1f) Ionic compounds + 1g) covalent compounds

Ionic bonding:

• strong electrostatic attraction 
• opposite charged ions 
• throughout lattice 

Properties of ionic compounds:

• high melting point 
• strong electrostatic attraction 
• giant ionic lattice 
• soluble in water 
• Ions attracted to polar water molecules 
• conduct electricity 
• ions can move and carry charge

A Lattice is a 3-D network of ions in fixed positions bonded together 

OIL RIG 

Oxidation- loses electrons                      Reduction- gains electrons 

Group	1	2	3	4	5	6	7	0/8
Charge	1+	2+	3+	X	3-	2-	1-	X

Covalent bonding:

• non metal with non metal 
• outer shells overlap 
• electron shared in pairs 
• atoms achieve outer shells (full)
• attracts both nuclei 

Properties of simple covalent molecules:

• very strong bonds
• low melting and boiling points 
• insoluble in water 
• no free electrons 
• Don't conduct electricity 
• soluble in organ solvents 

Intermolecular forces 

• weak bonds
• easily broken 

Giant covalent bonds 

• strong bonds 
• no free electrons 
• rigid 
• all atoms joined together 
• covalent unreactive 

Diamonds 

• rigid 
• hard 
• sparkly
• four covalent bonds  

Graphite

• layers three covalent bonds 
• slide over each other 
• free electrons 
• good conductor of electricity 
• lubricant