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

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

Answer 1

The correct answer is: The ionization energy increases because the stability of the half-full p subshell is increased.Explanation: The first ionization energy generally increases across a period due to the increasing nuclear charge, which pulls the electrons closer to the nucleus. However, between group 2 and group 13, the trend is not followed because the stability of the half-filled p subshell in group 13 elements is increased, making it harder to remove an electron from the p orbital compared to the s orbital in group 2 elements.

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