MCQ
The oxidation number of $Pt$ in ${[Pt({C_2}{H_4})C{l_3}]^ - }$ is
- A$+1$
- ✓$ +2$
- C$ +3$
- D$ +4$
✓
Answer
Correct option: B.
$ +2$
b
(b) $[\mathop {Pt}\limits_x \mathop {({C_2}}\limits_0 {H_4})\mathop {C{l_3}}\limits_{ - 1} {]^ - }$
$x + 0 + 3x( - 1) = - 1$, $x - 3 = - 1,$ $x = + 2.$
(b) $[\mathop {Pt}\limits_x \mathop {({C_2}}\limits_0 {H_4})\mathop {C{l_3}}\limits_{ - 1} {]^ - }$
$x + 0 + 3x( - 1) = - 1$, $x - 3 = - 1,$ $x = + 2.$
Need a full question paper?
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
Explore more
Similar questions
The structural formula of hypophosphorus acid is
Chlorine was discovered by
The variation of equilibrium constant with temperature is given below
→Temperature $\quad$ Equilibrium constant
$\begin{array}{ll} T _{1}=25^{\circ} C & K _{1}=100 \\ T _{2}=100^{\circ} C & K _{2}=100\end{array}$
The values of $\Delta H ^{\circ}, \Delta G ^{\circ}$ at $T _{1}$ and $\Delta G ^{\circ}$ at $T _{2}$ (in $kJ\, mol ^{-1}$ ) respectively, are close to $\left[\right.$ Use $\left. R =8.314\, JK ^{-1} mol ^{-1}\right]$
First ionization energy is the lowest with
Amongst the following, identify the species with an atom in $+6$ oxidation state
→Solubility product constant ( $\mathrm{K}_{\mathrm{sp}}$ ) of salts of types $\mathrm{MX}, \mathrm{MX}_2$ and $\mathrm{M}_3 \mathrm{X}$ at temperature ' $\mathrm{T}$ ' are $4.0 \times 10^{-8}, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$, respectively. Solubilities (mole dm ${ }^{-3}$ ) of the salts at temperature ' $\mathrm{T}$ ' are in the order
→Reason of lanthanoid contraction is
Equilibrium constant $(K_c)$ of $2HI_{(g)} \rightleftharpoons H_{2(g)} + I_{2(g)}$ is $5\times10^3$. What is the equilibrium concentration of $HI$, if equilibrium concentrations of $H_{2(g)}$ and $I_{2(g)}$ respectively are $2.2\times10^{-2}\, M$ and $2.2\times10^{-4}\, M$ ?
→The correct order for $E_2$ reaction with alc. $KOH$ will be
→Match List $I$ with List $II$
→| List-$I$ (Compound) | List-$II$ (Colour) |
| $A$ $\mathrm{Fe}_4\left[\mathrm{Fe}(\mathrm{CN})_6\right]_3 \cdot \mathrm{xH}_2 \mathrm{O}$ | $I$ Violet |
| $B$ $\left[\mathrm{Fe}(\mathrm{CN})_5 \mathrm{NOS}\right]^{4-}$ | $II$ Blood Red |
| $C$ $[\mathrm{Fe}(\mathrm{SCN})]^{2+}$ | $III$ Prussian Blue |
| $D$ $\left(\mathrm{NH}_4\right)_3 \mathrm{PO}_4 \cdot 12 \mathrm{MoO}_3$ | $IV$ Yellow |
Choose the correct answer from the options given below :