Among the elements of the main group, the general trend in the first ionization energy moving across a period is not followed between group 2 and group 13. Which best explains these exceptions?

The ionization energy decreases because the full s orbital shields the electron entering the p orbital.

The ionization energy increases because the full s orbital shields the electron entering the p orbital.

The ionization energy decreases because the stability of the half-full p subshell is increased.

The ionization energy increases because the stability of the half-full p subshell is increased.

Question

Chemistry

Richard Caldwell

18 May, 16:25

Among the elements of the main group, the general trend in the first ionization energy moving across a period is not followed between group 2 and group 13. Which best explains these exceptions?

The ionization energy decreases because the full s orbital shields the electron entering the p orbital.

The ionization energy increases because the full s orbital shields the electron entering the p orbital.

The ionization energy decreases because the stability of the half-full p subshell is increased.

The ionization energy increases because the stability of the half-full p subshell is increased.

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Answers (2)

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Dashawn Flores · Answer 1

The Ionization energy decreases because the full s orbital shields the electron entering the p orbital. This is known as "shielding", When each new electron experiences attraction from the nucleus and repulsion forces from the S orbitals, the net force on outer shell electrons is significantly smaller. Therefore, ionization energy decreases during these groups.

Robles · Answer 2

The Ionization energy decreases because the full s orbital shields the electron entering the p orbital.