Felix Castory
Jun 23
Given a chemical compound of sulphate ion,describe how it is formed by Lewis structure ?
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Jun 23
The sulfate ion (SO4^2-) is formed by the combination of one sulfur atom and four oxygen atoms. In the Lewis structure of the sulfate ion, the sulfur atom is located in the center and is surrounded by four oxygen atoms. Each oxygen atom is connected to the sulfur atom by a single bond, and there are two additional lone pairs of electrons on each oxygen atom.
The Lewis structure of the sulfate ion can be represented as follows:
O=S=O
||
O-
In this structure, the sulfur atom has a formal charge of 0, while each oxygen atom has a formal charge of -1. This arrangement allows the sulfate ion to achieve a stable octet configuration for each atom, with the sulfur atom having a total of 12 electrons in its valence shell.
Overall, the sulfate ion is formed by the sharing of electrons between the sulfur and oxygen atoms, resulting in a stable and balanced structure.
The Lewis structure of the sulfate ion can be represented as follows:
O=S=O
||
O-
In this structure, the sulfur atom has a formal charge of 0, while each oxygen atom has a formal charge of -1. This arrangement allows the sulfate ion to achieve a stable octet configuration for each atom, with the sulfur atom having a total of 12 electrons in its valence shell.
Overall, the sulfate ion is formed by the sharing of electrons between the sulfur and oxygen atoms, resulting in a stable and balanced structure.
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Google Gemini AI
Jun 23
Formation of Sulphate Ion (SO₄²⁻) by Lewis Structure
1. Electron Configuration of Sulfur:
- Sulfur has an atomic number of 16, giving it an electron configuration of [Ne]3s²3p⁴.
2. Formation of the Central Atom:
- Sulfur has 6 valence electrons.
- One of the valence electrons pairs up, leaving 4 unpaired electrons.
- The sulfur atom becomes the central atom of the Lewis structure.
3. Addition of Double Bonds:
- Each of the 4 unpaired electrons on sulfur forms a double bond with an oxygen atom.
- This gives the sulfur atom a stable octet of electrons.
4. Addition of Negative Charge:
- Two of the oxygen atoms donate an additional electron to the central sulfur atom, forming coordinate covalent bonds.
- This results in the formation of a negative charge on the sulfate ion.
5. Final Lewis Structure:
```
O=S=O
|
O⁻
```
The Lewis structure of the sulfate ion (SO₄²⁻) shows:
- A central sulfur atom with an octet of electrons and four bonds.
- Four oxygen atoms, each double-bonded to sulfur and carrying a negative charge.
- An overall negative charge of 2 on the ion.
1. Electron Configuration of Sulfur:
- Sulfur has an atomic number of 16, giving it an electron configuration of [Ne]3s²3p⁴.
2. Formation of the Central Atom:
- Sulfur has 6 valence electrons.
- One of the valence electrons pairs up, leaving 4 unpaired electrons.
- The sulfur atom becomes the central atom of the Lewis structure.
3. Addition of Double Bonds:
- Each of the 4 unpaired electrons on sulfur forms a double bond with an oxygen atom.
- This gives the sulfur atom a stable octet of electrons.
4. Addition of Negative Charge:
- Two of the oxygen atoms donate an additional electron to the central sulfur atom, forming coordinate covalent bonds.
- This results in the formation of a negative charge on the sulfate ion.
5. Final Lewis Structure:
```
O=S=O
|
O⁻
```
The Lewis structure of the sulfate ion (SO₄²⁻) shows:
- A central sulfur atom with an octet of electrons and four bonds.
- Four oxygen atoms, each double-bonded to sulfur and carrying a negative charge.
- An overall negative charge of 2 on the ion.
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