Bonding

Bonding (Chemistry)

• By Beth Buckley

Ionic Bonding

• An ionic bond is a bond between metals and non-metals which forms a giant ionic lattice.
• Strong electrostatic forces of attraction between the oppositely charged ions.
• Properties
• Very hard
• Conduct electricity wen molten/dissolved
• Solids at room temperature
• Very high melting/boiling points

Covelant Bonds

• Covelant bonds occur between non metals
• They form by sharing pairs of electrons and have a cooperative sharing area when being drawn.
• Covelant bonds within these molecules are strong but the intermolecular forces between them are easy to break.
• Properties
• Melting/boiling points are low
• Very small
• Gases at room temperature
• Bonds between non-metals
• Share pairs of electrons
• Do not conduct electricity as there is no free electrons to carry the charge

Giant Covelant Structures

• The larger the molecule the bigger the intermolecular force so the larger molecules have higher melting and boiling points as it takes more energy to overcome them.
• Diamond, Graphite and Silicone Dioxide:
• Giant covelant structures
• Hard
• High melting/boiling point
• Different forms of the same element: allotropes (diamond and graphite are made of carbon)
• Graphite can conduct electricity as it has one delocalised electron
• Each silicone atom is bonded to 4 oxygen atoms and each oxygen atom is bonded to 2 silicone atoms

Metallic Bonding

• Outer electrons of the metal atoms separate and form a sea of electrons
• These electrons are delocalised so are free to move through the structure
• The metal atoms become positively charged and are attracted to the sea of electrons. This is metallic bonding
• Part of a giant lattice
• Carry the charge through a giant lattice
• Metals are soft and malleble because they have sliding layers
• Alloys are mixtures of metals and at least one other element.

Additional Polymerisation

• Polymers form when many monomers join together to form a long chain molecule
• Polymers are plastics