Bonding

STATE: the bonding in metals

DESCRIBE; 

1) they form a giant metallic structure

2) made up of positive metal ions

3) delocalised electrons

DIAGRAM:

1) HIGH MELTING/BOILING POINTS

• giant metallic structure
• strong electrostatic attraction
• between positive metal ions and delocalised electrons

2) THEY CONDUCT ELECTRICITY

• delocalised electrons
• can move throughout the whole structure.

STATE: the bonding between a metal and a non-metal 

DESCRIBE: 

1) positive ions and negative ions form

2) electrons are transferred 

DIAGRAM: 

eg; calcuim chloride

1) HIGH MELTING/BOILING POINTS

• giant ionic structure 
• strong electrostatic attraction
• between positive and negative ions

2) CONDUCT ELECTRICITY WHEN MOLTEN OR AQUEOUS

• ions are free to move
• and carry a charge

3) SOLUABLE IN WATER

STATE: bonding between non-metals

DESCRIBE: sharing of electrons to form simple molecules 

DIAGRAMS:

1) LOW MELTING/BOILING POINTS

• it is a simple molecule
• weak intermolecular forces (between molecules)
• not much energy needed to overcome forces

2) DO NOT CONDUCT ELECTRICITY

• no delocalised electrons

STATE: bonding between non-metals

DESCRIBE; sharing electrons to form giant covalent structures; these are:

• DIAMOND - carbon
• GRAPHITE - carbon
• SILICA - silicon and oxygen

DIAMOND 

HARD

• each carbon is bonded to 4 others
• strong bonds between layers
• layers are unable to slide
• structure is rigid

DON'T CONDUCT ELECTRICITY

• no delocalised electrons, which can't carry a charge. 

GRAPHITE

Soft/slippery

• no bonds between layers
• layers can slide

conduct electricity

• delocalised electrons
• they can move through the whole structure 

Each carbon is bonded to 3 others 

HIGH MELTING POINTS 

• giant covalent structure
• lots of strong covalent bonds
• a lot of energy required to break bonds