Periodic Table Set-up. Periodic Trends. Atomic Radius :. 1/2 distance between 2 nuclei of the same element. Group Trend: Increases . Why: e-are being added to new energy levels further away, electron shielding occurs, so the nucleus can not pull electrons in a close. .
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1/2 distance between 2 nuclei of the same element.
Group Trend: Increases
Why: e-are being added to new energy levels
further away, electron shielding occurs, so the nucleus can not pull electrons in a close.
Period Trend: Decreases →
Why: e-are being added to the same energy level. As the nucleus becomes stronger, the electrons are drawn in closer.
The energy required to remove
Trend: Decrease →
Why: e-are further away (shielded) and easier to take away.
Period Trend: Increase →
Why: e-are closer to nucleus + harder to remove.
Atoms are closer to having a complete valence shell
and want to gain not lose e-.
: ability to attract e-
: Electrons are harder to bring in further away with the nucleus pulling less.
Period Trend: Increases →
due to a stronger nucleus
easier to bring in
Atoms want to complete their valence shell.
Electronegativity: ability to attract e-in a bond
→ scale of O-4
: lose valence e'
Effect on Radius:
decrease due to loss of
anions (+): gain electrons
increases due to addition
Effect on Radius :
of e- to the same energy level and not
changing the strength of the nucleus.