What is ionization energy?
Periodic Trends Practice

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Chemistry
•
10th - 11th Grade
•
Hard
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1.
FLASHCARD QUESTION
Front
Back
Ionization energy is the amount of energy required to remove an electron from an atom in its gaseous state.
2.
FLASHCARD QUESTION
Front
Why does ionization energy decrease down a group in the periodic table?
Back
Ionization energy decreases down a group because the valence electrons are farther from the nucleus, reducing the nuclear attraction.
3.
FLASHCARD QUESTION
Front
What is the trend of atomic radius as you move down a group?
Back
The atomic radius increases as you move down a group due to the addition of more electron shells.
4.
FLASHCARD QUESTION
Front
What is the trend of ionization energy as you move across a period?
Back
Ionization energy generally increases as you move from left to right across a period due to increasing nuclear charge.
5.
FLASHCARD QUESTION
Front
Which element has the highest ionization energy in Period 2?
Back
Neon (Ne) has the highest ionization energy in Period 2.
6.
FLASHCARD QUESTION
Front
What is the atomic radius of an element?
Back
The atomic radius is the distance from the nucleus to the outermost shell of electrons.
7.
FLASHCARD QUESTION
Front
How does the atomic radius change across a period?
Back
The atomic radius decreases across a period due to increased nuclear charge pulling electrons closer to the nucleus.
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