What is the hybridization of the central atom in NOCl? Hybridization- What are the approximate bond angles in this Bond angles substance
The correct answer and explanation is :
The central atom in NOCl is nitrogen (N). To determine its hybridization and bond angles, let’s go through the steps and concepts systematically.
Hybridization of Nitrogen in NOCl
- Valence Electrons of Nitrogen: Nitrogen (N) belongs to Group 15 and has 5 valence electrons.
- Bonding in NOCl: In the molecule NOCl, nitrogen forms one single bond with oxygen (O) and one single bond with chlorine (Cl). Additionally, nitrogen has one lone pair of electrons.
- Electron Domain Count: The electron domains around the nitrogen atom come from:
- Two single bonds (one to oxygen, one to chlorine)
- One lone pair of electrons
So, nitrogen has three electron domains in total. According to the VSEPR theory, three electron domains typically result in sp² hybridization, leading to a trigonal planar electron geometry. The bond angles in a trigonal planar geometry are approximately 120°, but this can be slightly altered due to the lone pair repulsion.
Bond Angles in NOCl
The presence of a lone pair of electrons on nitrogen distorts the ideal trigonal planar geometry. The lone pair is more repulsive than bonding pairs, causing the bond angles between the two bonds (N-O and N-Cl) to be slightly less than the ideal 120°. Hence, the bond angles in NOCl are slightly less than 120° but still close to this value.
Key Summary:
- Hybridization of nitrogen: sp²
- Electron Geometry: Trigonal Planar
- Molecular Geometry: Bent (due to the lone pair)
- Approximate Bond Angles: Slightly less than 120°
Explanation:
The nitrogen atom in NOCl undergoes sp² hybridization because it has three electron regions around it (two bonds and one lone pair). These electron regions repel each other and arrange themselves in a trigonal planar geometry. However, the lone pair takes up more space and pushes the bonding pairs closer together, causing the bond angles to be slightly reduced from the ideal 120°.
Hybridization and structure of NOCl.
Here is an image showing the molecular structure of Nitrosyl Chloride (NOCl) with the central nitrogen atom, its bonds to oxygen and chlorine, and a lone pair of electrons. The bond angles are slightly less than 120° due to the lone pair. This structure demonstrates the sp² hybridization of nitrogen in NOCl.