Q3 / 160 · AP EAMCET 2020 (22 Sep Shift 2) · Chemistry

Which of the following statement is incorrect? (i) $\mathrm{NaCl}$ being an ionic compound is a good conductor of electricity in the solid state. (ii) In canonical structures there is no difference in the arrangement of atoms. (iii) Hybrid orbitals form stronger bonds than pure orbitals. (iv) VSEPR theory can explain the square planar geometry of $\mathrm{XeF}_4$.

  • Correct answer
    A
    (i)
  • B
    (ii)
  • C
    (iii)
  • D
    (iv)

Solution

When sodium chloride is in solid state, it doesn't have free electrons due to the ionic/electrovalent bond between sodium and chorine but when $\mathrm{NaCl}$ dissolves in water, the bond is broken and sodium and chlorine separate forming ions like $\mathrm{Na}^{+}$and $\mathrm{Cl}^{-}$. Therefore, having free ions, it is able to conduct electricity. So, the option (1) is incorrect.

Hence, the correct answer is option: 'A'.

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