Question

answer the questions below about the highlighted atom in this lewis structure: in how many sigma bonds does the highlighted atom participate? in how many pi bonds does the highlighted atom participate? what is the orbital hybridization of the highlighted atom?

Answer 1

To determine the number of sigma (σ) bonds and pi (π) bonds the highlighted atom participates in, count the number of single bonds as σ bonds and the number of double or triple bonds as π bonds. The orbital hybridization of the highlighted atom can be determined by looking at the number of regions of electron density around the atom.

Step-by-step explanation:

In the Lewis structure, a highlighted atom is the central atom. To determine the number of sigma (σ) bonds and pi (π) bonds the highlighted atom participates in, count the number of single bonds as σ bonds and the number of double or triple bonds as π bonds. The orbital hybridization of the highlighted atom can be determined by looking at the number of regions of electron density around the atom.

1. In the Lewis structure, count the number of single bonds connected to the highlighted atom. Each single bond represents one σ bond.
2. In the Lewis structure, count the number of double bonds or triple bonds connected to the highlighted atom. Each double bond represents one σ bond and one π bond, and each triple bond represents one σ bond and two π bonds.
3. To determine the orbital hybridization of the highlighted atom, use VSEPR theory to find the geometry around the atom. Based on the geometry, assign the corresponding set of hybridized orbitals. For example, if there are four regions of electron density, the orbital hybridization is sp³.