Question

Which of the following is not the characteristics of ionic solid?
A.A very low value of electrical conductivity in a molten state
B.Brittle nature
C.Very strong forces of attraction
D.Anisotropic nature

Answer 1

To answer this question, you should recall the concept of ionic solids. Ionic solids refer to solids made up with ionic bonds. These ionic bonds result from the composition of oppositely charged ions

Complete Step by step solution:
This formation of bonds where there is the transference of electrons is known as ionic bonding. More charge disparity more the strength between the two atoms, i.e. the greater the charge disparity between the cation and the anion, the stronger the ionic bond. These solids tend to have high melting points. The electrons of their constituent charged ions are localized, this results in stiff and brittle like properties similar to covalent solids.
In solid states, they do not conduct electricity as conductance requires free electrons. However, in the liquid states, they conduct electricity due to the movement of ions. Examples of ionic solids include $NaCl{\text{ and }}Ca(C{O_3}).{\text{ }}\;$ Therefore to answer this question in the molten state, the ionic solids have free ions in them. Ions help in the conduction of electricity. Due to these free ions, the electrical conductivity of ionic compounds in the molten state is very high.
So, option A is not correct regarding the characteristics of ionic compounds.

Hence, we can conclude that the correct answer to this question is option A.

Note: The ideal conditions for the formation of an ionic bond are: low ionization energy of the atom forming the cation, High electron gain enthalpy of the atom forming the anion, High negative lattice enthalpy of the crystal formed. Generally, the ionic bond is formed between a metal cation and non-metal anion.