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Question

In which of the following arrangements the order is NOT according to the property indicated against it?
  1. Al3+<Mg2+<Na+<F - increasing ionic size
  2. B<C<N<O<P - increasing first ionization enthalpy
  3. I<Br<F<Cl - increasing electron gain enthalpy (with negative sign) 
  4. Li<Na<K<Rb - increasing metallic radius


Solution

The correct option is B B<C<N<O<P - increasing first ionization enthalpy
Nitrogen has half filled stable configuration, ns2np3 so, ionization enthalpy of nitrogen is greater than oxygen. Across the period with increasing effective nuclear charge and decreasing atomic size, the ionization energies increase  but down the group, decreases due to increasing atomic radii. So, the correct increasing order of the first ionization enthalpy is B<P<C<O<N.
(Ionisation energy in kJ mol1 B=801;P=1011;C=1086;O=1314;N=1402).
(A)  size of ionmagnitude of - ve chargemagnitude of +ve change
(for isoelectronic speies more the +ve charge, smaller will be the size a nd vice - versa)
(D) Down the group number of shells atomic radius 
(C) From 2nd period to 3rd period, e affinity increased due to less electron electron repulsion on Cl as compared to F and further on going down the group, e affinity decreases.

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