Li
B) Li < Sr < Ca
Answer: E
Ca
C) Ca < Sr < Li
D) Sr < Li < Ca
E) Li < Ca < Sr
39) Choose the orbital diagram that represents the ground state of N.
A)
D)
B)
E)
C)
Answer: A
Chapter 3 Molecules, Compounds, and Chemical Equations
1) An ionic bond is best described as
A) the sharing of electrons.
B) the transfer of electrons from one atom to another.
C) the attraction that holds the atoms together in a polyatomic ion.
D) the attraction between two nonmetal atoms.
E) the attraction between two metal atoms.
Answer: B
2) A covalent bond is best described as
A) the sharing of electrons between atoms.
B) the transfer of electrons.
C) a bond between a metal and a nonmetal.
D) a bond between a metal and a polyatomic ion.
E) a bond between two polyatomic ions.
Answer: A
3) Give a possible molecular formula for the empirical formula of C3H5ClO.
A) C6H10ClO2
B) C5H10Cl2O2
C) C6H10Cl2O2
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D) C6H10O2
Answer: C
E) C6H12Cl2O2
4) What is the empirical formula for Hg2(NO3)2?
A) Hg2(NO3)2
C) Hg(NO3)2
B) HgNO3
D) Hg2NO3
Answer: B
5) Give the name for SnO.
A) tin(I) oxide
B) tin(II) oxide
Answer: B
E) Hg4(NO3)4
C) tin(III) oxide
D) tin(IV) oxide
6) Give the name for TiCO3. Remember that titanium forms several ions.
A) titanium(II) carbonate
C) titanium carbonite
E) titanium(I) carbonate
B) titanium carbide
D) titanium(II) carbonite
Answer: A
7) Write the name for Sn(SO4)2. Remember that Sn forms several ions.
A) tin(I) sulfite
C) tin sulfide
E) tin(I) sulfate
B) tin(IV) sulfate
D) tin(II) sulfite
Answer: B
8) Give the name for KMnO4.
A) potassium manganese tetraoxide
B) potassium manganate
C) potassium permanganate
Answer: C
D) potassium permagnesium
E) potassium magnesate
9) Give the name for CoCl2∙6H2O. Remember that Co forms several ions.
A) cobalt chloride hydrate
D) cobalt(II) chloride hexahydrate
B) cobalt(I) chloride heptahydrate
E) cobalt(I) chloride
C) cobalt(II) chloride heptahydrate
Answer: D
10) Give the correct formula for aluminum sulfate.
A) Al2SO4
C) Al3(SO4)2
B) Al(SO4)3
D) Al2(SO4)3
Answer: D
11) Write the formula for copper (II) sulfate pentahydrate.
A) Cu2SO3∙H5
C) CuS∙5H2O
D) (CuSO4)5
B) Cu2S∙H2O
E) CuSO4∙5H2O
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Answer: E
12) Give the name for H2CO3.
A) carbonous acid
B) dihydrogen carbonate
Answer: C
C) carbonic acid
D) hydrocarbonic acid
13) Give the formula for sulfurous acid.
A) H2SO3
B) HSO3
Answer:
14) Give the name for P4O10.
A) phosphorus(IV) oxide
B) diphosphorus pentoxide
Answer: E
E) hydrocarbide acid
C) H2SO4
D) HSO4
C) phosphorus oxide
D) phosphorus(II) oxide
E) tetraphosphorus
decoxide
15) Identify the FALSE statement about acid rain.
A) Acid rain contains nitric acid and sulfuric acid.
B) Acid rain dissolves marble statues.
C) Acid rain comes from coal-powered electric power plants.
D) Acid rain corrodes steel bridges.
E) Acid rain comes from hydroelectric power plants.
Answer: E
16) Calculate the molar mass of Al(C2H3O2)3.
A) 86.03 g/mol
C) 56.00 g/mol
B) 204.13 g/mol
D) 258.09 g/mol
Answer: B
E) 139.99 g/mol
17) Calculate the molar mass of Ca3(PO4)2.
A) 87.05 g/mol
C) 310.18 g/mol
B) 215.21 g/mol
D) 279.21 g/mol
Answer: C
E) 246.18 g/mol
18) Calculate the molar mass of H2CO3.
A) 62.03 g/mol
C) 61.02 g/mol
B) 29.02 g/mol
D) 60.01 g/mol
Answer: A
E) 74.04 g/mol
19) The molecular weight of urea ((NH2)2CO), a compound used as a nitrogen fertilizer, is
________ amu (rounded to one decimal place).
A) 44.0
C) 60.1
E) 32.0
B) 43.0
D) 8.0
Answer: C
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20) How many millimoles of Ca(NO3)2 contain 4.78 × 1022 formula units of Ca(NO3)2? The
molar mass of Ca(NO3)2 is 164.10 g/mol.
