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Problem: Which member of the following pairs would you expect to be more energetically stable? Justify each choice.a. NaBr or NaBr 2

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

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The more energetically stable compound is, the lower energy it has. We will look at how the compounds are formed to determine which is more stable. 

Comparing the two compounds, both NaBr and NaBr2 have ionic bonds. Ionic bond is formed from the transfer of valence electrons from a metal to a non-metal. In this case, Na is our metal and Br is our non-metal.

Let us determine the valence electrons of our metal and non-metal:

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Problem Details

Which member of the following pairs would you expect to be more energetically stable? Justify each choice.

a. NaBr or NaBr 2

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 Bond Energy concept. If you need more Bond Energy practice, you can also practice Bond Energy practice problems.

What professor is this problem relevant for?

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

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.