Ionic Compounds

Notes:

Ionic Compounds

Chemistry

Chemical Bonds

▪ Created through gain, loss, or sharing of valence electrons

▪ Remember

– Electrons equal atomic number of the element
– Valence electrons equal the group number.

• Krypton

- 8 valence electrons

Example:

• Sodium

1 valence electron

Multiple Choice

Valence electrons are the electrons in the outermost orbit of an atom.

• True

• False

What is a Chemical Bond?

▪ A Chemical Bond is created when an atom attempts to fill

its outermost energy level to become stable, also called
the octet rule.
– An energy level is stable when it has 8 valence electrons.

▪ There are 3 types of chemical bonds

– Ionic bonds- transfer of electrons
– Covalent bonds- sharing of electrons
– Metallic bonds- two metals

Ionic Compounds

▪ An ionic bonds is an electrostatic attraction between atoms where

there is a transfer of valence electrons.
– Loss of electrons results in a positive charge (tend to be metals)
– Gain of electrons results in a negative charge. (tend to be nonmetals)
– The overall charge of the compound will be neutral.

▪ Two types of Ionic Compounds

– Salts-

▪ NaCl

MgSO4

– Oxides-

▪ CuO

Fe2O3

Multiple Choice

The word "transfer" best means

• move from one place to another

• Exchange

• Allocate

Multiple Choice

What will be the charge of oxygen if it had 8 protons and 10 electrons?

charge = protons - electrons

• 2+

• 2-

• 0

Ionic Compounds

▪ Properties of ionic Compounds

– Very high melting point
– Soluble in water
– Good conductors of electricity when dissolved

in water
▪ Electrolytes

– Atoms build upon each other to create

geometric patterns
▪ Crystal lattices

Creating Formulas for Ionic Compounds

▪ The formula of a compound can be determined

by using the Lewis dot structures for each atom.
– Example:
**Remember the
octet rule

Cl

Cl

AlCl3

▪When writing the formula, the cation
(metal) goes first.

Al

Cl

​Aluminum chloride

Multiple Choice

Take a look at the image. What would the charge be for the element oxygen (O)?

• 2-

• 0

• 1-

Writing & Naming Binary Ionic Compounds

▪ Name to Formula

– Write the symbol of the

elements
▪ Metal first

– Determine the charge for each

element
▪ If using a transition metal the

charge will be written as a
roman numeral

– Cross the charges

▪ Examples:

Ca Cl

Calcium Chloride

Iron (II) Oxide

Fe O

+2 -1

CaCl2

+2 -2

FeO

Writing & Naming Binary Ionic Compounds

▪ Binary ionic compounds will

contain two elements
– Positively charged cation (the

metal)

– Negatively charged anion (the

nonmetal)

▪ Formula to Name

– Name the metal

▪ If using a transition metal write the

charge as a roman numeral

– Name the nonmetal and change

the last syllable to -ide

▪ Examples:

Sodium chlorine

NaCl

Sodium chloride

MnBr2

manganese bromine

manganese (II) bromide

Writing & Naming Binary Ionic Compounds

Practice

▪ Strontium Chloride. SrCl₂

▪ KI. Potassium Iodide

▪ Aluminum Oxide. Al₂O₃

▪ AgCl

▪ Calcium Bromide

▪ Na2S. Sodium Sulfide

▪ Beryllium Iodide

▪ Potassium Fluoride. KF

▪ Cs3N

▪ Copper (I) oxide

Aluminum oxide

​Cs and N

Writing & Naming Ternary Ionic Compounds

Formula to Name
▪ Name the metal

▪ Name the polyatomic

ion

Name to Formula

▪ Determine the symbol of

the element and the
polyatomic ion.

▪ Cross the charges

A ternary ionic compound will contain an element bonded to a polyatomic ion, which is a
charged group of atoms acting as a single unit.

Polyatomic Ions
Nitrate

NO3

-1

Nitrite

NO2

-1

Sulfate

SO4

-2

Sulfite

SO3

-2

Phosphate

PO4

-3

Hydroxide

OH-1

Cyanide

CN-1

Ammonium

NH4

+1

Al2(SO4)3

Aluminum Sulfate

Calcium Nitrate

Ca (NO3)

2

+2 -1

Writing & Naming Ternary Ionic Compounds

Practice

▪

silver (I) nitrate ____________________

▪

CuSO4
________________________

▪

lithium nitrite ____________________

▪

Zn3(PO4)2 _______________________

▪

potassium hydroxide ______________

▪

Pb(NO3)2 ______________________

▪

Polyatomic Ions
Nitrate

NO3

-1

Nitrite

NO2

-1

Sulfate

SO4

-2

Sulfite

SO3

-2

Phosphate

PO4

-3

Hydroxide

OH-1

Cyanide

CN-1

Ammonium

NH4

+1