3.1.3.1 ionic bonding

Why do o if bonds have high boiling and melting points?

Strong electrostatic forces of attraction that take a lot of energy to overcome

attraction between oppositely charged ions

The higher the ——— the higher the———— point

Charge

Boiling point

What is the formula for hydrogen carbonate

HCO3-

Why is ionic compounds cant carry electricity when solid

The ions are not free to move

Why is aluminium oxide insoluble in water

The electrostatic attraction betweeen the positive and negative ions is so strong that water can’t break up the lattice

Another. Property is the high ——- when ——— or ———

High electrical conductivity when liquid or aqueous

Ions are red and not locked in and so can carry charge

What is the strength like of ionic bonding

BRITTLE

Layers shift -repulsion occurs between the ions of the same charge

Why is ionic bonding usually soluble?

Usually soluble - water molecule is polar and can break bonds

Higher charge = less soluble it gets (*harder to overcome electrostatic attraction*)

What are alll the properties of ionic bonding

High melting/ boiling point

High electrical conductivity when molten or aqueous

Brittle

Usually soluble

The greater the —— the stronger the ionic bonding. The —— the ions, the stronger the ionic bonding

The greater the charge the stronger the ionic bonding

The smaller the ions the stronger the ionic bonding

What has a higher melting point

Magnesium oxide or sodium chloride?

Magnesium oxide

(Higher charge)

What is smaller Na+ or K+

Na+

Do ions get smaller as you go along a group?

The ion gets smaller and higher charged

Why are aluminium ions smaller than sodium ions?

Higher charge density so more closer together

Describe the structure of ionic bonding

Lattice structure of positive and negative ions