Of2 Lewis Structure
When drawing Lewis structures for OF2 and CS2, why can CS2 have double bonds but not OF2? ۔
Lewis structure of cs2.
When calculating the Lewis structure, I usually count the electrons on the edges and draw the structure to see what the molecule would look like.
Let's use OF2, which cannot have double bonds, you will see why.
OF2 has 20 boundary electrons (O = 6 VE, F = 7 VE)
So when you draw a structure, you combine atoms and then subtract used electrons. (204 = 16VE)
Then add electrons to the outermost electrons and work with the whole bytes.
::: F: O: F ::::
It's hard to find your way here on the computer, but you have 3 wandering pairs around each fluorine and 2 wandering pairs around oxygen. If you count them, these are 4 in addition to the 16 limit electrons we used in the beginning. Everything has bytes, so be happy.
But let's see what happens when we add double bonds.
F == F
So to double bond, we take the right pair of fluorine electrons and leave it with two isolated pairs, and fluorine still has its bytes.
If you look at oxygen, it has not only 6 single and double bond electrons, but also two single pairs for a total of 10 VE, and we cannot get more than one byte.
As long as the atom fills its bytes, it can do so with single, double, or triple bonds.
Total 16 VE with CS2.
::: SK :::
In the wrong picture, only the sulfur atom completes the e-byte of the carbon bond and 3 pairs are separated.
So are we filling up with carbon bytes even though we've all used boundary electrons?
We can use one pair of each seller as double bond.
S = C = S.
The sulfur atom now has two single pairs of electrons and two pairs of double bond electrons.
Everything has bytes.
Unless you can see the structure, it will help you pull it out, count the electrons in multiples, and determine what kind of bond and how many pairs are isolated, and so on.
It helps !!