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2 cards from this section. Quick, good the night before a test.
Define atomic radius.
Think about how we measure an atom’s size.
What happens to atomic radius as you move down a group in the periodic table?
Consider the number of electron shells.
Does atomic radius generally increase or decrease as you go down a group in the periodic table?
Think about how many layers of electrons are added.
Isoelectronic species with the same number of electrons but different atomic numbers will have different sizes. Is this statement true or false?
What happens to size if protons increase?
Given the following ions: Cl⁻, K⁺, and Ca²⁺, list them in order of increasing ionic radius and justify your reasoning based on nuclear charge.
Consider how the number of protons pulls on the electrons.
Explain how the effective nuclear charge changes across Period 3 and how that impacts atomic size.
Think about charge pulling power.
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