Determine the formal charges on the highlighted atoms. if an atom is formally neutral, indicate a charge of zero. the molecule h 3 c c n o. the second c is connected to the c h 3 group with a single bond and to n with a triple bond. n is highlighted and is connected to c with a triple bond and o with a single bond. o is highlighted and is connected to n with a single bond and has 3 lone pairs of electrons.

Formal charge on n is +1

Formal charge on o is -1

Explanation:

Consider the atom n,

n is connected to o with a single bond and to c with a triple bond

In case of n, number of valence electrons are 5

Number of non-bonding electrons are 0

Number of bonding electrons are 8 (∵ n is attached to 4 bonds and each bond is equivalent to 2 electrons)

∴ Formal charge on n = 5 - 0 - (8 ÷ 2) = 5 - 4 = +1

∴ Formal charge on n is +1

Consider the atom o,

o is connected to n by a single bond

In case of o, number of valence electrons are 6

Number of non-bonding electrons are 6 (∵ it has 3 lone pair of electrons)

Number of bonding electrons are 2 (∵ it is connected to n by a single bond and that bond is equivalent to 2 electrons)

Formal charge on atom o = 6 - 6 - (2 ÷ 2) = -1

∴ Formal charge on o is -1

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