Select all of the below statements that accurately describe the proper Lewis structure for CBr2F2.- The formal charge on each br

Answer:

There exist 12 lone pairs of electrons in the molecule.

Carbon has a formal charge of zero.

This molecule contains 4 covalent bonds.

Explanation:

To compute the formal charge (FC), the formula used is:

FC = V - N - B/2, where V is the count of valence electrons from the neutral atom, N represents the non-bonding valence electrons, and B indicates the total number of electrons engaged in bonds.

The Lewis structure is displayed in the image below. Both F and Br possess 7 valence electrons, while C has 4.

Thus, for C, FC = 4 - 0 - 8/2 = 0

For both Br, FC = 7 - 6 - 2/1 = 0

For both F, FC = 7 - 6 - 2/1 = 0

This structure illustrates that the molecule has 12 lone pairs of electrons (3 for each Br and 3 for each F).

All bonds present are covalent since the atoms share pairs of electrons, confirming that there are 4 covalent bonds in the molecule.