Explanation:

To determine the number of sp3 hybridized carbons in the given compound, we need to analyze the molecular formula C4H5N.

Step 1: Calculate the number of carbons (C).

Given molecular formula: C4H5N
Number of carbons (C) = 4

Step 2: Calculate the number of hydrogens (H).

Given molecular formula: C4H5N
Number of hydrogens (H) = 5

Step 3: Calculate the number of nitrogens (N).

Given molecular formula: C4H5N
Number of nitrogens (N) = 1

Step 4: Determine the possible structures of the compound.

Since the compound is acyclic (meaning it does not contain any rings), we can consider different arrangements of the atoms to form a linear structure.

Step 5: Draw the possible structures of the compound.

Using the given molecular formula, we can draw the following possible structures for the compound:

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

Step 6: Analyze the structures to identify the number of sp3 hybridized carbons.

In the drawn structures, we can see that there is only one carbon atom (labeled as C) that is bonded to four other atoms (three hydrogens and one nitrogen). This carbon atom is sp3 hybridized because it forms four sigma bonds and has a tetrahedral geometry.

Therefore, the number of sp3 hybridized carbons in the given compound is 1.

Conclusion:

The number of sp3 hybridized carbons in the acyclic neutral compound with the molecular formula C4H5N is 1.