The correct option is(A): 1 and 2.
Only \(\left( NH _{4}\right)_{2} Cr _{2} O _{7}\) and \(NH _{4} NO _{2}\) give \(N _{2}\) on
heating.
(i) \(\left( NH _{4}\right)_{2} Cr _{2} O _{7} \stackrel{\Delta}{\longrightarrow} Cr _{2} O _{3}+4 H _{2} O + N _{2}\)
(ii) \({NH4NO2 ->[\text{Thermal decomposition}][{\Delta}] 2 H_2O +N2}\)
Given below are two statements.
In the light of the above statements, choose the correct answer from the options given below:
Given below are two statements:
Statement I: Nitrogen forms oxides with +1 to +5 oxidation states due to the formation of $\mathrm{p} \pi-\mathrm{p} \pi$ bond with oxygen.
Statement II: Nitrogen does not form halides with +5 oxidation state due to the absence of d-orbital in it.
In the light of the above statements, choose the correct answer from the options given below:
Given below are the pairs of group 13 elements showing their relation in terms of atomic radius. $(\mathrm{B}<\mathrm{Al}),(\mathrm{Al}<\mathrm{Ga}),(\mathrm{Ga}<\mathrm{In})$ and $(\mathrm{In}<\mathrm{Tl})$ Identify the elements present in the incorrect pair and in that pair find out the element (X) that has higher ionic radius $\left(\mathrm{M}^{3+}\right)$ than the other one. The atomic number of the element (X) is