The second ionisation enthalpies of elem...

The second ionisation enthalpies of elements are always higher than their first ionisation enthalpies because:

cation formed always have stable half-filled or completely filled valence shell electron configuration.

It is easier to remove electron process.

ionisation is an endothermic process.

the cation is smaller than its parent atom.

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The correct Answer is:

As elements are ionised, the proton to electron ratio increases, so the attraction between valence shell electron and nucles increases and as a result the size decreases. Therefore, the removal of electorns from smaller cation requires higher energy. Hence the second ionisation enthalpy is greater than its first ionisation enthalpy.

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The second ionisation enthalpy is

smaller than the first ionisation enthalpy

almost equal to the first ionisation enthalpy

smaller than the third ionisation enthalpy

equal to the second electron gain enthalpy.

The second ionisation energy is always higher than the first ionisation energy because the

ions become more stable by attaining an octet and duplet configuration

electron is more tightly bound to the nucleus in an ion

electron is attracted more by the core electrons

none of the above

The second ionisation enthalpy of an element M is the energy required to

remove one mole of electrons from one mole of gascous cations of the element

remove one mole of electrons from onc mole of gaseous anions

remove one mole of electrons from onc mole of monovalent gascous cations of the element

remove 2 moles of electrons from one mole of gaseous atoms.