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Home » The first ionization enthalpy values (in kJ/mol) of group 13 elements are given below. How would you explain this deviation from the general trend?
The first ionization enthalpy values (in kJ/mol) of group 13 elements are given below. How would you explain this deviation from the general trend?
CBSE | Chemistry | Class 12 | Classification of Elements and Periodicity in Properties | NCERT
The first ionization enthalpy values (in kJ/mol) of group 13 elements are given below. How would you explain this deviation from the general trend?
B Al Ga In Tl
801 577 579 558 589

 

Answer

The ionization enthalpy decreases with group size. B and Al agree. Ga has a higher ionization enthalpy than Al. Tend electrons in the inner shell of Ga are less piercing. Their shielding is inferior to s and p electrons. The nucleus firmly holds the outside electron. The ionization enthalpy rises. The rise from In to Tl is due to the existence of 14f electrons in the inner shell of Tl.

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