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In which of the following is there a consistent aecrease in atomic radius as the atomic number increases?
- a)halogens
- b)elements in a period
- c)transition elements
- d)lanthanides
Correct answer is option 'B'. Can you explain this answer?
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Most Upvoted Answer
In which of the following is there a consistent aecrease in atomic rad...
Consistent Decrease in Atomic Radius in Elements in a Period
Explanation:
- Atomic radius is the distance between the nucleus and the outermost electron shell of an atom.
- The atomic radius generally decreases as you move from left to right across a period in the periodic table.
- This is due to the increasing nuclear charge (number of protons) which attracts the electrons closer to the nucleus, making the atomic radius smaller.
- The electrons are in the same energy level or shell, but the effective nuclear charge increases, making the atomic radius smaller.
- The trend is not consistent throughout the periodic table, as there are some exceptions due to electron configurations and shielding effects.
Example:
- In period 3, the atomic radius decreases from sodium to chlorine.
- Sodium has the largest atomic radius in period 3 because it has only three energy levels and one electron in its outermost shell.
- Chlorine, on the other hand, has the smallest atomic radius because it has one more proton than sodium, increasing the effective nuclear charge and pulling the electrons closer to the nucleus.
Conclusion:
- The trend of decreasing atomic radius in elements in a period is due to the increasing nuclear charge and is a fundamental trend in the periodic table.
Explanation:
- Atomic radius is the distance between the nucleus and the outermost electron shell of an atom.
- The atomic radius generally decreases as you move from left to right across a period in the periodic table.
- This is due to the increasing nuclear charge (number of protons) which attracts the electrons closer to the nucleus, making the atomic radius smaller.
- The electrons are in the same energy level or shell, but the effective nuclear charge increases, making the atomic radius smaller.
- The trend is not consistent throughout the periodic table, as there are some exceptions due to electron configurations and shielding effects.
Example:
- In period 3, the atomic radius decreases from sodium to chlorine.
- Sodium has the largest atomic radius in period 3 because it has only three energy levels and one electron in its outermost shell.
- Chlorine, on the other hand, has the smallest atomic radius because it has one more proton than sodium, increasing the effective nuclear charge and pulling the electrons closer to the nucleus.
Conclusion:
- The trend of decreasing atomic radius in elements in a period is due to the increasing nuclear charge and is a fundamental trend in the periodic table.
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Community Answer
In which of the following is there a consistent aecrease in atomic rad...
As the number of electrons in a given shell increase along a period, effective nuclear charge increase.so, atomic size decrease because electrons are held by the atom more strongly.
In halogens, atomic size increase down the group.On the other hand, transition elements and lanthanides do not have consistent decrease.
so, option b is correct.
In halogens, atomic size increase down the group.On the other hand, transition elements and lanthanides do not have consistent decrease.
so, option b is correct.
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In which of the following is there a consistent aecrease in atomic radius as the atomic number increases?a)halogensb)elements in a periodc)transition elementsd)lanthanidesCorrect answer is option 'B'. Can you explain this answer?
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