Ch 5 – 8, 22, 23 Review Questions
AP Chemistry
Multiple Choice: Most of the following are actual questions from previous AP Exams. You may work on
them alone or with partners, but try to complete them using only a periodic table and calculator, if necessary.
These 30 questions should take you about 30 minutes to finish.
1. The substance likely to have the largest specific heat capacity at room temperature is:
(A) Fe
(B) H2O
(C) Cu
(D) Ag
(E) N2
2. The molar enthalpy of formation reaction for mercuric oxide is:
(A) 2 Hg (l) + O2 (g) → 2 HgO (s)
(B) Hg (l) + ½ O2 (g) → HgO (s)
(C) 4 Hg (l) + O2 (g) → 2 Hg2O (s)
(D) 2 Hg (l) + ½ O2 (g) → Hg2O (s)
(E) 2 Hg (l) + O2 (g) → Hg2O2 (s)
Given the following list of atomic and ionic species, find the appropriate match for questions 1-4.
(A) Fe2+ (B) Cl (C) K+ (D) Cs (E) Hg+
3.
4.
5.
6.
Has the electron configuration: 1s2 2s2 2p6 3s2 3p6 3d6.
Has a noble gas electron configuration.
Has electrons in f orbitals.
Is isoelectronic with gold.
7. For a neutral As atom in the ground state, how many electrons have quantum numbers n = 4, l = 1?
(A) 2
(B) 3
(C) 4
(D) 5
(E) 6
8. The electron configuration that is impossible is:
(A) 1s2 2s2 2p6
(B) 1s2 2s2 2p3
(C) 1s2 2s2 2p6 3s1
(D) 1s2 2s2 2p6 3s2
(E) 1s2 2s2 2p6 2d2
9. Atom X has 12 protons, 12 electrons, and 13 neutrons. Atom Y has 10 protons, 10 electrons, and 15 neutrons. It
can therefore be concluded that:
(A) atoms X and Y are isotopes.
(B) atom X is more massive than atom Y.
(C) atoms X and Y have the same mass number.
(D) atoms X and Y have the same atomic number.
10. How many unpaired electrons are found in the most stable electronic state (ground state) of a sulfur atom?
(A) 0
(B) 2
(C) 4
(D) 6
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11. Which of the following refers to the ground-state electron configuration of an atom?
(A) 1s1 2s1
(B) [Kr]5p1
(C) [Ne]3s1 3p2
(D) [Ar]4s2 3d6
12. Which of the following atoms would have the highest electron affinity?
(A) Ge
(B) As
(C) Se
(D) Sn
(E) Sb
13. Which series is ranked in order of increasing electronegativity?
(A) O, S, Se, Te
(B) Cl, S, P, Si
(C) In, Sn, N, O
(D) C, Si, P, Se
14. Given the following:
A: Ionization energy
B: Electron affinity
C: Atomic radius
In general, as one moves across a row of the periodic table from the alkali metals to the halogens:
(A) A, B, and C will decrease.
(B) A, B, and C will increase.
(C) A will increase, B and C will decrease.
(D) A and B will increase, C will decrease.
(E) A will decrease, B and C will increase.
15. In any one period of the periodic table, the element in Group I, as compared to the element in Group VII, has a
(A) larger number of valence electrons.
(B) lower electron affinity.
(C) smaller radius.
(D) higher ionization energy.
(E) none of the above.
16. Which of the following would have the largest second ionization energy?
(A) K
(B) Ne
(C) Cl
(D) Na
17. Which of the following would have the greatest shielding effect?
(A) Ba
(B) Ca
(C) Xe
(D) Rb
18. Which series is ranked in order of increasing electronegativity?
(A) N, P, As, Sb
(B) F, O, N, C
(C) I, Br, Cl, F
(D) Ga, Si, P, Se
19. Nitrogen has a higher first ionization energy than oxygen. This is principally the result of
(A) a nuclear charge effect.
(B) greater penetration of the nitrogen p orbitals.
(C) a crowding effect of the electrons.
(D) the extra neutrons of oxygen.
