4. Which of the following salts is insoluble in water?
(A) Na₂S
(B) K₂CO₃
(C) Pb(NO₃)₂
(D) CaCl₂
(E) All of these are soluble in water.

8.Which of the following salts is insoluble in water? (A) Na2S (B) K2CO3 (C) Pb(NO3)2 (D) All of these are soluble in water.

5. You have separate solutions of HCl and H2SO4 with the same concentrations in terms of molarity. You wish to neutralize a solution of NaOH. Which acid solution would require more volume (in mL) to neutralize the base? (A) The HCl solution. (B) The H2SO4 solution. (C) You need to know the acid concentrations to answer this question. (D) You need to know the volume and concentration of the NaOH solution to answer this question. (E) C and D

6. In which of the following does iodine have the lowest oxidation state? (A) LiIO3 (B) IO2 (C) I2O (D) NH4I (E) I2

7. Which of the following statements is correct? (A) The internal energy of a system increases when more work is done by the system than heat was flowing into the system. (B) The internal energy of a system decreases when work is done on the system and heat is flowing into the system. (C) The system does work on the surroundings when an ideal gas expands against a constant external pressure. (D) All statements are true. (E) All statements are false.

8. In the lab, you mix two solutions (each originally at the same temperature) and the temperature of the resulting solution decreases. Which of the following is true? (A) The chemical reaction is releasing energy. (B) The energy released is equal to s  m  T. (C) The chemical reaction is absorbing energy. (D) The chemical reaction is exothermic. (E) More than one of these.

9. Which of these is an isoelectronic series? (A) Na+, K+, Rb+, Cs+ (B) K+, Ca2+, Ar, S2– (C) Na+, Mg2+, S2–, Cl– (D) Li, Be, B, C (E) none of these (A-D)

10. 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.

11. Consider the ionization energy (IE) of the magnesium atom. Which of the following is not true? (A) The IE of Mg is lower than that of sodium. (B) The IE of Mg is lower than that of neon. (C) The IE of Mg is lower than that of beryllium. (D) The IE of Mg is higher than that of calcium (E) The IE of Mg is lower than that of Mg+.

12. In which pair do both compounds exhibit predominantly ionic bonding? (A) SCl6 and HF (B) Na2SO3 and NH3 (C) KI and O3 (D) LiF and H2O (E) LiBr and MgO

13. Which of the following statements concerning lattice energy is false? (A) It is often defined as the energy released when an ionic solid forms from its ions. (B) MgO has a larger lattice energy than NaF. (C) The lattice energy for a solid with 2+ and 2– ions should be two times that for a solid with 1+ and 1– ions. (D) MgO has a larger lattice energy than LiF. (E) All of these are true.

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