C.P. Chemistry
Study Guide
Test Chapter 6
Topics include but are not limited to:
 Describe the formation of a covalent bond between two nonmetallic elements.
 Describe double and triple covalent bonds
 Create Lewis structures for covalent molecules containing single, double, and triple bonds
 Create resonance structures
 Explain the formation of a coordinate covalent bond
 Describe the shapes of simple covalently bonded molecules using VSEPR theory
 Predict polarity of bonds and molecules
 Write names and chemical formulas for covalent and ionic compounds
(including acids)

C.P. Chemistry Name_____________
Ch 6 Review Covalent Compounds
A. Completion
Date_________Pd.__
Use this completion exercise to check your understanding of the concepts and terms introduced in this chapter. Each blank can be completed with a term, short phrase, or number. Word bank below: double or triple coordinate covalent bond stable electron
Resonance nonpolar lesser dipole single polar shared structural formula electronegativities equally
VSEPR covalent greater unequally
When atoms share electrons to gain the ____1___ configuration of a 1. ____________
Noble gases, the bonds formed are ____2___. A ____3___ pair of valence electrons constitutes a ___4____ covalent bond. Sometimes two or three
2. ____________ pairs of electrons may be shared to give ____5___ covalent bonds. In some 3. ____________ cases only one of the atoms in a bond provides the pair of bonding
4. ____________ electrons; this is a ___6____.
When like atoms are joined by a covalent bond, the bonding electrons
5. ____________ are shared ____7___, and the bond is ____8___. When the atoms in a bond
6. ____________ are not the same, the bonding electrons are shared ____9___, and the bond is ____10__. The degree of polarity of a bond between any two atoms is
7. ____________ determined by consulting a table of ____11__. Some molecules are
8. ____________
____12__ because they contain polar covalent bonds. Bond energies are
9. ____________ affected by bond polarity and the electronegativity of the joined atoms. The shorter the bond, the ____13__ the bond energy. Attractions between 10. ___________ opposite poles of polar molecules constitute a ___14___.
11. ___________
As a general rule, molecules adjust their three-dimensional shapes so that the valence electron pairs around a central atom are as far apart as 12. ___________ possible. This is the guiding principle in the valence shell electron pair
13. ___________ repulsion, or ___15___ theory of molecular geometries.
The ___16___ of a covalent compound shows the arrangement, number 14. ___________ and types of atoms in the molecule. ___17___ occurs when more than one
15. ___________ electron dot structure can be drawn for a particular molecule.

B. True-False
Classify each of these statements at always true, AT; sometimes true, ST; or never true, NT. For the statements that are ST and NT, explain why.
______ 1. In a polar covalent bond the more electronegative atom has a slight positive charge.
______ 2. In general, the electronegativity values of nonmetallic elements are greater than the electronegativity of metallic elements.
______ 3. A molecule with polar bonds must itself be polar.
______ 4. If two or more atoms are covalently bonded together, a molecule of a compound results.
______ 5. To attain a noble gas electron structure, a nitrogen atom must lose its five valence electrons.
______ 6. The compound OF
2
contains two double covalent bonds.
______ 7. Unshared pairs of electrons affect the shape of molecules.
______ 8. Covalent compounds are network solids.
C. Questions
Answer the following questions in the space provided.
1. Draw the Lewis Structures for each of the following compounds: a) Br
2 b) HCN C) NH
4
+
2. Draw three resonance structures for SO
3
.

NH
3
CO
2
3. For each compound, draw the Lewis structure, state the shape, polarity of the bonds and tell if the molecule is polar or nonpolar.
Formula Lewis Structure Shape Polarity of
Bonds
Polarity of
Molecule
H
2
O
CCl
4

D. Naming Covalent and Ionic Compounds (including acids)
Compound
16. Molecular (Covalent) Compound Name
Formula a. Carbon dioxide b. c. d. e. f.
Diphosphorus pentoxide
Dinitrogen monoxide
CCl
H
2
SeF
4
O
6 g. h. i. j. k.
17.
Ionic Compound
Name a. magnesium nitrate b. iron (III) oxide c. sodium phosphide d. calcium phosphate e. titanium (II) hydroxide f. lead (IV) chloride
Compound
Formula
(NH
V
2
O
SnCl
4
3
2
)
3
Ca(NO
CrSO
4
PO
3
)
2
4
18. a. b. c. d. f. g. h.
Name or Formula Covalent
CO
Potassium nitrate
CuSO
Sodium bicarbonate e. P
2
Fe
O
2
5
O
3
4
Zinc nitrate
Dihydrogen monoxide or Ionic

19. Acid Name a. Hydrochloric acid b. Chloric acid c. Sulfurous acid d. e.
HF
HNO
3
Acid
Formula