General Chemistry II Sample Page 1of 20
evssm_04
1. According to the Bronsted—Lowry definition, 8. The weakest of the bases listed is
which chemical species can function both as an
acid and as a base? Acid Conjugate Ka (Ionization
a. Cl— Base Constant of Acid)
b. SO42— HCl Cl— 100% ionized
c. NH4+ HSO4— SO42— 1.2 x 10-2
d. HCO3— H2S HS— 5.7x10-8
e. H3O+ HS— S2— 1.2x10-13
a. Cl—
2. In the reaction CN— + H2O HCN + OH— b. CN—
which is an acid—base conjugate pair? c. HS—
a. H2O and HCN d. S2—
b. H2O and OH— e. SO42—
c. CN— and H2O
d. HCN and OH— 9. The oxide of which element will react with water
to form the strongest acid?
3. Given that HX is a stronger Bronsted acid than
HY in aqueous solution, which is true of a 1 M Main Groups
solution of NaX Period I II II IV V VI VII O
a. It is less basic than a 1 M solution of NaY. I
b. It is more basic than a 1 M solution of NaY. First
c. It yields a neutral solution. Second X Y Z P Q S U
d. It is more concentrated than a 1 M solution Third W R T M
of NaY.
a. W
4. The pH of a 0.03 M HCl solution is
b. M
a. 1.5
c. P
b. 2.5
d. R
c. 3.5
e. Z
d. 12.5
10. Which statement is a logical inference from
5. The pH of a 1.0 x 10—3 M Ba(OH)2 solution at
the fact that a 0.10 M solution of potassium
25oC is
acetate KC2H3O2, is less alkaline than a 0.10 M
a. 2.7
solution of potassium cyanide, KCN?
b. 3.0
c. 11.0 a. Hydrocyanic acid is a weaker acid than
d. 11.3
acetic acid.
b. Hydrocyanic acid is less soluble in water
6. Which is the strongest acid?
than acetic acid.
c. Cyanides are less soluble than acetates
a. HClO
d. Acetic acid is a weaker acid than
b. HClO2
hydrocyanic acid
c. HClO3
d. HClO4
11. In the titration of 50.0 mL of 0.100 M
benzoic acid (a monoprotic acid) with 50.0 mL of
7. Which salt reacts with water (hydrolyzes) to
0.100 M NaOH, the properties of the solution at
produce a basic solution?
the equivalence point will correspond exactly to
the properties of
a. NaC2H3O2
a. a 0.100 M sodium solution.
b. NaNO3
b. a 0.0500 M sodium hydroxide solution.
c. NH4Cl
c. a 0.0500 M benzoic acid solution.
d. BaSO4
d. a 0.0500 M sodium benzoate solution.
,General Chemistry II Sample Page 2of 20
12. A mixture of which pair of 0.1 M aqueous 19. Which electron transition is associated with
solutions would constitute a buffer? the largest emission of energy?
a. NaOH and NaCl
b. HCl and NaOH a. n=2 to n=1
c. HCl and NaCl b. n=2 to n=4
d. NH3 and NH4NO3 c. n=2 to n=3
d. n=3 to n=2
13. What do these have in common?
20 19 1- 24
Ne F Mg2+ 20. If an electron moves from one energy level
in an atom to another energy level more remote
a. the same number of protons from the nucleus of the same atom
b. the same number of neutrons a. energy is absorbed.
c. the same number of electrons b. energy is liberated.
d. the same size c. there is no energy change.
d. the atom must assume a different ionic
14. The number of neutrons in the nucleus of valence
an atom of 13 27Al is e. light of a definite wave length is emitted.
a. 40
b. 13 21. A photon of light of 450 nm, when
c. 27 compared to light of wavelength 300 nm, has
d. 14 (1nm = 10-9 m)
e. 9
a. a higher frequency.
