Answer :
Step-by-Step Solution:
To determine the number of sigma ([tex]\(\sigma\)[/tex]) and pi ([tex]\(\pi\)[/tex]) bonds in the [tex]\( \text{H}_2\text{C}=\text{CH}_2 \)[/tex] molecule (ethene), we need to analyze the types of bonds formed by each carbon atom.
1. Structure of Ethene:
[tex]\[ \text{H}_2\text{C}=\text{CH}_2 \][/tex]
Ethene consists of two carbon atoms double-bonded to each other, and each carbon atom is also bonded to two hydrogen atoms.
2. Sigma ([tex]\(\sigma\)[/tex]) Bonds:
- Each [tex]\( \text{C} \)[/tex] atom forms one [tex]\(\sigma\)[/tex] bond with each [tex]\( \text{H} \)[/tex] atom, and there are two hydrogen atoms bonded to each carbon. Therefore, each carbon forms two [tex]\(\sigma\)[/tex] bonds with hydrogen atoms.
- Additionally, each carbon forms one [tex]\(\sigma\)[/tex] bond with the other carbon atom.
- Therefore, each carbon makes 3 [tex]\(\sigma\)[/tex] bonds in total: two with hydrogen atoms and one with the other carbon atom.
- Since there are two carbon atoms in the molecule, the total number of [tex]\(\sigma\)[/tex] bonds is:
[tex]\[ 3 \, \text{\(\sigma\) bonds per carbon} \times 2 \, \text{carbons} = 6 \, \text{\(\sigma\) bonds} \][/tex]
3. Pi ([tex]\(\pi\)[/tex]) Bonds:
- The double bond between the two carbon atoms consists of one [tex]\(\sigma\)[/tex] bond and one [tex]\(\pi\)[/tex] bond.
- Therefore, the total number of [tex]\(\pi\)[/tex] bonds in the molecule is:
[tex]\[ 1 \, \text{\(\pi\) bond} \][/tex]
By analyzing the bonding in the ethene molecule, we can conclude that there are:
[tex]\[ \boxed{6 \, \sigma \, \text{bonds} \; \text{and} \; 1 \, \pi \, \text{bond}} \][/tex]
Given the options:
- 3 and 2
- 4 and 3
- 3 and 4
- 2 and 3
- 5 and 1
None of these options match our conclusion since:
[tex]\[ \text{There are } 6 \, \sigma \, \text{bonds} \text{ and } 1 \, \pi \, \text{bond} \text{ in the ethene molecule.} \][/tex]
It seems there might be an error with the available answer choices, but our detailed analysis stands correct with [tex]\( \boxed{6 \, \sigma \, \text{bonds}} \)[/tex] and [tex]\( \boxed{1 \, \pi \, \text{bond}} \)[/tex].
To determine the number of sigma ([tex]\(\sigma\)[/tex]) and pi ([tex]\(\pi\)[/tex]) bonds in the [tex]\( \text{H}_2\text{C}=\text{CH}_2 \)[/tex] molecule (ethene), we need to analyze the types of bonds formed by each carbon atom.
1. Structure of Ethene:
[tex]\[ \text{H}_2\text{C}=\text{CH}_2 \][/tex]
Ethene consists of two carbon atoms double-bonded to each other, and each carbon atom is also bonded to two hydrogen atoms.
2. Sigma ([tex]\(\sigma\)[/tex]) Bonds:
- Each [tex]\( \text{C} \)[/tex] atom forms one [tex]\(\sigma\)[/tex] bond with each [tex]\( \text{H} \)[/tex] atom, and there are two hydrogen atoms bonded to each carbon. Therefore, each carbon forms two [tex]\(\sigma\)[/tex] bonds with hydrogen atoms.
- Additionally, each carbon forms one [tex]\(\sigma\)[/tex] bond with the other carbon atom.
- Therefore, each carbon makes 3 [tex]\(\sigma\)[/tex] bonds in total: two with hydrogen atoms and one with the other carbon atom.
- Since there are two carbon atoms in the molecule, the total number of [tex]\(\sigma\)[/tex] bonds is:
[tex]\[ 3 \, \text{\(\sigma\) bonds per carbon} \times 2 \, \text{carbons} = 6 \, \text{\(\sigma\) bonds} \][/tex]
3. Pi ([tex]\(\pi\)[/tex]) Bonds:
- The double bond between the two carbon atoms consists of one [tex]\(\sigma\)[/tex] bond and one [tex]\(\pi\)[/tex] bond.
- Therefore, the total number of [tex]\(\pi\)[/tex] bonds in the molecule is:
[tex]\[ 1 \, \text{\(\pi\) bond} \][/tex]
By analyzing the bonding in the ethene molecule, we can conclude that there are:
[tex]\[ \boxed{6 \, \sigma \, \text{bonds} \; \text{and} \; 1 \, \pi \, \text{bond}} \][/tex]
Given the options:
- 3 and 2
- 4 and 3
- 3 and 4
- 2 and 3
- 5 and 1
None of these options match our conclusion since:
[tex]\[ \text{There are } 6 \, \sigma \, \text{bonds} \text{ and } 1 \, \pi \, \text{bond} \text{ in the ethene molecule.} \][/tex]
It seems there might be an error with the available answer choices, but our detailed analysis stands correct with [tex]\( \boxed{6 \, \sigma \, \text{bonds}} \)[/tex] and [tex]\( \boxed{1 \, \pi \, \text{bond}} \)[/tex].
