Pergunta

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
Solução

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PedroMestre · Tutor por 5 anos
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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: .
- Oxygen (O) has 6 valence electrons.
Total valence electrons = .
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 electrons (one bond between C-H, another bond between C-H, and one bond between C-O).
- Remaining electrons = .
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.
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: .
- Oxygen (O) has 6 valence electrons.
Total valence electrons = .
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 electrons (one bond between C-H, another bond between C-H, and one bond between C-O).
- Remaining electrons = .
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.
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