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ianc1339
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- TL;DR Summary
- Why does the first ionization energy between group 1 and group 2 elements increase?
The first ionization energy decreases between group 5 and group 6 due to the repulsion between the electrons in the p orbital.
Although I understand that the effective nuclear charge increases between group 1 and group 2 elements, why isn't this the case between group 1 and group 2 elements? Shouldn't the first ionization energy decrease between group 1 and group 2 due to the repulsion between the electrons?
Although I understand that the effective nuclear charge increases between group 1 and group 2 elements, why isn't this the case between group 1 and group 2 elements? Shouldn't the first ionization energy decrease between group 1 and group 2 due to the repulsion between the electrons?