The electronic configuration 1s2 2s2 2p6 3s1 3p3 3d2 represents which state?
A) ground state
B)1st excited state
C)2nd excited state
D)3rd excited state
Answers
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answer is C) 2nd excited state.
since total no. of electrons here are 16 and original configuration(ground state) should be 1s2 2s2 2p6 3s2 3p4 3d0. So 1 electron each from 3s and 3p go into 3d in 2nd excited state.
since total no. of electrons here are 16 and original configuration(ground state) should be 1s2 2s2 2p6 3s2 3p4 3d0. So 1 electron each from 3s and 3p go into 3d in 2nd excited state.
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Answer:
The correct answer to this question is 2nd excited state.
Explanation:
Given - The electronic configuration 1s2 2s2 2p6 3s1 3p3 3d2
To Find - Choose the correct option.
An element's electronic configuration is a symbolic representation of how its atoms' electrons are arranged across distinct atomic orbitals.
Because there are 16 total electrons in this arrangement, the original configuration (ground state) should be 1s2 2s2 2p6 3s2 3p4 3d0. As a result, one electron from each of the 3s and 3p excited states enters the 2nd excited state of 3d.
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