Ionic Compounds
Determine the number of
subatomic particles in the
following elements:
Cl has a mass of 35 and an atomic # of 17
p+ = 17,
no = 18, e- = 17
K has a mass of 39 and an atomic # of 19
p+ = 19,
no = 20, e- = 19
Write the formula of each of the
following ionic compounds
Silver nitrate
Sodium oxalate
Magnesium hydroxide
Silver acetate
Forming Ionic Compounds w/
Variable Oxidation Numbers
 Some elements (metals) can have more than one
possible charge when they form ions
 Use Roman Numerals to indicate their charge
Example:
Copper(II) Sulfate
Chromium(III) Oxalate
Notes
Naming Ionic Compounds
Left  Right
Left Side:
Name the metal (cation)
If it is variable, you must use a roman numeral
to indicate its oxidation number/charge
Right Side
If polyatomic and on your reference chart,
write the name
If monatomic, write the name of the element
but change the ending to “-ide”
Practice
Write the name of each of the following
compounds
AgBr
Ca3(PO4)2
LiH
RaCl2
Notes
Naming Ionic Compounds w/
Variable Oxidation Numbers
 Start with what you know! (the anion)
 Calculate the total anion charge
 An ionic compound is neutral (no charge) so….
Total anion charge = Total cation charge
 Calculate the charge of the individual cation
 Name the compound by giving the cation a roman
numeral to represent its oxidation number (charge)
Naming Ionic Compounds w/
Variable Oxidation Numbers
Example:
Cu2S
Ni(OH)2
Name the compound
BiI3
CoBr2
Cu2S
CuS
Ionic Compounds Lab
Review: signs of a chemical
reaction
Ionic Compounds Lab
Goggle safety
Dropper safety
Silver Nitrate – Sodium hydroxide
safety
Equation set-up
 Double Displacement Reactions
Clean Up
Wrap Up
What does the roman numeral tell
you in an ionic compound?
Assignment: Finish writing out all
the reactions