Question

In the molecule \(\mathrm{CH}_{2}=\mathrm{C}=\mathrm{C}=\mathrm{CH}_{2}\), number of carbon atoms in sp hybrid state is

Short answer

There are 2 sp hybridized carbon atoms.

Step-by-step solution

Analyze the Molecular Structure

The molecule given is linear and consists of a series of double bonds: \(\mathrm{CH}_{2}=\mathrm{C}=\mathrm{C}=\mathrm{CH}_{2}\). This molecule can be written in a chain of carbons as \( H_2C=C=C=CH_2 \).

Determine Hybridization of Carbon Atoms

In determining the hybridization, remember: a carbon forms sp hybridized orbitals when it is involved in two double bonds or a single triple bond. Analyze the structure: \(\mathrm{C}_1 - \mathrm{C}_2=C_3=C_4-\mathrm{C}_5\).

Identify sp Hybridized Carbons

Check each carbon atom: 1. \(\mathrm{C}_1\) is bonded to two hydrogen atoms and one carbon with a double bond, so it is not sp hybridized.2. \(\mathrm{C}_3\) is bonded to two carbon atoms each with double bonds, 3. \(\mathrm{C}_4\) similarly is bonded to two carbon atoms each with double bonds. Since both \(\mathrm{C}_3\) and \(\mathrm{C}_4\) are involved in two double bonds, both are \(\mathrm{sp}\) hybridized.

Count the sp Hybridized Carbon Atoms

Given the analysis, we conclude that \(\mathrm{C}_3\) and \(\mathrm{C}_4\) are sp hybridized. Therefore, there are two carbon atoms in sp hybridization state.

Key concepts

sp Hybridization

In organic chemistry, understanding the concept of sp hybridization is crucial for analyzing molecular structures. When a carbon atom forms two double bonds or a single triple bond, it adopts the sp hybridization form.
The carbon atom mixes one s orbital with one p orbital to create two identical sp hybrid orbitals. This results in a linear geometry, with these orbitals being 180 degrees apart.

• sp hybridization involves one s and one p orbital.
• The carbon atom adopts a straight-line shape (linear).
• Each sp hybrid orbital participates in forming a sigma bond, often with another carbon or atom.

In the given molecule, the central carbons, specifically C3 and C4, each participate in two double bonds. This configuration leads both of them to adopt an sp hybridized state. Understanding this helps explain the molecule’s linear nature.

Carbon Hybridization

Carbon atoms exhibit various hybridization forms that dictate the molecular structure they participate in. Typically, carbons can be found in sp, sp2, or sp3 hybrid states.
Each state results in unique geometry and bonding properties.

• sp Hybridization: One s and one p orbital combine, leading to a linear geometry.
• sp2 Hybridization: One s and two p orbitals combine, resulting in a trigonal planar shape.
• sp3 Hybridization: One s and three p orbitals merge, forming a tetrahedral shape.

In the molecule exttt{CH}_2=C=C=CH_2, the presence of alternating double bonds suggests that certain carbons will need to be sp hybridized to accommodate the molecule's linear structure. This highlights the diversity and adaptability of carbon's hybridization to form complex structures.

Molecular Structure Analysis

Analyzing the molecular structure of organic compounds involves looking at the arrangement and hybridization of atoms. The geometry, type of bonds, and hybridization state significantly influence the molecule's chemical characteristics.
To better understand a molecule like exttt{CH}_2=C=C=CH_2, follow these steps:

• Identify the positions of atoms and types of bonds (single, double, triple).
• Determine each carbon atom’s hybridization state by examining its bonding partners.
• Evaluate the geometry derived from the hybridization states, confirming linearity in sp hybridized carbons.

In sum, for organic molecules, the hybridization of carbon atoms dictates their spatial arrangement and reactivity. This understanding helps chemists predict molecular behavior and reactivity in broader chemical contexts.