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:
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-.
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 +
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 Heteronuclear Diatomic Molecules concept. You can view video lessons to learn Heteronuclear Diatomic Molecules. Or if you need more Heteronuclear Diatomic Molecules practice, you can also practice Heteronuclear Diatomic Molecules practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Bellert's class at BAYLOR.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.