15. The orbitals of 2p electrons are often b. lower energy.
represented as being c. a greater velocity.
a. elliptical. d. a shorter wavelength
b. Pyramidal
c. Tetrahedral 22. Which set of quantum numbers is possible
d. dumbbell shaped for an electron in an atom?
e. spherical.
a. n=3, l=0, ml=1, ms = -½
16. The element in Period 5, Group 3A, has the b. n=2, l=2,ml= -2, ms = -½
outer electron configuration c. n=5, l=2, ml=2, ms =+½
a. 5s25p1 d. n=4, l=3, ml= -4, ms= -½
b. 3s23p5
c. 3s23p3 23. A compound consisting of an element
d. 5s25p3 having a low ionization potential and a second
element having a high electron affinity is likely
17. Which electron configuration is to have
impossible?
a. 1s22s22p63s2 a. covalent bonds
b. 1s22s22p63s23p6 b. metallic bonds
c. 1s22s22p62d2 c. coordinate covalent bonds
d. 1s22s22p53s1 d. ionic bonds.
18. The element X occurs naturally to the 24. According to modern bonding theory the
extent of 20.0% 12X and 80.0% 13X. The atomic number of sigma () and pi () bonds in the
mass of X is nearest ethylene molecule H2C=CH2 is
a. l and 4
a. 12.2 b. l and 1
b. 12.5 c. l and 5
c. 12.8 d. 2 and 4
d. 13.0 e. l and 6
, General Chemistry II Sample Page 3of 20
25. The number of bonds in N=N is Standard Potentials Eo
a. 1 Mg Mg2++2e 2.37V
b. 2 Al Al3++3e 1.66V
c. 3 Zn Zn2++2e 0.76V
d. 4 2+
FeFe +2e 0.44V
Cu Cu2++2e 0.34V
26. The elements in an ionic compound are Ag Ag++ e -0.80V
held together by 31. Using only the metals Mg, Al, Zn, Fe, Cu
and Ag, together with their 1 M salt solutions, a
a. electrostatic forces of attraction. voltaic cell of the highest possible voltage would
b. van der Waals forces be constructed using electrodes of these metals.
c. the spin of paired electrons. a. Mg and Ag
d. the formation of hybrid orbitals. b. Mg and Fe
e. an electron pair. c. Zn and Cu
d. Al and Ag
27. In every electrolytic and galvanic (voltaic) e. Mg and Al
cell the anode is that electrode
32. E = Eo - 0.059/n log Q (Nernst equation)
a. at which oxidation occurs. +
[H ] = 1.0 M initially, P02 = 1.0 atm
b. which attracts cations.
c. at which electrons are supplied to the 4e + O2(g)+4H+(aq) 2H2O(l) Eo=1.23V
solution. Based on the information above, which statement
d. at which reduction occurs. is correct?
28. Metal X was plated from a solution a. n = 1, since one mole of oxygen is being
containing cations of X. The passage of 48.25 C considered.
deposited 31 mg of X on the cathode. What is the b. Addition of base should result in an E
mass of X (in grams) per mole of electrons? value, which is less than 1.23 V.
a. 47 c. E is independent of the pH of the solution.
b. 62 d. Q = [H2O]2
c. 93 [O2] [H+]
d. 186
33. The equilibrium constant for the gaseous
29. In a galvanic (voltaic) cell in which the reaction C + D E + 2F is 3.0 at 50 oC. In a
reaction is Cd + Cu2+ Cu + Cd2+ 2.0 L flask at 50 oC are placed 1.0 mol of C, 1.0
and the ions are at unit concentration (activity), mol of D, 1.0 mol of E, and 3.0 mol of F.
the cell potential is Initially, the reaction will
a. proceed at equal rates in both directions.
Cd Cd2++ 2e- 0.4021 V b. proceed more rapidly to form E and F.
Cu Cu2+ + 2e- - 0.344 V c. proceed more rapidly to form C and D.
a. 0.1383 V d. not occur in either direction.
b. 0.4021 V
c. 0.344 V Compound Gof kJ/mol
d. 0.7461 V H2O(l) —237
e. 0.3677 V H2O(g) —229
34. At 298 K the equilibrium constant for
30. In which reaction will an increase in total
H2(g) + ½ O2(g) H2O(l)
pressure at constant temperature favor formation
of the products?
a. is larger than the Keq for
a. CaCO3(s) CaO(s) + CO2(g)
H2(g) + ½ O2(g) H2O(g)
b. H2(g) + Cl2(g) 2HCl(g)
c. 2NO(g) + O2(g) 2NO2(g) b. will have a value of 1 0 at equilibrium.
