1. How do we define ionization energy of H-atom in terms of the electron transit
ID: 476895 • Letter: 1
Question
1. How do we define ionization energy of H-atom in terms of the electron transition - from ground state to which energy level?
2. How is the energy of the electron is quantized in H-atom in terms of a quantum number n = 1,2,3,…? How does it depend on n mathematically?
3. What is the Rydberg constant for H-atom, and how does it relate to its ionization energy?
4. In the emission spectrum of H-atom, what are those series called Lyman, Balmer and Paschen? Between what values of main quantum number n the Lyman, Balmer and Paschen transitions do occur?
5. Why it is easier to ionize an H-atom in its excited state than to ionize it when the atom is in its ground state?
Explanation / Answer
1.
Ionization energy is defined as the energy required to remove the valence electron. Thus, for an H-atom, it corresponds to a transition of the electron from the ground state orbital to the orbital theortecially at infinite distance, i.e. at infinity such that it practically means that the electron gets removed form the atom.
2.
The electron in H-atom has fixed energy depending upon its quantum number, i.e., the orbit in which the electron is situated.
Mathematically, it is given by the following relation for the case of H-atom:
E = -13.6/n2 eV
4.
Lyman Balmer and Paschen series explain the occurence of the spectral lines observed in the H-spectrum.
Lyman series corresponds to the transition of electron from n2 = 2 to the ground state. Here, n2 denotes the excited state electron orbital number.
Similarly, for Balmer series n2 = 3, and for Paschen series n2 = 4.
5.
This is because in the excited state the electron is already at a higher energy level, so lesser input of extra energy is required in order to make up to the threshold level to finally attain ionization.
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