112年 - 112 國立嘉義大學_轉學生招生考試試題_獸醫學系：普通化學#143850

1. An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent). Molecules of what type are present in the substance? (A) neither polar nor nonpolar (B) polar (C) either polar or nonpolar (D) nonpolar (E) none of these

2. Which of the following is a strong acid? (A) HF (B) KOH (C) HClO₄ (D) HClO (E) HBrO

3. In the reaction C(s) + O₂(g) → CO₂(g) carbon is __________. (A) the reducing agent (B) the electron acceptor (C) reduced (D) the oxidizing agent (E) more than one of these

4. Which gas has the highest density? (A) He (B) Cl₂ (C) CH₄ (D) NH₃ (E) all gases the same

5. If M is the molar mass, R the gas constant, T the temperature, and P its pressure, which of the following expressions represents the density of a gas? (A)\( \frac{PM}{RT} \) (B)\( \frac{RM}{PT} \) (C)\( \frac{RMP}{T} \) (D)\( \frac{RTM}{p} \) (E)\(\frac{RT}{PM} \)

6. A gas absorbs 0.0 J of heat and then performs 15.8 J of work. The change in internal energy of the gas is (A) 31.6 J (B) 15.8 J (C) –31.6 J (D) –15.8 J (E) none of these

7. Calculate the work associated with the expansion of a gas from 42.0 L to 79.0 L at a constant pressure of 14.0 atm. (A) 518 L·atm (B) –518 L·atm (C) –1.11 × 10³ L·atm (D) 588 L·atm (E) 1.11 × 10³ L·atm

8. What is the specific heat capacity of a metal if it requires 169.6 J to change the temperature of 15.0 g of the metal from 25.00°C to 32.00°C? (A) 0.619 J/g°C (B) 11.3 J/g°C (C) 24.2 J/g°C (D) 1.62 J/g°C (E) 275 J/g°C

9. Choose the correct equation for the standard enthalpy of formation of CO(g), where ΔHf° for CO = –110.5 kJ/mol (gr indicates graphite).  (A) 2C(gr) + O₂(g) → 2CO(g), ΔH° = –110.5 kJ (B) C(gr) + O(g) → CO(g), ΔH° = –110.5 kJ (C) C(gr) + O₂(g) → CO(g), ΔH° = –110.5 kJ (D) C(gr) + CO₂(g) → 2CO(g), ΔH° = –110.5 kJ (E) CO(g) → C(gr) + O(g), ΔH° = –110.5 kJ

10. Which of the following statements best describes the Heisenberg uncertainty principle? (A) The exact position of an electron is always uncertain. (B) The velocity of a particle can only be estimated. (C) It is impossible to accurately know both the exact location and momentum of a particle. (D) The location and momentum of a macroscopic object are not known with certainty. (E) The location and momentum of a particle can be determined accurately, but not the identity of the particle.

11. Which of the following best describes an orbital? (A) space where electrons are unlikely to be found in an atom (B) space which may contain electrons, protons, and/or neutrons (C) the space in an atom where an electron is most likely to be found (D) small, walled spheres that contain electrons (E) a single space within an atom that contains all electrons of that atom

12. If n = 2, how many orbitals are possible? (A) 3 (B) 4 (C) 2 (D) 8 (E) 6

13. How many electrons can be described by the quantum numbers n = 2, l = 2, m_l = 2? (A) 0 (B) 2 (C) 6 (D) 10 (E) 14

14. Which of the following combinations of quantum numbers is not allowed? (A) n = 1, l = 1, ml = 0, ms = (B) n = 3, l = 0, ml = 0, ms = - (C) n = 2, l = 1, ml = -1, ms = (D) n = 4, l = 3, ml = -2, ms = - (E) n = 4, l = 2, ml = 0, ms =

15. Which of the following processes represents the ionization energy of bromine? (A) Br(s) Br+(g) + e^– (B) Br(l) Br+(g) + e^– (C) Br(g) Br+(g) + e^– (D) Br(s) Br+(s) + e^– (E) Br2(g) Br2+(g) + e^–

16. Which of the following groups contains no ionic compounds? (A) HCN, NO₂, Ca(NO₃)₂ (B) PCl₅, LiBr, Zn(OH)₂ (C) KOH, CCl₄, SF₄ (D) NaH, CaF₂, NaNH₂ (E) CH₂O, H₂S, NH₃

17. In which pair do both compounds exhibit predominantly ionic bonding? (A) SCl₄ and HF (B) Na₂SO₃ and NH₃ (C) KI and O₃  (D) BaF and H₂O (E) RbCl and MgS

18. Atoms with greatly different electronegativity values are expected to form (A) no bonds (B) covalent bonds (C) triple bonds (D) ionic bonds (E) none of these

19. Which of the following bonds is least polar? (A) C—O (B) H—C (C) S—Cl (D) Br—Br (E) They are all nonpolar.

20. For the elements Ba, F, and P, the order of increasing electronegativity is: (A) Ba < F < P (B) Ba < P < F (C) P < F < Ba (D) F < Ba < P (E) none of these

