A skeletal structure for sulfate (SO2) is 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.
**Diagram Explanation:**
The image displays a skeletal structure for the sulfate ion (SO₄²⁻). The diagram consists of:
- A central sulfur atom (S) represented by the letter "S".
- Four oxygen atoms (O) attached to the sulfur atom.
- Two of the oxygen atoms are singly bonded to the sulfur atom with a single line (–).
- Two of the oxygen atoms are doubly bonded to the sulfur atom with double lines (=).
**Instructions:**
To complete the Lewis structure that adheres to the octet rule for all atoms, follow these guidelines:
1. Ensure that each oxygen atom has eight electrons around it, implying that each oxygen forms bonds such that it acquires a full valence shell.
2. The sulfur atom must form a total of six bonds, as sulfur can have an expanded octet.
Using dot notation for electrons, the finalized Lewis structure should ensure:
- Each oxygen atom has either single bonds with additional lone pairs of electrons to complete its octet or double bonds without lone pairs.
- The central sulfur atom accommodates more than eight electrons due to its ability to expand its valence shell, featuring single and double bonds with surrounding oxygen atoms.
This skeletal structure forms the foundational framework for illustrating sulfate ion’s Lewis structure in a detailed and accurate manner.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf3280c8-8a53-4cd7-b227-b3a58aeda25e%2F38d116db-858b-4614-8442-7ac1152ad468%2Fowjq93f_processed.jpeg&w=3840&q=75)
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