Ionic bonding: Elements compounds and mixtures: Chemistry: (9:1)

Formation of metal ions

Atoms lose outer electrons

Metals

Elements that form positive ions

Formation of non-metal ions

Atoms gain electrons

Charge on non-metal ions

Negative

Group 1 ions charge

+1

Group 2 ions charge

+2

Group 6 (IUPAC group 16) ions charge

-2

Group 7 (IUPAC group 17) ions charge

-1

Electron structure of ions

Same as the nearest noble gas

Giant structure

A huge 3D network of atoms or ions

lattice

Regular arrangement of particles.

Giant ionic lattice

A huge, 3D, regular structure of oppositely charged ions, held together by electrostatic forces.

Examples of Ionic compounds

NaCl, MgO

Limitations of dot and cross diagram

Looks like the compound only contains a few ions

Limitations of a dot and stick diagram

Looks like each ion is only attracted to a few other ions

Limitations of a 3D diagram

Looks like it only contains a few ions

Melting and boiling points of ionic substances

high

Reason for melting and boiling points of ionic substances

Strong electrostatic forces between opposite ions need lots of energy to break

Movement of ions in a solid

Ions vibrate around fixed positions

Molten

Made liquid by heat

Movement of ions when molten

Ions can move past each other

Movement of ions in solution

Ions break apart and move freely

Conductivity of solid ionic compounds

don't conduct

Reason for conductivity of solid ionic compounds

Ions are fixed in place

Conductivity of molten/dissolved ionic compounds

good conductors

Reason for conductivity of liquid/dissolved ionic compounds

Ions are free to move and carry charge

Electrostatic force of attraction

The attractive force between oppositely charged particles.