Chemistry; bonding (models)

Metallic bonding

Attraction between delocalised electrons and positive metal ions

Ionic bonding

A chemical bond between a metal and non-metal where electrons are lost or gained , resulting in the formation of charged ions with electrostatic attraction.

Covalent bonding

A chemical bond between a non-metal and a non-metal with sharing of valence electrons to achieve noble gas configuration or a full outer shell. No ions present.

What are the three allotropes of carbon?

Diamond (C) graphite (C) and buckminsterfullerene (C60)

Electrostatic Attraction

The force of attraction between positively and negatively charged ions, crucial in ionic bonding.

Delocalised electrons

Electrons that are not associated with a single atom or bond and can move freely within a structure, contributing to properties like conductivity.

spd configuration of Ga

1s2,2s2,2p6,3s2,3p6,4s2,4p1

1

Mono

2

Di

3

Tri

4

Tetra

5

Penta

6

hexa

Diamond: Properties

Hard, does not conduct electricity because there are no delocalised electrons (no ions), insoluble in water (no polar molecules), high melting point, lustrous (transparent)

Diamond: chemical structure

Each carbon atom is joined to 4 other atoms by covalent bonding (tetrahedral structure).

Diamond: Uses

Cutting or drilling tools (Oil rigs)

Graphite: Properties

conducts electricity, slippery, black, shiny and opaque, high melting point

Graphite: Chemical structure

Each carbon atom is join to 3 other atoms. This forms a hexagonal structure (networked). Weak intermolecular forces and can slide over one another. Each carbon atome has a delocalised electron.

Graphite: Uses

Lubricant

Buckminsterfullerene: Properties

Cannot conduct electricity between molecules but can within itself, slippery, low melting point compared to other giant covalent structures

Buckminsterfullerene: chemical structure

60 electrons (carbon atoms) with strong covalent bonds. Molecules are spherical with hexagonal rings of carbon. Delocalised electrons stay within the structure with weak intermolecular forces. Has a hollow shape.

Buckminsterfullerene; uses

Drug delivery, storing hydrogen, fuel tank for fuel cell powered cars

ionic bonding properties

High boiling and melting point, soluble in polar solvent, a crystal lattice structure, solid form,

metallic bonding properties

malleability, ductility, good conducters of electricity, lustrousconductors

Covalent bonding properties

cannot conduct electricty, insoluble in water,

diamon: why is it hard?

Diamond is hard because it is a chemically rigid structure with a tetrahedral bond. Which signifies that one carbon atom is bonded to 4 other carbon atoms which means it takes much more energy to break the bonds.

Whys is diamond not a good conductor of electricity

diamond isnt a good conductor of electricity because it lacks the delocalised electrons moving freely within the structure hence its not a conductor of thermal/electricital conductivity.