The Lewis structure of nitrosyl chloride (NOCl) consists of a central nitrogen atom (N), an oxygen atom (O), and a chlorine atom (Cl). The nitrogen (N) and oxygen (O) atoms are connected by a double bond, and the nitrogen (N) and chlorine (Cl) atoms are connected by a single bond. The nitrogen atom (N) has one lone pair of electrons, the oxygen atom (O) has two lone pairs of electrons, and the chlorine atom (Cl) has three lone pairs of electrons. The detailed structural diagram is shown below:

Polarity and Molecular Configuration of Nitrosyl chloride

Nitrosyl chloride is a polar molecule. This polarity stems from the asymmetric curved geometry of the molecule and the difference in electronegativity among the nitrogen, oxygen, and chlorine atoms. The NOCl molecule has a curved shape or molecular geometry, also known as a angular or V-shaped molecule. Because the central nitrogen atom in the NOCl molecule has a lone pair of electrons, in addition to the repulsion between the N=O and N-Cl bond pairs, there is also electron repulsion between the lone pair and the bonding electron pairs. This strong repulsive force pushes the bonded oxygen and chlorine atoms away from the center. The N–O bond is highly polar (nitrogen is less electronegative than oxygen), while the N–Cl bond has opposite polarity (electronegativity: O > Cl > N). These two bond dipoles do not cancel each other out due to bending geometry. Therefore, NOCl has permanent dipoles and is a polar, V-shaped molecule.