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Which one of the following statements is incorrect in relation to ionization enthalpy?
(a) Ionization enthalpy increases for each successive electron.
(b) The greatest increase in ionization enthalpy is experienced on removal of electron from core noble gas configuration.
(c) End of valence electrons is marked by a big jump in ionization enthalpy.
(d) Removal of the electron from orbitals bearing lower n value is easier than from orbital having higher n value.
Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.
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?
What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group?
- Chemistry Textbook for Class 11 Part 1