A) 12.6 mmol Ca(NO3)2
C) 20.7 mmol Ca(NO3)2
E) 57.0 mmol Ca(NO3)2
B) 13.0 mmol Ca(NO3)2
D) 79.4 mmol Ca(NO3)2
Answer: D
21) How many molecules of N2O4 are in 76.3 g N2O4? The molar mass of N2O4 is 92.02
g/mol.
A) 5.54 × 1025 N2O4 molecules
D) 4.59 × 1025 N2O4 molecules
B) 7.26 × 1023 N2O4 molecules
E) 4.99 × 1023 N2O4 molecules
C) 1.38 × 1024 N2O4 molecules
Answer: E
22) How many moles of N2O4 are in 76.3 g N2O4? The molar mass of N2O4 is 92.02 g/mol.
C) 1.00 mole
E) 0.829 moles
A) 7.02 × 103 moles
D) 1.21 moles
B) 1.42 × 10-4 moles
Answer: E
23) How many C2H4 molecules are contained in 45.8 mg of C2H4? The molar mass of C2H4 is
28.05 g/mol.
A) 9.83 × 1020 C2H4 molecules
D) 3.69 × 1023 C2H4 molecules
B) 7.74 × 1026 C2H4 molecules
E) 4.69 × 1023 C2H4 molecules
C) 2.71 × 1020 C2H4 molecules
Answer: A
24) What is the mass (in kg) of 6.89 × 1025 molecules of CO2? The molar mass of CO2 is 44.01
g/mol.
A) 3.85 kg
C) 2.60 kg
E) 6.39 kg
B) 5.04 kg
D) 3.03 kg
Answer: B
25) Determine the number of moles of sodium in 3.20 moles of sodium hydrogen phosphate.
A) 6.40 moles of sodium
C) 9.60 moles of sodium
E) 12.80 moles of sodium
B) 3.20 moles of sodium
D) 1.60 moles of sodium
Answer: A
26) Determine the number of moles of oxygen in 3.20 moles of sodium hydrogen phosphate.
A) 6.40 moles of oxygen
C) 9.60 moles of oxygen
E) 12.80 moles of oxygen
B) 3.20 moles of oxygen
D) 1.60 moles of oxygen
Answer: E
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27) Calculate the mass percent composition of sulfur in Al2(SO4)3.
A) 28.12%
C) 42.73%
E) 35.97%
B) 9.372%
D) 21.38%
Answer: A
28) Calculate the mass percent composition of lithium in Li3PO4.
A) 26.75%
C) 30.72%
B) 17.98%
D) 55.27%
Answer: B
E) 20.82%
29) How many atoms of oxygen are contained in 47.6 g of Al2(CO3)3? The molar mass of
Al2(CO3)3 is 233.99 g/mol.
A) 1.23 × 1023 O atoms
C) 2.87 × 1025 O atoms
E) 3.68 × 1023 O atoms
B) 2.96 × 1024 O atoms
D) 1.10 × 1024 O atoms
Answer: D
30) How many atoms of carbon are contained in 47.6 g of Al2(CO3)3? The molar mass of
Al2(CO3)3 is 233.99 g/mol.
A) 1.23 × 1023 C atoms
C) 2.87 × 1025 C atoms
E) 3.68 × 1023 C atoms
B) 2.96 × 1024 C atoms
D) 1.10 × 1024 C atoms
Answer: E
31) Determine the volume of hexane that contains 5.33 × 1022 molecules of hexane. The density
of hexane is 0.6548 g/mL and its molar mass is 86.17 g/mol.
A) 8.59 mL
C) 7.40 mL
E) 11.6 mL
B) 13.5 mL
D) 12.4 mL
Answer: E
32) How many molecules of butane are contained in 25.0 mL of butane? The density of butane
is 0.6011 g/mL and the molar mass is 58.12 g/mol.
A) 2.59 × 1023 molecules butane
D) 1.56 × 1023 molecules butane
B) 1.46 × 1027 molecules butane
E) 7.14 × 1025 molecules butane
C) 6.87 × 1023 molecules butane
Answer: D
33) Determine the molecular formula of a compound that has a molar mass of 183.2 g/mol and
an empirical formula of C2H5O2.
