102年 - [無官方正解]102 國立嘉義大學_轉學生招生考試試題_應用化學系：普通化學#145292

1. Which of the following description is true for 12Mg2+ (A) 12 protons, 12 neutrons, and 12 electrons
(B) 12 protons, 12 neutrons, and 10 electrons
(C) 10 protons, 12 neutrons, and 12 electrons
(D) 12 protons, 10 neutrons, and 12 electrons

2. How many state function in the following: work, temperature, internal energy, and enthalpy.
(A) 1 (B) 2 (C) 3 (D) 4

3. Which of the following contain most number of hydrogen atoms ? (A) 2.0 x 102 mg H2O (B) 10 ppm H2 in 10kg dry ice
(C) 1.0 x 105 ng H2 (D) 10-4 mole CH4

4. Which of the following nomenclature is correct for CuCl ? (A) cupric chloride (B) cupric chlorine (C) copper (I) chloride (D) copper chloride

5. What is the coefficient for water when the following equation is balanced ?
Fe2O3 + HNO3 → Fe(NO3)3 + H2O
(A) 1 (B) 2 (C) 3 (D) 4

6. Which of the following atoms has the highest first ionization energy?
(A) O (B) C (C) Na (D) Mg

7. Consider the following reaction: 2A + 3B → 2C + D
3.0 mol A and 2.0 mol B react to form 1.0 mol C. What is the percent yield of this reaction? (A) 33% (B) 67% (C) 75% (D) 100%

8. Which of the following salts is expected to be soluble in water?
(A) Sodium sulfide (B) lead (II) chloride (C) calcium sulfate (D) silver chloride

9. Which of the following statement is correct when 0.1 M of AgNO3(aq) and 0.1M of KI(aq) are mixed?
(A) KNO3 will precipitate; Ag+ and I- will be spectator ions.
(B) No precipitate will form
(C) AgI will precipitate; K+ and I- will be spectator ions.
(D) AgI will precipitate; K+ and NO3- will be spectator ions.

10. Diamond has unusual hardness and melting point. What type of solid is it?
(A) ionic crystal (B) molecular crystal (C) metal crystal (D) covalent crystal

11. Which of the following sets of quantum numbers are not allowed?
(A) n=3, l=2, ml=0 (B) n=4, l=2, ml=1
(C) n=1, l=1, ml=1 (D) n=2, l=1, ml=0

12. As the volume of a gas increases, the pressure decreases due to
(A) a decrease in temperature of the gas molecules.
(B) an increase in the density of the gas system.
(C) a decrease in the number of collisions occurring per unit time.
(D) an increase in the kinetic energy of the gas molecules.

13. When an hydrogen electron makes transition from n = 2 to n = 1, which of the following statements is (are) true?
I. Energy is emitted.
II. Energy is absorbed.
III. The electron loses energy.
IV. The electron gains energy.
V. The electron cannot make this transition.
(A) II, III (B) V (C) I, III (D) II, III

14. Which of the following subshell orbital has the quantum numbers n = 3, l = 2?
(A) 2p (B) 3p (C) 3d (D) 4d

15. In the gaseous phase, which of the following diatomic molecules would be the most polar? (A) LiF (B) CsF (C) NaCl (D) CsCl

16. How many species could have  bond(s) in the following? NO2- , NF3 , CO32- , SO2 , CO2
(A) 1 (B) 2 (C) 3 (D) 4

17. How many of the molecules does not have dipole moment in the gaseous phase? (A) N2O (B) NO2 (C) H2O (D) CO2

18. How many of the following molecule(s) have London dispersion force?
N2O, NO2, H2O, and CO2
(A) 1 (B) 2 (C) 3 (D) 4

19. The atomic number of Bi is 83. What orbital is the highest energy level with electron(s)?
(A) 6s (B) 6p (C) 6d (D) 5d

20. The C-C  bond of H2C=CH2 is formed by two orbitals. What are these orbitals?
(A) s and s (B) s and sp2 (C) s and sp3 (D) sp2 and sp2

21. Given the following acids and Ka values: HClO4 HOAc HCN HF
1 × 107 1.76 × 10-5 4.93 × 10-10 3.53 × 10-4
Which is correct in term of base strength?
(A) CN- ＜ F- ＜ OAc- ＜ ClO4- (B) CN- ＜ OAc- ＜ F- ＜ ClO4- (C) ClO4- ＜ OAc-＜ CN- ＜ F- (D) ClO4-＜ F-＜ OAc- ＜ CN-

22. How much heat is required to raise the temperature of a 4.48-g sample of iron (specific heat = 0.450 J/g℃) from 25.0℃ to 79.8℃?
(A) 1.98 J (B) 246 J (C) 110 J (D) 546 J

23. In the reaction P4(s) + 10Cl2(g) → 4PCl5(s), the reducing agent is
(A) Chlorine (B) PCl5 (C) phosphorus (D) Cl-

24. Four identical 1.0-L flasks contain the gases He, Cl2, CH4, and NH3, each at 0℃ and 1 atm pressure. For which gas do the molecules have the highest average velocity? (A) H2 (B) O2 (C)CO2 (D) NH3

25. In which case must a reaction be spontaneous at all temperatures?
(A) ΔH is positive, ΔS is positive. (B) ΔH = 0, ΔS is negative. (C) ΔS = 0, ΔH is positive (D) ΔH is negative, ΔS is positive.