Using formal charge as a guide, choose the most favorable Lewis structure for the sulfate ion, SO42-. (Note: electronegativity values: S = 2.5, O = 3.5) Answer Options: A.) All three structures are equally favorable B.) Structure II C.) Structure I D.) Structure III
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.
Using formal charge as a guide, choose the most favorable Lewis structure for the sulfate ion, SO42-. (Note: electronegativity values: S = 2.5, O = 3.5)
Answer Options:
A.) All three structures are equally favorable
![The image presents three structural diagrams of a sulfate ion (SO₄²⁻), each labeled as Structure I, Structure II, and Structure III. These diagrams illustrate different resonance structures, demonstrating the delocalization of electrons within the sulfate ion.
**Structure Details:**
1. **Structure I:**
- The sulfur (S) atom is at the center, surrounded by four oxygen (O) atoms.
- Each oxygen has a single bond with the sulfur, and carries three lone pairs of electrons.
- The overall charge of the ion is -2, as indicated by the 2- sign outside the brackets.
2. **Structure II:**
- Similar central arrangement with sulfur bonded to four oxygens.
- One of the oxygen atoms forms a double bond with sulfur, while the others form single bonds.
- The double-bonded oxygen has two lone pairs, whereas each single-bonded oxygen has three lone pairs.
- The ion has a -2 charge overall.
3. **Structure III:**
- The arrangement mirrors Structure II, with a different oxygen forming the double bond with sulfur.
- Similar distribution of lone pairs as Structure II.
- The ion maintains a -2 charge.
These resonance structures illustrate how electrons can be distributed among the sulfur and oxygen atoms in the sulfate ion, showing different possible configurations that stabilize the ion through delocalization of electron density.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1290e653-b206-4ea8-8527-a4dd2bf5953e%2F3cb3cbfe-08eb-4d52-b4a9-04806a3d18c8%2Ftu8awb_processed.png&w=3840&q=75)
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