11. Consider the reaction below:

N₂(g) + 3H₂(g) 2NH₃(g)

What will happen when more N₂ is added?
(A) The reaction will stop.
(B) Equilibrium will shift to the right.
(C) Equilibrium will shift to the left.
(D) There will be no noticeable change.
(E) One more product will be formed.

12. A complex ion is a charged species consisting of a metal ion surrounded by (A) other transition metals (B) hydrogen ions (C) ligands (D) ligands and counter ions (E) none of these

13. What is the electron configuration of the Ni(II) ion? (A) [Ar] 4s23d6 (B) [Ar] 4s13d7 (C) [Ar] 4s23d8 (D) [Ar] 3d8 (E) none of these

14. Which of the following is the Arrhenius definition of a base? (A) A substance that produces H+ ions in aqueous solution. (B) A substance that produces OH- ions in aqueous solution. (C) A substance that is an H+ donor (D) A substance that is an H+ acceptor (E) A substance that is an OH- donor

15. Calculate the [H+] in a solution that has a pH of 9.00. (A) M (B) M (C) M (D) M (E) none of these

16. Choose the correct equilibrium expression for the following reaction.  (A) (B) (C) (D) (E) none of these

17. Order the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen- bonding) from weakest to strongest. (A) dipole-dipole, London dispersion, ionic, and hydrogen-bonding (B) London dispersion, dipole-dipole, hydrogen-bonding, and ionic (C) hydrogen-bonding, dipole-dipole, London dispersion, and ionic (D) dipole-dipole, ionic, London dispersion, and hydrogen-bonding (E) London dispersion, ionic, dipole-dipole, and hydrogen-bonding

18. What volume of a 0.687 M solution of CaCl2 contains 1.28 g of solute? (A) 59.6 mL (B) 16.8 mL (C) 1.86 mL (D) 7.92 mL (E) 83.2 mL

19. Which of the following is a conjugate acid/base pair? (A) HCl/OCl– (B) H2SO4/SO42– (C) NH4+/NH3 (D) H3O+/OH– (E) more than one of these

20. Which form of electromagnetic radiation has the longest wavelengths? (A) gamma rays (B) microwaves (C) radio waves (D) infrared radiation (E) x-rays

21. 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

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