chapter 8 periodic properties of the elements · p a g e | 1 chapter 8 periodic properties of the...
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P a g e | 1
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.
B) Hund's rule.
C) Aufbau principle.
D) Heisenberg uncertainty principle.
Answer: A
2) Electrons filling up the orbitals from low to high is known as (the)
A) Pauli exclusion principle.
B) Hund's rule.
C) Aufbau principle.
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.
B) Hund's rule.
C) Aufbau principle.
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.
B) vanadium.
C) chromium.
D) manganese.
E) iron.
Answer: C
6) Give the ground state electron configuration for Se.
A) [Ar]4s23d104p4
B) [Ar]4s24d104p4
C) [Ar]4s23d104p6
D) [Ar]4s23d10
E) [Ar]3d104p4
Answer: A
7) Give the ground state electron configuration for Sr.
A) [Kr]5s24d2
B) [Kr]5s24d105p2
C) [Kr]5s2
D) [Kr]5s25d105p2
E) [Kr]5s24d10
Answer: C
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8) Give the ground state electron configuration for Pb.
A) [Xe]6s26p2
B) [Xe]6s25d106p2
C) [Xe]6s25f146d106p2
D) [Xe]6s24f145d106p2
E) [Xe]6s24f145d106s26p
Answer: D
9) How many valence electrons do the alkali metals possess?
A) 1
B) 2
C) 7
D) 6
E) 8
Answer: A
10) How many valence electrons do the noble gases possess?
A) 1
B) 2
C) 7
D) 6
E) 8
Answer: E
11) A cation of +2 indicates that an element has
A) lost two electrons.
B) lost two protons.
C) lost two neutrons.
D) gained two electrons.
E) gained two protons.
Answer: A
12) Give the ground state electron configuration for F⁻.
A) 1s22s22p6
B) 1s22s22p5
C) 1s22s22p4
D) 1s22s22p3
E) 1s22s22p2
Answer: A
13) Choose the ground state electron configuration for Zn2⁺.
A) [Ar]4s23d8
B) [Ar]3d10
C) [Ar]4s23d6
D) [Ar]
E) [Ar]3d8
Answer: B
14) Choose the ground state electron configuration for Cr3⁺.
A) [Ar]4s13d2
B) [Ar]
C) [Ar]4s23d6
D) [Ar]3d3
E) [Ar]4s23d1
Answer: D
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-, At-
B) N3-, S2-, Br-, Cs+, Sr2+
C) P3-, S2-, C1-, K+, Ca2+
D) Zn2+, Co2+, Cu2+, Cr2+, Cd2+
E) Ne, Ar, Kr, Xe, He
Answer: C
17) For a particular element, identify the species that has the smallest radius.
A) cation
B) anion
C) neutral
D) radical
E) They are all the same
size.
Answer: A
18) Identify the elements correctly shown by decreasing radii size.
A) N3- > N
B) K+ > K
C) N > N3-
D) Cu2+ > Cu+
E) S- > S2-
Answer: A
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)
B) Li(g) → Li⁺(g) + e⁻ C) Li(g) + e⁻ → Li⁺(g)
D) Li⁺(g) → Li(g) + e⁻ E) Li⁺(g) + e⁻ → Li(g)
Answer: A
21) Which reaction below represents the electron affinity of S?
A) S(g) + e⁻ → S⁻(g)
B) S⁻(g) + e⁻ → S2⁻(g)
C) S(g) → S⁺(g) + e⁻ D) S⁻(g) → S(g) + e⁻
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
C) K > P > As
D) As > K > P
E) K > As > P
Answer: E
23) Place the following in order of increasing metallic character.
Rb Cs K Na
A) K < Cs < Na < Rb
B) Na < K < Rb < Cs
C) Cs < Rb < K < Na
D) K < Cs < Rb < Na
E) Na < Rb < Cs < K
Answer: B
24) Describe the reaction of the noble gases with metals.
A) inert
B) vigorous
C) mild reaction
D) forms water
E) dissolves
Answer: A
25) Describe the reaction of the alkali metals with non-metals.
A) inert
B) vigorous
C) mild reaction
D) forms water
E) dissolves
Answer: B
26) Identify the most reactive alkali metal with water.
A) Cs
B) Rb
C) K
D) Na
E) Li
Answer: A
27) Identify a characteristic of halogens.
