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Trends in Ionization Energy

Ionization energy trends show that down a group, first ionization energy decreases due to increased atomic radius and shielding, leading to weaker nuclear attraction. Conversely, across a group, first ionization energy increases as atomic radius decreases and nuclear charge increases, resulting in stronger attraction between the nucleus and electrons. The balance of shielding and nuclear charge is key to understanding these trends.

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Maahil. M
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17 views1 page

Trends in Ionization Energy

Ionization energy trends show that down a group, first ionization energy decreases due to increased atomic radius and shielding, leading to weaker nuclear attraction. Conversely, across a group, first ionization energy increases as atomic radius decreases and nuclear charge increases, resulting in stronger attraction between the nucleus and electrons. The balance of shielding and nuclear charge is key to understanding these trends.

Uploaded by

Maahil. M
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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Download as DOCX, PDF, TXT or read online on Scribd
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Trends in ionization energy

Down the group

Number of protons increase which means nuclear charge increases.

Number of shielding increases.

Electron is removed from a higher energy quantum shell.

Atomic radius increases

Increase in shielding is more significant than increase in protons.

Weaker attraction between nucleus and electrons

Less energy to remove one electron from the outermost shell

First ionization energy decreases down the group.

Across the group

Number of protons increases which means nuclear charge increases.

Number of shielding remains same across the group.

Electron is removed from the same quantum shell.

Atomic radius decreases

Increase in proton number is more significant than increase in shielding.

Stronger attraction between nucleus and electrons from the outermost shell.

More energy is required to remove electron

First ionization energy increases across the group

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