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NEETChemistryClassification of Elements and Periodicity in Properties

How would you explain the fact that the first ionisation enthalpy of sodium is lower than that of magnesium, but its second ionisation enthalpy is higher than that of magnesium?

Options

  1. ASodium has a larger atomic size, leading to weaker electron-nucleus attraction, resulting in a lower first ion
  2. BMagnesium has a completely filled inner electron shell, reducing its affinity to lose electrons, resulting in
  3. CThe removal of the first electron in sodium requires breaking a stable, fully filled electron shell, making it
  4. DThe removal of the second electron in sodium requires breaking a stable, fully filled electron shell, making i

Correct answer

D. The removal of the second electron in sodium requires breaking a stable, fully filled electron shell, making i

Step-by-step solution

Correct Option is : (D) The removal of the second electron in sodium requires breaking a stable, fully filled electron shell, making it energetically unfavourable and resulting in a higher ionisation enthalpy.

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