(Polar molecules, Non-polar molecules, etc.)

Moderators: Chem_Mod, Chem_Admin

nshahwan 1L
Posts: 100
Joined: Fri Aug 30, 2019 12:18 am


Postby nshahwan 1L » Thu Nov 14, 2019 11:41 pm

Can someone explain part b to me?
2E.3 Draw the structures and name the shapes of the following molecules: (a) HCN; (b) CH2F2 .

Daniel Martinez 1k
Posts: 50
Joined: Wed Sep 18, 2019 12:16 am

Re: 2E.3

Postby Daniel Martinez 1k » Thu Nov 14, 2019 11:45 pm

The lewis structure would have 4 bonded pairs. So, the C would have a bond pair with 2 Fs and 2 Hs. Since there are 4 bonded pairs and no lone pairs, the shape of the molecule is a tetrahedral.

Jasmine Fendi 1D
Posts: 108
Joined: Sat Aug 24, 2019 12:15 am

Re: 2E.3

Postby Jasmine Fendi 1D » Thu Nov 14, 2019 11:55 pm

To add on to the comment above, the name of the shape of the molecule only depends on the number of atoms attached to the central atoms and the number of lone pairs on the central atom. Single, double and triple bonds are considered the same as "one unit" and lone pairs on outside atoms do not matter.

Posts: 55
Joined: Wed Sep 18, 2019 12:16 am

Re: 2E.3

Postby Aprice_1J » Fri Nov 15, 2019 12:02 am

I was also confused by this. Why is it that the hydrogens are closer to each other rather than all of them being in two intersecting lines with the fluorine as far away and the hydrogen as far away from each other.

Return to “Determining Molecular Shape (VSEPR)”

Who is online

Users browsing this forum: No registered users and 2 guests