This document provides a study guide for a chapter 8 test on covalent bonding. It includes definitions and characteristics of ionic compounds and covalent compounds. It outlines steps to draw Lewis electron dot structures and provides example questions to practice this. It also covers drawing resonance structures, defining polar bonds and molecules, denoting partial charges on polar molecules, and ranking intermolecular forces. The review sheet is intended to guarantee covering all topics that will be on the 12-15 question test, with an option to use the sheet during the test with a maximum grade of 90%.

1. Name __________________________________________ Date ___________________
Chapter 8 Study Guide
Covalent Bonding
• What is a covalent bond?
• What are the characteristics of molecular compounds (covalently bonded compounds)
Characteristics of Ionic and Covalent Compounds
Characteristics
Ionic compound Covalent compound
Representative element Formula unit
Bond formation Transfer of one or more
electrons between atoms
Type of elements Metallic and nonmetallic
Physical state Solid
Melting point High (usually above 300
deg. Celcius)
Solubility in water Usually high
Electrical conductivity of Good conductor
aqueous solution
• Know how to write the Lewis electron dot structure for a molecular compound given
its molecular formula.
• The trick part is figuring out how many bonds to draw. It’s easy if you follow these
steps.
1. Count the number of ____________________________________________________
2. Subtract that number from ________________________________________________
3. Divide your answer by _________
4. That number equals _____________________________________________________
5. Draw the structure with the correct number of bonds and don’t forget to make sure
every octet is full.

2. Example Questions
(Use the steps above to figure out how many bonds there are in each molecule, then draw
the structures of each of the molecules.)
1.) Br2
2.) CH4
3.) H20
4.) S2
5.) As2
• Know how to draw resonance structures
Example Question
(Draw all the possible resonance structures for the molecule below.)
O3
• What is a polar bond?
• Know how to use Table S to determine the electronegativity difference and the chart
below to determine what kind of bond will be made.

3. Electronegativity Differences and Bond Types
Electronegativity Difference Range Most Probably type of bond
0.0-0.4
0.4-1.0
1.0-2.0
> 2.0
Example Problems
1.) What kind of bond will be produced between H and Cl?
2.) What kind of bond will be produced between N and N?
3.) What kind of bond will be produced between Li and Br?
• What is a polar molecule?
• Know how to denote the partial charges of a polar bond on a molecule with symbols
Example Problems
First draw the structure of each molecule, then using symbols, write the partial charges
cause by polar bonds on each molecule.
1.) HCl 2.) H20 3.) CF4 4.) CO2
• What is a polar molecule? (Explain why a molecule which has polar bonds can either
be polar or non polar)

4. Example problems
1.) Is CO2 polar? Why? (use a drawing of the molecule in your explanation)
2.) Is H2C polar? Why? (use a drawing of the molecule in your explanation)
• Rank the strengths of the intermolecular attraction forces
1.
2.
3.
4.
***This test will only be 12-15 questions, due to the shortened class time tomorrow. This
review sheet will have the basis of how to answer each question guaranteed. Know this
review sheet and you’ll do great on the test***
***Even though I don’t think you’ll need it, I will allow offer you the opportunity to use
this review sheet on tomorrows test. However if you choose to use it, the highest grade
you may receive will be a 90%***