A) powerful reducing agents
B) forms water in reactions
C) powerful oxidizing agents
D) absorbs water in reactions
E) inert
Answer: C
28) How many valence electrons does an atom of Tl possess?
A) 3
B) 5
C) 0
D) 4
E) 7
Answer: A
29) How many valence electrons does an atom of Ar possess?
A) 2
B) 4
C) 7
D) 0
E) 8
Answer: E
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30) How many valence shell electrons does an atom of thallium have?
A) 1
B) 4
C) 3
D) 81
E) 7
Answer: C
31) An element that has the valence electron configuration 5s25p5 belongs to which period and
group?
A) period 5; group 5A
B) period 5; group 7A
C) period 6; group 5A
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
B) neon
C) helium
D) iodine
E) oxygen
Answer: C
33) Give the number of core electrons for Te.
A) 2
B) 6
C) 46
D) 50
E) 11
Answer: C
34) How many unpaired electrons are present in the ground state N atom?
A) 0
B) 3
C) 1
D) 2
E) 4
Answer: B
35) How many unpaired electrons are present in the ground state Xe atom?
A) 2
B) 3
C) 0
D) 5
E) 8
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
C) Br; O
D) Br; Se
Answer: C
37) Place the following elements in order of increasing atomic radius.
S Te O
A) Te < S < O
B) S < O < Te
C) O < S < Te
D) O < Te < S
E) Te < O < S
Answer: C
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38) Place the following in order of increasing atomic radius.
Sr Li Ca
A) Sr < Ca < Li
B) Li < Sr < Ca
C) Ca < Sr < Li
D) Sr < Li < Ca
E) Li < Ca < Sr
Answer: E
39) Choose the orbital diagram that represents the ground state of N.
A)
B)
C)
D)
E)
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 E) C6H12Cl2O2
Answer: C
4) What is the empirical formula for Hg2(NO3)2?
A) Hg2(NO3)2
B) HgNO3
C) Hg(NO3)2
D) Hg2NO3
E) Hg4(NO3)4
Answer: B
5) Give the name for SnO.
A) tin(I) oxide
B) tin(II) oxide
C) tin(III) oxide
D) tin(IV) oxide
Answer: B
6) Give the name for TiCO3. Remember that titanium forms several ions.
A) titanium(II) carbonate
B) titanium carbide
C) titanium carbonite
D) titanium(II) carbonite
E) titanium(I) carbonate
Answer: A
7) Write the name for Sn(SO4)2. Remember that Sn forms several ions.
A) tin(I) sulfite
B) tin(IV) sulfate
C) tin sulfide
D) tin(II) sulfite
E) tin(I) sulfate
Answer: B
8) Give the name for KMnO4.
A) potassium manganese tetraoxide
B) potassium manganate
C) potassium permanganate
D) potassium permagnesium
E) potassium magnesate
Answer: C
9) Give the name for CoCl2∙6H2O. Remember that Co forms several ions.
A) cobalt chloride hydrate
B) cobalt(I) chloride heptahydrate
C) cobalt(II) chloride heptahydrate
D) cobalt(II) chloride hexahydrate
E) cobalt(I) chloride
Answer: D
10) Give the correct formula for aluminum sulfate.
A) Al2SO4
B) Al(SO4)3
C) Al3(SO4)2
D) Al2(SO4)3
Answer: D
11) Write the formula for copper (II) sulfate pentahydrate.
A) Cu2SO3∙H5
B) Cu2S∙H2O
C) CuS∙5H2O
D) (CuSO4)5
E) CuSO4∙5H2O
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Answer: E
12) Give the name for H2CO3.
A) carbonous acid
B) dihydrogen carbonate
C) carbonic acid
D) hydrocarbonic acid
E) hydrocarbide acid
Answer: C
13) Give the formula for sulfurous acid.
A) H2SO3
B) HSO3
C) H2SO4
D) HSO4
Answer:
14) Give the name for P4O10.
A) phosphorus(IV) oxide
B) diphosphorus pentoxide
C) phosphorus oxide
D) phosphorus(II) oxide
E) tetraphosphorus
decoxide
Answer: E
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
B) 204.13 g/mol
C) 56.00 g/mol
D) 258.09 g/mol
E) 139.99 g/mol
Answer: B
17) Calculate the molar mass of Ca3(PO4)2.
