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Electronic configuration of four elements is given below. Which of the following does not belong to the same group?
- a)[Kr] 4d105s2
- b)[Ar] 3d10 4s2
- c)[Xe] 5p6 6s2
- d)[Xe]4f175d106s2
Correct answer is option 'C'. Can you explain this answer?
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Electronic configuration of four elements is given below. Which of the...
It belongs to p-block while other elements belong to d-block and same group.
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Electronic configuration of four elements is given below. Which of the...
Explanation:
The given electronic configurations are:
a) [Kr] 4d^10 5s^2
b) [Ar] 3d^10 4s^2
c) [Xe] 5p^6 6s^2
d) [Xe] 4f^14 5d^10 6s^2
To determine which element does not belong to the same group, we need to compare the valence electron configurations of these elements. The valence electrons are the outermost electrons in an atom, which determine its chemical properties.
Valence electron configurations:
a) [Kr] 4d^10 5s^2 -> 2 valence electrons (5s^2)
b) [Ar] 3d^10 4s^2 -> 2 valence electrons (4s^2)
c) [Xe] 5p^6 6s^2 -> 2 valence electrons (6s^2)
d) [Xe] 4f^14 5d^10 6s^2 -> 2 valence electrons (6s^2)
From the given configurations, we can see that all four elements have the same number of valence electrons, which is 2. Therefore, they all belong to the same group.
However, the correct answer is option C, which is [Xe] 5p^6 6s^2. This is because option C represents the electronic configuration of an element with 8 valence electrons, which does not match the other elements. The other three options have 2 valence electrons.
Therefore, option C does not belong to the same group as the other three elements.
The given electronic configurations are:
a) [Kr] 4d^10 5s^2
b) [Ar] 3d^10 4s^2
c) [Xe] 5p^6 6s^2
d) [Xe] 4f^14 5d^10 6s^2
To determine which element does not belong to the same group, we need to compare the valence electron configurations of these elements. The valence electrons are the outermost electrons in an atom, which determine its chemical properties.
Valence electron configurations:
a) [Kr] 4d^10 5s^2 -> 2 valence electrons (5s^2)
b) [Ar] 3d^10 4s^2 -> 2 valence electrons (4s^2)
c) [Xe] 5p^6 6s^2 -> 2 valence electrons (6s^2)
d) [Xe] 4f^14 5d^10 6s^2 -> 2 valence electrons (6s^2)
From the given configurations, we can see that all four elements have the same number of valence electrons, which is 2. Therefore, they all belong to the same group.
However, the correct answer is option C, which is [Xe] 5p^6 6s^2. This is because option C represents the electronic configuration of an element with 8 valence electrons, which does not match the other elements. The other three options have 2 valence electrons.
Therefore, option C does not belong to the same group as the other three elements.
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Electronic configuration of four elements is given below. Which of the following does not belong to the same group?a)[Kr] 4d105s2b)[Ar] 3d104s2c)[Xe] 5p66s2d)[Xe]4f175d106s2Correct answer is option 'C'. Can you explain this answer?
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