Which of the following statements is incorrect for ionic compounds?

Soluble in a polar solvent

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Low melting and boiling points

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Commonly present in lattice structures

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Insulators in solid form but good conductors in dissolved or molten form

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Solution

The correct option is B Low melting and boiling points
In ionic compounds, the force of attraction between the opposite charges i.e. between the anions and cations is quite strong. Therefore, if we want to separate these ions by heating them, it requires a lot of heat to distort the lattice which results in higher melting and boiling points for the ionic compounds. Hence, statement (b) is wrong.

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Similar questions

Q. Give the reasons for following
(i) Ionic compounds are bad conductors in the solid state but conduct electricity in solution form and in the molten state
(ii) Ionic solids are soluble in polar solvents but not in non-polar solvents

Question 10
Which one of the following properties is not generally exhibited by ionic compounds?
(a) Solubility in water
(b) Electrical conductivity in solid state
(c) High melting and boiling points
(d) Electrical conductivity in molten state

Question 10
Which one of the following properties is not generally exhibited by ionic compounds?
(a) Solubility in water.
(b) Electrical conductivity in solid state.
(c) High melting and boiling points.
(d) Electrical conductivity in molten state.

Explain the following:
(a) Covalent compounds are generally gases or liquids or soft solids.
(b) Covalent compounds have low melting point and boiling point.
(c) Non-polar covalent compounds are insoluble in water.
(d) Polar covalent compounds are good conductors of electricity.

why ionic compounds are bad conductors of electricity and good conductor in molten or aqueous

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