Problem: Using the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders. Which ones are paramagnetic? Place the species in order of increasing bond length and bond energy.a. CN + b. CN c. CN–

FREE Expert Solution
80% (356 ratings)
FREE Expert Solution

To calculate bond order of CN+, CN and CN- and predict other properties, we will start by drawing the molecular orbital diagram for all three.


Let’s start with the CN+ ion

CN+ is composed of two atoms from 2nd period. The electronic configurations of C and N are:


null


Carbon is a group 4A element having 4 valence electrons and nitrogen has 5 valence electrons (Group 5A). There is 1 positive charge, so we will subtract 1 electron from the total for the positive charge.


Total valence electrons are 4+5-1 = 8 e-.


80% (356 ratings)
Problem Details

Using the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders. Which ones are paramagnetic? Place the species in order of increasing bond length and bond energy.

a. CN + 

b. CN 

c. CN

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the MO Theory: Bond Order concept. You can view video lessons to learn MO Theory: Bond Order Or if you need more MO Theory: Bond Order practice, you can also practice MO Theory: Bond Order practice problems .

How long does this problem take to solve?

Our expert Chemistry tutor, Rae-Anne took 15 minutes to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Davis' class at UCF.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in . You can also practice practice problems .