Write the configuration of `Cr^(3+), Cu^(+), Co^(2+), Mn^(2+)`

The d-electron configurations of Cr^(2+), Mn^(2+), Fe^(2+) and Co^(2+) are d^4, d^5, d^6 and d^7 respectively. Which one of the following will exhibit minimum paramagnetic behaviour?

Which of the following pairs of ions have the same electronic configuration A) Cr^(+3),Fe^(+3) B) Fe^(+3),Mn^(+2) C) Fe^(+3),Co^(+3) D) Sc^(+3),Cr^(+3)

Which of the following pairs of ions have the same electronic configuration A) Cr^(+3),Fe^(+3) B) Fe^(+3),Mn^(+2) C) Fe^(+3),Co^(+3) D) Sc^(+3),Cr^(+3)

Write down the electronic configuration of: Co ^(2+)

Write down the electronic configuration of: (i). Cr^(3+) (ii). Prn^(3+) (iii). Cu^(o+) (iv). Ce^(4+) (v). Co^(2+) (iv). Lu^(2+) (vii). Mn^(2+) (viii). Th^(4+)

The electronic configuration of Co^(2+) and Cu^(2+) is d^7 and d^(9) respectively. Which of these ions will be more paramagnetic ?

Write the electronic configuration of (i) Mn4+, (ii) Fe3+ (iii) Cr2+ Mention the number of unpaired electrons in each case.

Write down the number of 3d electrons in each of the following ions : Ti^(2+), V^(2+), Cr^(3+), Mn^(2+), Fe^(2+), Co^(2+), Ni^(2+) and Cu^(2+) . Indicate how would you expect the five 3d orbitals to be occupied for these hydrated ions (octahedral).

Out of the following ions Ti^(3+), V^(3+), Cu^(+), Sc^(3+), Mn^(3+) and Co^(2+) the colourless ions will be

The electronic configuration of Mn^(2+) is: