Which of the following correctly represents the Lewis dot structure for the neutral compound CHF?

• A. C is the central atom with single bonds to H and F; C has no lone pairs, F has three lone pairs, H has none.
• B. C is the central atom with single bonds to H and F; C has two lone pairs, F has three lone pairs, H has none.
• C. C is the central atom with single bonds to H and F; C has one lone pair, F has two lone pairs, H has one lone pair.
• D. C is the central atom with double bonds to H and F; C has one lone pair, F has two lone pairs, H has none.

Answer: (A)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for the molecule CHF. Carbon (C) has 4 valence electrons, hydrogen (H) has 1, and fluorine (F) has 7. Add these together to find the total valence electrons available for bonding and lone pairs.
2. Step 2: Identify the central atom. Carbon is less electronegative than fluorine and hydrogen, so it will be the central atom. Arrange the atoms with carbon in the center, and hydrogen and fluorine bonded to it.
3. Step 3: Draw single bonds between the central carbon atom and each of the other atoms (H and F). Each single bond represents 2 electrons shared between atoms.
4. Step 4: Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each atom where applicable. Hydrogen only needs 2 electrons (a duet), carbon aims for 8 electrons, and fluorine also aims for 8 electrons. Remember that carbon typically does not have lone pairs in simple molecules like CHF.
5. Step 5: Verify the Lewis structure by checking that the total number of electrons used (bonding and lone pairs) equals the total valence electrons calculated in Step 1, and that each atom satisfies its electron requirements (octet or duet).