c. cannot be computed since data on O2 and
d. COCl2(g) CO(g) + Cl2(g)
evssm_04
1. According to the Bronsted—Lowry definition, 8. The weakest of the bases listed is
which chemical species can function both as an
acid and as a base? Acid Conjugate Ka (Ionization
a. Cl— Base Constant of Acid)
b. SO42— HCl Cl— 100% ionized
c. NH4+ HSO4— SO42— 1.2 x 10-2
d. HCO3— H2S HS— 5.7x10-8
e. H3O+ HS— S2— 1.2x10-13
a. Cl—
2. In the reaction CN— + H2O HCN + OH— b. CN—
which is an acid—base conjugate pair? c. HS—
a. H2O and HCN d. S2—
b. H2O and OH— e. SO42—
c. CN— and H2O
d. HCN and OH— 9. The oxide of which element will react with water
to form the strongest acid?
3. Given that HX is a stronger Bronsted acid than
HY in aqueous solution, which is true of a 1 M Main Groups
solution of NaX Period I II II IV V VI VII O
a. It is less basic than a 1 M solution of NaY. I
b. It is more basic than a 1 M solution of NaY. First
c. It yields a neutral solution. Second X Y Z P Q S U
d. It is more concentrated than a 1 M solution Third W R T M
of NaY.
a. W
4. The pH of a 0.03 M HCl solution is
b. M
a. 1.5
c. P
b. 2.5
d. R
c. 3.5
e. Z
d. 12.5
10. Which statement is a logical inference from
5. The pH of a 1.0 x 10—3 M Ba(OH)2 solution at
the fact that a 0.10 M solution of potassium
25oC is
acetate KC2H3O2, is less alkaline than a 0.10 M
a. 2.7
solution of potassium cyanide, KCN?
b. 3.0
c. 11.0 a. Hydrocyanic acid is a weaker acid than
d. 11.3
acetic acid.
b. Hydrocyanic acid is less soluble in water
6. Which is the strongest acid?
than acetic acid.
c. Cyanides are less soluble than acetates
a. HClO
d. Acetic acid is a weaker acid than
b. HClO2
hydrocyanic acid
c. HClO3
d. HClO4
11. In the titration of 50.0 mL of 0.100 M
benzoic acid (a monoprotic acid) with 50.0 mL of
7. Which salt reacts with water (hydrolyzes) to
0.100 M NaOH, the properties of the solution at
produce a basic solution?
the equivalence point will correspond exactly to
the properties of
a. NaC2H3O2
a. a 0.100 M sodium solution.
b. NaNO3
b. a 0.0500 M sodium hydroxide solution.
c. NH4Cl
c. a 0.0500 M benzoic acid solution.
d. BaSO4
d. a 0.0500 M sodium benzoate solution.
,General Chemistry II Sample Page 2of 20
12. A mixture of which pair of 0.1 M aqueous 19. Which electron transition is associated with
solutions would constitute a buffer? the largest emission of energy?
a. NaOH and NaCl
b. HCl and NaOH a. n=2 to n=1
c. HCl and NaCl b. n=2 to n=4
d. NH3 and NH4NO3 c. n=2 to n=3
d. n=3 to n=2
13. What do these have in common?
20 19 1- 24
Ne F Mg2+ 20. If an electron moves from one energy level
in an atom to another energy level more remote
a. the same number of protons from the nucleus of the same atom
b. the same number of neutrons a. energy is absorbed.
c. the same number of electrons b. energy is liberated.
d. the same size c. there is no energy change.
d. the atom must assume a different ionic
14. The number of neutrons in the nucleus of valence
an atom of 13 27Al is e. light of a definite wave length is emitted.
a. 40
b. 13 21. A photon of light of 450 nm, when
c. 27 compared to light of wavelength 300 nm, has
d. 14 (1nm = 10-9 m)
e. 9
a. a higher frequency.
