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The first ionization enthalpy values (in kJmol–1) of group 13 elements are:-
How would you explain this deviation from the general trend?
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?
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?
Among the second period elements the actual ionization enthalpies are in the
order Li < B < Be < C < O < N < F < Ne.
Explain why O has lower ΔiH than N and F?
- Chemistry Textbook for Class 11 Part 1