Name: ___________________
Class: ___________
Unit 5 Test Review
1. How many valence electrons are in each of the following atoms AND what are their charges when they
form ions:
a) P
b) Ca
c) B
2. Define:
a) Valence electron –
b) Ionic Bondc) Covalent Bondd) Unshared (Lone) Pair –
e) VSEPR –
f)
Resonance Structure –
g) Subscript –
h) Polar –
i)
Nonpolar –
j)
Hydrogen bond –
k) Dispersion force –
l)
Dipole-dipole interaction –
3. What is the overall charge of any ionic compound?
4. Which subatomic particles are free to drift in metallic compounds?
5. Circle all of the elements below that are diatomic.
O
Ar
H
N
U
Zn
Cl
6. What do the following elements do to gain an octet (become stable)
a) Mg
b) S
7. Fill in each of the blanks below with the word metal or nonmetal.
a. An ionic compound is made of a ______________ and a ________________.
b. A covalent compound is made of ______________________.
c. A metallic bond is made of _______________________.
9. Write I if the compound is ionic and C if the compound is covalent
a. CCl4 _______
b. KCl _______
c. CuI _______
10. What are the properties of ionic and covalent compounds?
11. Circle all of the elements in the list below that CAN form double bonds.
H
Br
C
N
O
Cl
12. How do you determine which atom should be the central atom in a Lewis structure?
13. Circle the words that correctly complete the statement: Breaking a chemical bond requires/releases
energy, while forming a chemical bond requires/releases energy.
14. Which intermolecular force(s) is/are present in the molecules below:
a. I2
b.
c.
Choose at least 3 of the problems from the chart to solve. O3 MUST be one that you choose.
Lewis Structure
Formula
VSEPR Geometry
Polar or NonPolar
NH4 +1
OCN-1
CF2H2
F2O
CH2O
O3
SF6
14. How many electrons are shared in a single bond? A double bond? A triple bond?
15. Magnesium combines with 2 chlorine atoms. Draw the dot structures, use arrows to show the transfer of
electrons, and write the formula for the compound.