Inorganic Chemistry PYQ — Page 12

The number of species from the following that have pyramidal geometry around the central atom is _______. \(\mathrm{S}_2 \mathrm{O}_3^{2-}, \mathrm{SO}_4^{2-}, \mathrm{SO}_3^{2-}, \mathrm{S}_2 \mathrm{O}_7^{2-}\)

Arrange the following elements in the increasing order of number of unpaired electrons in it. (A) \(\mathrm{Sc}\) (B) \(\mathrm{Cr}\) (C) \(\mathrm{V}\) (D) \(\mathrm{Ti}\) (E) Mn Choose the correct answer from the options given below :

Number of Complexes with even number of electrons in \(t_{2 g}\) orbitals is - \(\left[\mathrm{Fe}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+},\left[\mathrm{Co}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+},\left[\mathrm{Co}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{3+},\left[\mathrm{Cu}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+},\left[\mathrm{Cr}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+}\)

Match List I with List II \(\begin{array}{llll} \text{List - I} & \text{List - II} \\ \text{(A) } \mathrm{ICl} & \text{(I) T - shape} \\ \text{(B) } \mathrm{ICl}_3 & \text{(II) pyramidal} \\ \text{(C) } \mathrm{ClF}_5 & \text{(III) Pentagonal bipyramidal} \\ \text{(D) } \mathrm{IF}_7 & \text{(IV) Linear} \\ \end{array}\) Choose the correct answer from the options given below :

Number of colourless lanthanoid ions among the following is ________ \(\mathrm{Eu}^{3+}, \mathrm{Lu}^{3+}, \mathrm{Nd}^{3+}, \mathrm{La}^{3+}, \mathrm{Sm}^{3+}\)

If an iron (III) complex with the formula \(\left[\mathrm{Fe}\left(\mathrm{NH}_3\right)_x(\mathrm{CN})_y\right]^{-}\)has no electron in its \(e_g\) orbital, then the value of \(x+y\) is

The correct sequence of electron gain enthalpy of the elements listed below is A. Ar B. Br C. F D. S Choose the most appropriate from the options given below:

In which one of the following pairs the central atoms exhibit \(\mathrm{sp}^2\) hybridization ?

Match List I with List II \(\begin{array}{|l|l|l|l|} \hline & \text{List - I} & & \text{List - II} \\ & \text{(Molecule/Species)} & & \text{(Property/Shape)} \\ \hline \text { A. } & \mathrm{SO}_2 \mathrm{Cl}_2 & \text { I. } & \text { Paramagnetic } \\ \hline \text { B. } & \mathrm{NO} & \text { II. } & \text { Diamagnetic } \\ \hline \text { C. } & \mathrm{NO}_2^{-} & \text {III. } & \text { Tetrahedral } \\ \hline \text { D. } & \mathrm{I}_3^{-} & \text {IV. } & \text { Linear } \\ \hline \end{array}\) Choose the correct answer from the options given below:

Given below are two statements : Statement I : The correct order of first ionization enthalpy values of \(\mathrm{Li}, \mathrm{Na}, \mathrm{F}\) and \(\mathrm{Cl}\) is \(\mathrm{Na} < \mathrm{Li} < \mathrm{Cl} < \mathrm{F}\). Statement II : The correct order of negative electron gain enthalpy values of \(\mathrm{Li}\), \(\mathrm{Na}, \mathrm{F}\) and \(\mathrm{Cl}\) is \(\mathrm{Na} < \mathrm{Li} < \mathrm{F} < \mathrm{Cl}\) In the light of the above statements, choose the correct answer from the options given below :

Given below are two statements: One is labelled as Assertion A and the other is labelled as Reason R. Assertion A : ${H}_{2}\mathrm{Te}$ is more acidic than ${H}_{2}S$. Reason R: Bond dissociation enthalpy of ${H}_{2}\mathrm{Te}$ is lower than ${H}_{2}S$. In the light of the above statements. Choose the most appropriate from the options given below.

The number of non-polar molecules from the following is $\mathrm{HF},{H}_{2}O,{\mathrm{SO}}_{2},{H}_{2},{\mathrm{CO}}_{2},{\mathrm{CH}}_{4},{\mathrm{NH}}_{3},\mathrm{HCl},{\mathrm{CHCl}}_{3},{\mathrm{BF}}_{3}$

Choose the correct option having all the elements with ${d}^{10}$ electronic configuration from the following:

Number of compounds / species from the following with non-zero dipole moment is ______ \(\mathrm{BeCl}_2, \mathrm{BCl}_3, \mathrm{NF}_3, \mathrm{XeF}_4, \mathrm{CCl}_4, \mathrm{H}_2 \mathrm{O}, \mathrm{H}_2 \mathrm{~S}, \mathrm{HBr}, \mathrm{CO}_2, \mathrm{H}_2, \mathrm{HCl}\)

Number of molecules having bond order 2 from the following molecules is ________ \(\mathrm{C}_2, \mathrm{O}_2, \mathrm{Be}_2, \mathrm{Li}_2, \mathrm{Ne}_2, \mathrm{~N}_2, \mathrm{He}_2\)

The total number of species from the following in which one unpaired electron is present, is _______ \(\mathrm{N}_2, \mathrm{O}_2, \mathrm{C}_2^{-}, \mathrm{O}_2^{-}, \mathrm{O}_2^{2-}, \mathrm{H}_2^{+}, \mathrm{CN}^{-}, \mathrm{He}_2^{+}\)

$\mathrm{NaCl}$ reacts with conc. ${H}_{2}{\mathrm{SO}}_{4}$ and ${K}_{2}{\mathrm{Cr}}_{2}{O}_{7}$ to give reddish fumes (B), which react with $\mathrm{NaOH}$ to give yellow solution (C). (B) and (C) respectively are ;

Yellow compound of lead chromate gets dissolved on treatment with hot $\mathrm{NaOH}$ solution. The product of lead formed is a :

The Spin only magnetic moment value of square planar complex $[\mathrm{Pt}{({\mathrm{NH}}_{3})}_{2}\mathrm{Cl}({\mathrm{NH}}_{2}{\mathrm{CH}}_{3})]\mathrm{Cl}$ is _______ B.M. (Nearest integer) ( Given atomic number for $\mathrm{Pt}=78)$

In alkaline medium. ${\mathrm{MnO}}_{4}^{-}$ oxidises ${I}^{-}$ to

Iron (III) catalyses the reaction between iodide and persulphate ions, in which A. \(\mathrm{Fe}^{3+}\) oxidises the iodide ion B. \(\mathrm{Fe}^{3+}\) oxidises the persulphate ion C. \(\mathrm{Fe}^{2+}\) reduces the iodide ion D. \(\mathrm{Fe}^{2+}\) reduces the persulphate ion Choose the most appropriate answer from the options given below:

The number of element from the following that do not belong to lanthanoids is \(\mathrm{Eu}, \mathrm{Cm}, \mathrm{Er}, \mathrm{Tb}, \mathrm{Yb}\) and \(\mathrm{Lu}\)

The correct IUPAC name of ${K}_{2}{\mathrm{MnO}}_{4}$ is:

Identify the incorrect statements about group 15 elements : (A) Dinitrogen is a diatomic gas which acts like an inert gas at room temperature. (B) The common oxidation states of these elements are \(-3,+3\) and +5 . (C) Nitrogen has unique ability to form \(\mathrm{p} \pi-\mathrm{p} \pi\) multiple bonds. (D) The stability of +5 oxidation states increases down the group. (E) Nitrogen shows a maximum covalency of 6. Choose the correct answer from the options given below :