## Module Question

$\Delta p \Delta x\geq \frac{h}{4\pi }$

Jolie Sukonik 2B
Posts: 41
Joined: Wed Sep 30, 2020 9:44 pm

### Module Question

The hydrogen atom has a radius of approximately 0.05 nm. Assume that we know the position of an electron to an accuracy of 1 % of the hydrogen radius, calculate the uncertainty in the speed of the electron using the Heisenberg uncertainty principle.

How do I find the uncertainty in the position first? I know once I find it I can just calculate the uncertainty in velocity, but I am struggling on how to find deltax.

Quentin Scarborough 1A
Posts: 45
Joined: Wed Sep 30, 2020 9:59 pm
Been upvoted: 1 time

### Re: Module Question

If you know the radius of a Hydrogen atom, you can just find 1% of that to find your uncertainty. In this case it would be .05nm * .01= 5*10^-13, which would be your uncertainty position.

Posts: 49
Joined: Wed Sep 30, 2020 9:40 pm

### Re: Module Question

Since it says that we know the position of an electron to an accuracy of 1 % of the hydrogen radius, and the radius is 0.05 nm, the uncertainty in position is
.01(.05 nm)= 5 x 10^-13 m. From there, you can find delta(v).