Questions and Answers
What describes atomic radii as one moves from top to bottom within a group?
The atomic radius increases from top to bottom within a group.
What describes atomic radii as one travels across a period (from left to right)?
The atomic radius decreases as one moves across a period.
What is true of the first ionization energy within a group?
The first ionization energy decreases from top to bottom within a group.
What is a measure of how readily an atom attracts electrons when it is part of a compound?
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Which of the following is true about the radii of Na and Na+?
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Study Notes
Atomic Radii Trends
- Atomic radius increases from top to bottom within a group in the periodic table due to the addition of electron shells, resulting in larger atoms.
- Atomic radius decreases as one moves from left to right across a period due to the increased positive charge in the nucleus, which pulls the electrons closer.
First Ionization Energy Trends
- The first ionization energy decreases from top to bottom within a group, as increased distance from the nucleus and electron shielding reduce the energy required to remove an electron.
Electronegativity
- Electronegativity is defined as the measure of an atom's ability to attract electrons in a chemical bond; a key property that influences bond formation and molecular structure.
Comparison of Atomic Radii
- Sodium (Na) has a larger atomic radius than its ionized form, sodium ion (Na+), because removal of an electron reduces electron-electron repulsion, bringing remaining electrons closer to the nucleus.
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Description
Test your knowledge on the trends within the periodic table with this quiz. It covers concepts such as atomic radii variations and ionization energy as you move across periods and down groups. Perfect for reinforcing your understanding of chemistry concepts related to elements.
