Chemistry - Ionic Bonding

Ion

-an atom that losses or gains an electron

-Lower ionisation energy, more likely to lose electrons

=i.e. group 1-3 (lose electrons), group 5-7 (gain electrons)

ionic bonding

-occur by transferring electrons from a metal to non-metal.

-Now the two atoms become oppositely charge and attract becoming stable

ionic Model

-Cations and anions form and will arrange themselves in a continuous 3D lattice

-They bond through electrostatic attraction between the + and - natures of the ion

-They find themselves in fixed position with ‘directional bonds’

Properties

1.High melting/boiling point

2.Hard and brittle (not malleable or ductile)

3.Conductivity (only in liquid form)

4.Solubility (more will cover in Sem 2)

High melting/boiling point

-Caused by strong attractive forces (more energy to change state)

-attractive forces between + and - ion is relatively strong so high amounts of energy needed to disrupt (to melt)

Hard and brittle (not malleable or ductile)

-Due to strict formation of ions in a lattice, a shift or change in this structure causes bonds to break

-if force is applied, Movement of ions will result in repulsion of like ions, causing lattice to break

-Ionic hardness is due to strength of attraction (particles close) and directional bonds

Conductivity (charged particles must be mobile for electricity to flow)

-As a solid, ions are in rigid formation and unable to move if there was an electric current

-As a liquid or solution- ions are not in a lattice and can move towards electric terminals, allowing electricity to flow

Solubility (more will cover in Sem 2)

-Some compounds dissolve, some don’t

*info in data booklet