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How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?
Among the second period elements the actual ionization enthalpies are in the
order Li < B < Be < C < O < N < F < Ne.
Explain why Be has higher ΔiH than B?
Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.
What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group?
Energy of an electron in the ground state of the hydrogen atom is –2.18 × 10–18 J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol–1.
- Chemistry Textbook for Class 11 Part 1