Download Covalent Bonding and Molecular Structures

C.P. Chemistry
Test Chapter 6
Study Guide
Covalent Bonding and Molecular Structures
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
Ch 6 Review Covalent Compounds
Name_____________
Date_________Pd.__
A. Completion
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
Noble gases, the bonds formed are ____2___. A ____3___ pair of valence
electrons constitutes a ___4____ covalent bond. Sometimes two or three
1. ____________
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
affected by bond polarity and the electronegativity of the joined atoms. The
9. ____________
shorter the bond, the ____13__ the bond energy.
Attractions between 10. ___________
opposite poles of polar molecules constitute a ___14___.
As a general rule, molecules adjust their three-dimensional shapes so
11. ___________
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
repulsion, or ___15___ theory of molecular geometries.
13. ___________
The ___16___ of a covalent compound shows the arrangement, number 14. ___________
and types of atoms in the molecule. ___17___ occurs when more than one
electron dot structure can be drawn for a particular molecule.
15. ___________
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 OF2 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) Br2
b) HCN
C) NH4+
2. Draw three resonance structures for SO3.
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
H2 O
CCl4
NH3
CO2
Lewis Structure
Shape
Polarity of
Bonds
Polarity of
Molecule
D. Naming Covalent and Ionic Compounds (including acids)
16. Molecular (Covalent) Compound Name
a.
Carbon dioxide
b.
Diphosphorus pentoxide
c.
Dinitrogen monoxide
Compound
Formula
d.
CCl4
e.
H2O
f.
SeF6
17.
Ionic Compound
Name
a.
magnesium nitrate
b.
iron (III) oxide
c.
sodium phosphide
Compound
Formula
18.
Name or Formula Covalent
or Ionic
a.
CO
b.
Potassium nitrate
c.
CuSO4
d.
calcium phosphate
e.
titanium (II)
hydroxide
d.
Sodium
bicarbonate
f.
lead (IV) chloride
e.
P2O5
f.
Zinc nitrate
g.
Fe2O3
h.
Dihydrogen
monoxide
g.
(NH4)3PO4
h.
V2O3
i.
SnCl2
j.
Ca(NO3)2
k.
CrSO4
19.
Acid Name
a.
Hydrochloric acid
b.
Chloric acid
c.
Sulfurous acid
Acid
Formula
d.
HF
e.
HNO3