Draw the Lewis Structure for the Hydrogen Cyanide Molecule (HCN) with C as the Center Atom

To draw the Lewis structure for the hydrogen cyanide molecule (HCN) with carbon (C) as the center atom, follow these steps:

1. Determine the total number of valence electrons:
   • Hydrogen (H) has 1 valence electron.
   • Carbon (C) has 4 valence electrons.
   • Nitrogen (N) has 5 valence electrons.

   Total valence electrons = 1 (H) + 4 (C) + 5 (N) = 10 valence electrons.

2. Place the atoms in the structure:

   Carbon (C) is the center atom, with hydrogen (H) on one side and nitrogen (N) on the other side.

3. Connect the atoms with single bonds:

   Draw a single bond between carbon (C) and hydrogen (H), and another single bond between carbon (C) and nitrogen (N). This uses up 4 valence electrons (2 electrons per bond).

4. Distribute the remaining electrons:

   You have 6 valence electrons left. Place these electrons around the nitrogen (N) atom to complete its octet. Nitrogen will have a lone pair and a triple bond with carbon (C).

5. Check the octet rule:
   • Hydrogen (H) has 2 electrons (satisfying the duet rule).
   • Carbon (C) has 8 electrons (satisfying the octet rule).
   • Nitrogen (N) has 8 electrons (satisfying the octet rule).

The final Lewis structure for HCN looks like this:

    H
    |
    C≡N

In this structure, the carbon (C) atom is triple-bonded to the nitrogen (N) atom, and single-bonded to the hydrogen (H) atom.