In the following brown complex, the oxidation state of iron is +_____________.

${[Fe{({H_2}O)_6}]^{2 + }} + NO \to \mathop {{{[Fe{{({H_2}O)}_5}(NO)]}^{2 + }}}\limits_{\text{Brown complex}} + {H_2}O$

Amongst FeCl₃.3H₂O, K₃[Fe(CN)₆] and [Co(NH₃)₆]Cl₃, the spin-only magnetic moment value of the inner-orbital complex that absorbs light at shortest wavelength is ____________ B.M. [nearest integer]

Total number of unpaired electrons in the complex ions $[\mathrm{Co}(\mathrm{NH}_3)_6]^{3+}$ and is ________.

The spin-only magnetic moment value of the ion among $\mathrm{Ti}^{2+}, \mathrm{V}^{2+}, \mathrm{Co}^{3+}$ and , that acts as strong oxidising agent in aqueous solution is _________ BM (Near integer).

For a given chemical reaction

$\gamma$₁A + $\gamma$₂B $\to$ $\gamma$D

${[Fe{(CN)_6}]^{4 - }}$

The observed magnetic moment of the complex $\left.\left[\operatorname{Mn}(\underline{N} C S)_{6}\right)\right]^{x^{-}}$ is . The numerical value of is __________.

The ratio of spin-only magnetic moment values $\mu_{\text {eff }}\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]^{3-} / \mu_{\text {eff }}\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}$ is _________.

For a metal ion, the calculated magnetic moment is $4.90 ~\mathrm{BM}$. This metal ion has ___________ number of unpaired electrons.

If [Cu(H₂O)₄]²⁺ absorbs a light of wavelength 600 nm for d-d transition, then the value of octahedral crystal field splitting energy for [Cu(H₂O)₆]²⁺ will be ____________ $\times$ 10^$-$21 J. [Nearest Integer]

(Given : h = 6.63 $\times$ 10 ms)

For the reaction given below :

CoCl₃ . xNH₃ + AgNO₃ (aq) $\to$

If two equivalents of AgCl precipitate out, then the value of x will be _____________.

The spin-only magnetic moment value of an octahedral complex among CoCl₃.4NH₃, NiCl₂.6H₂O and PtCl₄.2HCl, which upon reaction with excess of AgNO₃ gives 2 moles of AgCl is ___________ B.M. (Nearest integer)

$\mathrm{KClO}_{3}+6 \mathrm{FeSO}_{4}+3 \mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{KCl}+3 \mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}+3 \mathrm{H}_{2} \mathrm{O}$