🔴 BOHR'S MODEL for Hydrogen Atom and its Limitations || Chemistry for Class 11 in Hindi

In this Chemistry video in Hindi for class 11 we explained Bohr's model for hydrogen atom and also discussed on its limitations. Niels Bohr stated that there are some fixed orbits with fixed energy for hydrogen atoms. There were two developments leading to Bohr's atomic model, viz., Hydrogen atomic spectra and particle nature of electromagnetic radiation. Bohr's model explains the elusive hydrogen spectral lines. But this model has its limitations / drawbacks. Bohr's atomic model can not explain the Zeeman effect or Stark effect. And it also fails to explain the complicated spectral lines for atoms with more than one electron.
🔴 Link for the playlist on the chapter ‘Structure of Atom’ for Class 11 - Chemistry
• Discovery of Electron ...
Some related videos :
🔴 Rutherford Atomic Model and it's Drawback
• 🔴 Rutherford Atomic Mo...
🔴 Developments Leading to the Bohr's Model of Atom
• 🔴 Developments Leading...
🔴 Wave Nature of Electromagnetic Radiation
• 🔴 Wave Nature of Elect...
🔴 Planck's Quantum Theory
• 🔴 Planck's Quantum The...
🔴 Photoelectric Effect
• 🔴 Photoelectric Effect...
🔴 ABSORPTION and EMISSION SPECTRA || ATOMIC SPECTRA
• 🔴 ABSORPTION and EMISS...
🔴 LINE SPECTRUM of HYDROGEN || Balmer and Rydberg Equations
• 🔴 LINE SPECTRUM of HYD...

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[@shantachattopadhyay6897]

I have a question...for Hydrogen atom ..we know there is only 1s orbital...so when energy is supplied..electron moves to another higher orbital which doesn't exist for hydrogen(i.e.2s)...but we get of the hydrogen spectrum as different lines(Balmer,Paschen etc)...so where does the electron go actually for hydrogen atom when energy is supplied to it?

[@mathsfanatics]

Good Question. Firstly energy level doesn't necessary means the orbit. There are different energy levels possible where the single electron can jump when get excited.
Electrons in a hydrogen atom must be in one of the allowed energy levels. If an electron is in the first energy level, it must have exactly -13.6 eV of energy. If it is in the second energy level, it must have -3.4 eV of energy.
Energy Level and Energy
1 -54.4 eV
2 -13.6 eV
3 -6.04 eV
And so on.... Different energy level means where the electron can revolve around the nucleus with fixed L and E. Also remember the concept of orbital was not introduced in this time.

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