1.
Given the following thermochemical equations:
 
H2S(g) + 3/2 O2(g) → H2O (l) + SO2(g)
ΔH° = -562.3 kJ
1/8 S8(s) + O2(g) → SO2(g)
       ΔH° = -297.0 kJ
2H2(g) + O2(g) → 2H2O (l)
       ΔH° = -533.8 kJ
 
Calculate ΔH° for H2(g) + 1/8 S8 (s) → H2S(g) in kJ.
A.
265.3 kJ
B.
562.3 kJ
C.
276.6 kJ
D.
-1.6 kJ
E.
20.5 kJ


2.
When 745.0 J of energy in the form of heat is transferred from the environment to gas, the expansion of the gas does 312.0 J of work on the environment. What is the change in internal energy of the gas?
A.
433.0 J
B.
-433.0 J
C.
1057 J
D.
-1057 J
E.
105.7 J


3.
Which statement is FALSE about a chemical reaction proceeding under constant volume conditions?
A.
The pressure also remains constant.
B.
The change in internal energy, ΔU, is equal to qv
C.
No PV work is done.
D.
ΔU is a state function.
E.
∆V equals 0.


4.
When 2.065 g of styrene (C8H8) is burned in a constant-volume calorimeter at 298 K, 87.14 kJ of heat is evolved. Calculate the ∆U for the reaction on a molar basis.
A.
+ 5695 kJ/mol
B.
- 2054 kJ/mol
C.
- 5695 kJ/mol
D.
+ 3780 kJ/mol
E.
- 4395 kJ/mol


5.
The reaction of iron with hydrochloric acid is represented by the following thermochemical equation.
Fe(s)     +      2HCl(aq) →     FeCl2(aq)     + H2(g)      ΔH° = –87.9 kJ/mol
How much heat is liberated at constant pressure if 0.358 g of iron reacts with 34.1 mL of 0.588 M HCl?
A.
0.563 kJ
B.
0.881 kJ
C.
87.9 kJ
D.
31.5 kJ
E.
4.09 kJ


6.
The decrease in the atomic radius from left to right across a period is due to:
A.
the increase in electrostatic attraction between the effective nuclear charge and the charge on the valence shell.
B.
the increase in the outer shell of an atom across the group.
C.
the decrease of the inner electrons from left to right across a period.
D.
the increase of the inner electrons from left to right across a period.
E.
the decrease in the electron affinity from left to right across a period.


7.
The electron configuration of the copper and chloride in CuCl2 are respectively:
A.
[Ar] 4s13d10 and [Ne] 3s23p5
B.
[Ar] 3d9 and [Ne] 3s23p6
C.
[Ar] 4s23d8 and [Ne] 3s23p6
D.
[Ar] 3d10 and [Ne] 3s23p5
E.
[Ar] 4s13d9 and [Ne] 3s23p6


8.
The effective nuclear charge for the following elements O, B, F and C are respectively: 4.45, 2.42, 5.10 and 3.14. Therefore, the expected effective nuclear charge for the N element is:
A.
3.83
B.
4.50
C.
3.11
D.
4.83
E.
2.99


9.
The element with the electron configuration [Ar] 3d104s24p5 belongs to:
A.
Chalcogen
B.
Transition metals
C.
Halogen
D.
Group 5A
E.
Group 4A


10.
The successive ionization energies of a certain element are I1 = 589.5 kJ/mol, I2 =1145 kJ/mol, I3= 4900 kJ/mol, I4 = 6500 kJ/mol, and I5 = 8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is
A.
N
B.
K
C.
Al
D.
Ca
E.
B


11.
Calculate the ΔH° for the following reaction:
8Mg(s) + S8(s) → 8MgS(s)
 
Using the information provided below:
ΔH° = ?
 
Mg(s) → Mg(g)
ΔH° = 148 kJ/mol
Mg(g) → Mg2+(g) + 2e–
ΔH° = 2186 kJ/mol
S8(s) → 8S(g)
ΔH° = 2232 kJ/mol
S(g) + 2e– → S2–(g)
ΔH° = 450 kJ/mol
Mg2+(g) + S2–(g) → MgS(s)
ΔH°lattice = –3406 kJ/mol
 
A.
–2744 kJ/mol
B.
–2720 kJ/mol
C.
2720 kJ/mol
D.
-3406 kJ/mol
E.
–2340 kJ/mol


12.
In which substance(s) shown below does the central atom have the lowest formal charge? Assume that the Lewis structure for each species obeys the octet rule and ignore resonance.

         I. NO3-      II. CO32-     III. SO3


A.
II only
B.
I only
C.
III only
D.
I and II only
E.
All of them


13.
Which one of the following statements is false concerning ionic bonds and compounds?
A.
Elements of an ionic compound usually carry the same charge.
B.
Ionic bonds are a result of electrostatic forces.
C.
Ionic bonds usually occur between elements with high and low electron affinities.
D.
Lewis dot symbols are useful for tracking electrons.
E.
Two non-metals can not form ionic bonds.                                        


14.
Estimate the enthalpy change for the reaction below given the following bond energies:
Bond
C-H
C-C
C-Cl
H-Cl
Cl-Cl
Bond energy (kJ/mol)
414
347
327
431
242
C2H6(g) + Cl2(g) → C2H5Cl(g) + HCl(g)
A.
-68 kJ/mol
B.
-113 kJ/mol
C.
-102 kJ/mol
D.
-334 kJ/mol
E.
-276 kJ/mol


15.
Which of the following Lewis structure(s) is (are) incorrect?
 
A.
III and IV
B.
I and III
C.
II and IV
D.
II only
E.
IV only


16.
The retina of a human eye can detect light when radiant energy incident on it is at least 4.00 x 10-17 J. For light of 575 nm wavelength, how many photons does this have?
A.
116 photons
B.
1160 photons
C.
11.6 photons
D.
11600 photons
E.
116000 photons


17.
Calculate the wavelength (in nm) of the photon emitted when an electron drops from the n = 4 to the n = 3 level in a hydrogen atom.
A.
1.88 x 103 nm
B.
2.48 x 103 nm
C.
4.88 x 103 nm
D.
8.88 x 103 nm
E.
2.68 x 103 nm


18.
An electron in an atom is in the n = 3 quantum level. What are the possible values of ℓ and mℓ it can have.
A.
ℓ =0 and mℓ =0 ,    ℓ =1 and mℓ = -1, 0, 1 ,   ℓ =2 and mℓ = -2, -1, 0, 1 , 2
B.
ℓ =0 and mℓ =0 ,    ℓ =1 and mℓ = -1, 0, 1 , ℓ =3 and mℓ = -3, -2, -1, 0, 1 , 2, 3
C.
ℓ =2 and mℓ = -2, -1, 0, 1 , 2
D.
ℓ =0 and mℓ =0 ,    ℓ =1 and mℓ = -1, 0, 1
E.
ℓ =1 and mℓ =1


19.
The number of waves that pass through a particular point in one second is called
A.
frequency.
B.
wavelength.
C.
magnitude.
D.
amplitude.
E.
light.


20.
Which of the following statement(s) is/are TRUE?
   I.    The d orbitals can have maximum five orientation orbitals.
   II.   All orbitals in a given atom are roughly the same size.
   III. Atomic orbitals developed using quantum mechanics describe regions of space in which one is most likely to find an electron.
   IV. Since electrons have mass, we must always consider them to have particle properties and never wavelike properties.
A.
I only
B.
II and III only
C.
I, II and IV only
D.
II and IV only
E.
I and III only


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