TEST OF CHEMISTRY FOR STUDY AT FUDAN
Total credits: 30 points （45 minutes）
Name_________________
Date_______________
Time________________
Part A (18 points, 18 questions): For each statement or question, select only one that
best completes the statement or answers the question.
1．As the elements in Group 17 on the Periodic Table are considered from top to bottom, what
happens to the atomic radii and the metallic character of each successive element? _____
(A) The atomic radius increases and the metallic character decreases.
(B) The atomic radius and the metallic character both increase.
(C) The atomic radius decreases and the metallic character increases.
(D) The atomic radius and the metallic character both decrease.
2．If the ionization energy for an electron in the first quantum state of a hydrogen atom is 13.6 eV,
what is the ionization energy (in eV) for an electron in the second quantum state? _____
(A) 13.6
(B) 27.2
(C) 3.4
(D) 6.8
3．If a copper bearing material weighing 40 grams yielded 5 grams of CuO (MW 79.55), the
percentage of copper (atomic weight 63.55) in the sample is: _____
(A) 5/40 × 100
(B) 40/5 × 79.55/63.55 × 100
(C) 5/40 × 79.55/63.55 × 100
(D) 5/40 × 63.55/79.55 × 100
4．A covalent bond is unlikely to exist in the product of which of the following reactions? _____
(A) H + H  H2
(B) Br + Br  Br2
(C) Si + 2 F2  SiF4
(D) 2 Ca + O2  2 CaO
5．Which of these substances has the strongest intermolecular force? _____
(A) H2O
(B) H2S
(C) H2Se
(D) H2Te
6．The compound CH3CH==CH2 has a bond formed by the overlap of which of the following
hybrid orbitals? ———
(A) sp2–sp3
(B) sp–sp2
(C) sp–sp3
(D) sp3–sp3
7．Which of the following is most acidic? _____
(A) HF
(B) HCl
(C) HClO4
(D) H3PO4
8．Which of the following ions can act as both a Brônsted acid and base in water? _____
(A) HCO3–
(B) SO42–
(C) NH4+
(D) NO3–
9．Which of the following can function as a Lewis acid? _____
(A) I+
(C) CN–
(B) NH3
(D) CH3–O–CH3
10．Which pH change represents a hundred fold increase in the concentration of H3O+?_____
(A) pH 5 to pH 7
(B) pH 13 to pH 14
(C) pH 3 to pH 1
(D) pH 4 to pH 3
11．Which of the following is the closet to the pH of a 10–9 M HCl? _____
(A) 5
(B) 7
(C) 9
(D) 11
12．For a reaction: NH3 (aq) + H2O (l)  NH4+ (aq) + OH– (aq), if [NH4+] is 10-4 M, [NH3] is 1.0
M, [OH–] is 0.18 M, what is the equilibrium constant of NH3 (aq) hydrolysis? _____
(A) 1.8 × 10–5
(B) 1.8 × 10–4
(C) 1.8 × 10–3
(D) 10–5
13．Given the reaction at equilibrium: H2 (g) + Br2 (g)  2 HBr (g). The rate of the forward
reaction is _____
(A) greater than the rate of the reverse reaction
(B) less than the rate of the reverse reaction
(C) equal to the rate of the reverse reaction
(D) independent of the rate of the reverse reaction
14．Which half-reaction correctly represents reduction? _____
(A) Ag  Ag+ + e–
(B) F2  2 F + 2 e–
(C) Fe2+ + e–  Fe3+
(D) Au3+ + 3e–  Au
15．The equation ΔG = ΔH – T ΔS tells us that which of the following conditions will always be an
exothermic, spontaneous reaction? _____
(A) ΔH > 0, ΔS > 0
(B) ΔH < 0, ΔS > 0
(C) ΔH > 0, ΔS < 0
(D) ΔH < 0, ΔS < 0
16．The activation energy of a reaction can be determined from the slope of which of the following
graphs? _____
(A) ln K vs 1/T
(B) (ln K)/T vs T
(C) ln K vs T
(D) (ln K)/T vs 1/T
17．Given the balanced equation: 4 Fe (s) + 3 O2 (g)  Fe2O3 (s) + 1640 kJ. Which phrase best
describes this reaction? _____
(A) endothermic with H = +1640 kJ
(B) endothermic with H = –1640 kJ
(C) exothermic with H = +1640 kJ
(D) exothermic with H = –1640 kJ
18．For a certain first-order reaction, the time required for half of an initial amount to decompose
is 3 minutes. If the initial concentration of the reaction is 1 molar, how long does it take to
reduce the concentration of A to 0.125 M? _____
(A) 3 min
(B) 6 min
(C) 8 min
(D) 9 min
Part B (12 points, 6 questions): Write down your answers in the spaces.
19．Write ionic equation of the reaction:
NaOH + CH3COOH
20．Balance the oxidation-reduction reactions below.
(a)
(b)
HNO3 + Cu
FeSO4
 Cu(NO3)2
+ NO + H2O
+ KMnO4 + H2SO4  MnSO4 + Fe2(SO4)3 + K2SO4 + H2O
21．Calculate the pH values of the following aqueous solutions (at 25 oC):
(a) 0.010 mol/L NH4Cl
(NH3 ∙ H2O: Kb = 1.8 ×10-5)
(b) Use 1.0 M KOH solution to titrate 20.0 ml 0.50 M HCN solution to the end point (i.e. the
equivalent point) (HCN: Ka = 4.9 ×10-10)
22．Calculate the amount of heat released or absorbed from 1 mol of the following chemical
reaction, 2 NO + O2  2 NO2 , given that the bond energy of the following bonds
are: N–O (165 kJ/mol);
N=O (430 kJ/mol);
O–O (145 kJ/mol);
O=O (498 kJ/mol)