(E) the half-filled subshell of nitrogen.
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20. Which of the following ions is largest in size?
(A) O2(B) Al3+
(C) Na+
(D) F-
(E) Mg2+
21. The elements in which of the following have most nearly the same atomic radius?
(A) Be, B, C, N
(B) Ne, Ar, Kr, Xe
(C) Mg, Ca, Sr, Ba
(D) C, P, Se, I
(E) Cr, Mn, Fe, Co
22. What is the correct order of decreasing first ionization energies for the elements Be, B, and C?
(A) Be>B>C
(B) B>Be>C
(C) B>C>Be
(D) C>Be>B
(E) Be>C>B
23. Assume that an element has the following ionization energies:
1st IE = 600 kJ/mol
2nd IE = 1,800 kJ/mol
3rd IE = 2,750 kJ/mol
4th IE = 11,600 kJ/mol
5th IE = 15,000 kJ/mol
Which of the following is the most probable electron configuration for this element?
(A) 1s2 2s2 2p6
(B) 1s2 2s2 2p6 3s2
(C) 1s2 2s2 2p6 3s1
(D) 1s2 2s2 2p6 3s2 3p1
(E) 1s2 2s2 2p6 3s2 3p3
24. Which chemical species is the smallest in size?
(A) Cl
(B) Cl(C) Cl2-
(D) Cl3-
25. A molecule of which of the following compounds contains a double bond?
(A) C3H8
(B) C2H6
(C) C2H4
(D) C2H6O
(E) CH4
26. A compound that best represents resonance is:
(A) SO2
(B) N2
(C) CO2
(D) HCl
(E) NH3
27. Which of the following compounds does not follow the Octet Rule?
(A) H2O
(B) PH3
(C) PCl3
(D) PCl5
(E) SO3
28. Which species is a free radical?
(A) N2O
(B) NO2-
(C) NO2+
(D) NO
29. The elemental form of carbon is:
(A) diamond (B) coal
(C) graphite
(D) coal
(E) buckminsterfullerene
30. The oxidation number of manganese in potassium permanganate is:
(A) +1
(B) + 3
(C) + 5
(D) + 7
(E) cannot be determined
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ANSWER KEY:
1.
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5.
6.
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30.
B
Water absorbs the most energy without changing temperature
B
Hg (l) + ½ O2 (g) → HgO (s): forms 1 mole
A
transition metals lose their “s” e- before their “d” eC
potassium ion is isoelectronic with argon
E
Hg+ has a filled 4f subshell
E
Hg+ has 79 eB
Arsenic is [Ar] 4s2 3d10 4p3
E
2d does not exist
C
both have mass number 15 (n + p)
B
S is [Ne] 3s2 3p4, and the 3p e- are | |, |, and |
D
represents Fe
C
EA “increases” (becomes more neg) as you move right across a period
C
EN increases as you move right across a period and up the table
D
IE and EA “increase” (although EA gets more neg) as you move right across a period, but radius
decreases
B
Group I(A) elements have 1 valence e- (compared to 7), lower EA, larger radii, and lower IE
D
2nd IE is removing an e- from a filled shell in Na and K, but since the e- is being removed from a
shell closer to the nucleus in Na, it is larger.
A
most inner e- shells, most shielding
C
EN increases as you go up a group
E
removing an e- from a half-filled p subshell in N takes more energy
A
All are isolectronic with Ne, but O has lowest nuclear charge so is largest
E
Periodic trends in transition metals show little variation
B
C (s2 p2) is greatest, then Be (s2) since filled subshell, B is easiest (s2 p1)
D
Major increase from 3rd IE to 4th IE represents 4th IE is removing an inner shell eA
Fewest e- / e- repulsion and fewest shells (compared to Cl2- and Cl3-)
C
Has a C=C double bond (have to draw the Lewis structures)
A
Has O-S=O and O=S-O resonance structures
D
Lewis structure shows P with 10 eD
Has an odd number of eC
graphite
D
KMnO4: K + Mn + 4(O) = zero; 1 + Mn + -8 = 0; Mn = 7
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