I don't even know how to start this...The valence electron configurations of several atoms are shown below. How many bonds can each atom make without hybridization?
1. Si 3S2 3P2
2. P 3S2 3P3
3. F 2S2 2P5
Hey! So remember electron orbitals will fill up one by one. If you have Si notated by 3s2 3p2, you have 2 electrons that are unpaired, right? That means you can have 2 bonds.
With P (3s2 3p3), you have 3 electrons that are each unpaired in the 3 p orbitals, so P can make 3 bonds without hybridization.
With F (2s2 2p5), you'll have 1 unpaired electron. Since p has 3 orbitals, and you have 5 electrons, you'll start with one in each orbital (3 electrons) then the 2 left over will each join an orbital, so 2 of your 3 p orbitals are full. That means you have 1 unpaired electron, so you can have 1 bond without hybridization.
I realize I'm answering this question 4 years later, but hopefullly others can benefit from the explanation. :)