hybridization

$sp, sp^{2}, sp^{3}, dsp^{3}, d^{2}sp^{3}$

curry 1E
Posts: 55
Joined: Wed Sep 18, 2019 12:15 am

hybridization

Hello I am still very confused on hybridization. How do we derive the hybridization by looking at the lewis structure? Or do we have to look at each valence shell of each atom?

Montana James 4G
Posts: 46
Joined: Wed Sep 18, 2019 12:21 am

Re: hybridization

from what I understand, you look at how many regions of electron density there are and using that number to choose a hybridization scheme. In the end, the number of regions of electron density should equal the number of hybridized orbitals.

BCaballero_4F
Posts: 94
Joined: Wed Nov 14, 2018 12:22 am

Re: hybridization

You begin with the Lewis Structure which then allows you to use VSEPR to predict the shape, and from these two you should know the number of regions of electron density which would then allow you to derive the hybridization.

BNgo_2L
Posts: 95
Joined: Wed Sep 11, 2019 12:17 am

Re: hybridization

The number of hybrid orbitals are consistent with the number of electron densities of the molecule determined using its VSEPR model. In hybrid orbitals, the max number of orbitals of each shape are s:1, p:3, d:5, etc. The orbitals are then filled using the number of electrons in the atomic orbital of the atom in question.

EvanWang
Posts: 101
Joined: Sat Sep 07, 2019 12:16 am

Re: hybridization

Look at the lewis structure to help figure out the hybridization of an atom. If a central atom has four areas of electron density around it, then you need a hybridization that corresponds to those four areas. In this case, sp3. If an atom has three areas of electron density, the hybridization is sp2. For Five areas, the hybridization is sp3d, etc.

Tauhid Islam- 1H
Posts: 64
Joined: Fri Aug 02, 2019 12:15 am

Re: hybridization

EvanWang wrote:Look at the lewis structure to help figure out the hybridization of an atom. If a central atom has four areas of electron density around it, then you need a hybridization that corresponds to those four areas. In this case, sp3. If an atom has three areas of electron density, the hybridization is sp2. For Five areas, the hybridization is sp3d, etc.

So the number of electron densities in the central atom of a molecule corresponds to an orbital that is hybridized or a combination of the various orbitals in a particular energy level? Also does that mean that sp^3d can only exist for central atoms that have an energy level of three of higher as an atom in the second energy level can not reach the third energy level? So atoms in period 3 or higher can have hybridized orbitals containing a d or is this not the only case?

Cassandra_1K
Posts: 49
Joined: Wed Sep 18, 2019 12:16 am

Re: hybridization

how do you go about selecting a hybridization scheme?

Ruth Glauber 1C
Posts: 100
Joined: Wed Sep 18, 2019 12:20 am

Re: hybridization

^^ What is a step by step method?

Sean Cheah 1E
Posts: 105
Joined: Wed Sep 18, 2019 12:20 am

Re: hybridization

Ruth Glauber 3L wrote:^^ What is a step by step method?

I don't think there is any kind of step-by-step method. All you need to determine the hybridization scheme of a certain central atom is the number of regions of electron density around that atom (which one can very easily determine using the Lewis dot structure). 2 regions = sp, 3 = sp2, 4 = sp3, 5 = sp3d, etc.

ValerieChavarin 4F
Posts: 99
Joined: Wed Sep 18, 2019 12:18 am

Re: hybridization

You begin with the Lewis structure that will provide you with the regions of electron density of the center atom. Form their you can determine the hybridization. 2 regions corresponds with $sp$; 3= $sp^{2}$ and so on.

RobertXu_2J
Posts: 104
Joined: Fri Aug 30, 2019 12:17 am

Re: hybridization

Hybridization has to do with molecule shape. You can look at the shape of the molecule to derive the hybridization of the orbitals.

Rodrigo2J
Posts: 102
Joined: Sat Jul 20, 2019 12:16 am

Re: hybridization

To determine hybridization simply count the number of regions of electron density around the central atom, or the atom in question.