A skeletal structure for sulfurous acid (H₂SO₃) shown below. Starting from this structure, complete the Lewis structure that follows the octet rule on all atoms.
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
A skeletal structure for sulfurous acid (H₂SO₃) shown below. Starting from this structure, complete the Lewis structure that follows the octet rule on all atoms.
![## Sulfurous Acid (H2SO3) Lewis Structure
### Introduction
The skeletal structure for sulfurous acid (H₂SO₃) is shown below. This structure is a basis to help you complete the Lewis structure that adheres to the octet rule for all atoms.
### Instructions
Starting from this structure, complete the Lewis structure that follows the octet rule on all atoms.
### Skeletal Structure
Below is the initial skeletal structure of the sulfurous acid molecule:
- **Sulfur (S)**: The central sulfur atom is bonded to three oxygen (O) atoms.
- **Double Bond**: One oxygen atom forms a double bond with the sulfur atom, contributing two pairs of electrons in the bond.
- **Single Bonds**: The other two oxygen atoms form single bonds with the sulfur atom. These oxygen atoms each have a hydrogen (H) atom attached.
- **Hydrogen (H)**: There are two hydrogen atoms, each bonded to a different oxygen atom.
#### Lewis Structure of Sulfurous Acid (H₂SO₃)
```
O
..
:O:
/ \
H--O S--O
. . .
: O .
: .
H
```
### Step-by-Step Guide to Completing the Lewis Structure:
1. **Identify Valence Electrons**:
- Sulfur: 6 valence electrons
- Oxygen: 6 valence electrons each
- Hydrogen: 1 valence electron each
2. **Determine Total Electrons**:
- Total valence electrons = 1(2) + 6(3) + 6 = 24 electrons
3. **Draw Skeletal Structure**:
- Place sulfur (S) in the center.
- Attach each oxygen (O) to sulfur with single bonds.
- Attach one hydrogen (H) to each of the two single-bonded oxygen atoms.
4. **Distribute Remaining Electrons to Fulfill Octet Rule**:
- Distribute electrons around each oxygen to complete their octets.
- Add double bonds if needed to ensure sulfur follows the octet rule.
### Conclusion
Completing the Lewis structure ensures that the octet rule is satisfied for all atoms. This representation helps in understanding the electron configuration and the bonding nature in sulfurous acid molecules. If you have any questions or need further clarification,](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F42c9ca3c-cb39-47fb-a603-0de5ef67ab03%2F0e7ea94e-2021-4f11-9c36-1ed4678bf2ef%2Fdqvlyf_processed.png&w=3840&q=75)
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