3.Orbital Hybridisation

Atomic orbitals

Regions where electrons are statistically most likely to be found.

s orbitals

Spherical shaped orbitals

p orbitals

two lobes along the X, Y and Z axis.

Covalent bonding

The sharing of atomic orbitals when atoms come together to form molecules.

Hybridisation

The mixing of atomic orbitals to form new hybrid orbitals.

sp3 hybridisation

where one s orbital and three p orbitals combine to form four equivalent sp3 orbitals.

Tetrahedral geometry

Results from sp3 hybridisation with bond angles of 109.5 degrees.

sp2 hybridisation

It involves one s orbital and two p orbitals, resulting in three equivalent sp2 orbitals.

Trigonal planar

Results from sp2 hybridisation with bond angles of 120 degrees.

sp hybridisation

It involves one s orbital and one p orbital, forming two equivalent sp orbitals.

Linear geometry

Results from sp hybridisation with a bond angle of 180 degrees.

p-bonding

Its weaker than s-bonding, and contributes to double and triple bonds.

Bond dissociation energy

The energy required to break a bond

An example of a molecule with sp3 hybridised nitrogen, exhibiting tetrahedral geometry.

Ammonia (NH3)

A molecule with sp3 hybridised oxygen, exhibiting a bent shape due to lone pair repulsion.

Water (H2O)

A molecule where each carbon undergoes sp hybridisation, resulting in a linear structure.

Ethyne (C2H2)

A molecule featuring sp2 hybridised carbon, exhibiting trigonal planar geometry.

Ethene (C2H4)

sp3d hybridisation

A hybridisation involving one s, three p, and one d orbital, resulting in a trigonal bipyramidal molecule.

octet rule

says atoms prefer having eight electrons in their valence shell.

A chemical compound where phosphorus is hybridised to form five equivalent bonds via sp3d hybrid orbitals.

PCl5

sp3d2 hybridisation

A hybridisation involving one s, three p, and two d orbitals, which leads to an octahedral molecule.

Lewis Acid

A substance that can accept an electron pair from a Lewis base, often creating bonds.

A chemical compound that possesses a trigonal planar geometry due to sp2 hybridisation of boron.

Boron trifluoride (BF3)

σ bond

A type of covalent bond formed by atomic orbitals overlapping.

π bond

A type of covalent bond formed by the side-to-side overlap of p orbitals.

bond angles

The angles formed between adjacent bonds in a molecule.

Hybrid orbitals

Orbitals formed from the combination of atomic orbitals to create new orbitals that are degenerate in energy.