For COF2 draw an appropriate Lewis structure (carbon is the central atom).
The Correct Answer and Explanation is:
Lewis Structure for COF₂:
To draw the Lewis structure of COF₂ (carbonyl fluoride), where carbon is the central atom:
- Count the total valence electrons:
- Carbon (C) has 4 valence electrons.
- Oxygen (O) has 6 valence electrons.
- Each fluorine (F) has 7 valence electrons, and there are 2 of them.
- Total = 4 (C) + 6 (O) + 7×2 (F) = 24 valence electrons.
- Place carbon in the center, as it is the least electronegative element except hydrogen.
- Attach oxygen and both fluorine atoms to the carbon using single bonds.
- So far, 3 single bonds = 6 electrons used.
- Distribute remaining electrons (18 left) to complete octets:
- Start with outer atoms: give 6 electrons (3 lone pairs) to each fluorine.
- Each F now has a full octet (2 from the bond with C + 6 nonbonding).
- That uses 12 electrons (6 for each F).
- 6 electrons remain. Oxygen currently has 2 from the bond, so it needs 6 more to complete its octet.
- Assign 6 electrons (3 lone pairs) to oxygen.
- Check carbon’s octet:
- Carbon has only 6 electrons (3 single bonds). It needs 2 more.
- Convert the C–O bond into a double bond (share one lone pair from O).
- Now carbon has 8 electrons: 2 from each C–F bond, and 4 from the double bond with O.
Final Lewis Structure:
rCopyEdit ..
:F–C=O:
..
:F:
Each F has three lone pairs. The O has two lone pairs after sharing one in a double bond with C.
Explanation:
The Lewis structure of COF₂ illustrates the bonding and lone pairs around each atom while ensuring the octet rule is satisfied. Carbon, as the central atom, forms one double bond with oxygen and single bonds with each fluorine atom. This arrangement ensures that all atoms achieve stable electron configurations. The molecule contains a total of 24 valence electrons, which are correctly distributed in bonds and lone pairs. This structure also explains the molecular geometry, which is trigonal planar, with bond angles close to 120 degrees.
