Name_____________________________________________Period________________________
Ionic Compounds – Study Guide
Fill in the blank
Elements tend to
or
to be like their nearest
. Elements that have more than
tend to gain some until they have
, and those with less than
tend to lose until
they have
. In their ion form, they are said to have a
. The
charges of ions attract to form
. These ionic
“salts” tend to
when mixed with water and can
electricity.
Noble gas configuration
8 valence electrons
4 valence electrons
Opposite
Lose
Electrons
No valence electrons
Dissolve
Ionic Compounds
Gain
4 valence electrons
Conduct
Noble Gas
Identify the number of valence electrons and most common charge formed by each of the following
# valence electrons
Common charge
1)
Mg
_______________
2)
Na
_______________
3)
Te
_______________
4)
I
_______________
5)
Al
_______________
Fill in the blank
When naming ionic compounds the
tends to be a metal with a
charge and
is written
. If it is an element that can form multiple charges, then the charge should be written in
after the name of the element. You (should/should not) alter the name of the cation. The second half
of the name is for the
which tends to be a non-metal with a
charge. If it is an element,
then you (should/should not) alter its name by changing the ending to
. Either the cation or anion can be a
polyatomic ion, in which case you (should/should not) alter its name.
Anion
positive
first
cation
negative
Write the name of each compound. Example – CaCl2  “Calcium Chloride”
6)
NaF
___________________
7)
Al2O3
___________________
8)
ZnCO3
___________________
parentheses
-ide
Fill in the blank
To write the formula for a compound from its name, you must first identify the
that
represent each ion/polyatomic ion. Next, identify the
of each ion. The charges on each must be
by adding
that indicate how many of each ion is in the molecule. Polyatomic
ions use
to show that there are multiples of the entire ion within a molecule.
Charge
symbols
parentheses
subscripts
balanced
Write the formula for each compound. Example – “Magnesium Fluoride”  MgF2
9)
Sodium Bromide
___________________
10)
Aluminum Sulfide
___________________
11)
Silver Nitrate
12)
Mercury (II) Sulfate
13) How do you know whether a compound is ionic or covalent? Example CH3OH vs MgSO4
HONORS
“Complex salts” contain more than one type of cation or anion. We have already seen an example: (NH4)2Fe(SO4)2,
known as “ammonium iron (II) sulfate” or “ammonium ferrous sulfate”.
Name the following: KCr(SO4)2, BaCa(CO3)2, (NH4)2V(SO4)2, K2Co(SO4)2