The molecular geometry of ClNO can be predicted using VSEPR (Valence Shell Electron Pair Repulsion) theory. In this molecule, nitrogen (N) is the central atom.
First, we need to determine the number of valence electrons for the atoms involved: chlorine (Cl) has 7 valence electrons, nitrogen (N) has 5, and oxygen (O) has 6, giving us a total of 18 valence electrons to work with.
Next, we can draw the Lewis structure:
- Place nitrogen in the center, since it is less electronegative than oxygen.
- Connect chlorine and oxygen to nitrogen with single bonds.
- Distribute the remaining electrons to satisfy the octets of chlorine and oxygen. You will find that nitrogen is left with one lone pair.
Now, we need to consider the number of bonded atoms and lone pairs around the nitrogen atom:
- Nitrogen is bonded to one chlorine and one oxygen atom, making two bonded pairs.
- There is also one lone pair on nitrogen.
According to VSEPR theory, the arrangement of the two bonded pairs and one lone pair results in a trigonal planar electron geometry. However, the presence of the lone pair causes the molecular geometry to be bent or angular, not linear.
Therefore, the predicted molecular geometry of ClNO, with nitrogen as the central atom, is bent.