Problem: Would you expect Fe3+ or Fe2+ to be the stronger Lewis acid? Explain.

🤓 Based on our data, we think this question is relevant for Professor Chamberlain's class at UCD.

We’re being asked which of the given compounds is a better Lewis acid.

Based on the Lewis definition:

Lewis acid is an electron pair acceptor.

Some characteristics of a Lewis acid:

• When hydrogen is connected to an electronegative element such as P, O, N, S or halogens

▪ hydrogen gains a partially positive charge → makes hydrogen act as a Lewis acid

• Positively charged metal ions

▪ can accept negative electron pairs → can act as Lewis Acids

• Central element that has less than 8 valence electrons around it

▪ more likely to accept an electron pair to follow the octet rule
▪ can accept electron pair → can act as Lewis acid

Would you expect Fe³⁺ or Fe²⁺ to be the stronger Lewis acid? Explain.

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 Lewis Acid and Base concept. You can view video lessons to learn Lewis Acid and Base. Or if you need more Lewis Acid and Base practice, you can also practice Lewis Acid and Base practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Chamberlain's class at UCD.

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 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.