Practice Final Exam: AP Chemistry
Name: _________________________
Match the notation below with the atom described in questions 1-4:
1) Represents an atom that is in an excited state
2) Represents an atom that is a noble gas
3) Represents an atom that is a transition metal
4) Represents an atom of an alkali earth metal
Questions 5-8 refer to the following descriptions of bonding in different types of solids.
a) Lattice of positive and negative ions held together by electrostatic forces
b) Closely packed lattice with delocalized electrons throughout giving ability to conduct electricity
and permitting ductility
c) Strong single covalent bonds making up a molecule with a low molecular mass
d) Double and/or triple bonds are used to hold atoms together
e) Expanded octet of electrons on the central atom
5)
6)
7)
8)
Potassium Chloride, KCl(s)
Gold, Au(s)
Methane, CH4(s)
Sulfur Hexafluoride, SF6(g)
Questions 9-12 refer to the reactions represented below. Answers may be used more than once.
--
+
a)
H2SeO4(aq) + 2Cl + 2H (aq)
b)
C2H2(g) + O2(g)
CO2(g)+H2O(g)
--
c)
3I2(aq) + 6OH (aq)
++
d)
e)
Ba
(aq)
2--
+ SO4
Ag(s) + 2Cl
--
H2SeO3(aq) +Cl2(g) +H2O(l)
(aq)
(aq)
5I
--
(aq)
--
+ IO3 (aq) + 3H2O(l)
BaSO4(s)
AgCl(s)
9) A reaction with both a weak and a strong acid as reactants
10) A precipitation reaction in which Ca++ could be a spectator ion
11) A reaction in which the same reactant undergoes both oxidation and reduction
12) A combustion reaction
Practice Final Exam AP Chemistry
Page (1)
13)
A 0.10M aqueous solution of potassium phosphate, K3PO4, is a better conductor of electricity
than a 0.10M aqueous solution of potassium bromide, KBr. Which of the following best explains
this observation?
a) K3PO4 is more soluble in water than KBr
b) K3PO4 has a higher molar mass than KBr has.
c) To prepare a given volume of 0.10M solution, the mass of K3PO4 needed is more than
twice the mass of KBr needed.
d) More moles of ions are present in a given volume of 0.10M K3PO4 than in the same
volume of 0.10M KBr.
e) The degree of dissociation of K3PO4 in solution is significantly greater than that of
KBr.
14)
The element rubidium (atomic mass 85.47) consists of two isotopes, one of mass number 85 (Rb85) and the other of mass number 87 (Rb-87). Which one of the following statements about the
isotopes of rubidium is correct?
A. Rb-85 is approximately twice as abundant as Rb-87.
B. Rb-85 is approximately three times as abundant as Rb-87.
C. Rb-87 is approximately twice as abundant as Rb-85.
D. Rb-87 is approximately three times as abundant as Rb-85
15)
How many protons, neutrons and electrons are present in the ion, 3919K+?
a) 39,19,19
b) 20,19,19
c) 19,20,18
d) 19,20,19
e) 19,19,19
16)
Which two species contain the same number of electrons?
A.
B.
C.
D.
17)
Na+ and Ar
F- and Na+
Cl+ and Ar
Fe3+ and Co2+
If an electron shifts from one energy level in an atom to a lower level, energy is emitted. Which
one of the following electron transitions would release the most energy?
A.
B.
C.
D.
Second level to first level
Third level to second level
Third level to first level
First level to fourth level
18)
Which one of the following compounds contains both ionic and covalent bonds?
A. NH4Cl (s)
B. Na2S(s)
C. CO2 (g)
D. ClO2 (g)
19)
Which one of the following species has a lone pair of electrons on the nitrogen atom?
A. NI4+
20)
B. NH4+
C. HCN
bonds?
