Editing Atomic physics (section)

===Bohr Model of the Atom===

The Bohr model, proposed by '''Niels Bohr in 1913''', is a revolutionary theory describing the structure of the hydrogen atom. It introduced the idea of quantized orbits for electrons, combining classical and quantum physics.

'''Key Postulates of the Bohr Model'''

'''1. Electrons Move in Circular Orbits:'''

• Electrons revolve around the nucleus in fixed, circular paths called '''orbits''' or '''energy levels'''.

• These orbits are '''stable''' and do not radiate energy.

'''2. Quantization of Angular Momentum:'''

• The angular momentum of an electron is quantized and given by:

:<math>\ L = m_{e}vr = n_{\hbar}, \quad n = 1, 2, 3, \ldots </math>

where:

• <math> m_e : </math> Mass of the electron.

• <math> v : </math> Velocity of the electron.

• <math> r : </math> Radius of the orbit.

• <math> \hbar : </math> Reduced Planck's constant (<math>\hbar = \frac{h}{2\pi}</math>).

• <math> n : </math> Principal quantum number, representing the orbit.

'''3. Energy Levels:'''

• Each orbit has a specific energy. The total energy of an electron in the <math>n</math>th orbit is:

:<math>\ E_n = -\frac{13.6}{n^2} \ \text{eV}, </math>

where <math> 13.6 \ \text{eV} </math> is the ground-state energy of the hydrogen atom.

'''4. Emission or Absorption of Energy:'''

• Electrons can transition between orbits by '''absorbing''' or '''emitting''' energy equal to the difference between the energy levels:

:<math>\ \Delta E = E_f - E_i = h\nu, </math>

where:

• <math> h : </math> Planck's constant.

• <math> \nu : </math> Frequency of emitted/absorbed radiation.

• <math> E_f, E_i : </math> Final and initial energy levels.