What Orbitals Are Involved in Bond Formation for Common Molecules and Ions?

[Soaring Crane]

For the following molecules and ions, indicate the obitals involved in bond formation.


1) SO2
The central atom is S, and it has 1 double bond with a O and a single bond with the remaining O. There is also 1 lone electron pair. Therefore, a S-O bond is sp^2-p while a S=O bond is sp^2-sp^3?


2) NO3-
N is central atom, and there are 2 single bonds between 2 O atoms and a double bond between the other O. A N-O bond is sp^2-p while a N=O bond is sp^2-sp^3?


3) NO2+
N is central atom, and there are 2 double bonds between both O atoms and N. Thus, a N=O bond is sp-sp^3?


4) NO2-
There is 1 single bond between a O atom and N and 1 double bond with the other O. One lone e- pair exists for N. A N-O bond is sp^2-p and a N=O bond is sp^2-sp^3?

Thanks.

 

[Soaring Crane]

Any volunteers?

Thanks again.

 

[Blueshift5]

Your analysis is correct. In general, the orbitals involved in bond formation are determined by the hybridization of the central atom and the type of bond (single, double, or triple). In the case of SO2, the sulfur atom is sp^2 hybridized and forms a sigma bond with each oxygen atom using a sp^2 orbital. The double bond between sulfur and one oxygen atom is formed by overlapping of a p orbital from sulfur and a p orbital from oxygen. The remaining p orbital on sulfur is used to form a pi bond with the other oxygen atom. Similarly, for NO3-, the nitrogen atom is sp^2 hybridized and forms a sigma bond with each oxygen atom using a sp^2 orbital. The double bond between nitrogen and one oxygen atom is formed by overlapping of a p orbital from nitrogen and a p orbital from oxygen. The remaining p orbital on nitrogen is used to form a pi bond with the other oxygen atom. For NO2+, the nitrogen atom is sp hybridized and forms a sigma bond with each oxygen atom using a sp orbital. The double bonds between nitrogen and both oxygen atoms are formed by overlapping of a p orbital from nitrogen and a p orbital from each oxygen atom. Finally, for NO2-, the nitrogen atom is sp^2 hybridized and forms a sigma bond with one oxygen atom using a sp^2 orbital. The remaining p orbital on nitrogen is used to form a pi bond with the other oxygen atom. Overall, the orbitals involved in bond formation are determined by the hybridization of the central atom and the type of bond being formed.