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Jessica Chen 2C
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Postby Jessica Chen 2C » Sun Nov 03, 2019 11:14 pm

What is an easy way to remember the trends of polarizability/polarizing power on the periodic table?

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Re: Trends

Postby madawy » Sun Nov 03, 2019 11:19 pm

honestly i find it easiest to try and understand the reasons behind them !! Most of it corresponds to the amount of orbitals/amount of electrons in a single orbital. E.g. the more electrons in a single orbital means the stronger of an attraction it’ll feel to the nucleus etc etc which correlates to ionization and affinity. I’m sure there are a ton of questions/ on it :)

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Re: Trends

Postby ALegala_2I » Mon Nov 04, 2019 9:00 am

Cations with a smaller radius and a more positive charge have greater polarizing power. For example, K+ > K in polarizing power. Anions with a larger radius and a more negative charge have greater polarizability because they have more electrons. So I->Br-, in polarizability.

Emily Chirila 2E
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Joined: Sat Jul 20, 2019 12:16 am

Re: Trends

Postby Emily Chirila 2E » Mon Nov 04, 2019 9:05 am

If all else fails an easy way to remember is that ionization energy, electron affinity, and electronegativity all increase up and to the right, and atomic radius is the opposite (increase down and to the left). It is important to know the meaning behind them but that's a simple way to remember :)

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