Question

What is Heisenberg's uncertainty principle?​

Answer 1

Heisenberg's uncertainty principle states that-

"the exact position as well as momentum of an electron in an atom cannot be determined at a particular instant"

it further established a relationship between the uncertainties in the above mention quanities as–

if dx and dp and dv are the uncertainties in the position, momentum and velocity of an electron in an atom respectively, then

$dx.dp \: ≥ \:\frac{h}{4\pi}$

where 'h' is the Planck's constant

$(h = 6.626 \times {10}^{ - 34} \: joule \: per \: second)$

Answer 2

Answer:

What is Heisenberg's Uncertainty Principle ?

Statement:

At the level of Quantum Mechanics,

the position and velocity of any object cannot be measured accurately at the same time.

Meaning:

During measurement of velocity or position , there is bound to be some error during theoritical calculations.

Mathematical Statement:

∆x × ∆P > h/(4π) ,

=>∆x × m × ∆v > h/(4π)

where ∆x is the error in calculating position,

∆P is the error in calculating momentum.

and ∆v is the error in calculating velocity.

This Principle considers electron to have both particle as well as wave nature. Hence its position and velocity calculation becomes unpredictable.