Inorganic Chemistry PYQ — Page 40

The secondary valency and the number of hydrogen bonded water molecule(s) in ${\mathrm{CuSO}}_{4}\cdot 5{H}_{2}O$, respectively, are

In the structure of the dichromate ion, there is a :

Which pair of oxides is acidic in nature?

Which one of the following statements for D.I. Mendeleeff, is incorrect ?

In which of the following order the given complex ions are arranged correctly with respect to their decreasing spin only magnetic moment? (i) ${[{\mathrm{FeF}}_{6}]}^{3-}$ (ii) ${[\mathrm{Co}{({\mathrm{NH}}_{3})}_{6}]}^{3+}$ (iii) ${[{\mathrm{NiCl}}_{4}]}^{2-}$ (iv) ${[\mathrm{Cu}{({\mathrm{NH}}_{3})}_{4}]}^{2+}$

The sum of oxidation states of two silver ions in $[\mathrm{Ag}{({\mathrm{NH}}_{3})}_{2}][\mathrm{Ag}(\mathrm{CN}{)}_{2}]$ complex is _____ .

Given below are two statement : one is labelled as Assertion A and the other is labelled as Reason R : Assertion A : Size of ${\mathrm{Bk}}^{3+}$ ion is less than ${\mathrm{Np}}^{3+}$ ion. Reason R : The above is a consequence of the lanthanide contraction. In the light of the above statements, choose the correct answer from the options given below :

Given below are two statements : Statement I: ${[\mathrm{Mn}(\mathrm{CN}{)}_{6}]}^{3-},{[\mathrm{Fe}(\mathrm{CN}{)}_{6}]}^{3-}$ and ${[\mathrm{Co}{({C}_{2}{O}_{4})}_{3}]}^{3-}$ are ${d}^{2}{\mathrm{sp}}^{3}$ hybridised. Statement II : ${[{\mathrm{MnCl}}_{6}]}^{3-}$ and ${[{\mathrm{FeF}}_{6}]}^{3-}$ are paramagnetic and have $4$ and $5$ unpaired electrons, respectively. In the light of the above statements, choose the correct answer from the options given below:

The type of hybridisation and magnetic property of the complex ${[{\mathrm{MnCl}}_{6}]}^{3-},$ respectively, are:

The atomic number of the element unnilennium is :

The number of unpaired electrons in Fe²⁺ ion is:

The oxidation states of iron atoms in compounds $(A)$, $(B)$ and $(C)$, respectively, are $x,y$ and $z$. Then sum of $x,y$ and $z$ is ........... $\underset{(A)}{{\mathrm{Na}}_{4}[\mathrm{Fe}{(\mathrm{CN})}_{5}(\mathrm{NOS})]} \underset{(B)}{{\mathrm{Na}}_{4}[{\mathrm{FeO}}_{4}]} \underset{(C)}{[{\mathrm{Fe}}_{2}{(\mathrm{CO})}_{9}]}$

The IUPAC name of the complex $[Pt{(N{H}_{3})}_{2}Cl(N{H}_{2}C{H}_{3})]Cl$ is

The ionic radii of ${O}^{2–},{F}^{–},{\mathrm{Na}}^{+}$ and ${\mathrm{Mg}}^{2+}$ are in the order:

Three elements $X,Y$ and $Z$ are in the ${3}^{\text{rd }}$period of the periodic table. The oxides of$X,Y$ and $Z$, respectively, are basic, amphoteric and acidic. The correct order of the atomic numbers of $X,Y$ and $Z$ is:

Complex A has a composition of ${H}_{12}{O}_{6}{\mathrm{Cl}}_{3}Cr$. If the complex on treatment with conc. ${H}_{2}{\mathrm{SO}}_{4}$ loses $13.5%$ of its original mass, the correct molecular formulas of $A$ is: [Given : atomic mass of $Cr=52$ amu and $CI=35$amu]

The increasing order of the atomic radii of the following elements is: $(a)C$ $(b)O$ $(c)F$ $(d)Cl$ $(e)Br$

The one that can exhibit highest paramagnetic behaviour among the following is : $\mathrm{gly}=$ glycinato; $\mathrm{bpy}=2,2$'$-$bipyridine

‘ $X$ ’ melts at low temperature and is a bad conductor of electricity in both liquid and solid state. $X$ is:

Among the statements $(a)-(d)$ , the incorrect ones are: $(a)$ Octahedral $Co(III)$ complexes with strong field ligands have very high magnetic moments $(b)$ When ${\Delta }_{0}<P$ , the d-electron configuration of $Co(III)$ in an octahedral complex is ${t}_{eg}^{4}{e}_{g}^{2}$ $(c)$ Wavelength of light absorbed by ${[Co{(en)}_{3}]}^{3+}$ is lower than that of ${[{CoF}_{6}]}^{3-}$ $(d)$ If the ${\Delta }_{0}$ for an octahedral complex of $Co(III)$ is $18,000c{m}^{-1}$, the ${\Delta }_{t}$ for its tetrahedral complex with the same ligand will be $16,000c{m}^{-1}$.

Arrange the following bonds according to their average bond energies in descending order: $C-Cl,C-Br,C-F,C-I$

Of the species, $\mathrm{NO},{\mathrm{NO}}^{+},{\mathrm{NO}}^{2+}$ and ${\mathrm{NO}}^{-},$ the one with minimum bond strength is :

The complex that can show optical activity is :

The electronic spectrum of ${[\mathrm{Ti}{({H}_{2}O)}_{6}]}^{3+}$ shows a single broad peak with a maximum at $20,300{\mathrm{cm}}^{-1}.$The crystal field stabilization energy (CFSE) of the complex ion, in ${\mathrm{kJmol}}^{-1},$ is : $(1{\mathrm{kJmol}}^{-1}=83.7{\mathrm{cm}}^{-1})$