Chemistry ionic bonds and ions

An ammonium ion

NH₄⁺

A silver ion

Ag⁺

A copper ion

Cu²⁺

A lead ion

Pb²⁺

An Iron II ion

Fe²

An Iron III ion

Fe³⁺

Electrostatic force

An attraction between positive and negative species

Ionic bond 

An electrostatic attraction between oppositely charged ions in all directions

How ionic bonds form

Electrons transferred from metal atom to nonmetal atom

Lattice

A regular giant 3D structure

Structure of ionic compounds

A giant ionic lattice

Type of bond formed between a metal atom and a non metal atom

Ionic

What happens when a substance melts

Forces or bonds between particles are overcome

Why different substances have different melting points

Forces or bonds between particles may be weaker or stronger

Melting point of an ionic substance

High

Reasons why ionic substances have a high melting point

Ionic structure with a giant lattice structure. There are electrostatic forces of attraction between oppositely charged ions. Requires a lot of energy to break the ions/bonds apart.

What is needed to allow a substance to conduct electricity

Mobile charged particles (ions for ionic compounds or electrons in metals)

Do ionic substances conduct electricity when solid

No

What can you do to an ionic substance to make it conduct electricity

Melt it or dissolve it in water

Why don’t solid ionic substances conduct electricity

Ions are fixed in position

Properties of ions

Strong bonds, giant lattice, high melting and boiling point and do not conduct electricity when is solid

How do molten or dissolved ionic substances conduct electricity

Mobile ions carry the charge through the substance

What is a hydroxide ion?

OH^-

What is a sulfate ion?

SO₄^2-

What is a carbonate ion?

CO₃^2-

What is a nitrate ion?

NO₃^-

Why does an ion conduct electricity when molten but not as a solid

When solid, ions are in a fixed position so cannot carry the charge, when molten there are free ions to carry the charge