D. NO3-
All of the following possess a dipole moment except
A. HF
Practice Final Exam AP Chemistry
B. SF2
C. BF3
D. CH2F2
Page (2)
21)
An unknown solid melts at high temperature, is insoluble in water, and does not conduct
electricity in the solid or liquid states. This substance is most likely to be
A. Al B. I2 C. CO2 D. SiO2 E. Ni
22)
What molecular geometry (shape) is expected for BH3?
A) Linear B) Planar
23)
50 cm3 of 1 M hydrochloric acid
25 cm3 of 5 M sodium chloride
100 cm3 of 0.5 M nitric acid
50 cm3 of 2 M sulphuric acid
Which of the molecules given below has/have a nonzero molecular electric dipole?
HCl
I
A. I only
25)
D) Tetrahedral E) Octahedral
Which of the following solutions contains the largest number of moles of solute?
A.
B.
C.
D.
24)
C) Pyramidal
H2O
II
NH3
III
B. I and II only
BF3
IV
CH4
V
C. IV and V only
Use the bond energies below to calculate H for the reaction,
H2C=CH2 + H2  H3C—CH3
energy / kJ mol-1
348
612
436
412
Bond
C—C
C==C
H—H
C—H
A. H = -124 kJ
C. H = 48 kJ
26)
B. H = -48 kJ
D. H = 124 kJ
Ignoring heat lost to the surroundings, which of the following is closest to the final temperature
of a mixture of water if 100.0 grams of water with a temperature of 40ºC is added to 50.0 g of
water at 0.0ºC?
A. 30ºC
27)
D. I, II, and III only
B. 25ºC
C. 20ºC
D. 15ºC
Which of the following processes is/are exothermic?
I. H2O(s)  H2O(g)
II. CO2(g)  CO2(s)
III. O2(l) O2(g)
A. II only
Practice Final Exam AP Chemistry
B. III only
C. I and II only D. I and III only
Page (3)
28)
In the graph below, what quantity is plotted against the atomic number of the third period
elements (sodium to argon)?
•
•
•
•
•
•
•
•
11
12
13
A. Atomic radius
29)
14
15
16
Atomic number
B. Ionisation energy
17
C. Melting point
18
D. Density
In which of the following series are the elements arranged in the order of increasing electrical
conductivity?
A. Mg<Si<S
B. Si<S<Mg
C. S<Mg<Si
D. S<Si<Mg
30)
Use the following reaction to assist answering the next three questions
3A + 2B + C  2D + E
If there is 1.0 mole of each reactant, which substance is the limiting reagent?
a) A
b) B
c) C
d) Both A and B
e) Both A and C
31)
If 2.0 moles of B react with an excess of A and C, how many moles of products D and E
(respectively) are produced?
a) 2, 1
b) 3, 2
c) 4, 2
d) 2, 3
e) none of the above are correct choices
32)
3.0 moles of A react with an excess of B and C. If the reaction produces a 50% yield of reactant
E, what is the actual yield (in moles) of E?
a) 2 moles
b) 1.5 moles
c) 1.0 moles
d) 0.5 moles
e) 0.25 moles
33)
Look at the reaction below.
2--
2+
+
3+
4+
Cr2O7 (aq)+3Sn (aq)+14H (aq)
2Cr (aq)+3Sn (aq)+7H2O(l)
Which lists the element oxidized followed by the element reduced?
a) Cr, Sn b) O, Sn c) O, Cr d) Cr, H e) Sn, Cr
Practice Final Exam AP Chemistry
Page (4)
34)
Which is closest to the molar concentration of K+ in 0.2M K3PO4?
a) 0.30M b) 0.60M c) 1.2M d) 1.6M e) 2.2M
35)
Approximately what mass of CuSO4∙5H2O (250 g∙mol-1) is required to prepare 100.0 mL of
0.50M copper (II) sulfate solution?
a) 6.125 b) 12.5 c) 25.0 d) 37.5 e) 250
36)
A 1.0L solution of 1.0M lithium phosphate, Li3PO4, is diluted to 0.25M. Which is closest to the
amount of water _added_ to dilute the solution?
