We have to predict if the N–O bonds in NO3- are stronger or weaker than the N–O bonds in NO+.
To solve this problem, we need the Lewis structure and resonance forms for the NO3- and NO+ ions.
A resonance structure shows the delocalization of electrons in a molecule.
Resonance structures differ only in the placement of electrons over the atoms in the molecule.
We will be following these steps:
Step 1: Determine the central atom in the molecule.
Step 2: Calculate the total number of valence electrons present.
Step 3: Draw the Lewis structure for the molecule.
Step 4: Draw the resonance structures.
Predict whether the N-O bonds in NO3- are stronger or weaker than the N-O bond in NO+.
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 Average Bond Order concept. You can view video lessons to learn Average Bond Order. Or if you need more Average Bond Order practice, you can also practice Average Bond Order practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Zhang's class at USF.