MCQ
The complex ion which has no $ ‘d ’ $ electrons in the central metal atom is
- ✓${[Mn{O_4}]^ - }$
- B${[Co{(N{H_3})_6}]^{3 + }}$
- C${[Fe{(CN)_6}]^{3 - }}$
- D${[Cr{({H_2}O)_6}]^{3 + }}$
The electronic configuration of $Mn$ is $[ Ar ] 3 d^{5} 4 s ^{2} .$ In $MnO _{4}^{-}$, oxidation number of $Mn$ is +7 i.e. all
the $3 d$ and $4 s$ electrons are lost to form $\left[M n O_{4}\right]^{-}$ complex. Hence, it has no $d$ -electron.
The electronic configuration of $Mn ( V \|)$ is $[A r] 3 d^{0} 4 s^{0} .$
The complex ions $\left[ Co \left( NH _{3}\right)_{6}\right]^{3+},\left[ Fe ( CN )_{6}\right]^{3-}$ and $\left[ Cr \left( H _{2} O \right)_{6}\right]^{3+}$ have 6, 5 and 3 $d$ -electrons
respectively in the central metal atom.
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$CH_3COCH_{3(aq)} + Br_{2(aq)} \rightarrow $$CH_3COCH_2Br_{(aq)} + H^+_{(aq)}+ Br^-_{(aq)}$
These kinetic data were obtained for given reaction concentrations.
Initial concentrations, $M$
| $[CH_3COCH_3]$ | $[Br_2]$ | $[H^+]$ |
| $0.30$ | $0.05$ | $0.05$ |
| $0.30$ | $0.10$ | $0.05$ |
| $0.30$ | $0.10$ | $0.10$ |
| $0.40$ | $0.05$ | $0.20$ |
Initial rate, disappearance of $Br_2, \,\,Ms^{-1}$
$5.7 \times 10^{-5} ,$ $5.7 \times 10^{-5} ,$ $1.2 \times 10^{-5} ,$ $3.1 \times 10^{-5}$
Based on these data, the rate equation is