Problem: The ionic radii of the ions S2–, Cl–, and K+ are 184, 181, 138 pm respectively. Explain why these ions have different sizes even though they contain the same number of electrons.

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

FREE Expert Solution

We’re being asked to explain why the ionic radius of the following ions have different sizes even though they contain the same number of electrons. 


Recall that ionic radius is the size of an ion. The trend for ionic radius is as follows: it increases from right to left and down a period in the periodic table. Ionic radius also increases with increasing number of electrons.


For this problem, we need to do the following:

Step 1: Determine the electrons in each species.

Step 2: Compare the charges if they are isoelectronic.


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Problem Details

The ionic radii of the ions S2–, Cl, and K+ are 184, 181, 138 pm respectively. Explain why these ions have different sizes even though they contain the same number of electrons.

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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 Periodic Trends: Ionic Radius concept. You can view video lessons to learn Periodic Trends: Ionic Radius. Or if you need more Periodic Trends: Ionic Radius practice, you can also practice Periodic Trends: Ionic Radius practice problems.

What professor is this problem relevant for?

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

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.