Inorganic Chemistry PYQ — Page 7

The correct order of the following complexes in terms of their crystal field stabilization energies is :

Identify the inorganic sulphides that are yellow in colour : (A) $\left(\mathrm{NH}_4\right)_2 \mathrm{~S}$ (B) $\mathrm{Pbs}$ (C) $\mathrm{Cus}$ (D) $\mathrm{As}_2 \mathrm{~S}_3$ (E) $\mathrm{As}_2 \mathrm{~S}_5$ Choose the correct answer from the options given below :

The spin-only magnetic moment value of $\mathrm{M}^{\mathrm{n+-}}$ ion formed among $\mathrm{Ni}, \mathrm{Zn} \mathrm{Mn}$ and Cu that has the least enthalpy of atomisation is ________. (in nearest integer) Here n is equal to the number of diamagnetic complexes among $\mathrm{K}_2\left[\mathrm{NiCl}_4\right],\left[\mathrm{Zn}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right] \mathrm{Cl}_2$, $\mathrm{K}_3\left[\mathrm{Mn}(\mathrm{CN})_6\right] \text { and }\left[\mathrm{Cu}\left(\mathrm{PPh}_3\right)_3 \mathrm{I}\right]$

The correct statements from the following are : (A) $\mathrm{Tl}^{3+}$ is a powerful oxidising agent (B) $\mathrm{Al}^{3+}$ does not get reduced easily (C) Both $\mathrm{Al}^{3+}$ and $\mathrm{Tl}^{3+}$ are very stable in solution (D) $\mathrm{Tl}^{+}$is more stable than $\mathrm{Tl}^{3+}$ (E) $\mathrm{Al}^{3+}$ and $\mathrm{Tl}^{+}$are highly stable Choose the correct answer from the options given below :

The incorrect relationship in the following pairs in relation to ionisation enthalpies is :

The elements of Group 13 with highest and lowest first ionisation enthalpies are respectively:

Which of the following statements are correct? A. The process of the addition an electron to a neutral gaseous atom is always exothermic B. The process of removing an electron from an isolated gaseous atom is always endothermic C. The $1^{\text {st }}$ ionization energy of the boron is less than that of the beryllium D. The electronegativity of C is 2.5 in $\mathrm{CH}_4$ and $\mathrm{CCl}_4$ E. Li is the most electropositive among elements of group I Choose the correct answer from the options gives below

The type of oxide formed by the element among $\mathrm{Li}, \mathrm{Na}, \mathrm{Be}, \mathrm{Mg}, \mathrm{B}$ and Al that has the least atomic radius is :

The incorrect decreasing order of atomic radii is

Match List-I with List-II. $\begin{array}{llll} & \text{List-I} & & \text{List-II} \\(A) & \mathrm{Al}^{3+} < \mathrm{Mg}^{2+} < \mathrm{Na}^{+} < \mathrm{F}^{-} & (I) & \text{Ionisation Enthalpy} \\(B) & \mathrm{B} < \mathrm{C} < \mathrm{O} < \mathrm{N} & (II) & \text{Metallic character} \\(C) & \mathrm{B} < \mathrm{Al} < \mathrm{Mg} < \mathrm{K} & (III) & \text{Electronegativity} \\(D) & \mathrm{Si} < \mathrm{P} < \mathrm{S} < \mathrm{Cl} & (IV) & \text{Ionic radii}\end{array}$ Choose the correct answer from the options given below :

Which of the following molecules(s) show/s paramagnetic behavior? (A) $\mathrm{O}_2$ (B) $\mathrm{N}_2$ (C) $\mathrm{F}_2$ (D) $\mathrm{S}_2$ (E) $\mathrm{Cl}_2$ Choose the correct answer from the options given below :

Given below are two statements : Statement (I): Experimentally determined oxygen-oxygen bond lengths in the $\mathrm{O}_3$ are found to be same and the bond length is greater than that of a $\mathrm{O}=\mathrm{O}$ (double bond) but less than that of a single $(O-O)$ bond. Statement (II) : The strong lone pair-lone pair repulsion between oxygen atoms is solely responsible for the fact that the bond length in ozone is smaller than that of a double bond $(\mathrm{O}=\mathrm{O})$ but more than that of a single bond $(\mathrm{O}-\mathrm{O})$. In the light of the above statements, choose the correct answer from the options given below :

Which of the following statement is true with respect to $\mathrm{H}_2 \mathrm{O}, \mathrm{NH}_3$ and $\mathrm{CH}_4$ ? A. The central atoms of all the molecules are $\mathrm{sp}^3$ hybridized. B. The $\mathrm{H}-\mathrm{O}-\mathrm{H}, \mathrm{H}-\mathrm{N}-\mathrm{H}$ and $\mathrm{H}-\mathrm{C}-\mathrm{H}$ angles in the above molecules are $104.5^{\circ}, 107.5^{\circ}$ and $109.5^{\circ}$, respectively. C. The increasing order of dipole moment is $\mathrm{CH}_4 \lt \mathrm{NH}_3 \lt \mathrm{H}_2 \mathrm{O}$. D. Both $\mathrm{H}_2 \mathrm{O}$ and $\mathrm{NH}_3$ are Lewis acids and $\mathrm{CH}_4$ is a Lewis base. E. A solution of $\mathrm{NH}_3$ in $\mathrm{H}_2 \mathrm{O}$ is basic. In this solution $\mathrm{NH}_3$ and $\mathrm{H}_2 \mathrm{O}$ act as Lowry-Bronsted acid and base respectively. Choose the correct answer from the options given below:

