Reply answr immediatly

Reply answr immediatly of •i' fro—sy of 5800 A

According to the Heisenberg's Uncertainty principle, it is impossible to determine simultaneously the exact position and the exact momentum of an electron (microscopic particle) with absolute accuracy and certainty. Mathematically, it can be represented as

Δ x × Δp _x ≥ 

Or, Δx × Δ(mv _x ) ≥ 

Or, Δx × Δv _x ≥ 

Where,

Δ x is the uncertainty in position

Δ v _x is the uncertainty in velocity

Δ p _x is the uncertainty in momentum

If the uncertainty in position (Δx) is less, then the uncertainty in momentum (Δp _x ) would be large. On the other hand, if the uncertainty in momentum (Δp) is less, the uncertainty in position (Δx) would be large.

Significance of Uncertainty Principle

• Heisenberg’s uncertainty principle rejects the existence of definite paths or trajectories of electrons and other similar particles (subatomic or microscopic).

• The effect of Heisenberg’s uncertainty principle on the motion of macroscopic objects is negligible.

• However, this is not the case with the motion of microscopic objects.

Limitations of Bohr’s model of atom:

• Bohr’s model was unable to explain the multi electron atom spectra but explained the spectra of simple atom containing single electron i.e. hydrogen.
• The model was unable to explain the splitting of spectral lines in electric ( Zeeman effect )and magnetic field ( stark effect ).
• It failed to explain the three dimensional model of atom which it proposed as flat model.
• It failed to explain the shape of molecules.
• It failed to explain the de Broglie and Heisenberg uncertainty principle.