Question #aad44

1 Answer
Sep 17, 2016

Answer:

Here's what I got.

Explanation:

The thing to remember here is that

  • a single bond #-># contains one sigma bond
  • a double bond #-># contains one sigma bond and one pi bond
  • a triple bond #-># contains one sigma bond and two pi bonds

In order to find the number of sigma and pi bonds present in a molecule of cyanogen, #"C"_2"N"_2#, you must examine its Lewis structure.

http://chemistry.about.com/od/factsstructures/ig/Chemical-Structures---C/Cyanogen.htm

As you can see, the cyanogen molecule contains one #"C"-"C"# single bond and two #"C"-="N"# triple bonds.

This means that you will have

  • a total of three sigma bonds

Here you have one sigma bond from the #"C"-"C"# single bond and one sigma bond from each of the two #"C"-="N" #triple bonds

  • a total of four pi bonds

Here you get two pi bonds from each of the two #"C" -= "N"# triple bonds