Name____________________________________ Period__________
Chapter 7, 8, 9 Review Sheet
Date__________
Fredericks/Weis
Section 1: Naming Binary and Polyatomic Ionic Compounds
Cation
(charge)
Anion(charge) Formula
Name
Li2O
Barium chloride
K1+
I1MgSO4
(pick one)
Section 2: Molar Mass Conversions (SHOW ALL WORK)
1 mole = “molar mass”
1 mole = 6.02 x 1023 “formula units”
1. What is the mass of 1.7 moles of copper (I) chloride?
Formula: ______________
Molar Mass:______________
2. How many moles are in 6.3g of iron (III) sulfide?
Formula:_________________
Molar Mass:________________
3. How many formula units are in 2.3g of potassium chloride?
Formula:______________
Molar Mass:_____________
Section 3: Diagrams and Molecular Geometry
Compound
Lewis Dot
Diagram
VSEPR Diagram
Molecular
Shape
Bond Angle
Polar/ Non-polar
SO4
CO2
CHCl3
Section 4: Bonding and Electronegativity
1. If atoms in a bond have very different electronegativity values (the difference in
electronegativity is greater than 1.7), that would mean that electrons are transferred in
a(n) __________________________bond.
2. If atoms have the similar electronegativity (the difference in electronegativity is less
than 1.7), that would mean they share electrons in a(n)
__________________________bond. When atoms share electrons, they may share them
equally or they may share them unequally.
3. List some properties comparing Metallic Solids to Ionic Solids:








Use the Electronegativity Table below to identify the EN between
the following atoms. Then determine what kind of bond it is.
Li-Cl in LiCl
BOND
K-O in K2O
Ni-F in NiF
BOND
Mg-O in MgO
4.0
Ionic
BOND
BOND
Be-S in BeS
BOND
Ca-Br in CaBr2
BOND
Difference in electronegativity
1.7>=
0.4>=
0
Non-polar
Polar-covalent
covalent
bond
bond