Why are the trends and exceptions to the trends in ionization energy observed? Check all that apply.

Ionization energy tends to increase down a group because the electrons get farther away from the nucleus.

Ionization energy tends to increase across a period because the nuclear charge increases.

Ionization energy tends to increase across a period because electrons are added to the same main energy level.

The ionization energies of the elements in Group 16 tend to be slightly smaller than the elements in Group 15 because the fourth electron is added to an unfilled p orbital.

The ionization energies of elements in Group 13 tend to be lower than the elements in Group 2 because the full s orbital shields the electron in the p orbital from the nucleus.

Question

Peyton Cardenas

Chemistry

17 January, 01:40

Why are the trends and exceptions to the trends in ionization energy observed? Check all that apply.

Ionization energy tends to increase down a group because the electrons get farther away from the nucleus.

Ionization energy tends to increase across a period because the nuclear charge increases.

Ionization energy tends to increase across a period because electrons are added to the same main energy level.

The ionization energies of the elements in Group 16 tend to be slightly smaller than the elements in Group 15 because the fourth electron is added to an unfilled p orbital.

The ionization energies of elements in Group 13 tend to be lower than the elements in Group 2 because the full s orbital shields the electron in the p orbital from the nucleus.

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Answers (1)

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Trenton · Answer 1

By definition, the ionisation energy is the term used to describe as the energy required to remove an electrical from the outermost orbital of an atom. In addition, the general trend of ionisation energy in a periodic table is that the energy required to remove an electron increases across a period due to decreasing atomic radius.