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.
Ionization enthalpy is the minimum amount of energy which is needed to remove the loosely bound electron from a isolated gaseous atom to form a cation.
It is given that the energy of an electron in the ground state of the hydrogen atom is –2.18 × 10–18 J.
Therefore, the energy required to remove that electron from the ground state of hydrogen atom is 2.18 × 10–18 J.
so Ionization enthalpy of atomic hydrogen = 2.18 × 10–18 J
Hence, ionization enthalpy of atomic hydrogen in terms of J mol–1 = 2.18 × 10–18 × 6.02 × 1023 J mol–1 = 1.31 × 106 J mol–1
NCERT questions are designed to test your understanding of the concepts and theories discussed in the chapter. Here are some tips to help you answer NCERT questions effectively:
Welcome to the NCERT Solutions for Class 11 Chemistry - Chapter . This page offers a step-by-step solution to the specific question from Excercise 1 , Question 15: Energy of an electron in the ground state of the hydrogen atom is –2.18 × 10–18 J.....
Comments
Energy of electron has negative value which shows that electron has loosened that energy to come to the hydrogen nucleus hence it is required to give back that same amount of energy to the electron to get out of the hydrogen atom
Very well understood
I got it. Thanks
thanks