Question

A Lewis structure of OCI ion is drawn below. What is the formal charge on each atom? OC a. Cl atom- +1 and each O atom --1 b. Cl atom-0 and each O atom --1 c. Cl atom- -1 and each O atom-0 d. Cl atom +3 and each O atom2 e. Cl atom-0, one O atom 0, one O atom +1 20.

Answer 1

The formal charges in the hypochlorite ion, OCI-, are Oxygen -1 and Chlorine 0, hence the correct answer is (b) Cl atom-0 and each O atom --1.

Step-by-step explanation:

The student is asking for the formal charge on each atom in the hypochlorite ion, OCI-. With 6 valence electrons from the oxygen atom and 7 from the chlorine atom, plus one additional electron for the negative charge, we have a total of 14 valence electrons. After placing a bonding pair between O and Cl, we assign six electrons (as three lone pairs) to each atom to fulfill their octet requirements.

Now, let's calculate the formal charge for each atom:

• Oxygen (O): 6 valence electrons (for the neutral atom) - [6 non-bonding + 1/2(2 bonding)] = 6 - 7 = -1.
• Chlorine (Cl): 7 valence electrons (for the neutral atom) - [6 non-bonding + 1/2(2 bonding)] = 7 - 7 = 0.

Thus, the formal charges are Oxygen -1 and Chlorine 0, making the correct answer (b) Cl atom-0 and each O atom --1.