Select all of the below statements that accurately describe the proper Lewis structure for CBr2F2.- The formal charge on each bromine is -1.- There are 12 lone pairs of electrons on the molecule.- The formal charge on carbon is zero.- There are 4 covalent bonds within the molecule.- The formal charge on each fluorine is -1.

FC = V - N - B/2, where V is the number of the valence electrons of the neutral element, N is the number of non-bonding valence electrons, and B is the total of electrons shared in bond.

The Lewis structure is represented in the image below. F and Br have 7 valence electrons and C 4 valence electrons.

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

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

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

For the structure, we can see that there are 12 lone pairs of electrons on the molecule (3 in each Br and 3 in each F).

All the bonds are covalent because the atoms are sharing a pair of electrons, so there are 4 covalent bonds within the molecule.

pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-10-03T07:20:45+02:00

The Lewis structure shows the valence electrons in a molecule as dots around the symbols of its constituent atoms. Shared electrons are shown as two dots or a dash.

The true statements about the molecule CBr2F2 are;

There are 12 lone pairs of electrons on the molecule

The formal charge on carbon is zero

There are 4 covalent bonds within the molecule

The formal charge an an atom is the charge assigned to the atom assuming equal sharing of electrons in chemical bonds within the molecule. From the structure of the molecule shown in the image attached to this answer, the formal charge on carbon is zero.

From the image attached, we can also see that each of bromine and fluorine atoms has three lone pairs of electrons making a total of 12 lone pairs in the CBr2F2 molecule.

Finally, two bromine and two fluorine atoms are attached to carbon central atom in CBr2F2 giving a total of four covalent bonds in the molecule.

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