Which one of the following statements is incorrect in relation to ionisation enthalpy?
- AIonization enthalpy increases for each successive electron.
- BThe greatest increase in ionization enthalpy is experienced on removal of electron from core of noble gas configuration.
- CDetermination of valence electrons is marked by a large jump in ionization enthalpy.
- DRemoval of electron from orbitals bearing lower $n$ value is easier than from orbital having higher $n$ value.
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Which of the following has the least ionization potential?
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View SolutionAn element has successive ionization enthalpies as $940 \, kJ \, mol^{-1}$ (first),$2080 \, kJ \, mol^{-1}$,$3090 \, kJ \, mol^{-1}$,$4140 \, kJ \, mol^{-1}$,$7030 \, kJ \, mol^{-1}$,$7870 \, kJ \, mol^{-1}$,$16000 \, kJ \, mol^{-1}$ and $19500 \, kJ \, mol^{-1}$. To which group of the periodic table does this element belong?
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View SolutionWhat is the definition of ionization energy for an atom?
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View SolutionThe incorrect statement among the following is:
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View SolutionAmong the second period elements,the actual ionization enthalpies are in the order $Li < B < Be < C < O < N < F < Ne$. Explain why:
$(i)$ $Be$ has higher $\Delta_{i}H$ than $B$
$(ii)$ $O$ has lower $\Delta_{i}H$ than $N$ and $F$?
$(i)$ $Be$ has higher $\Delta_{i}H$ than $B$
$(ii)$ $O$ has lower $\Delta_{i}H$ than $N$ and $F$?
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