Atomic and Physical Properties of Group 17 Elements

The correct increasing order of the magnitude of enthalpies of formation for alkali metal halides is:

The property of halogens which is not correctly matched is

In liquid ${\mathrm{CCl}}_4$, which of the following has maximum solubility

Arrange the following in the order of property indicated for each set: $\mathrm{M}-\mathrm{F}, \mathrm{M}-\mathrm{Cl}, \mathrm{M}-\mathrm{Br}, \mathrm{M}-\mathrm{I}$ - decreasing ionic character.

Arrange the following in the order of property indicated for each set: ${\mathrm{F}}_2,{\mathrm{Cl}}_2,{\mathrm{Br}}_2,{\mathrm{I}}_2$-increasing bond energy.

The colour deepens from fluorine iodine in halogen family. Explain.

Name the elements which are collectively known as halogens. Write the general electronic structures of halogen atoms.

Name the halogen with the lowest ionization energy.

Why do halogens exist as diatomic molecules ?

Electron gain enthalpies of halogens are largely negative. Give reason.

Fluoride ion has higher hydration enthalpy than chloride ion. Give reasons.

Iodine is more soluble in $\mathrm{KI}$ than in water. Why ?

${\mathrm{F}}_2$ has lower bond dissociation enthalpy than ${\mathrm{Cl}}_2$. Why?

Bond dissociation energy of ${\mathrm{F}}_2$ is less than that of ${\mathrm{Cl}}_2$. Explain.

The negative value of electron gain enthalpy is less for fluorine than for chlorine. Give reason.

Electron gain enthalpies of halogens are largely negative. Give reasons.

Which of the following orders is not in accordance with the property stated against it?

Explain the variation of melting and boiling points of group 17 elements down the group.

The highest bond enthalpy is shown by halogen

Which halogen has deep violet colour?