1. Unit 4 Test Review

2. Identify the following as covalent or ionic.
water (H2O)
salt (NaCl)
iron (II) sulfide (FeS)
calcium bromide (CaBr2)
covalent
ionic

3. CS2 BaI2 N2O4 PCl3 covalent ionic
Identify the following as covalent or ionic.
CS2
BaI2
N2O4
PCl3
covalent
ionic

4. Identify the following as covalent or ionic.
compound is a gas at room temperature
compound, when melted, conducts an electric current
compound is composed of a metal and a nonmetal
compound is composed of a nonmetal and a nonmetal

5. What is a polyatomic ion?
An ion that contains more than 1 element

6. What is meant by binary ionic?
2 elements (metal and nonmetal) joined by ionic bonds

7. What is meant by binary molecular?
2 elements (both nonmetals) joined by covalent bonds

8. What is meant by ternary ionic?
3 elements (metal and nonmetals) joined by ionic bonds

9. What part of the atom is involved in chemical reactions?
Valence electrons

10. Why do atoms share electrons?
To gain the electron configuration of a noble gas

11. Which intermolecular attractive force is the strongest?
Hydrogen bonds

12. Why is carbon special?
it has four electrons in its outermost energy level
it readily bonds with other carbon atoms
it can form single, double, or triple bonds with other atoms

13. What is the Octet Rule?
in chemical compounds, atoms tend to have the electron configuration of a noble gas

14. What is the electron configuration of the sulfide ion (S-2)?
1s22s22p63s23p6

15. A compound that ends in -ate or -ite contains ____.
A polyatomic ion

16. How many valence electrons are transferred from the aluminum atom to oxygen in the formation of the compound aluminum oxide? 3

17. Why are metal good electrical conductors?
They have mobile electrons

18. Which elements can form diatomic molecules joined by a single covalent bond?
halogens and hydrogen

19. Which elements can form diatomic molecules joined by double covalent bonds?
oxygen

20. Which elements can form diatomic molecules joined by triple covalent bonds?
nitrogen

21. What is VESPR Theory?
molecules adjust their shapes to keep valence electrons as far apart as possible

22. What is a polar molecule?
A molecule that has partial positive and negative charges

23. Which of the following covalent bonds is the most polar?
a. H—F
b. H—C
c. H—H
d. H—N

24. What is the charge on the cation in the ionic compound magnesium chloride?+2

25. What is the net charge of the ionic compound potassium fluoride?

26. What is the formula unit of calcium nitride?
Ca3N2

27. What is the formula for potassium sulfate
K2SO4

28. What is the formula unit for sodium sulfide?
Na2S

29. What is the name of the following compound? NaClO2
Sodium chlorite

30. Are the following pairs of elements likely to form ionic or covalent compounds?
phosphorus and sulfur
magnesium and oxygen
aluminum and chlorine

31. What are some properties of ionic compounds?
High melting points
Metal and nonmetal
Conducts electricity in solution
solid

32. What is a cation?
An ion with a positive charge due to loss of electrons
The metal part of an ionic compound

33. What is an anion?
An ion with a negative charge due to gain of electrons
The nonmetal part of an ionic compound

34. Will group 6A elements gain or lose electrons when forming ions
Will group 6A elements gain or lose electrons when forming ions? How many electrons will be gained or lost?
gain 2

35. What is the purpose of a Roman numeral following the name of an element?
To indicate the presence of a transition metal that can have more than one common ionic charge.

36. What ion will sulfur form?
sulfide

37. What is the formula for iron (III) oxide?
Fe2O3

38. What is the formula for phosphorus tetrachloride?
PCl4

39. What is the formula for trisulfur dioxide?
S3O2

40. Reactions between atoms involve which part of the atom?
Valence electrons

41. What is the name of the following compound? CrF3
Chromium (III) fluoride