Question

Calculate the uncertainty in the position of an electron moving at a speed of (3.00±0.01)×105m/s. (Take the mass of the electron m=9.109×10−31kg.) Express your answer using two significant figure.

Answer 1

use Heisenberg uncertainty principle,

Δx*Δv = h/(4*pi*m)

Here:

Δv = 0.01*10^5 m/s = 1*10^3 m/s

mass, m = 9.109*10^-31 Kg

Putting values,

Δx*(1*10^3) = (6.626*10^-34)/(4*3.14*9.109*10^-31)

Δx*(1*10^3) = 5.792*10^-5

Δx = 5.792*10^-8 m

Answer: 5.8*10^-8 m

Answer 2

Use sketches of 2s and 2p orbitals to distinguish between (a) the radial wavefunction and (b) the radial distribution function.