*Hybridization- came from native orbitals that form a newly-hybrid orbital.

All s orbital have a sphere-like shape, for p orbitals they have a dumbbell- like shape and for the d orbitals it’s look-like a clove in shape.

All orbitals have its own maximum capacity. For s orbital it can only hold 2 e-, for p it can hold up to 6 e-, for d orbital it can hold up to 10 e-, and for the f orbital it can hold 14 e-.

 

Let’s find out how to do hybridization.

The first kind is sp3.

The first thing you have to do is know the atomic number of the given element.

Given:  AlCl3

 

Now that you know the atomic number, make the electron distribution for the given elements.

Make a box for the last to electron distribution. One box for s orbital,  three boxes for p orbital and 5 boxes for d orbitals then place the electron in each designated box (singly first before pairing).

            

 

 

 

 

 

 

Since the chemical formula is AlCl3, the central is Aluminum, then it’s connected to 3 Chlorine that will form a trigonal planar. So we have to separate the electron in 3s2 to be able to bond in Chlorine.

Do the separation and promotion just like on the illustration below.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

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Just like on what we do on the first (sp2) get the atomic number, make an electron distribution and a box orbital.

Given: CH4

 

 

 

 

 

 

Since the hydrogen have only one electron it is capable for bonding but the electron for carbon are not enough for bonding so, we will do the separation by transferring one electron to the next orbital then do the promotion.

                                   6C                                                                                                        1H

             

 

 

 

                                              

 

 

 

 

 

 

 

 

 

 

Next is sp3d.

Take first the atomic number, make an electron distribution the make a box orbital for the last two orbitals.

Given: PCl5

                                  15 P                                                                                                         17Cl

    

Since in the orbital 3s2 it has a 2 electron so it’s not capable for bonding. So we will separate the one electron by transferring one electron to the next orbital then do the promotion.

 

 

 

 

                                              

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Just like in the first three, take the atomic number, make a electron distribution then make a box orbital for the last two orbitals.

Given: SF6

    

 

 

 

 

 

             

The orbital 3s and 3px have 2 electrons so making it not capable for bonding so separate the one electron from 3s then promote it the next orbital. Then separate also the one electron from 3px then promote it to the next orbital which is d orbital.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Notes:

In every last two box orbitals, there should not be 2 electrons.

And for promotion the one electron will be transferred to the next orbital.

 

 

 

written by: Bernadeth Castilleja