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Ionic radius in a group while moving down.
- a)Remains same from top to bottom
- b)Decreases from top to bottom
- c)Increases from top to bottom
- d)First increases and then decreases
Correct answer is option 'C'. Can you explain this answer?
Most Upvoted Answer
Ionic radius in a group while moving down.a)Remains same from top to b...
Ionic radius in a group increases from top to bottom since one energy shell is added with each period
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Ionic radius in a group while moving down.a)Remains same from top to b...
Understanding Ionic Radius in a Group
As we move down a group in the periodic table, the ionic radius of elements generally increases. Here's why:
1. Increased Electron Shells
- Each successive element in a group has an additional electron shell.
- This results in a larger distance between the nucleus and the outermost electrons.
2. Shielding Effect
- With more electron shells, the inner electrons repel the outer electrons.
- This shielding reduces the effective nuclear charge felt by the outermost electrons, allowing them to spread out more.
3. Size of the Ions
- Cations (positively charged ions) often decrease in size compared to their parent atoms due to the loss of outer electrons.
- Anions (negatively charged ions) increase in size due to the addition of electrons.
4. Group Trends
- For alkali metals (Group 1), the ionic radius increases significantly as we move from lithium to cesium.
- Similarly, for halogens (Group 17), the ionic radius increases from fluoride to iodide.
Conclusion
- Overall, as we move down a group in the periodic table, the ionic radius increases due to the addition of electron shells and the corresponding increase in shielding.
- This trend is crucial for understanding chemical bonding and reactivity in various elements.
In summary, the correct answer regarding ionic radius in a group while moving down is option 'C', indicating that the ionic radius increases from top to bottom.
As we move down a group in the periodic table, the ionic radius of elements generally increases. Here's why:
1. Increased Electron Shells
- Each successive element in a group has an additional electron shell.
- This results in a larger distance between the nucleus and the outermost electrons.
2. Shielding Effect
- With more electron shells, the inner electrons repel the outer electrons.
- This shielding reduces the effective nuclear charge felt by the outermost electrons, allowing them to spread out more.
3. Size of the Ions
- Cations (positively charged ions) often decrease in size compared to their parent atoms due to the loss of outer electrons.
- Anions (negatively charged ions) increase in size due to the addition of electrons.
4. Group Trends
- For alkali metals (Group 1), the ionic radius increases significantly as we move from lithium to cesium.
- Similarly, for halogens (Group 17), the ionic radius increases from fluoride to iodide.
Conclusion
- Overall, as we move down a group in the periodic table, the ionic radius increases due to the addition of electron shells and the corresponding increase in shielding.
- This trend is crucial for understanding chemical bonding and reactivity in various elements.
In summary, the correct answer regarding ionic radius in a group while moving down is option 'C', indicating that the ionic radius increases from top to bottom.
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