Molecules of life (bonds)

working through checklist

Orbital Hybridisation - what is it

mixing of atomic orbitals to form new hybrid orbitals.

• hybrid orbitals have different shapes and energies than the original atomic orbitals.

• used to explain geometry of molecules and the types of bonds that can be formed

Orbital Hybridisation - process

atoms bond together to form a molecule

• atomic orbitals overlap to create new hybrid orbitals that can accommodate the shared electrons

• The type of hybridization that occurs depends on the number and types of orbitals involved in the bonding.

states of different hybridizations - sp

one s orbital and one p orbital are combined to form two hybrid orbitals

• 180 degrees.

• CH=CH

• linear

states of different hybridizations - sp2

one s orbital and 2 p orbitals are combined to form three hybrid orbitals

• 120 degrees

• Ch2=CH2

• triagonally

states of different hybridizations - sp3

one s orbital and three p orbitals are combined to form four hybrid orbitals

• 109.5 degrees

• tetrahedral

• CH4

Covalent bonds and properties

Forms when two atoms share one or more pairs of electrons to achieve stable elec config (non metal atoms)

• Both atoms contribute one or more electrons to form a shared electron pair in the region of space between two nuclei

• Electrons are attracted to both nuclei, holding the two atoms together in a stable molecule

• sharing lowers the energy state of both atoms compared to their isolated states.

Polarity of Covelent Bonds (non polar and polar)

NON- polar = electrons shared equally - no dipole movement - no significant charge separation (example H2, O2)

POLAR - electrons shared unequally - dipole movement and partial charge separation

• One atom attracted shared electronsg stronger than other

• Water (H20) - oxygen attracts shared electrons more strongly than hydrogen so partial negative charge on oxygen and partial positive charge on hydrogen.

Covalent - Sigma bonds