Chemistry -- Ionic Compounds Study Guide
True/False
Indicate whether the statement is true or false.
____ 1. A positively charged ion is called an anion.
____ 2. Elements tend to react so that they acquire the electron structure of a halogen.
____ 3. A sodium atom tends to lose one electron when it reacts.
____ 4. The electron structure of a zinc ion (Zn2+) is an example of a pseudo-noble gas formation.
____ 5. A Cl– ion is an example of a cation.
____ 6. The ending -ide is used to designate an anion.
____ 7. Nonmetals form a stable outer electron configuration by losing electrons and becoming anions.
____ 8. Elements in group 1 lose their one valence electron, forming an ion with a 1+ charge.
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 9. The overall charge of a formula unit for an ionic compound ____.
a. / is always zero. / c. / is always positive.b. / is always negative. / d. / may have any value.
____ 10. How many chloride (Cl–) ions are present in a formula unit of magnesium chloride, given that the charge on a Mg ion is 2+?
a. / one-half / c. / twob. / one / d. / four
____ 11. Ionic bonds generally occur between ____.
a. / metals.. / c. / a metal and a nonmetalb. / nonmetals. / d. / noble gases.
____ 12. Salts are examples of ____.
a. / nonionic compounds. / c. / nonmetals.b. / metals. / d. / ionic compounds.
____ 13. A three-dimensional arrangement of particles in an ionic solid is called a(n) ____.
a. / crystal lattice. / c. / formula unit.b. / sea of electrons. / d. / electrolyte.
____ 14. The anion that has the formula ClO— is called the ____.
a. / chloride ion. / c. / hypochlorite ion.b. / chlorate ion. / d. / perchlorate ion.
____ 15. Where does a subscript that indicates the number of atoms appear, relative to a chemical symbol in a formula?
a. / to the upper left / c. / to the upper rightb. / to the lower left / d. / to the lower right
____ 16. What is the formula of calcium phosphate, which is made up of the ions Ca2+ and PO43–?
a. / Ca3PO4 / c. / Ca3(PO4)2b. / Ca6PO4 / d. / Ca2(PO4)3
____ 17. In a crystal lattice of an ionic compound, ____.
a. / ions of a given charge are clustered together, far from ions of the opposite charge.b. / ions are surrounded by ions of the opposite charge.
c. / a sea of electrons surrounds the ions.
d. / neutral molecules are present.
Matching
Match the terms below with their correct definitions.
a. / alloy / j. / ionic bondb. / anion / k. / lattice energy
c. / cation / l. / metallic bond
d. / chemical bond / m. / monatomic ion
e. / delocalized electrons / n. / oxidation number
f. / electrolyte / o. / oxyanion
g. / electron sea model / p. / polyatomic ion
h. / formula unit / q. / salts
i. / interstitial alloy
____ 18. Electrons that are free to move in metals
____ 19. For a monatomic ion, is equal to the charge
____ 20. The force that holds two atoms together
____ 21. A charged particle containing more than one atom
____ 22. A positively charged ion
____ 23. A negatively charged ion
____ 24. Represents the way electrons exist in metals
____ 25. A charged particle containing only one atom
____ 26. The electrostatic force that holds oppositely charged particles together
____ 27. A polyatomic ion composed of an element bonded to at least one oxygen atom
____ 28. Shows the simplest ratio of ions in an ionic compound
____ 29. The attraction of a metallic cation for delocalized electrons
Short Answer
For each of the following chemical formulas, write the correct name of the ionic compound represented.
30. Mg(ClO)2
31. Li2O2
32. (NH4)2CO3
33. Fe(IO3)2
34. Which of other element’s Lewis electron dot structures is the same as the Lewis electron dot structure for the ion S2-? Explain your answer.
35. Which of the other element’s Lewis electron dot structures is the same as that for the ion Cl-? Explain your answer.
36. Which of the other element’s Lewis electron dot structures is like that for the ion K+? Explain your answer.
37. Explain how Ca2+ could have similar properties to argon.
For each of the following ionic compounds, write the correct formula for the compound.
38. nickel(II) chloride
39. copper(I) oxide
40. calcium iodate