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Question

Which of the following ion is diamagnetic?


A

Zn+2

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B

Cr+3

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C

Fe+3

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D

Mn+2

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Solution

The correct option is A

Zn+2


Explanation for the correct option

A. Zn+2

  • The diamagnetic ions one those that do not have unpaired electrons.
  • Atomic number of zinc (Zn) = 30
  • Thus, the number of electrons in Zn+2=30-2=28e-
  • Therefore, the electronic configuration of Zn+2is - 1s22s22p63s23p63d10
  • As all the orbitals are completely filled in Zn+2, that means there is no unpaired electron present. Hence, Zn+2 is a diamagnetic ion.

Explanation for the incorrect options:

B. Cr+3

  1. Atomic number of Chromium (Cr) = 24
  2. Thus, the number of electrons in Cr+3=24-3=21e-
  3. Therefore, the electronic configuration of Cr+3is - 1s22s22p63s23p63d3
  4. As the d orbital in Cr+3 is only partially filled with 3 unpaired electrons, that means Cr+3 is a paramagnetic ion.

C. Fe+3

  1. Atomic number of Iron (Fe) = 26
  2. Thus, the number of electrons in Fe+3=26-3=23e-
  3. Therefore, the electronic configuration of Fe+3is - 1s22s22p63s23p63d5
  4. As the d orbital in Fe+3 is half with 5 unpaired electrons, that means Fe+3 is a paramagnetic ion.

D. Mn+2

  1. Atomic number of Manganese (Mn) = 25
  2. Thus, the number of electrons in Mn+2=25-2=23e-
  3. Therefore, the electronic configuration of Mn+2is - 1s22s22p63s23p63d5
  4. As the d orbital in Mn+2 is half with 5 unpaired electrons, that means Mn+2 is a paramagnetic ion.

Hence, the correct option is A, Zn+2.


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