What is the hybridization about the nitrogen center in #"NCl"_2^(+)#?
1 Answer
- Distributing
#3# lone pairs on each chlorine atom, we use#12# of these electrons. - Making two bonds off of nitrogen uses
#4# more. - The remaining
#2# become a lone pair.
But then nitrogen only has 6 valence electrons. So, instinctively, the next best thing is to make a second
Since
This gives for formal charge:
#"7 valence" - "6.5 owned" = +0.5# on each chlorine atom#"5 valence" - "5 owned" = 0# on the nitrogen atom
which adds up to a total charge of
#2+2+1+2+1/2(2) = 8# total around each chlorine atom#2+2+2+1/2(2)+1/2(2) = 8# total around the nitrogen atom
Assuming this is the correct structure, this indicates a hybridization of