Draw the lewis dot structure for two different isomers for C2H5N

Draw the lewis dot structure for two different isomers for C2H5N. Name the geometrical shapes of the molecules with their bond angles, and determine whether they or polar or non-polar.

The correct answer and explanation is :

The compound C₂H₅N can form two distinct isomers: ethylamine and dimethylamine. Let’s draw the Lewis dot structures for both and discuss their geometry, bond angles, and polarity.

1. Ethylamine (C₂H₅N)

Lewis Dot Structure:

In ethylamine, the nitrogen (N) is bonded to an ethyl group (C₂H₅). The structure looks like this:

   H   H
   |   |
H - C - C - N - H
   |   |
   H   H

Explanation:

• The nitrogen atom has a lone pair of electrons and forms three single bonds, one with each hydrogen atom and one with the ethyl group.
• Carbon atoms form single bonds with the hydrogen atoms and a single bond with nitrogen.

Geometry:

• The geometry around the nitrogen atom is trigonal pyramidal, as nitrogen has a lone pair. The bond angles are approximately 107°, which is less than the ideal tetrahedral angle (109.5°) due to the repulsion from the lone pair.

Polarity:

• Ethylamine is polar because the nitrogen atom has a lone pair and a higher electronegativity than carbon and hydrogen. This creates a dipole moment with a partial negative charge on the nitrogen and a partial positive charge on the hydrogen atoms.

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2. Dimethylamine (C₂H₅N)

Lewis Dot Structure:

In dimethylamine, the nitrogen is bonded to two methyl groups (CH₃) and one hydrogen atom. The structure looks like this:

     H
     |
H₃C - N - CH₃

Explanation:

• The nitrogen atom bonds to two methyl groups and one hydrogen atom, and it also has a lone pair.
• Carbon atoms in the methyl groups are bonded to hydrogen atoms.

Geometry:

• The geometry around the nitrogen in dimethylamine is trigonal pyramidal, as it also has a lone pair of electrons. The bond angles are again 107°, similar to ethylamine.

Polarity:

• Dimethylamine is also polar. The lone pair on nitrogen, along with the difference in electronegativity between nitrogen and carbon, results in a dipole moment.

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Summary:

1. Ethylamine (C₂H₅N):

• Geometry: Trigonal pyramidal, bond angle ~107°
• Polarity: Polar

1. Dimethylamine (C₂H₅N):

• Geometry: Trigonal pyramidal, bond angle ~107°
• Polarity: Polar

Both molecules are polar due to the lone pair on nitrogen and the difference in electronegativity between nitrogen and hydrogen or carbon. However, they differ in the type of alkyl groups attached to the nitrogen.