Draw the Lewis structure re for the formaldehyde (CH_(2)O) molecule. Be sure to in include all resonance structures es that satisfy the octet rule. square

To draw the Lewis structure for formaldehyde (CH₂O), we need to follow these steps:

1. **Count the total number of valence electrons:**
- Carbon (C) has 4 valence electrons.
- Hydrogen (H) has 1 valence electron each, so for 2 hydrogen atoms: $2 \times 1 = 2$.
- Oxygen (O) has 6 valence electrons.

Total valence electrons = $4 + 2 + 6 = 12$.

2. **Determine the central atom:**
- The central atom is usually the least electronegative atom that can form the most bonds. In this case, carbon is the central atom because it can form four bonds.

3. **Place the atoms and distribute the electrons:**
- Place carbon in the center, with two hydrogen atoms and one oxygen atom around it.
- Connect the atoms with single bonds initially.

4. **Distribute the remaining electrons to complete the octet rule:**
- After forming initial single bonds, we have used $2 \times 3 = 6$ electrons (one bond between C-H, another bond between C-H, and one bond between C-O).
- Remaining electrons = $12 - 6 = 6$.

5. **Complete the octet for oxygen:**
- Place the remaining 6 electrons as lone pairs on the oxygen atom.

6. **Check for octet completion and adjust bonds if necessary:**
- The oxygen atom now has 8 electrons (2 from the C-O bond and 6 as lone pairs).
- The carbon atom needs to complete its octet. Since carbon already has 6 electrons from the two C-H bonds and the C-O bond, it needs one more bond to complete its octet.

7. **Form a double bond between carbon and oxygen:**
- Move one lone pair from oxygen to form a double bond between carbon and oxygen.

Here is the Lewis structure for formaldehyde (CH₂O):

```
H
|
H - C = O
|
H
```

In this structure:
- Carbon forms two single bonds with hydrogen atoms and one double bond with the oxygen atom.
- Oxygen has two lone pairs of electrons.

This structure satisfies the octet rule for all atoms involved.