21. In which case is the bond polarity incorrect? (A) δ⁺H–Fδ^– (B) δ⁺K–Oδ^– (C) δ⁺Mg–Hδ^– (D) δ⁺Cl–Iδ^– (E) δ⁺Si–Sδ^–

22. Which of these is an isoelectronic series? (A) Na⁺, K⁺, Rb⁺, Cs⁺ (B) K⁺, Ca²⁺, Ar, S^2– (C) Na⁺, Mg²⁺, S^2–, Cl^– (D) Li, Be, B, C (E) none of these (A-D)

23. Which of the following ionic compounds has the largest lattice energy (i.e., the lattice energy most favorable to a stable lattice)? (A) BaO (B) BeO (C) CsI (D) NaBr (E) BaS

24. How many of the following molecules possess dipole moments?

BH₃, CH₄, PCl₅, H₂O, HF, H₂ (A) 1 (B) 2 (C) 3 (D) 4 (E) 5

25. Which of the following is the correct order for molecules from most to least polar? (A) CH₄ > CF₂Cl₂ > CF₂H₂ > CCl₄ > CCl₂H₂ (B) CH₄ > CF₂H₂ > CF₂Cl₂ > CCl₄ > CCl₂H₂ (C) CF₂Cl₂ > CF₂H₂ > CCl₂H₂ > CH₄ = CCl₄ (D) CF₂H₂ > CCl₂H₂ > CF₂Cl₂ > CH₄ = CCl₄ (E) CF₂Cl₂ > CF₂H₂ > CCl₄ > CCl₂H₂ > CH₄

26. Which of the following molecules are nonlinear?

NO₂^–, C₂H₂, N₃^–, HCN, CO₂, H₂O₂ (A) C₂H₂, HCN (B) CO₂, N₃^– (C) NO₂^–, H₂O₂ (D) N₃^–, NO₂^– (E) all are linear

27. The bond angles about the carbon atom in the formaldehyde molecule, H₂C=O, are about: (A) 120° (B) 60° (C) 109° (D) 180° (E) 90°

28. The hybridization of the central atom in O3 is: (A) sp (B) sp² (C) sp³ (D) dsp³ (E) d²sp³

29. Which of the following does not contain at least one pi bond? (A) H₂CO (B) CO₂ (C) C₂H₂ (D) C₃H₈ (E) All of the above (A-D) contain at least one pi bond.

30. How many electrons are involved in pi bonding in benzene, C₆H₆? (A) 12 (B) 30 (C) 3 (D) 6 (E) 18

31. In a 0.1 molar solution of NaCl in water, which one of the following will be closest to 0.1? (A) The mole fraction of NaCl. (B) The mass fraction of NaCl. (C) The mass percent of NaCl. (D) The molality of NaCl. (E) All of these are about 0.1.

32. Which of the following chemical or physical changes is an endothermic process? (A) the evaporation of water (B) the combustion of gasoline (C) the mixing of sulfuric acid and water (D) the freezing of water (E) none of these

33. Rank the following compounds according to increasing solubility in water.

I. CH₃–CH₂–CH₂–CH₃ II. CH₃–CH₂–O–CH₂–CH₃ 

III. CH₃–CH₂–OH        IV. CH₃–OH (A) I < III < IV < II (B) I < II < IV < III (C) III < IV < II < I (D) I < II < III < IV (E) None of these (A-D) is correct.

34. Indicate the mass action expression for the following reaction: 2X(g) + Y(g) 3W(g) + V(g) (A) [X]²[Y][W]³[V] (B)\( \frac{[W]^3 [V]}{[X]^2 [Y]} \) (C)\( \frac{[3w][v]}{[2x][y]} \) (D)\( \frac{[x]^2 [y]}{[w]^3 [v]} \) (E) none of these

35. For a reaction in which A and B react to form C, the following initial rate data were obtained:

What is the rate law?  (A) Rate = k[A][B] (B) Rate = k[A]²[B] (C) Rate = k[A][B]² (D) Rate = k[A]²[B]² (E) Rate = k[A]³

36. Which letter shows the activation energy using a catalyst?

(A) a (B) b (C) c (D) d (E) e

37. Which letter shows the change in energy for the overall reaction?

(A) a (B) b (C) c (D) d (E) e

38. Which of the following atoms or ions has three unpaired electrons? (A) N (B) O (C) Al (D) S₂^– (E) Ti₂⁺

39. Which of the following substances contains two pi bonds? (A) C₂H₄ (B) C₃H₈ (C) C₂H₂ (D) C₂H₆ (E) CH₄

40. How many milliliters (mL) of 18.2 M H₂SO₄ are needed to prepare 600.0 mL of 0.10 M H₂SO₄? (A) 0.30 mL (B) 109 mL (C) 3.3 mL (D) 1.6 mL (E) 4.3 mL