To draw the Lewis structure for CH2F2, we first need to identify the central atom. In this case, carbon (C) is the central atom, as it is less electronegative than fluorine (F) and it can form more bonds.
Next, we count the total valence electrons available for bonding. Carbon has 4 valence electrons, each hydrogen (H) contributes 1 valence electron, and each fluorine contributes 7 valence electrons. Therefore, the total number of valence electrons is:
4 (C) + 2 × 1 (H) + 2 × 7 (F) = 4 + 2 + 14 = 20 valence electrons.
In the Lewis structure, we place the carbon atom in the center and arrange hydrogen and fluorine atoms around it. Carbon will form bonds with each of the hydrogen and fluorine atoms. The structure looks like this:
H | H-C-F | F
This shows that carbon is bonded to two hydrogens and two fluorines. Now, we can see that there are a total of 4 bonds around the central carbon atom (2 with H and 2 with F).
As for the shape of this molecule, we can use VSEPR (Valence Shell Electron Pair Repulsion) theory to determine it. With four bonded atoms and no lone pairs on the central carbon, the shape around the carbon is tetrahedral. In a tetrahedral geometry, the bond angles are approximately 109.5 degrees.
In summary, after analyzing the Lewis structure for CH2F2, we can conclude that there are 4 bonds around the central carbon atom, and the overall shape of the molecule is tetrahedral.