Draw the Overlap Between P Atomic Orbitals to Show the Covalent

Question

Examlex · Accepted Answer

The Answer is In chlorine gas (Cl₂), the covalent bond between the two chlorine atoms is formed by the overlap of their unpaired p atomic orbitals. Each chlorine atom has seven valence electrons, and its electron configuration ends in 3s²3p⁵. This means that in the p orbital, there are three p orbitals (p_x, p_y, and p_z), and five electrons are distributed among them, with one of the p orbitals having an unpaired electron.

To form a Cl-Cl bond, the unpaired electron in the p orbital of one chlorine atom overlaps with the unpaired electron in the p orbital of the other chlorine atom. This overlap is a head-on overlap, known as a sigma (σ) bond, which is the strongest type of covalent bond.

Here's a simplified representation of the overlap:

```
Cl: [Ne] 3s² 3p⁵

* Each Cl atom has an unpaired electron in one of its p orbitals.

Cl atom 1: ...3p: ↑↓ ↑↓ ↑
Cl atom 2: ...3p: ↑↓ ↑↓ ↑

* The unpaired electrons (indicated by single arrows ↑) are in the same type of p orbital (e.g., p_z).

Overlap:
Cl atom 1: ...3p: ↑↓ ↑↓ ↑
\
σ bond formation
/
Cl atom 2: ...3p: ↑↓ ↑↓ ↑

* The resulting molecule is Cl₂ with a single covalent bond between the two Cl atoms.
```

In this diagram, the single arrows represent the unpaired electrons that overlap to form the σ bond. The paired electrons (indicated by arrows pointing in opposite directions ↑↓) do not participate in the bond formation and are considered as part of the filled inner orbitals or lone pairs.

Please note that this is a simplified representation and does not show the actual shape and orientation of the p orbitals, which are dumbbell-shaped and oriented at right angles to each other. The actual overlap occurs in three-dimensional space and involves the correct alignment of the p orbitals to allow for effective overlap and bond formation.

Draw the Overlap Between P Atomic Orbitals to Show the Covalent

Definitions: