First ionization energy of group 1 and group 2 elements

  • #1
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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?
 

Answers and Replies

  • #2
DrClaude
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s orbitals extend to the nucleus, so there is a strong increase in potential energy when the nuclear charge increases. This more than compensates for the added electron-electron repulsion.
 
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