The number of molecules/ions that show linear geometry among the following is ________ $\mathrm{SO}_2, \mathrm{BeCl}_2, \mathrm{CO}_2, \mathrm{~N}_3^{-}, \mathrm{NO}_2, \mathrm{~F}_2 \mathrm{O}, \mathrm{XeF}_2, \mathrm{NO}_2^{+}, \mathrm{I}_3^{-}, \mathrm{O}_3$

The metal ions that have the calculated spin only magnetic moment value of 4.9 B.M. are A. $\mathrm{Cr}^{2+}$ B. $\mathrm{Fe}^{2+}$ C. $\mathrm{Fe}^{3+}$ D. $\mathrm{Co}^{2+}$ E. $\mathrm{Mn}^{3+}$ Choose the correct answer from the options given below

Given below are two statements : Statement I: $\mathrm{H}_2 \mathrm{Se}$ is more acidic than $\mathrm{H}_2 \mathrm{Te}$. Statement II : $\mathrm{H}_2 \mathrm{Se}$ has higher bond enthalpy for dissociation than $\mathrm{H}_2 \mathrm{Te}$. In the light of the above statements, choose the correct answer from the options given below.

Identify the diamagnetic octahedral complex ions from below ; A. $\left[\mathrm{Mn}(\mathrm{CN})_6\right]^{3-}$ B. $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+}$ C. $\left[\mathrm{Fe}(\mathrm{CN})_6\right]^{4-}$ D. $\left[\mathrm{Co}\left(\mathrm{H}_2 \mathrm{O}\right)_3 \mathrm{~F}_3\right]$ Choose the correct answer from the options given below :

The amphoteric oxide among $\mathrm{V}_2 \mathrm{O}_3, \mathrm{~V}_2 \mathrm{O}_4$ and $\mathrm{V}_2 \mathrm{O}_5$, upon reaction with alkali leads to formation of an oxide anion. The oxidation state of V in the oxide anion is :

Total number of molecules/species from following which will be paramagnetic is ______ $\mathrm{O}_2, \mathrm{O}_2^{+}, \mathrm{O}_2^{-}, \mathrm{NO}, \mathrm{NO}_2, \mathrm{CO}, \mathrm{K}_2\left[\mathrm{NiCl}_4\right],\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right] \mathrm{Cl}_3, \mathrm{~K}_2\left[\mathrm{Ni}(\mathrm{CN})_4\right]$

An element ' \(E^{\prime}\) has the ionisation enthalpy value of \(374 \mathrm{~kJ} \mathrm{~mol}^{-1}\). ' \(E\) ' reacts with elements \(\mathrm{A}, \mathrm{B}, \mathrm{C}\) and D with electron gain enthalpy values of \(-328,-349,-325\) and \(-295 \mathrm{~kJ} \mathrm{~mol}^{-1}\), respectively. The correct order of the products EA, EB, EC and ED in terms of ionic character is :

Match the LIST-I with LIST-II. $\begin{array}{|l|l|l|l|}\hline & \begin{array}{c} \text{LIST-I} \\ \text{(Family)} \end{array} & & \begin{array}{c} \text{LIST-II} \\ \text{(Symbol of Element)} \end{array} \\ \hline \text{A.} & \begin{array}{l} \text{Pnicogen} \\ \text{(group 15)} \end{array} & \text{I.} & \text{Ts} \\ \hline \text{B.} & \text{Chalcogen} & \text{II.} & \text{Og} \\ \hline \text{C.} & \text{Halogen} & \text{III.} & \text{Lv} \\ \hline \text{D.} & \text{Noble gas} & \text{IV.} & \text{Mc} \\ \hline\end{array}$ Choose the correct answer from the options given below :

The number of paramagnetic metal complex species among $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+}, \quad\left[\mathrm{Co}\left(\mathrm{C}_2 \mathrm{O}_4\right)_3\right]^{3-}$, $\left[\mathrm{MnCl}_6\right]^{3-},\left[\mathrm{Mn}(\mathrm{CN})_6\right]^{3-},\left[\mathrm{CoF}_6\right]^{3-},\left[\mathrm{Fe}(\mathrm{CN})_6\right]^{3^{3-}}$ and $\left[\mathrm{FeF}_6\right]^{3-}$ with same number of unpaired electrons is ________.

Preparation of potassium permanganate from $\mathrm{MnO}_2$ involves two step process in which the 1st step is a reaction with KOH and $\mathrm{KNO}_3$ to produce

Identify $\mathrm{A}, \mathrm{B}$ and C in the given below reaction sequence $\mathrm{A} \xrightarrow{\mathrm{HNO}_3} \mathrm{~Pb}\left(\mathrm{NO}_3\right)_2 \xrightarrow{\mathrm{H}_2 \mathrm{SO}_4}$ B $\xrightarrow[\substack{\text { (2) Acetic acid } \\ \text { (3) } \mathrm{K}_2 \mathrm{CrO}_4}]{\substack{\text { (1) Ammonium } \\ \text { acetate }}}$