Which of the following compounds has an "arrowed" carbon atom that is sp2 hybridized? A C H₂C=C=CH₂ CH3 H₂C-C-CH₂ NH B H₂C-C-CH3 D Compounds B and C
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 on Hybridization
**Question:** Which of the following compounds has an “arrowed” carbon atom that is sp² hybridized?
### Descriptions of Each Option:
- **Option A:**
\[
\text{H}_2\text{C} = \text{C} = \text{CH}_2
\]
The arrow points to the central carbon atom in a structure where two hydrogen atoms are single-bonded to a carbon atom. This carbon atom is double-bonded to another carbon atom, which is again double-bonded to a third carbon atom, which is single-bonded to two hydrogen atoms.
- **Option B:**
\[
\text{H}_3\text{C} - \text{C} = \text{N}
\]
The arrow points to a carbon atom that is single-bonded to a nitrogen atom (which is single-bonded to a hydrogen atom) and double-bonded to another carbon atom, which is single-bonded to three hydrogen atoms.
- **Option C:**
\[
\text{H}_3\text{C} - \text{C} - \text{CH}_3
\]
The arrow points to the central carbon atom that is single-bonded to two other carbon atoms, each of which is single-bonded to three hydrogen atoms.
- **Option D:**
\[
\text{Compounds B and C}
\]
This option suggests that both compounds B and C might have the arrowed carbon atom in the specified hybridization state.
### Analysis:
The hybridization of a carbon atom depends on the types of bonds it forms:
- **sp³ hybridization:** Carbon forms four single bonds.
- **sp² hybridization:** Carbon forms one double bond and two single bonds.
- **sp hybridization:** Carbon forms triple bonds or two double bonds.
Based on this understanding:
- In **Option A**, the central carbon atom has two double bonds. Therefore, it is sp hybridized.
- In **Option B**, the arrowed carbon atom forms a double bond and two single bonds, indicating sp² hybridization.
- In **Option C**, the arrowed carbon atom forms four single bonds, indicating sp³ hybridization.
So, the correct answer is:
**Option B:**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F127f63d9-8f89-4c37-8cc0-122cae65c6f1%2F25cc5f22-a762-44c7-b0d6-cf31f76af372%2Fgzr08wn_processed.jpeg&w=3840&q=75)
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