Metals generally melt at very high temperature. Amongst the following, the metal with the highest melting point will be :

The dark purple colour of $${\mathrm{KMnO}}_4$$ disappears in the titration with oxalic acid in acidic medium. The overall change in the oxidation number of manganese in the reaction is :

Given below are two statements. Statement I : Iron (III) catalyst, acidified $${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$$ and neutral $${\mathrm{KMnO}}_4$$ have the ability to oxidise $${\mathrm{I}}^{-}$$ to $${\mathrm{I}}_2$$ independently. Statement II : Manganate ion is paramagnetic in nature and involves $$\mathrm{p}\pi -\mathrm{p}\pi$$ bonding. In the light of the above statements, choose the correct answer from the options given below.

The total number of $$\mathrm{Mn}=\mathrm{O}$$ bonds in $${\mathrm{Mn}}_2{\mathrm{O}}_7$$ is __________.

In neutral or alkaline solution, $${\mathrm{MnO}}_4^{-}$$ oxidises thiosulphate to :

Match List - I with List - II, match the gas evolved during each reaction. .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-c3ow{border-color:inherit;text-align:center;vertical-align:top} .tg .tg-7btt{border-color:inherit;font-weight:bold;text-align:center;vertical-align:top} .tg .tg-fymr{border-color:inherit;font-weight:bold;text-align:left;vertical-align:top} .tg .tg-0pky{border-color:inherit;text-align:left;vertical-align:top} List - I List - II (A) $${\left({\mathrm{NH}}_4\right)}_2{\mathrm{Cr}}_2{\mathrm{O}}_7\stackrel{\Delta }{⟶}$$ (I) $${\mathrm{H}}_2$$ (B) $${\mathrm{KMnO}}_4+\mathrm{HCl}\to$$ (II) $${\mathrm{N}}_2$$ (C) $$\mathrm{Al}+\mathrm{NaOH}+{\mathrm{H}}_2\mathrm{O}\to$$ (III) $${\mathrm{O}}_2$$ (D) $${\mathrm{NaNO}}_3\stackrel{\Delta }{⟶}$$ (IV) $${\mathrm{Cl}}_2$$ Choose the correct answer from the options given below :

Which of the following has least tendency to liberate $${\mathrm{H}}_2$$ from mineral acids?

Which of the following pair is not isoelectronic species? (At. no. Sm, 62; Er, 68; Yb, 70; Lu, 71; Eu, 63; Tb, 65; Tm, 69)

The reaction of zinc with excess of aqueous alkali, evolves hydrogen gas and gives :

In following pairs, the one in which both transition metal ions are colourless is :

In neutral or faintly alkaline medium, $${\mathrm{KMnO}}_4$$ being a powerful oxidant can oxidize, thiosulphate almost quantitatively, to sulphate. In this reaction overall change in oxidation state of manganese will be :

Which of the following $$3\mathrm{d}$$-metal ion will give the lowest enthalpy of hydration $$\left({\Delta }_{\text{hyd }}\mathrm{H}\right)$$ when dissolved in water ?

Consider the species CH4, NH$${}_4^{+}$$ and BH$${}_4^{-}$$. Choose the correct option with respect to the these species.

Number of lone pair(s) of electrons on central atom and the shape BrF3 molecule respectively, are

In the structure of SF4, the lone pair of electrons on S is in.

Identify the incorrect statement for PCl5 from the following.

The correct order of increasing intermolecular hydrogen bond strength is :

Based upon VSEPR theory, match the shape (geometry) of the molecules in List-I with the molecules in List-II and select the most appropriate option. .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-1wig{font-weight:bold;text-align:left;vertical-align:top} .tg .tg-0lax{text-align:left;vertical-align:top} List - I (Shape) List - II (Molecules) (A) T-shaped (I) XeF$${}_4$$ (B) Trigonal planar (II) SF$${}_4$$ (C) Square planar (III) ClF$${}_3$$ (D) See-saw (IV) BF$${}_3$$

Consider the ions/molecule O$${}_2^{+}$$, O2, O$${}_2^{-}$$, O$${}_2^{2-}$$ For increasing bond order the correct option is :

Bonding in which of the following diatomic molecule(s) become(s) stronger, on the basis of MO Theory, by removal of an electron? (A) NO (B) N2 (C) O2 (D) C2 (E) B2 Choose the most appropriate answer from the options given below :