所屬科目：研究所、轉學考(插大)◆普通化學
1. How many significant figures are in 0.0035? (A) 5 (B) 3 (C) 4 (D) 2
2. Perform the following calculation to the correct number of significant figures. 56.55×0.920÷34.2585= (A) 1.519 (B) 1.5186 (C) 1.52 (D) 1.5185
3. Aluminum metal melts at 660 °C. What is the temperature in Kelvin? (A) 387 °K (B) 423 °K (C) 897 °K (D) 933 °K
4. What is the mass in grams of 0.172 moles of NaHCO3? (A) 10.4 (B) 14.4 (C) 12.8 (D) 11.4
5. Which sample contains the greatest number of molecules? (A) 1.0 g of CH4 (B) 1.0 g of H2O (C) 1.0 g of HNO3 (D) 1.0 g of N2O4
6. The total number of electrons allowed in a ℓ = 1 sublevel is (A) 2 (B) 6 (C) 8 (D) 10
7. What is the mass in grams of 5.00×1012 water molecules? (A) 1.67×1012 g (B) 6.69×109 g (C) 4.61×10-13 g (D) 1.50×10-10 g
8. Arrange these elements in order of increasing atomic radius. Ca, F, Li, N (A) Li < N < F < Ca (B) Ca < Li < N < F (C) F < N < Li < Ca (D) Ca < F < N < Li
9. What is the oxidation state for I in the NaIO4 molecule? (A) +7 (B) +5 (C) +3 (D) +1
10. For which of the following compounds does 1.0 g represent 5.55×10-2 mol? (A) NO2 (B) H2O (C) C2H6 (D) NH3
11. A 12.0-g sample of HF is dissolved in water to give 3.1×102 mL of solution. The concentration of the solution is (A) 3.9 M (B) 3.7 M (C) 0.19 M (D) 1.9 M
12. Lead(II) nitrate reacts with sodium chloride in aqueous solution to form a precipitate. What is the net ionic equation for this reaction?(A) \( \text{Pb}^{2+}(aq) + 2\text{NO}_3^-(aq) \rightarrow \text{Pb}(\text{NO}_3)_2(s) \) (B) \( \text{Na}^+(aq) + \text{Cl}^-(aq) \rightarrow \text{NaCl}(s) \) (C) \( \text{Pb}^{2+}(aq) + 2\text{Cl}^-(aq) \rightarrow \text{PbCl}_2(s) \) (D) \( \text{Na}^+(aq) + \text{NO}_3^-(aq) \rightarrow \text{NaNO}_3(s) \)
13. Air is 79% N2 and 21% O2 by volume. Calculate the density of air at 1.0 atm, 25°C. (A) 0.590 g/L (B) 1.18 g/L (C) 2.46 g/L (D) 14.1 g/L
14. Which of the following is a conjugate acid-base pair? (A) HCl/ClO2- (B) H2PO4-/PO43- (C) NH3/NH4+ (D) H2O/OH-
15. The strong acid HA is added to water. Which of the following is the strongest base in the system? (A) HA (B) A– (C) H2O (D) H3O+
16. Identify the strongest base. (A) CH3O– (B) CH3OH (C) CN– (D) NO3–
17. What concentration of HF (Ka = 7.2×10–4) has the same pH as that of 0.068 M HCl? (A) 0.068 M (B) 0.16 M (C) 6.4 M (D) 0.011 M
18. A calorimeter contains 123 g of water at 27.0°C. A block of metal with a mass of 28 g is heated to 95.8°C and then placed in the water in the calorimeter. After sufficient time, the temperature of the water is measured and found to be 28.8°C. Calculate the heat capacity per gram of metal. Assume no heat is lost to the calorimeter or the surroundings. (A) 2.0 J/g°C (B) 0.12 J/g°C (C) 6.8×102 J/g°C (D) 0.49 J/g°C
19. 75.0 mL of a pure liquid at 245 K is mixed with 100.0 mL of the same pure liquid at 365. K. What is the final temperature of the mixture? (A) 295 K (B) 305 K (C) 314 K (D) 325 K
20. For which process is ΔS negative? (A) evaporation of 1 mol of CCl4(l) (B) mixing 5 mL of ethanol with 25 mL of water (C) compressing 1 mol of Ne at constant temperature from 1.5 atm to 0.5 atm (D) raising the temperature of 100 g of Cu from 275 K to 295 K
21. Which of the following frequencies corresponds to light with the longest wavelength? (A) \( 3.00 \times 10^{11} \text{ s}^{-1} \) (B) \( 4.12 \times 10^{6} \text{ s}^{-1} \) (C) \( 8.50 \times 10^{10} \text{ s}^{-1} \) (D) \( 9.12 \times 10^{11} \text{ s}^{-1} \)
22. In Bohr's atomic theory, when an electron moves from one energy level to another energy level more distant from the nucleus, (A) energy is emitted. (B) energy is absorbed. (C) no change in energy occurs. (D) light is emitted.