a) 1.0L b) 2.0L c) 3.0L d) 4.0L e) 5.0L
37)
From the information below, calculate the enthalpy change, ∆Ho, for the reaction:
S(s) + O2(g) ---> SO2(g)
S(s) + 3/2 O2(g) ---> SO3(g)
SO2(g) + 1/2 O2(g) ---> SO3(g)
∆Ho = -395 kJ
∆Ho = -98.3 kJ
A. +494 kJ
C. -297 kJ
38)
B. +297 kJ
D. -494 kJ
Given the following thermochemical data:
N2O4(g)  2NO2(g) ∆Ho = +100 kJ
2NO(g) + O2(g)  2NO2(g) ∆Ho = -50 kJ
determine the heat of reaction
NO(g) + 1/2O2(g)  1/2N2O4(g)
a) -100 b) -75 c) -50 d) -25 e) 0
39)
Which two species are isoelectronic, i.e., they contain the same number of electrons?
A. Rb+ and K+
B. Cl and Na+ C. Cl- and Br- D. Fe2+ and Co2+ E. N-3 and Na+
40)
Which orbital has a spherical shape?
a) 5s b) 4p c) 3d d) 4f e) 5g
41)
The atom of which element, in the ground state, has 2 electrons in each of the three p orbitals?
a) N b) O c) F d) F+ e) O-1
42)
Which set of three quantum numbers (n,l,ml) corresponds to a 2p orbital?
a) 2,1,1
b) 2,0,0
c) 2,2,2
d) 2,1,-2
e) 2,0,1
43)
An electron in a(n) _____ subshell experiences the greatest effective nuclear charge in a
polyelectronic atom.
a) 4f
b) 4p
c) 3d
d) 3s
e) 4s
Practice Final Exam AP Chemistry
Page (5)
44)
Which are the formal charges respectively of H, C, O in this resonance form of the formate ion:
[H-C=O::]-1
A.
B.
C.
D.
E.
45)
A crystalline solid of formula MX is formed by the reaction of an alkali metal with a halogen.
Which of the following conditions will lead to the formation of a crystal with the greatest lattice
energy?
a)
b)
c)
d)
46)
0,0,0,
0, 0, -1
0,+1,0
0, +1,-1
–2, 0, +1
M+ has a small ionic radius and X- has a small ionic radius
M+ has a small ionic radius and X- has a large ionic radius
M has a small ionisation energy and X has a large electron affinity
M has a small heat of vaporisation and X has a small heat of dissociation
Which specie illustrates resonance?
a)
b)
c)
d)
e)
47)
Which molecule is NOT polar?
a. H2CO b. CCl c. PBrCl d. SCO
4
48)
c. tetrahedral
d. square planar e. octahedral
What is the maximum amount of copper that could be obtained from a mixture of 5.0 moles of
Cu2O and 6.0 moles of C according to the balanced equation below?
Cu2O + C  2Cu + CO
B. 6.0 moles
C. 9.0 moles
D. 10.0 moles
Which is closest to the volume of 0.20 M sodium hydroxide solution could be made from 20.0 g of
solid sodium hydroxide (and an unlimited supply of water)?
A. 1.0 dm3
51)
3
2
b. bent
A. 5.0 moles
50)
e. O
What is the shape of the XeCl molecule?
a. linear
49)
4
CO32HCN
H2CO
Br2
NH4+
B. 0.5 dm3
C. 0.25 dm3
D. 2.5 dm3 E. none of these
A sample of a pure compound was found to contain only 0.250 g of hydrogen, 1.500 g of carbon,
and 8.875g of chlorine. What is the empirical formula of the compound? (H= 1, C = 12, Cl = 35.5)
A. CHCl3
Practice Final Exam AP Chemistry
B. CH2Cl2
C. CH2Cl
D. CH3Cl
Page (6)