JEE Main 2013 — Inorganic Chemistry

Which has trigonal bipyramidal shape ?

When a small amount of $\mathrm{KMnO}_4$ is added to concentrated $\mathrm{H}_2 \mathrm{SO}_4$, a green oily compound is obtained which is highly explosive in nature. Compound may be :

Which one of the following molecules is expected to exhibit paramagnetic behaviour?

Which is the correct order of second ionization potential of $\mathrm{C}, \mathrm{N}, \mathrm{O}$ and $\mathrm{F}$ in the following ?

In which of the following sets, all the given species are isostructural ?

Which one of the following molecules is polar?

The shape of $\mathrm{IF}_6^{-}$is :

Given ${\text{E}}_{{\text{Cr}}^{3+}/\text{Cr}}^{o}=-0.74{\text{ V; E}}_{{\text{MnO}}_{4}^{-}/{\text{Mn}}^{2+}}^{o}=1.51V$ ${\text{E}}_{{\text{Cr}}_{2}{\text{O}}_{7}^{2-}/{\text{Cr}}^{3+}}^{o}=1.33{\text{ V; E}}_{{\mathrm{Cl}}_{2}|{\mathrm{Cl}}^{-}}^{o}=1.36V$ Based on the data given above, strongest oxidising agent will be:

Oxidation state of sulphur in anions $\mathrm{SO}_3^{2-}, \mathrm{S}_2 \mathrm{O}_4^{2-}$ and $\mathrm{S}_2 \mathrm{O}_6^{2-}$ increases in the orders :

Which of the following complex species is not expected to exhibit optical isomerism?

The first ionisation potential of Na is 5.1 eV. The value of electron gain enthalpy of Na $^{+}$ will be :

The solubility order for alkali metal fluoride in water is :

Which of the following arrangements does not represent the correct order of the property stated against it?

Electron gain enthalpy with negative sign of fluorine is less than that of chlorine due to :

The structure of which of the following chloro species can be explained on the basis of $\mathrm{dsp}^2$ hybridization?

Trigonal bipyramidal geometry is shown by:

$\mathrm{XeO}_4$ molecule is tetrahedral having:

The element with which of the following outer electron configuration may exhibit the largest number of oxidation states in its compounds :

Which of the following represents the correct order of increasing first ionization enthalpy for $\mathrm{Ca},\mathrm{Ba},S,\mathrm{Se}\text{and}\mathrm{Ar}$?

In which of the following octahedral complex species the magnitude of $\Delta_0$ will be maximum?

The order of increasing sizes of atomic radii among the elements O, $\mathrm{S}$, Se and As is :

Which one of the following cannot function as an oxidising agent?

Bond distance in $\mathrm{HF}$ is $9.17 \times 10^{-11} \mathrm{~m}$. Dipole moment of $\mathrm{HF}$ is $6.104 \times 10^{-30} \mathrm{Cm}$. The percentage ionic character in $\mathrm{HF}$ will be : (electron charge $=1.60 \times 10^{-19} \mathrm{C}$ )

Type of isomerism which exists between $\left[\mathrm{Pd}\left(\mathrm{C}_6 \mathrm{H}_5\right)_2(\mathrm{SCN})_2\right]$ and $\left[\mathrm{Pd}\left(\mathrm{C}_6 \mathrm{H}_5\right)_2(\mathrm{NCS})_2\right]$ is :

Which of the following is wrong statement?

The internuclear distances in $\mathrm{O}-\mathrm{O}$ bonds for $\mathrm{O}_2^{+}, \mathrm{O}_2, \mathrm{O}_2^{-}$and $\mathrm{O}_2^{2-}$ respectively are :

Potassium dichromate when heated with concentrated sulphuric acid and a soluble chloride, gives brown-red vapours of :

Stability of the species ${\text{Li}}_{2} \text{,} {\text{Li}}_{2}^{-} \text{and} {\text{Li}}_{2}^{+}$ increases in the order of

The magnetic moment of the complex anion $\left[\mathrm{Cr}(\mathrm{NO})\left(\mathrm{NH}_3\right)(\mathrm{CN})_4\right]^{2-}$ is :

Identify incorrect statement :

Which of the following is diamagnetic ?

Identify the incorrect statement:

Bond order normally gives idea of stability of a molecular species. All the molecules viz. $\mathrm{H}_2, \mathrm{Li}_2$ and $\mathrm{B}_2$ have the same bond order yet they are not equally stable. Their stability order is :

In which of the following ionization processes the bond energy has increased and also the magnetic behaviour has changed from paramagnetic to diamagnetic ?

Which of the following statements is incorrect?

In which of the following pairs of molecules/ions, both the species are not likely to exist?

The catenation tendency of $\mathrm{C}, \mathrm{Si}$ and $\mathrm{Ge}$ is in the order $\mathrm{Ge} < \mathrm{Si} < \mathrm{C}$. The bond energies (in $\mathrm{kJ} \mathrm{~mol}^{-1}$ ) of $\mathrm{C}-\mathrm{C}, \mathrm{Si}-\mathrm{Si}$ and $\mathrm{Ge}-\mathrm{Ge}$ bonds are respectively ;