Chapter 8:  Covalent Bonding Review Worksheet						

Section 8.1  Molecular Compounds

1.  Classify each of the following as an atom or molecule:

	a.  Be		b. N2		c.  CO2		d.  H2O		e.  Ne

2.  Which of the following are diatomic molecules?

	a.  CO2		b.  N2		c.  O2		d.  H2O		e.  CO

3. What types of elements tend to combine to form molecular compounds?

4.  What information does a molecule’s molecular structure give?

5.  How do ionic compounds and molecular compounds differ in their relative melting and boiling points?

Section 8.2  The Nature of Covalent Bonding & Section 8.3  Bonding Theories

1.  Draw the electron dot structure for the following compounds AND predict the shape and bond angle for each:

a.  HF

	b.  PF3
	
c.  NCl3

	d.  C2H2
	
e.  CF4

	f.  CO2
	
g.  BCl3

	h. SiF4	
i.  F2O

	j.  H2O	

Section 8.4 Polar Bonds & Molecules

1.  What type of bond – nonpolar covalent, polar covalent, or ionic – will form between each pair of atoms?

	a.  Na and O			b.  O and O			c.  P and O

2.  Explain why most chemical bonds would be classified as either polar covalent or ionic.

3.  Would you expect carbon monoxide and carbon dioxide to be polar or nonpolar molecules?

4.  Draw the structural formulas for each molecule and identify the partial positives & partial negatives, as well as the pulling arrow to the more electronegative atom.

	a.  NH3					b.  CF4

5.  Are the following molecules polar or nonpolar?

	a.  H2O		b.  CO2		c.  NH3		d.  HCl		e.  CH4

General Review Questions

1.  How many shared electron-pairs are represented by each of the following types of bonds:

	a.  single				b.  double			c.  triple

2.  What are nonbonding pairs and how do you tell how many pairs a central element may have?

3.  What is a coordinate covalent bond and what is an example of one?

4.  Define the following types of Intermolecular Attractions:

	a.  Dispersion Forces

	b.  Dipole Interactions

	c.  Hydrogen Bonding