Hybridization
Started by mass
Get help with your application
Use all the free resources available to you from SDN: articles, guides, expert advising, forums discussions, and school research.
Its plain and simple, you have two types of orbitals:
Atomic: your S P D F orbitals
Molecular: your SP, SP2, SP3, SP3D etc...
S orbitals hold 2 electrions
P orbitals hold 6 electrions (in 3d, theres Px Py & Pz) hence a single P orbital can create from SP - SP3 hybrid.
You get Hybrid (molecular) orbitals by merging two or more atomic orbitals hence if you merge an S and Px you get a molecular SP orbital.
Another thing to remember is you will always get out what you put in.
1 S + 1 P = 2 SP (an SP bonding orbital and an SP Antibonding oribital)
1S + 1Px + 1Py + 1Pz = 4 SP orbitals aka SP3 hybridization.
"Antibonding > bonding" in energy, therefore electrons naturally lie in the bonding orbital unless energy is put in (such as heat or pressure etc) and the electrons move to the anti-bonding and the bond breaks.
Atomic: your S P D F orbitals
Molecular: your SP, SP2, SP3, SP3D etc...
S orbitals hold 2 electrions
P orbitals hold 6 electrions (in 3d, theres Px Py & Pz) hence a single P orbital can create from SP - SP3 hybrid.
You get Hybrid (molecular) orbitals by merging two or more atomic orbitals hence if you merge an S and Px you get a molecular SP orbital.
Another thing to remember is you will always get out what you put in.
1 S + 1 P = 2 SP (an SP bonding orbital and an SP Antibonding oribital)
1S + 1Px + 1Py + 1Pz = 4 SP orbitals aka SP3 hybridization.
"Antibonding > bonding" in energy, therefore electrons naturally lie in the bonding orbital unless energy is put in (such as heat or pressure etc) and the electrons move to the anti-bonding and the bond breaks.
