Question

The angle between the overlapping of one s-orbital and one p-orbital is

• A. 180$^{\circ}$
• B. 120$^{\circ}$
• C. 109$^{\circ}$28'
• D. $120^{\circ}$ 60'

Answer 1

The Correct Option is A

To solve the given problem, we need to determine the angle between the overlapping of one s-orbital and one p-orbital. Let's explore the concept of orbital overlapping:

• s-Orbital: The s-orbital has a spherical shape. It is evenly distributed around the nucleus, allowing it to overlap from any direction equally.
• p-Orbital: The p-orbital has a dumbbell shape and is directional, meaning its maximum probability density is aligned along a particular axis in space. For instance, the p_x, p_y, and p_z orbitals are oriented along the x, y, and z axes, respectively.

When an s-orbital overlaps with a p-orbital, the maximum overlap occurs when the orbitals are aligned directly along the axis of the p-orbital. This overlap gives rise to directional bonding, characteristic of the angle between the s and p orbitals.

Typically, the angle formed in such a linear arrangement is 180° owing to the linear geometry along a straight axis. This happens because the most effective overlap (and thereby bond formation) occurs along a straight line linearly through the center.

Based on this understanding, the correct answer for the angle between the overlapping of one s-orbital and one p-orbital is 180°.

Let's verify the other options:

1. 120°: This angle is characteristic of trigonal planar geometry, not applicable for simple s-p orbital overlapping.
2. 109°28': This angle represents the tetrahedral bond angles, common in sp³ hybridization, which involves the mixture of one s-orbital and three p-orbitals, not a single s-p overlap.
3. 120°60': This is incorrect as it does not correspond to any known angle resembling simple s-p orbital overlap.

Therefore, the correct choice is 180°, as it accurately represents the linear overlap between an s-orbital and a p-orbital, typically in sp hybridization where linear geometry is expected.