Chemistry ionic bonds and ions

NH₄⁺ – An ammonium ion

Ag⁺ – A silver ion

Cu²⁺ – A copper ion

Pb²⁺ – A lead ion

Fe²⁺ – An Iron II ion

Fe³⁺ – An Iron III ion

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 non

metal 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 – Giant structure and strong ionic bonds

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

Feature of molten or dissolved ionic substances that allow them to conduct electricity – Ions can flow

How molten or dissolved ionic substances conduct electricity – Mobile ions carry the charge through the substance