NAMING IONIC
COMPOUNDS
CHEMICAL NAMES
 Always has 2 parts
 The first part is a POSITIVE ion and is always a metal
 An example is Sodium (Na)
 The second part is a NEGATIVE ion and is always a non -metal
 An example is Chlorine ( Cl)
CHEMICAL NAMES
We always have to change the non-metal’s
name
We change the ending from
“ine” to “ide”
Example: Chlorine becomes Chloride
Table salt is then called Sodium Chloride, not
Sodium Chlorine)
PRACTICE
Calcium and Nitrogen
Potassium and Oxygen
Lithium and Chlorine
Magnesium and sulphur
Silver and Fluorine
CHEMICAL FORMULA
We write sodium chloride as NaCl
We write aluminum chloride as AlCl 3
Why?
CHEMICAL FORMULA
 We must examine that charges that each ion has.
 Na has a charge of +1
 Cl has a charge of -1
 Together, they cancel each other out, and can be
NaCl
CHEMICAL FORMULA
Al has a charge of +3
Cl has a charge of -1
If these are going to bond properly, we will
need 3 Cl to match the Al
So 1 Al and 3 Cl
We write this as:
AlCl 3
CHEMICAL FORMULA
Practice with Zinc and Nitrogen (Zn and N)
Zn is +2
N is -3
How can we make these equal?
We need 3 Zn and 2 N
We write this as Zn 3 N 2
PRACTICE
In pairs, complete the practice problems on
pages 86 and 87. Work with another team.
After every 5 questions, switch, and mark the
other teams answers.
Tell the other team if they are on the wrong
track. Help them correct errors.
MULTIVALENT IONS
As you have noticed, some ions have more
than one charge!
Example: Iron can be +2 or +3
If we use the +2 charge, we say “iron two”
Iron (II) Oxide is said “Iron two oxide”
How would you say
Iron (III) Oxide?
PRACTICE
Chromium (II) chloride
Copper (I) sulphide
Iron (III) phosphide
Tin (IV) nitride
How do you write these as formulas?
MULTIVALENT FORMULAS
Identify each ion’s charge
Make each ion’s charge equal
Use subscripts to write the formula
Example: Iron (III) sulphide
Iron is +3
Sulphur is -2
We need 2 Iron and 3 Sulphur (totals 6)
We write Fe 2 S 3
PRACTICE
In pairs, complete the practice problems on
page 89. Work with another team. After every
3 questions, switch, and mark the other teams
answers.
Tell the other team if they are on the wrong
track. Help them correct errors.
Remember to use the positive ion charge that
is in the roman numerals!
MULTIVALENT IONS
If we see Fe0, how do we know which iron was
used? Iron (III) or Iron (II)?
O is -2
Since there are no subscripts, in order to be
balanced, that Fe must be +2!
So the answer is Iron (II)
MULTIVALENT IONS
If we see Fe 2 0 3 , how do we know which iron
was used? Iron (III) or Iron (II)?
O is -2 x 3 = -6
There are 2 irons…if they are going to equal 6,
they MUST each have a charge of +3
So the answer is Iron (III)
PRACTICE
In pairs, complete the practice problems on
pages 90. Work with another team. After
every 3 questions, switch, and mark the other
teams answers.
Tell the other team if they are on the wrong
track. Help them correct errors.
QUESTIONS
Complete questions 4 and 5 on page 95.
Remember to check if the metal is
multivalent.
If it is multivalent, you must use the
correct charge! Look closely, and make
sure things balance.
You must also use roman numerals if you
are writing out the name!
NEXT DAY
Bring any products from home…shampoo,
deodarant, hairspray, cologne, food, etc.
Whatever you bring, make sure it has labels!
POLYATOMIC IONS
 Polyatmoic ions do not exist on their own.
 They are ALWAYS paired up with an opposite
charge
 Each polyatomic ion has a charge…so you can
balance it the same way you were doing the
others!
Example: Iron (III) hydroxide is Fe(OH) 3
Look at the charge of OH on page 92.
Put brackets around it!
Say it just like it says on page 92.
TWO POLYATOMIC IONS
Instead of using a metal and a polyatomic ion,
you can link 2 polyatomic ions together
Ammonium (NH 4 ) is +1
Carbonate (CO 3 ) is -2
You will need 2 ammonium ions and 1
carbonate ion.
(NH 4 ) 2 CO 3
PRACTICE
In pairs, complete the practice problems on
pages 91. Work with another team. After every
3 questions, switch, and mark the other teams
answers.
Tell the other team if they are on the wrong
track. Help them correct errors.
QUESTIONS
On page 95, complete questions 3 and 5
BUILD A COMPOUND
With clay, build a compound.
Tell you partner what elements are in your
compound, and see if they can write out
the chemical name and the chemical
formula.
Use the internet to help you if you need to
look at where electrons are shared, or
gained or lost.
Use polyatomic ions to make it harder!
Destroy, and try another one!
PRODUCTS
Find a chemical listed on a container, and see
if you can model it with clay.
If it’s a complicated chemical, you may need
to use the internet for help.
See if you partner can guess the chemical
model you made.