Name ______________________
Per. ____
Chapter 7 & 8 Study Guide
Ch 7) Ions – page 187-192
A. Valence electrons:
1. Define valence electrons:
2. Label the number of valence electrons for each column on the table below.
B. Most Common Ion formed:
1. Define octet rule:
2. All atoms will gain or lose electrons to have a filled valence shell of electrons. List the
most common ion formed for each column on the table below.
Example:
Na has1 valence electron, it is easier to lose the one electron then to try and gain 7
more. So sodium will form a 1+ ion.
Therefore, the Na ion has p= 11, e= 10 giving it a 1+ charge since protons are
positive and electrons are negative. All of the alkali metals have one valence electron so they
will all form a 1+ ion.
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____
___ ___ ___ ___
___
___
___
___ ___Valence Electrons
___ ___ ___ ___ ___Most common Ion
Label the metals, non-metals and semi-metals location on the chart above.
3. Which of the above columns form cations and which form anions?
C) Ionic Compounds – pg. 194-198
1. Define ionic bond:
2. What types of elements form an ionic bond? Explain why and give an example of an ionic
compound.
3. What are three properties of ionic compounds?
Ch 8) Molecular Compounds – page 213
Part A)
1. Define covalent bond:
2. Define molecule:
3. Why is oxygen gas a diatomic molecule?
4. Why isn’t sodium chloride a molecule?
5. List three properties of molecular compounds.
Part B) Bond Polarity – page 237
6. Define non-polar covalent bond:
7. Give an example of a non-polar covalent bond.
8. Define polar covalent bond and give an example.
9. Define electronegativeity:
10. Complete the chart below:
Electronegativity difference
Most probable type of bond
0-0.4
0.4-1.0
1.0-2.0
> 2.0
Example