L2 - Orbital Theory, E- Configuration And Hybridisation

electrons that are moving through space

wavefunctions behave as a particle and a wave

finding an electron at any given location round the nucleus

• the pattern of probabilities of positions of electrons around the nucleus • depending on its energy level, it exists in certain regions around the nucleus

s p d f

• electrons fill the lowest energy shells first • form pairs

orbitals that are spherical - centred on the nucleus - have the highest probability of finding the electron at the nucleus

orbitals that are 2 ellipsoids - have a point of tangency at the nucleus - no probability of finding an electron at the nucleus

orbitals that are 3 pear-shaped lobes - they are all in one plane

the number of bonds needed to complete the shell

mixing up the atomic orbitals to give new molecular orbitals?

with an energy input to promote electrons within the atomic orbital shells

tetrahedral (109.5) - s-orbital and all 3 p-orbitals

trigonal planar (120) - s-orbital and 2 p-orbitals

linear (180) - s-orbital and p-orbitals

single bond - strongest type of covalent chemical bond - form when atomic orbitals overlap in a head on arrangement

• s-orbital and p-orbital = σs-p • s-orbital and sp-orbital = σs-sp hybrid • the lobe of the orbital opposite is involved in a substitution reactions

• covalent bonds formed from overlap of 2 orbital lobes on one atom with 2 of another in a lateral sense • there is a plane between the molecular orbitals with no electron density

paired electrons occupying one or more of the hybridised orbitals

lone pairs are held closer to the atom than bonding electrons exert more repulsion on other valence electrons = compressed bonding angles

sigma bonds - free rotation pi bonds - fixed rotation = leads to isomers (stereochemistry)