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Questions and Answers
Atomic radius increases from left to right across a period.
Atomic radius increases from left to right across a period.
False
Atomic radius decreases from top to bottom down a group.
Atomic radius decreases from top to bottom down a group.
False
A larger nucleus with more protons results in a stronger attraction to its electrons.
A larger nucleus with more protons results in a stronger attraction to its electrons.
True
A larger atomic radius corresponds to a weaker attraction between the nucleus and valence electrons.
A larger atomic radius corresponds to a weaker attraction between the nucleus and valence electrons.
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An increase in metallic property is associated with a decrease in atomic radius.
An increase in metallic property is associated with a decrease in atomic radius.
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The nucleus is larger than an atom.
The nucleus is larger than an atom.
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What is the main factor that determines the size of the nucleus?
What is the main factor that determines the size of the nucleus?
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What trend is observed in atomic radius as you move down a group on the periodic table?
What trend is observed in atomic radius as you move down a group on the periodic table?
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What is the main reason for the decrease in atomic radius across a period?
What is the main reason for the decrease in atomic radius across a period?
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How does the strength of attraction between the nucleus and valence electrons affect the metallic property of an element?
How does the strength of attraction between the nucleus and valence electrons affect the metallic property of an element?
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Study Notes
Atomic Radius
- Atomic radius is the distance from the nucleus to the outermost electron orbital.
- Atomic radius increases down a group (top to bottom) in the periodic table.
- This increase is due to the addition of electron shells, placing the outermost electrons further from the nucleus.
- The weaker attraction between the nucleus and these valence electrons makes them easier to delocalize.
- This trend correlates with increased metallic behavior.
- Atomic radius decreases across a period (left to right) in the periodic table.
- The increasing number of protons in the nucleus pulls the valence electrons closer resulting in a stronger attraction and tighter binding.
- This trend corresponds to decreased metallic behavior.
Nuclear Size
- Nuclear size is determined by the number of protons and neutrons.
- A larger nucleus (more protons and neutrons) results in a larger nucleus.
- A larger nucleus with more protons exerts a stronger attraction on its electrons, which leads to a smaller atomic radius.
- Larger atomic radius correlates with increased metallic property since it's easier to delocalize valence electrons.
- Smaller atomic radius corresponds to decreased metallic property since it's harder to delocalize valence electrons.
- The nucleus is significantly smaller than the entire atom.
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Description
Test your understanding of atomic radius and nuclear size with this quiz. Dive into the trends of atomic size in the periodic table and how nuclear size relates to the number of protons and neutrons. Perfect for students of chemistry!
