Name: __________________________ Date: _____________
1. Use the following data to calculate the standard enthalpy of formation of COCl2(g).
CO(g) + Cl2(g)
COCl2(g)
ΔH° = -108 kJ/mol
The standard enthalpy of combustion of carbon graphite, C(gr), and CO(g) are -393.5
kJ/mol and -283 kJ/mol, respectively.
A) -219 kJ/mol
B) -153 kJ/mol
C) -185 kJ/mol
D) -167 kJ/mol
E) -152 kJ/mol
2. A gas absorbs 300 J of heat and it expands from 10.0 L to 20.0 L against a constant
pressure of 2.00 atm. Calculate the ∆U for the system. (1 L·atm = 101.3 J )
A) -1.73 x 103 J
B) +1.73 x 103 J
C) -2.33 x 103 J
D) +2.33 x 103 J
E) 300. J
3. Which one of the following statements is FALSE?
A) w is a state function
B) ∆U is a state function
C) P, V, and T are state functions
D) An open system can exchange mass and energy with its surrounding.
E) ∆H is equal to the heat change at constant pressure
4. A 3.5 g sample of NH4NO3 was added to 80. mL of water in a coffee cup calorimeter of
negligible heat capacity. As a result, the temperature of solution decreased from 21.6 oC
to 18.1 oC. Calculate the enthalpy change of the solution (∆Hsol ). (specific heat of the
solution = 4.18 J/g. oC; density of water 1.00 g/mL)
A) +28 kJ/mol
B) +1.2 kJ/mol
C) -28 kJ/mol
D) -1.2 kJ/mol
E) -13 kJ/mol
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5. Given the Hfo for NH3(g) and H2O(l) are –46.11 kJ/mol and –241.82 kJ/mol,
respectively, and heat of reaction for the following reaction:
4NH3(g) + 5O2(g)
4 NO(g)
+ 6H2O(l)
H = -905.4 kJ
Determine the heat of formation for the NO(g):
A) +90.3 kJ/mol
B) – 96.7 kJ/mole
C) – 390. kJ/mole
D) +361. kJ/mole
E) +468 kJ/mol
6. Calculate the binding energy of an electron in a metal ejected by a photon with a
wavelength of 4.00 x 104 nm and having the kinetic energy of 4.1 x 10-22 J.
A) 4.6 x 10-21 J
B) 4.0 x 10-22 J
C) 3.8 x 10-21 J
D) – 4.0 x 10-22 J
E) 3.7 x 10-22 J
7. The number of unpaired electrons in the ground state for nitrogen (N) and copper (Cu),
respectively are:
A) 3 e- and 1 eB) 3 e- and 2 eC) 2 e- and 1 eD) 1 e- and 3 eE) 2 e- and 3 e-
8. The number of orbitals allowed in a subshell of the angular momentum quantum
number (l) of 1 and 2, respectively are:
A) 3 and 5 orbitals
B) 7 and 5 orbitals
C) 3 and 7 orbitals
D) 5 and 7 orbitals
E) 1 and 5 orbitals
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9. In the hydrogen atom emission spectrum, calculate the wavelength of a photon emitted
when its electron drops from the n = 7 state to the n = 2 state.
(Rydburg constant = 1.097373 x107 m-1 or -2.18 x10-18 J)
A) 397 nm
B) 300. nm
C) 3.00 x 10-7 nm
D) 2.73 x 10-7 nm
E) 2.52 x 106 nm
10. In a px orbital, the subscript x denotes the ________.
A) axis along which the orbital is aligned
B) energy of the electron
C) spin of the electrons
D) probability of the shell
E) size of the orbital
11. How many valence electrons does S2- have?
A) 8
B) 2
C) 6
D) 4
E) 18
12. Which statement is true about effective nuclear charge?
A) Effective nuclear charge increases as you move to the right across a row in the
periodic table and decreases as you move down a column.
B) Effective nuclear charge increases as you move to the right across a row in the
periodic table and increases as you move down a column.
C) Effective nuclear charge decreases as you move to the right across a row in the
periodic table and decreases as you move down a column.
D) Effective nuclear charge decreases as you move to the right across a row in the
periodic table and increases as you move down a column.
E) Effective nuclear charge is an exception; there is no certain pattern for it across the
periodic table.
13. Which of the following species make an isoelectronic pair?
A) Cl– and Ca2+
B) Co3+ and Fe3+
C) O2– and S2–
D) Ba2+ and Br–
E) Al3+ and P3–
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14. Concerning the electron configuration of fluorine, 1s22s22p5, which of the following
represents the core electrons only?
A) 1s2
B) 1s22s2
C) 2s22p5
D) 2p5
E) 1s22s22p5
15. Rank the two elements rubidium (Rb) and strontium (Sr) with respect to higher first
ionization (IE1), higher second ionization (IE2) and higher first electron affinity (EA1):
A) Sr, Rb, Rb
B) Rb, Rb, Sr
C) Rb, Sr, Rb
D) Rb, Sr, Sr
E) Sr, Sr, Sr
16. Which one of the following ionic solids would have the highest melting pont?
A) AlN
B) NaI
C) MgBr2
D) CaO
E) CsBr
17. Which one of the following statements is TRUE?
A) A covalent bond has a lower potential energy than the two separate atoms.
B) A pair of electrons involved in a covalent bond are sometimes referred to as “lone
pairs”.
C) A covalent bond is formed through the transfer of electrons from one atom to
another.
D) Single bonds are shorter than double bonds.
E) It is not possible for two atoms to share more than two electrons.
18. Choose the bond below that is least polar.
A) C-I
B) N-F
C) C-Br
D) C-Cl
E) C-F
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19. Use the bond energies provided to estimate the enthalpy of the reaction below.
CH3OH(l) + 2 O2(g)
Bond
→
Bond Energy(kJ/mol)
C-H
414
C-O
360
C=O
799
O=O
498
O-H
A)
B)
C)
D)
E)
CO2(g) + 2 H2O(g)
464
-392 kJ
+473 kJ
-91 kJ
486 kJ
+206 kJ
20. Which one of the central atom in the following species obey the octet rule? (Note: The
first atom is the central atom)
A) BrO2B) NO2
C) BH3
D) ICl2E) PCl5
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Answer Key
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