Chemistry: Atomic Structure & Periodicity Flashcards
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Read the first 7 Chemistry: Atomic Structure & Periodicity flashcards as text
Across a period from left to right, atomic radius generally:
Answer: decreases
Increasing nuclear charge pulls electrons in the same shell closer, shrinking the radius.
Which element has the highest first ionization energy?
Answer: Cl
Chlorine is farthest right in the period, giving it the highest first ionization energy among these.
Why does oxygen have a slightly lower first ionization energy than nitrogen?
Answer: Oxygen's paired 2p electron experiences repulsion
Removing the paired electron in oxygen's 2p^4 is easier due to electron-electron repulsion.
Which element is the most electronegative?
Answer: Fluorine
Fluorine is the most electronegative element on the periodic table.
The second ionization energy of sodium is much larger than its first because:
Answer: It removes a core electron from a noble-gas configuration
After losing one electron, Na+ has a stable neon core, making the next removal very difficult.
Which trend correctly describes electron affinity moving down a group?
Answer: Generally becomes less negative
Larger atoms down a group add electrons less readily, so electron affinity becomes less negative.
Which cation is smaller than its parent neutral atom?
Answer: Mg2+ vs Mg
Mg2+ loses its outer shell and has greater effective nuclear charge per electron, making it smaller than Mg.