Lewis structure for C2F6

Answer 1

To draw the Lewis structure for C2H4, the total number of valence electrons must be known. Carbon has 4 and hydrogen has 1, making a grand total of 12 e- (4*2 + 4*1). All electrons are shared within bonds in this compound.

Carbon and Carbon are double bonded to each other, with each carbon having two hydrogens attached. Each element in this arrangement has a full outer shell. Hydrogen has 2 and each carbon has 8.

Answer 2

There are 14 Valence electrons in this compound. Knowing hydrogen can only contain one bond and carbon can only contain four bonds, we can make a structure that resembles this:

H

|

H - C - F

|

H

If you add all the valence electrons used (two for each bond) you will get 8 valence electrons used. Since 14-8=6, we know that we still need to place 6 valence electrons on the compound. Since the hydrogen and carbon atoms cannot recieve any more electron domains (bonds or electron pairs), the only plausible solution if to add 6 electrons (or 3 electron pairs) to Fluoride. This will result in:

H

| _

H - C - F|

| -

H

With the lines around F representing electron pairs.

You can check this lewis structure by using the formal charge equation:

Formal Charge = Valence electrons - (Number of bonds/2) - number of valence electrons attatched to the atom.

Using the formula you want the formal charge to be as close to zero as possible.

We know that it is tetrahedral because there are four bond sites to the central atom and no lone pairs.

Answer 3

F F
F - C - C - F
F F

Six electrons around each of the F Atoms...

Answer 4

you put f and then two dots on the top, two dots on the left side, and then two dots on the bottom of the f

Answer 5

H h

/ /

c=c

/ /

h h

Answer 6

double bond between the 2 carbon atoms, each carbon atom has 2 F

Answer 7

The 6 Carbon atoms are aranged in a ring, with 2 H atoms bonded to each C atom.

Answer 8

Tetrahedral.