A) C2H5O2
C) C3H7O3
E) C8H20O8
B) C6H15O6
D) C4H10O4
Answer: B
34) Determine the molecular formula of a compound that has a molar mass of 92.0 g/mol and an
empirical formula of NO2.
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A) N2O3
B) N3O6
Answer: C
C) N2O4
D) NO2
E) N2O5
35) Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.
A) NO
C) NO2
E) NO3
B) N2O
D) N2O3
Answer: D
36) Determine the empirical formula for a compound that is found to contain 10.15 mg P and
34.85 mg Cl.
A) P3Cl
C) PCl2
E) PCl3
B) PCl
D) P2Cl3
Answer: E
37) Determine the empirical formula for a compound that contains C, H and O. It contains
52.14% C and 34.73% O by mass.
A) C2H6O
C) C4H13O2
E) CH3O
B) CHO
D) CH4O3
Answer: A
38) Determine the molecular formula of a compound that is 49.48% carbon, 5.19% hydrogen,
28.85% nitrogen, and 16.48% oxygen. The molecular weight is 194.19 g/mol.
A) C8H12N4O2
C) C8H10N4O2
B) C4H5N2O
D) C8H10N2O
Answer: C
39) Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg
of CO2 and 59.38 mg of H2O. What is the empirical formula for the compound?
A) C5H2O
C) C3H6O
E) C6HO3
B) CHO
D) C3H7O
Answer: C
40) Write a balanced equation to show the reaction of sulfurous acid with lithium hydroxide to
form water and lithium sulfite.
A) H2SO4(aq) + LiOH(aq) → H2O(l) + Li2SO4(aq)
B) H2SO3(aq) + 2 LiOH(aq) → 2 H2O(l) + Li2SO3(aq)
C) HSO3(aq) + LiOH(aq) → H2O(l) + LiSO3(aq)
D) HSO4(aq) + LiOH(aq) → H2O(l) + LiSO4(aq)
E) H2S(aq) + 2 LiOH(aq) → 2 H2O(l) + Li2S(aq)
Answer: B
41) Write a balanced equation to show the reaction of gaseous ethane with gaseous oxygen to
form carbon monoxide gas and water vapor.
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A) 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)
B) C2H6(g) + 5 O(g) → 2 CO(g) + 3 H2O(g)
C) 2 C2H6(g) + 5 O2(g) → 4 CO(g) + 6 H2O(g)
D) C2H6(g) + 7 O(g) → 2 CO2(g) + 3 H2O(g)
E) 2 CH3(g) + 5 O(g) → 2 CO(g) + 3 H2O(g)
Answer: C
42) Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous
ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate.
A) Al(C2H3O2)2(aq) + (NH4)2PO4(aq) → AlPO4(s) + 2 NH4C2H3O2(aq)
B) Al(C2H3O2)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3C2H3O2(aq)
C) Al(CO3)2(aq) + (NH3)2PO4(aq) → AlPO4(s) + 2 NH3CO3(aq)
D) Al(C2H3O2)3(aq) + (NH4)3PO4(aq) → AlPO4(s) + 3 NH4C2H3O2(aq)
E) Al(CO2)3(aq) + (NH4)3PO3(aq) → AlPO3(s) + 3 NH4CO2(aq)
Answer: D
43) Identify rubbing alcohol.
A) CH3CH2CH2OH
B) CH3CH2OH
Answer: D
C) CH3OH
D) (CH3)2CHOH
44) Identify the alcohol in fermented drinks.
A) CH3CH2CH2OH
C) CH3OH
B) CH3CH2OH
D) (CH3)2CHOH
Answer: B
45) Identify the compound with covalent bonds.
A) CH4
C) LiBr
D) Mg
B) Ar
Answer: A
E) HOCH2CH2OH
E) HOCH2CH2OH
E) NaI
46) Which of the following contains BOTH ionic and covalent bonds?
A) BaF2
D) SF6
covalent bonds.
B) Cl2
E) None of the above
contains both ionic and
C) MgSO4
Answer: C
47) Identify the element that chlorine forms a covalent bond with.
A) carbon
C) barium
B) sodium
D) copper
Answer: A
E) nickel
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48) Identify the compound with ionic bonds.
A) Ne
C) N2
B) CO
D) H2O
Answer: E
49) What is the empirical formula for C10H20O5?
A) C2H5O
C) C2H4O
B) CHO
D) CHO2
Answer: C
50) Write a possible molecular formula for C4H4O.
A) C24H24O6
C) C2H2O
D) C8H8O
B) C12H12O2
Answer: A
E) KCl
E) CH2O