ClO – Draw the Lewis structure for the ion. Show the formal charges of all atoms in the correct structure. Include all lone pairs of electrons.
The Correct Answer and Explanation is :
To draw the Lewis structure for the hypochlorite ion (ClO⁻), follow these steps:
Steps to Draw the Lewis Structure:
- Count the Total Valence Electrons:
- Chlorine (Cl) has 7 valence electrons.
- Oxygen (O) has 6 valence electrons.
- Add 1 electron for the negative charge (⁻).
- Total: 7+6+1=147 + 6 + 1 = 14 valence electrons.
- Connect the Atoms with a Single Bond:
- Chlorine is less electronegative than oxygen, so it will be the central atom.
- Draw a single bond between Cl and O, which uses 2 electrons (leaving 14−2=1214 – 2 = 12 electrons).
- Distribute Remaining Electrons as Lone Pairs:
- Start by completing the octet of oxygen. Place 6 electrons (3 lone pairs) on oxygen.
- Then, place 6 electrons (3 lone pairs) on chlorine.
- Check the Octet Rule and Formal Charges:
- Oxygen: 6 nonbonding electrons + 2 bonding electrons = 8 electrons (octet satisfied).
- Chlorine: 6 nonbonding electrons + 2 bonding electrons = 8 electrons (octet satisfied).
- Calculate Formal Charges:
- Formal charge formula: Formal charge=Valence electrons−(Nonbonding electrons+Bonding electrons2)\text{Formal charge} = \text{Valence electrons} – (\text{Nonbonding electrons} + \frac{\text{Bonding electrons}}{2})
- Oxygen: 6−(6+22)=−16 – (6 + \frac{2}{2}) = -1
- Chlorine: 7−(6+22)=07 – (6 + \frac{2}{2}) = 0
- Formal charge formula: Formal charge=Valence electrons−(Nonbonding electrons+Bonding electrons2)\text{Formal charge} = \text{Valence electrons} – (\text{Nonbonding electrons} + \frac{\text{Bonding electrons}}{2})
Thus, the oxygen has a formal charge of −1-1, and the chlorine has a formal charge of 00.
Final Lewis Structure:
- Chlorine (Cl) is bonded to oxygen (O) with a single bond.
- Oxygen has 3 lone pairs and a −1-1 formal charge.
- Chlorine has 3 lone pairs and no formal charge.
Explanation:
This structure satisfies the octet rule for both atoms. The negative charge resides on the more electronegative oxygen atom, making the structure stable. The distribution of formal charges aligns with the expected behavior of oxygen and chlorine based on their electronegativities. Hypochlorite ions play essential roles in disinfectants and bleaching agents, showcasing the stability of this electronic configuration.