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Periodic Trends- Chemistry with 100% correct answers
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Atomic Radius half the distance between adjacent nuclei or bonded nuclei *no defined edge of atom because of electron cloud- can't measure from edge Atomic Radius- Period Trend -left to right decrease -increase in number of protons and valence electrons but same energy level; no further shielding s...

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  • January 4, 2023
  • 3
  • 2022/2023
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  • atomic radius half the distance between adjacent nuclei or bonded nuclei no defined edge of atom because of electron cloud cant measure from edge atomic radius period trend left to right de

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Periodic Trends- Chemistry



Atomic Radius - half the distance between adjacent nuclei or bonded nuclei
*no defined edge of atom because of electron cloud- can't measure from edge

Atomic Radius- Period Trend - -left to right decrease
-increase in number of protons and valence electrons but same energy level; no further
shielding so stronger nuclear pull

Atomic Radius- Group Trend - -going down atomic radius increases -there are more
energy levels causing more shielding and less nuclear pull

Ion - a charged atom; formed when giving up or taking electrons; form ionic bonds

Cations - -positively charged ion due to electron loss
-usually metal

Anion - -negatively charged ion due to electron gain
-usually nonmetal

Ionic radius - -half the distance between adjacent charged nuclei or bonded charged
nuclei (cations and anions)

Cation- Period Trend - -radius decreases left to right
-losing electrons, nuclear pull greater because there are more protons than electrons

Transition from Anion to Cation- crossing over stair step line - -radius increases
-gaining electrons, nuclear pull less because electrons outnumber protons
-more electron repulsion

Anion- Period Trend - -radius decreases left to right
-gaining fewer electrons with each element
-electrons don't outnumber protons as much

Atomic radius of Anion versus atomic radius of Cation - anionic radius is bigger than
cationic radius if they're in the same period

Valence electrons - the electrons that are on the outermost energy level- are involved in
a chemical reaction

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