23. The ionization energy for a hydrogen atom is \( 1.31 \times 10^4 \) J/mol. What is the ionization energy for He+? (A) \( 8.72 \times 10^4 \) J/mol (B) \( 1.31 \times 10^4 \) J/mol (C) \( 5.25 \times 10^4 \) J/mol (D) \( 2.18 \times 10^4 \) J/mol
24. How many electrons can be described by the quantum numbers n = 4, l = 3, ml = 0? (A) 0 (B) 2 (C) 6 (D) 10
25. Of the following elements, which needs 3 electrons to complete its valence shell? (A) Ba (B) K (C) Si (D) P
26. Choose the compound with the most ionic bond. (A) LiCl (B) KF (C) NaBr (D) RbI
27. Which of the following elements forms the most ionic bond with chlorine? (A) Rb (B) Ga (C) N (D) Ar
28. Which of the following is nonpolar? (A) Cl2O (B) CS2 (C) SF4 (D) NCl3
29. Which of the following molecules contains a double bond? (A) CO2 (B) NH3 (C) H2O (D) CH3OH
30. What is the hybridization of S in the molecule H2S? (A) sp (B) sp2 (C) sp3 (D) dsp3
31. For which order reaction is the half-life of the reaction independent of the initial concentration of the reactant(s)? (A) zero order (B) first order (C) second order (D) all of these
32. Which intermolecular force is the strongest? (A) dipole-dipole interactions (B) London dispersion forces (C) hydrogen bonding (D) ionic bonding
33. Which of the following is the correct order of boiling points for NaNO3, CH3OH, C2H6, and Ne? (A) Ne < CH3OH < C2H6 < NaNO3 (B) NaNO3 < CH3OH < C2H6 < Ne (C) Ne < C2H6 < NaNO3 < CH3OH (D) Ne < C2H6 < CH3OH < NaNO3
34. A solution is made of 178.0 g of methanol (CH3OH) in 153.0 g of water. What is the mole fraction of methanol? (A) 0.538 (B) 0.562 (C) 0.395 (D) 0.605
35. A salt solution sits in an open beaker. Assuming constant temperature and pressure, the vapor pressure of the solution (A) increases over time. (B) decreases over time. (C) stays the same over time. (D) We need to know which salt is in the solution to answer this.
36. Within a group, as the atomic numbers of the elements increase, the (A) ionization energies decrease. (B) atomic masses decrease. (C) elements become less metallic. (D) atomic radii decrease.
37. The Haber process (A) is used to manufacture ammonia. (B) transforms nitrogen to other nitrogen-containing compounds. (C) is used to recover sulfur from underground deposits. (D) is used to produce nitric acid.
38. The color of a transition metal complex results from (A) bending vibrations. (B) stretching vibrations. (C) transition of an electron between d orbitals. (D) transition of an electron between an s orbital and a p orbital.
39. Which of the following processes decreases the atomic number by 2? (A) gamma-ray production (B) beta production (C) positron-particle production (D) alpha-particle production
40. The half-life for electron capture for K is 1.30×109 years. What percent of the original K remains after 3.90×109 years? (A) 33.3% (B) 12.5% (C) 50.0% (D) 25.0%
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