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 $^{24}_{12}$Mg²⁺ (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 10⁶ mg H₂O (B) 10 ppm H₂ in 10kg dry ice (C) 1.0 x 10⁴ 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 ? Fe₃O₄ + 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 $\pi$ bond(s) in the following? NO$_{2}^{-}$, NF$_{3}$, CO$_{3}^{2-}$, SO$_{2}$, CO$_{2}$ (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 $\sigma$ 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: HOAc HCN HF HClO₄ 1 x 10⁷ 1.76 x 10⁴ 4.93 x 10⁻¹⁰ 3.53 x 10⁻⁸ 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 P_4(s) + 10Cl_2(g) → 4PCl_3(l), the reducing agent is (A) Chlorine (B) PCl₃ (C) phosphorus (D) Cl^-

24. Four identical 1.0-L flasks contain the gases He, Cl₂, CH₄, and NH₃, each at 0°C 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.

3. Both of NaOH and Al(OH)₃ are solid at room temperature. However, NaOH is soluble in water while Al(OH)₃ is insoluble. Please explain this difference in terms of lattice energies.

4. A balloon is becoming its full extent after heating the air inside. In the final stage of this process the volume of the balloon changes from 4.0 x 10⁸ L to 4.5 x 10⁸ L by addition of 1.3 x 10⁴ J of the energy as heat.
Assuming the balloon expand against a constant pressure of 1.0 atm, please calculate \( \Delta E \) for the process.

5. Use the MO model to predict the electron configuration, bond order and magnetism. (a) N₂ (b) O₂⁺