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Chapter 7: Problem 16

In going across a row of the periodic table, electrons are added and ionization energy generally increases. In going down a column of the periodic table, electrons are also being added but ionization energy decreases. Explain

Short Answer

Expert verified
In general, ionization energy increases across a row of the periodic table because the atomic radius decreases, resulting in a stronger attraction between the nucleus and outermost electrons. Ionization energy decreases down a column due to an increase in atomic radius and electron shielding, causing weaker attraction between the nucleus and outermost electrons, making them easier to remove.

Step by step solution

01

Understand ionization energy

Ionization energy is the energy required to remove an electron from an atom or ion in its gaseous state. In general, ionization energy increases when it becomes harder to remove an electron due to a stronger attraction between the nucleus and the electrons.
02

Atomic radius and its impact on ionization energy

Atomic radius is the distance between the nucleus of an atom and its outermost electrons. As we move across a row in the periodic table, the number of protons and electrons increases, while the number of electron shells remains the same. This causes the atomic radius to decrease because the increased positive charge of the nucleus attracts the electrons more strongly, pulling them closer. As a result, the ionization energy required to remove an electron increases.
03

Electron shielding and its effect on ionization energy

Electron shielding occurs when inner electrons shield the outer electrons from the full attractive force of the nucleus. As we move down a column in the periodic table, the number of electron shells increases, causing an increase in atomic radius and electron shielding. This means that the outermost electrons are farther from the nucleus and experience a weaker attraction due to the shielding effect of inner electrons. As a result, less ionization energy is required to remove an electron, causing a decrease in ionization energy. To summarize:
04

Ionization energy in the periodic table

In general, ionization energy increases while moving across a row of the periodic table because the atomic radius decreases as the number of protons and electrons increases. This results in the outermost electrons being more tightly held by the nucleus, requiring more energy to remove them. Ionization energy decreases while moving down a column of the periodic table due to an increase in the atomic radius and electron shielding. This causes the outermost electrons to have a weaker attraction to the nucleus, making them easier to remove, and thus requiring less ionization energy.

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Most popular questions from this chapter

Mars is roughly 60 million km from Earth. How long does it take for a radio signal originating from Earth to reach Mars?

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