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Problem: Silver and rubidium both form +1 ions, but silver is far less reactive. Suggest an explanation, taking into account the ground-state electron configurations of these elements and atomic radii.

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We are asked to explain why Silver (Ag) is far less reactive than Rubidium (Rb) taking into account the ground-state electronic configuration of these elements and atomic radii.


Silver and rubidium belong in the 5th period of the periodic table


The condensed electronic configuration of the atoms are as follows:

 Rb: [Kr] 5s1

 Ag: [Kr] 4d105s1

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Problem Details

Silver and rubidium both form +1 ions, but silver is far less reactive. Suggest an explanation, taking into account the ground-state electron configurations of these elements and atomic radii.

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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 concept. If you need more Periodic Trends practice, you can also practice Periodic Trends practice problems.

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Based on our data, we think this problem is relevant for Professor Grimes' class at Thomas Jefferson University.