A) 87.05 g/mol
B) 215.21 g/mol
C) 310.18 g/mol
D) 279.21 g/mol
E) 246.18 g/mol
Answer: C
18) Calculate the molar mass of H2CO3.
A) 62.03 g/mol
B) 29.02 g/mol
C) 61.02 g/mol
D) 60.01 g/mol
E) 74.04 g/mol
Answer: A
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
B) 43.0
C) 60.1
D) 8.0
E) 32.0
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
B) 13.0 mmol Ca(NO3)2
C) 20.7 mmol Ca(NO3)2
D) 79.4 mmol Ca(NO3)2
E) 57.0 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
B) 7.26 × 1023 N2O4 molecules
C) 1.38 × 1024 N2O4 molecules
D) 4.59 × 1025 N2O4 molecules
E) 4.99 × 1023 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.
A) 7.02 × 103 moles
B) 1.42 × 10-4 moles
C) 1.00 mole
D) 1.21 moles
E) 0.829 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
B) 7.74 × 1026 C2H4 molecules
C) 2.71 × 1020 C2H4 molecules
D) 3.69 × 1023 C2H4 molecules
E) 4.69 × 1023 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
B) 5.04 kg
C) 2.60 kg
D) 3.03 kg
E) 6.39 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
B) 3.20 moles of sodium
C) 9.60 moles of sodium
D) 1.60 moles of sodium
E) 12.80 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
B) 3.20 moles of oxygen
C) 9.60 moles of oxygen
D) 1.60 moles of oxygen
E) 12.80 moles of oxygen
Answer: E
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27) Calculate the mass percent composition of sulfur in Al2(SO4)3.
A) 28.12%
B) 9.372%
C) 42.73%
D) 21.38%
E) 35.97%
Answer: A
28) Calculate the mass percent composition of lithium in Li3PO4.
A) 26.75%
B) 17.98%
C) 30.72%
D) 55.27%
E) 20.82%
Answer: B
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
B) 2.96 × 1024 O atoms
C) 2.87 × 1025 O atoms
D) 1.10 × 1024 O atoms
E) 3.68 × 1023 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
B) 2.96 × 1024 C atoms
C) 2.87 × 1025 C atoms
D) 1.10 × 1024 C atoms
E) 3.68 × 1023 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
B) 13.5 mL
C) 7.40 mL
D) 12.4 mL
E) 11.6 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
B) 1.46 × 1027 molecules butane
C) 6.87 × 1023 molecules butane
D) 1.56 × 1023 molecules butane
E) 7.14 × 1025 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
B) C6H15O6
C) C3H7O3
D) C4H10O4
E) C8H20O8
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
C) N2O4
D) NO2
E) N2O5
Answer: C
35) Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.
A) NO
B) N2O
C) NO2
D) N2O3
E) NO3
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
B) PCl
C) PCl2
D) P2Cl3
E) PCl3
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
B) CHO
C) C4H13O2
D) CH4O3
E) CH3O
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
B) C4H5N2O
C) C8H10N4O2
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
B) CHO
C) C3H6O
D) C3H7O
E) C6HO3
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
C) CH3OH
D) (CH3)2CHOH
E) HOCH2CH2OH
Answer: D
44) Identify the alcohol in fermented drinks.
A) CH3CH2CH2OH
B) CH3CH2OH
C) CH3OH
D) (CH3)2CHOH
E) HOCH2CH2OH
Answer: B
45) Identify the compound with covalent bonds.
A) CH4
B) Ar
C) LiBr
D) Mg
E) NaI
Answer: A
46) Which of the following contains BOTH ionic and covalent bonds?
A) BaF2
B) Cl2
C) MgSO4
D) SF6
E) None of the above
contains both ionic and
covalent bonds.
Answer: C
47) Identify the element that chlorine forms a covalent bond with.
A) carbon
B) sodium
C) barium
D) copper
E) nickel
Answer: A
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48) Identify the compound with ionic bonds.
A) Ne
B) CO
C) N2
D) H2O
E) KCl
Answer: E
49) What is the empirical formula for C10H20O5?
A) C2H5O
B) CHO
C) C2H4O
D) CHO2
E) CH2O
Answer: C
50) Write a possible molecular formula for C4H4O.
A) C24H24O6
B) C12H12O2
C) C2H2O
D) C8H8O
Answer: A