P-block elements practice · Medium

Assertion (A): Chlorine has higher electron affinity than fluorine.

Reason (R): Chlorine is a weak oxidising agent than fluorine.

Statement I: Iodine is more soluble in $\mathrm{CCl}_4$ than in water

Statement II: Non-polar solutes are more soluble in non-polar solvents

Find the incorrect statement

In $3^{\text {rd }}$ group cationic analysis, ${NH}_4 {Cl}$ is added before adding ${NH}_4 {OH}$. This is due to

The correct order of acidic nature is:

Bleaching action of $S{O_2}$ is due to

Assertion (A) : $\mathrm{N}_3 \mathrm{H}$ is a weak acid and $\mathrm{NH}_3$ is a weak base.

Reason (R) : There is proton-donor acceptor equilibrium

$\mathrm{N}_3 \mathrm{H}+\mathrm{NH}_3 \rightleftharpoons \mathrm{N}_3^{-}+\mathrm{NH}_4^{+}$

Assertion (A): ${H}_2 {S}$ is less acidic than ${H}_2 {Te}$

Reason (R): ${S}-{H}$ bond is stronger than ${Te}-{H}$ bond

Which of the following is least likely to exist?

Hot concentrated sulphuric acid is a moderately strong oxidizing agent. Which of the following reactions does not show oxidizing behavior?

Assertion (A): $\mathrm{XeF}_6$ cannot be handled in glass or quartz apparatus.

Reason (R): Reaction between $\mathrm{XeF}_6$ and $\mathrm{SiO}_2$ of glass form explosive $\mathrm{XeO}_3$.

$BrF_3$ and $IF_5$ both exist in ionic form, in solid state. What are the hybridizations of cationic parts of
both, respectively?

The $\mathrm{H-N-H}$ angle in ammonia is $107.6^{\circ}$, while the $\mathrm{H}-\mathrm{P}-\mathrm{H}$ angle in phosphine is $93.5^{\circ}$. Relative to phosphine, the $\mathrm{p}$-character of the lone pair on ammonia is expected to be

S-I: No. of lone pairs in ${XeOF}_4$ is 15.

S-II: ${XeF}_2$ is hydrolysed gives ${Xe}, {HF}$ and ${O}_2$.

Assertion (A): The halogens absorb visible light.

Reason (R): All halogens are coloured.

Oxidation states of nitrogen in ${N}_2 {O}_3, {HN}_3$ and ${HCN}$ respectively are

The type of bonds present in $\mathrm{N}_2 \mathrm{O}_5(\mathrm{~g})$ are;

Which of the following property does not correspond to the order ${HI} < {HBr} < {HCl} < {HF}$ ?

Assertion (A): While moving from $\mathrm{N}$ to $\mathrm{P}$ covalent radius increases significantly but from $\mathrm{As}$ to $\mathrm{Bi}$ only a small increase is observed.
Reason (R): For a particular oxidation state covalent radii and ionic generally radii increases down the group.

Which one of the following reacts with conc. ${H}_2 {SO}_4$ ?

Assertion (A): $\mathrm{H}_3 \mathrm{PO}_4$ is less acidic than $\mathrm{H}_3 \mathrm{PO}_3.$

Reason (R): Oxidation state of phosphorus in $\mathrm{H}_3 \mathrm{PO}_4< \mathrm{H}_3 \mathrm{PO}_3.$

$C{l_2}$ on reaction with cold and dilute NaOH gives

A compound which leaves behind no residue on heating is:

Choose the correct statements from the following

A. All group 16 elements form oxides of general formula $\mathrm{EO}_2$ an $\mathrm{EO}_3$, where $\mathrm{E}=\mathrm{S}, \mathrm{Se}, \mathrm{Te}$ and Po. Both the types of oxides are acidic in nature.

B. $\mathrm{TeO}_2$ is an oxidising agent while $\mathrm{SO}_2$ is reducing in nature.

C. The reducing property decreases from $\mathrm{H}_2 \mathrm{~S}$ to $\mathrm{H}_2 \mathrm{Te}$ down the group.

D. The ozone molecule contains five lone pairs of electrons.

Choose the correct answer from the options given below:

I. Melting point of rhombic sulphur is higher than that of monoclinic sulphur.

II. Specific gravity of rhombic sulphur is lower than that of rhombic sulphur.

III. Sulphurous acid $\left(\mathrm{H}_2 \mathrm{SO}_3\right)$ has two one pairs on S-atom. The incorrect statement(s) is/are

Platinum, palladium and iridium are called noble metals because

The halogen which has greater bond dissociation energy after ${Cl}_2$ is

When potassium ferrocyanide crystals are heated with conc. $\mathrm{H}_2 \mathrm{SO}_4$, the gas evolved is

Among $\mathrm{HClO}_2,$ $\mathrm{HClO}_3,$ $\mathrm{HClO}$ and $\mathrm{HClO}_4$ which is most acidic in nature:

Which of the following is more acidic in nature?