Inorganic Chemistry PYQ — Page 6

$SF_4$ is isostructural with: A. $BrF_4^{\ominus}$ B. $CH_4$ C. $IF_4^{\oplus}$ D. $XeF_4$ E. $XeO_2 F_2$ Choose the correct answer from the options given below:

Correct statements from the following are: A. Nitrogen in oxidation states from $+1$ to $+4$ disproportionates in acid medium. B. Nitrogen has the ability to form $d\pi - p\pi$ multiple bonds with itself and other elements with small size and high electronegativity. C. N-N single bond is stronger than P-P single bond. D. Nitrogen has highest density in its group due to small size. E. The maximum covalency of nitrogen is four since it has only four valence orbitals for bonding. Choose the correct answer from the options given below:

The correct statements about metal carbonyls are A. The metal-carbon bonds in metal carbonyls possess both $\sigma$ and $\pi$-character. B. Due to synergic bonding interactions between metal and CO ligand, the metal-carbon bond becomes weak. C. The metal-carbon $\sigma$ bond is formed by the donation of lone pair of electrons on the carbonyl carbon into a vacant orbital of metal. D. The metal-carbon $\pi$ bond is formed by the donation of electrons from filled d-orbital of metal into vacant $\pi^*$ orbital of CO. Choose the correct answer from the options given below:

The electronegativity of a group 13 element 'E' is same as that of Ge (on Pauling scale and upto one decimal point). The CORRECT statements about $E^{3+}$ are A. It can act as a reducing agent. B. It can act as an oxidizing agent. C. $E^{3+}$ is more stable than $E^+$. D. The standard electrode potential value for $E^{3+}/E$ is positive. Choose the correct answer from the options given below:

Among $Fe^{3+}$, $Pb^{2+}$, $Cu^{2+}$ and $Mn^{2+}$, identify the one that gets precipitated out while passing $H_2S$ in presence of $NH_4OH$ as group reagent. The highest possible oxidation state of the corresponding metal is

Given below are two statements : Statement I : The number of compounds among SO$_2$, SO$_3$, SF$_4$, SF$_6$ and H$_2$S in which sulphur does not obey the Octet rule is $3$. Statement II : Among [H$_2$O, ClF$_3$, SF$_4$], [NH$_3$, BrF$_5$, SF$_4$], [BrF$_5$, ClF$_3$, XeF$_4$] and [XeF$_4$, ClF$_3$, H$_2$O], the number of sets in which all the molecules have one lone pair of electrons on the central atom is $1$. In the light of the above statements, choose the correct answer from the options given below :

Given below are two statements : Statement I: $\quad\left[\mathrm{CoBr}_{4}\right]^{2-}$ ion will absorb light of lower energy than $\left[\mathrm{CoCl}_{4}\right]^{2-}$ ion. Statement II : In $\left[\mathrm{CoI}_{4}\right]^{2-}$ ion, the energy separation between the two set of d-orbitals is more than $\left[\mathrm{CoCl}_{4}\right]^{2-}$ ion. In the light of the above statements, choose the correct answer from the options given below :

Given below are two statements : Statement I: Presence of large number of unpaired electrons in transition metal atoms results in higher enthalpies of their atomisation. Statement II: $d_{xy} = d_{xz} = d_{yz} < d_{x^2-y^2} = d_{z^2}$ and $d_{x^2-y^2} = d_{z^2} < d_{xy} = d_{xz} = d_{yz}$ are the d-orbital splittings in $[Fe(H_2O)_6]^{3+}$ and $[Ni(Cl)_4]^{2-}$ complex ions respectively. In the light of the above statements, choose the correct answer from the options given below :

Identify the correct statements from the following A. $[Fe(C_2O_4)_3]^{3-}$ is the most stable complex among $[Fe(OH)_6]^{3-}$, $[Fe(C_2O_4)_3]^{3-}$ and $[Fe(SCN)_6]^{3-}$ B. The stability of $[Cu(NH_3)_4]^{2+}$ is greater than that of $[Cu(en)_2]^{2+}$ C. The hybridization of Fe in $K_4[Fe(CN)_6]$ is $d^2sp^3$ D. $[Fe(NO_2)_3Cl_3]^{3-}$ exhibits linkage isomerism E. $NO_2^-$ and $SCN^-$ ligands are NOT ambidentate ligands Choose the correct answer from the options given below :

Consider ' $n$ ' is the number of lone pair of electrons present in the equatorial position of the most stable structure of $\mathrm{ClF}_3$. The ions from the following with ' $n$ ' number of unpaired electrons are A. $\mathrm{V}^{3+}$ B. $\mathrm{Ti}^{3+}$ C. $\mathrm{Cu}^{2+}$ D. $\mathrm{Ni}^{2+}$ E. $\mathrm{Ti}^{2+}$ Choose the correct answer from the options given below:

The incorrect statement among the following is options ${ }_1$.

From the magnetic behaviour of $\left[\mathrm{NiCl}_4\right]^{2-}$ (paramagnetic) and $\left[\mathrm{Ni}(\mathrm{CO})_4\right]$ (diamagnetic), choose the correct geometry and oxidation state.

A metal complex with a formula $\mathrm{MC} \ell_4 \cdot 3 \mathrm{NH}_3$ is involved in $\mathrm{sp}^3 \mathrm{~d}^2$ hybridisation. It upon reaction with excess of $\mathrm{AgNO}_3$ solution gives ' x ' moles of AgCl. Consider ' x ' is equal to the number of lone pairs of electron present in central atom of $\mathrm{BrF}_5$. Then the number of geometrical isomers exhibited by the complex is ______.

Given below are two statements : Statement (I) : The first ionization energy of Pb is greater than that of Sn . Statement (II) : The first ionization energy of Ge is greater than that of Si . In the light of the above statements, choose the correct answer from the options given below :

Identify the homoleptic complexes with odd number of d electrons in the central metal : (A) $\left[\mathrm{FeO}_4\right]^{2-}$ (B) $\left[\mathrm{Fe}(\mathrm{CN})_6\right]^{3-}$ (C) $\left[\mathrm{Fe}(\mathrm{CN})_5 \mathrm{NO}\right]^{2-}$ (D) $\left[\mathrm{CoCl}_4\right]^{2-}$ (E) $\left[\mathrm{Co}\left(\mathrm{H}_2 \mathrm{O}\right)_3 \mathrm{~F}_3\right]$ Choose the correct answer from the options given below :

An octahedral complex having molecular composition Co. $5 \mathrm{NH}_3. \mathrm{Cl}. \mathrm{SO}_4$ has two isomers A and B. The solution of A gives a white precipitate with $\mathrm{AgNO}_3$ solution and the solution of B gives white precipitate with $\mathrm{BaCl}_2$ solution. The type of isomerism exhibited by the complex is,

Given below are the atomic numbers of some group 14 elements. The atomic number of the element with lowest melting point is :

The group 14 elements A and B have the first ionisation enthalpy values of $708$ and $715 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively. The above values are lowest among their group members. The nature of their ions $\mathrm{A}^{2+}$ $\mathrm{B}^{4+}$ respectively is

Match List-I with List-II  Choose the correct answer from the options given below :

In the given structure, number of sp and $\mathrm{sp}^2$ hybridized carbon atoms present respectively are : 

Which of the following electronegativity order is incorrect?

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 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 :

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