15. The orbitals of 2p electrons are often b. lower energy.
represented as being c. a greater velocity.
a. elliptical. d. a shorter wavelength
b. Pyramidal
c. Tetrahedral 22. Which set of quantum numbers is possible
d. dumbbell shaped for an electron in an atom?
e. spherical.
a. n=3, l=0, ml=1, ms = -½
16. The element in Period 5, Group 3A, has the b. n=2, l=2,ml= -2, ms = -½
outer electron configuration c. n=5, l=2, ml=2, ms =+½
a. 5s25p1 d. n=4, l=3, ml= -4, ms= -½
b. 3s23p5
c. 3s23p3 23. A compound consisting of an element
d. 5s25p3 having a low ionization potential and a second
element having a high electron affinity is likely
17. Which electron configuration is to have
impossible?
a. 1s22s22p63s2 a. covalent bonds
b. 1s22s22p63s23p6 b. metallic bonds
c. 1s22s22p62d2 c. coordinate covalent bonds
d. 1s22s22p53s1 d. ionic bonds.
18. The element X occurs naturally to the 24. According to modern bonding theory the
extent of 20.0% 12X and 80.0% 13X. The atomic number of sigma () and pi () bonds in the
mass of X is nearest ethylene molecule H2C=CH2 is
a. l and 4
a. 12.2 b. l and 1
b. 12.5 c. l and 5
c. 12.8 d. 2 and 4
d. 13.0 e. l and 6
, General Chemistry II Sample Page 3of 20
25. The number of bonds in N=N is Standard Potentials Eo
a. 1 Mg Mg2++2e 2.37V
b. 2 Al Al3++3e 1.66V
c. 3 Zn Zn2++2e 0.76V
d. 4 2+
FeFe +2e 0.44V
Cu Cu2++2e 0.34V
26. The elements in an ionic compound are Ag Ag++ e -0.80V
held together by 31. Using only the metals Mg, Al, Zn, Fe, Cu
and Ag, together with their 1 M salt solutions, a
a. electrostatic forces of attraction. voltaic cell of the highest possible voltage would
b. van der Waals forces be constructed using electrodes of these metals.
c. the spin of paired electrons. a. Mg and Ag
d. the formation of hybrid orbitals. b. Mg and Fe
e. an electron pair. c. Zn and Cu
d. Al and Ag
27. In every electrolytic and galvanic (voltaic) e. Mg and Al
cell the anode is that electrode
32. E = Eo - 0.059/n log Q (Nernst equation)
a. at which oxidation occurs. +
[H ] = 1.0 M initially, P02 = 1.0 atm
b. which attracts cations.
c. at which electrons are supplied to the 4e + O2(g)+4H+(aq) 2H2O(l) Eo=1.23V
solution. Based on the information above, which statement
d. at which reduction occurs. is correct?
28. Metal X was plated from a solution a. n = 1, since one mole of oxygen is being
containing cations of X. The passage of 48.25 C considered.
deposited 31 mg of X on the cathode. What is the b. Addition of base should result in an E
mass of X (in grams) per mole of electrons? value, which is less than 1.23 V.
a. 47 c. E is independent of the pH of the solution.
b. 62 d. Q = [H2O]2
c. 93 [O2] [H+]
d. 186
33. The equilibrium constant for the gaseous
29. In a galvanic (voltaic) cell in which the reaction C + D E + 2F is 3.0 at 50 oC. In a
reaction is Cd + Cu2+ Cu + Cd2+ 2.0 L flask at 50 oC are placed 1.0 mol of C, 1.0
and the ions are at unit concentration (activity), mol of D, 1.0 mol of E, and 3.0 mol of F.
the cell potential is Initially, the reaction will
a. proceed at equal rates in both directions.
Cd Cd2++ 2e- 0.4021 V b. proceed more rapidly to form E and F.
Cu Cu2+ + 2e- - 0.344 V c. proceed more rapidly to form C and D.
a. 0.1383 V d. not occur in either direction.
b. 0.4021 V
c. 0.344 V Compound Gof kJ/mol
d. 0.7461 V H2O(l) —237
e. 0.3677 V H2O(g) —229
34. At 298 K the equilibrium constant for
30. In which reaction will an increase in total
H2(g) + ½ O2(g) H2O(l)
pressure at constant temperature favor formation
of the products?
a. is larger than the Keq for
a. CaCO3(s) CaO(s) + CO2(g)
H2(g) + ½ O2(g) H2O(g)
b. H2(g) + Cl2(g) 2HCl(g)
c. 2NO(g) + O2(g) 2NO2(g) b. will have a value of 1 0 at equilibrium.
c. cannot be computed since data on O2 and
d. COCl2(g) CO(g) + Cl2(g)
