Hybridization question

[TigerLilies]

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I need help as I am studying hybridization in Chemistry and while I understand that four bonds is sp3, three is sp2, two is sp, etc. When I am asked to explain the bonding in terms of valence bond theory and draw a picture of the hybridized orbitals showing sigma and pi bonds, I am not able to. I am stuck on doing this for NO2-.

Does anyone have tips or explanation? Or books or resources I could use to better understand this?

Thanks

 

[Compass]

OK. I haven't got my super chem textbook with me right now, so I had to brush up.

http://en.wikipedia.org/wiki/Pi_bond

Drawing a Lewis structure of NO2-(2 oxygens I presume)

O(3 e pairs) - N (2 e pairs) - O (3 e pairs)

Since these are both single bonds, they are both sigma bonds. No other bonds = no pi bonds.

If you meant nitrous oxide (NO^2-)

It would be N (2 e pairs) = O (2 e pairs)

Since this is double bonded, in reality you'd have something like this:

:___:
N=O
: :

With the outside molecules bending outward.

Now, a pi bond requires 2 pairs of electrons.

Each electron pair would be represented by something like an 8 <-- with the center of the eight being the center of the atom.

Now, to form a pi bond, you need 2 8s. 8-8 (Imagine the - is a sigma bond)

Those 4 electrons are going to be shared, creating ONE pi bond. 4 electrons = 1 pi bond. That's the second bond, locking the shape in place. If you have an orgo model kit, take a single bond and connect two 6-sided balls together. Now have two more sticks for each vertically so it looks like an H (assume these represent single electrons, not a pair)

The vertical parts that are parallel form a pi bond. And that's basically it.

Someone check my chemistry, I don't trust myself.

 

[TigerLilies]

OK. I haven't got my super chem textbook with me right now, so I had to brush up.

http://en.wikipedia.org/wiki/Pi_bond

Drawing a Lewis structure of NO2-(2 oxygens I presume)

O(3 e pairs) - N (2 e pairs) - O (3 e pairs)

Since these are both single bonds, they are both sigma bonds. No other bonds = no pi bonds.

If you meant nitrous oxide (NO^2-)

It would be N (2 e pairs) = O (2 e pairs)

Since this is double bonded, in reality you'd have something like this:

:___:
N=O
: :

With the outside molecules bending outward.

Now, a pi bond requires 2 pairs of electrons.

Each electron pair would be represented by something like an 8 <-- with the center of the eight being the center of the atom.

Now, to form a pi bond, you need 2 8s. 8-8 (Imagine the - is a sigma bond)

Those 4 electrons are going to be shared, creating ONE pi bond. 4 electrons = 1 pi bond. That's the second bond, locking the shape in place. If you have an orgo model kit, take a single bond and connect two 6-sided balls together. Now have two more sticks for each vertically so it looks like an H (assume these represent single electrons, not a pair)

The vertical parts that are parallel form a pi bond. And that's basically it.

Someone check my chemistry, I don't trust myself.

Hi, thanks I understand that but I have to do a drawing showing the hybrid orbitals involved (like s, p etc) thats what i dont understand

I know that it is sp2 hybridized but i dont know how to represent this in a picture

 

[Kuba]

why is this posted in every forum?

 

[Compass]

I'll make one in Flash, please hold.

 

[MollyMalone]

Duplicate, so closing.