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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?
What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group?
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?
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.
The first ionization enthalpy values (in kJmol–1) of group 13 elements are:-
How would you explain this deviation from the general trend?
- Chemistry Textbook for Class 11 Part 1