Which of the following pairs represent resonance structures? :0= and I. .. S=C: and s=c=S: II. .. :N= :N=Cö: N C=O: and III. :N=c=ö: and :C N O: IV.
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.
![**Question: Which of the following pairs represent resonance structures?**
**I.**
- **Structure 1:**
O==O—O:
(Oxygen atoms are connected with a double bond followed by a single bond. The oxygen atoms have lone pairs of electrons.)
- **Structure 2:**
O—O==O
(Oxygen atoms are connected with a single bond followed by a double bond. The oxygen atoms have lone pairs of electrons.)
**II.**
- **Structure 1:**
:S==S—C:
(Sulfur and carbon atoms are connected with single and double bonds. Sulfur has lone pairs.)
- **Structure 2:**
:S—C==S:
(Sulfur and carbon atoms are connected with double and single bonds. Sulfur has lone pairs.)
**III.**
- **Structure 1:**
[:N==C==O:]^-
(Nitrogen and oxygen atoms are connected with two double bonds through carbon. Nitrogen and oxygen have lone pairs. The structure carries a negative charge.)
- **Structure 2:**
[:N≡C—O:]^-
(Nitrogen and oxygen atoms are connected with a triple bond and a single bond through carbon. Nitrogen and oxygen have lone pairs. The structure carries a negative charge.)
**IV.**
- **Structure 1:**
[:N==C==O:]^-
(Nitrogen and carbon atoms are connected with double bonds. Oxygen has a single bond. Nitrogen and oxygen have lone pairs. The structure carries a negative charge.)
- **Structure 2:**
[:C—N==O:]^-
(Carbon and nitrogen have a single bond and nitrogen has a double bond with oxygen. Nitrogen and oxygen have lone pairs. The structure carries a negative charge.)
**Explanation:**
Pairs of resonance structures have the same arrangement of atoms but differ in the distribution of electrons (bonds and lone pairs). They are valid Lewis structures that depict molecules where electron distribution can be represented in multiple ways.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd38f8f8d-3c67-4950-8636-439a4de702d1%2Fd8b45b56-8227-476a-a2ee-0358e803892b%2Fm0y2rp_processed.jpeg&w=3840&q=75)
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