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Estimated time: 8 minutes
CBSE: Class 12

Definition: Ionisation

Completely removing an electron from atom is called ionisation.

CBSE: Class 12

Definition: Luminescence

The atom emits a photon with energy equal to the difference between the two energy levels, a phenomenon known as luminescence.

CBSE: Class 12

Formula: Wave Number / Wavelength Formula (Rydberg Formula)

\[\bar{v}=\frac{1}{\lambda}=RZ^2\left[\frac{1}{n_1^2}-\frac{1}{n_2^2}\right]\mathrm{m}^{-1}\]

where \[R=1.097\times10^7\mathrm{m}^{-1}\] (Rydberg constant)

CBSE: Class 12

Formula: Ionisation Energy (Hydrogen Atom)

\[E_\text{ionisation}=13.6Z^2\mathrm{~eV}\]

CBSE: Class 12

Formula: Energy of Electron at Level n

\[E_n=-Rhc\left(\frac{1}{n^2}\right)\]

CBSE: Class 12

Key Points: Energy Levels

  • For hydrogen (Z = 1): ground state energy = −13.6 eV; at n = ∞, energy = 0 eV.
  • Energy levels for hydrogen: n=1: −13.6 eV, n=2: −3.4 eV, n=3: −1.511 eV, n=4: −0.850 eV, n=5: −0.544 eV.
  • In normal conditions, electrons are in the ground state, occupying orbitals closest to the nucleus.
  • Beyond ionisation potential, the electron is no longer bound — energy levels form a continuum (starts at 13.6 eV above ground in hydrogen).
  • Electrons in orbitals close to the nucleus are stable (need more energy to remove); electrons farther away are less stable.
  • If energy supplied ≥ ionisation energy, ionisation occurs.
  • Spectral Series (from energy level transitions): Lyman, Balmer, Paschen, Bracket, Pfund series.

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