Review AP Chem
In questions 1 and 2, refer to the
electron configuration shown below.
(A) 1s22s22p63s23p4
(B) 1s22s22p63s23p64s13d5
(C) 1s22s22p83s23p6
(D) 1s22s22p63s23p64s23d4
(E) 1s22s22p63s23p6
1. violates the Pauli Exclusion principle
2. electron configuration of Cr
In questions 1 and 2, refer to the
electron configuration shown below.
(A) 1s22s22p63s23p4
(B) 1s22s22p63s23p64s13d5
(C) 1s22s22p83s23p6
(D) 1s22s22p63s23p64s23d4
(E) 1s22s22p63s23p6
1. violates the Pauli Exclusion principle C
2. electron configuration of Cr B
3. Which of the following has the most
polar bond?
(A) N2
(B) F2
(C) HF
(D) HCl
(E) PCl3
3. Which of the following has the most
polar bond?
(A) N2
(B) F2
(C) HF
(D) HCl
(E) PCl3
4. Molecules that have planar configurations
include which of the following?
I. BF3
II. XeF4
III. NH3
(A)
(B)
(C)
(D)
(E)
I only
III only
I and II
II and III
I, II and III
4. Molecules that have planar configurations
include which of the following?
I. BF3
II. XeF4
III. NH3
(A)
(B)
(C)
(D)
(E)
I only
III only
I and II
II and III
I, II and III
5. Which of the following is most likely to
deviate from ideal gas behavior?
(A) H2
(B) He
(C) Ne
(D) N2
(E) CCl4
5. Which of the following is most likely to
deviate from ideal gas behavior?
(A) H2
(B) He
(C) Ne
(D) N2
(E) CCl4
6. Which of the following explains why,
at room temperature, I2 is a solid, Br2 is
a liquid and Cl2 is a gas?
(A) Hydrogen bonding
(B) Hybridization
(C) Ionic Bonding
(D) Resonance
(E) London dispersion forces
6. Which of the following explains why,
at room temperature, I2 is a solid, Br2 is
a liquid and Cl2 is a gas?
(A) Hydrogen bonding
(B) Hybridization
(C) Ionic Bonding
(D) Resonance
(E) London dispersion forces
7. electron configuration of Cr. Which
set of quantum numbers (n, l ml, ms) is
not possible?
(A) 1, 0, 0 ½
(B) 1, 1, 0 ½
(C) 1, 0, 0 -½
(D) 2, 1 -1, ½
(E) 3, 2 1, ½
7. electron configuration of Cr. Which
set of quantum numbers (n, l ml, ms) is
not possible?
(A) 1, 0, 0 ½
(B) 1, 1, 0 ½
(C) 1, 0, 0 -½
(D) 2, 1 -1, ½
(E) 3, 2 1, ½
8. Which of the following has a dipole
moment of zero?
(A) CCl4
(B) HCN
(C) NO2
(D) NH3
(E) H2O
8. Which of the following has a dipole
moment of zero?
(A) CCl4
(B) HCN
(C) NO2
(D) NH3
(E) H2O
9. Exactly 4.0 g of helium gas, He, is placed into a container
at constant temperature and pressure. Next to the
container of helium is a 28.0 g sample of nitrogen gas, N2,
placed in an identical container and the same temperature
and pressure as the helium. From the list of statements
below, select all that are TRUE.
I. The number of atoms of He is identical to the number
of molecules of N2.
II. The average kinetic energy of the He atoms is the
same as the average kinetic energy of the
nitrogen molecules.
III. The average speed of the helium atoms is the same
as the average speed of the nitrogen molecules.
(A) I only
(B) II only
(C) III only
(D) I and II
(E) I, II and III
9. Exactly 4.0 g of helium gas, He, is placed into a container
at constant temperature and pressure. Next to the
container of helium is a 28.0 g sample of nitrogen gas, N2,
placed in an identical container and the same temperature
and pressure as the helium. From the list of statements
below, select all that are TRUE.
I. The number of atoms of He is identical to the number
of molecules of N2.
II. The average kinetic energy of the He atoms is the
same as the average kinetic energy of the
nitrogen molecules.
III. The average speed of the helium atoms is the same
as the average speed of the nitrogen molecules.
(A) I only
(B) II only
(C) III only
(D) I and II
(E) I, II and III
N2(g) + 3 F2(g)  2 NF3(g)
∆H°= – 264 kJ mol–1; ∆S°= – 278 J K–1 mol–1
The following questions relate to the synthesis reaction
represented by the chemical equation in the box above.
(a) Calculate the value of the standard free energy change, for the
reaction.
(b)Determine the temperature at which the equilibrium constant,
Keq, for the reaction is equal to 1.00. (Assume that ∆H˚ and ∆S˚
are independent of temperature.)
(c) Calculate the standard enthalpy change, ∆H˚, that occurs when
a 0.256 mol sample of NF3(g) is formed from N2(g) and F2(g) at
1.00 atm and 298 K.
The enthalpy change in a chemical reaction is the difference
between energy absorbed in breaking bonds in the reactants and
energy released by bond formation in the products.
(d)How many bonds are formed when two molecules of NF3 are
produced according to the equation in the box above?
(e)Use both the information in the box above and the table of
average bond enthalpies below to calculate the average enthalpy
of the F–F bond.
Bond Average Bond Enthalpy in kJ/mol-1:
NΞN = 946, N-F = 272, F-F = ?
HF(aq) + H2O(l)  H3O+(aq) + F–(aq) Ka = 7.210–4
1. Hydrofluoric acid, HF(aq), dissociates in water as
represented by the equation above.
(a) Write the equilibrium-constant expression for the
dissociation of HF(aq) in water.
(b) Calculate the molar concentration of H3O+ in a 0.40 M
HF(aq) solution.
HF(aq) reacts with NaOH(aq) according to the reaction
represented below.
HF(aq) + OH–(aq)  H2O(l) + F–(aq)
A volume of 15 mL of 0.40 M NaOH(aq) is added to 25 mL of
0.40 M HF(aq) solution. Assume that volumes are additive.
(c) Calculate the number of moles of HF(aq) remaining in the
solution.
(d) Calculate the molar concentration of F–(aq) in the
solution.
(e) Calculate the pH of the solution.