Solution: According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 x 103 m/s, the uncertainty in its position (in m) is at least.66 m 17 m 6.6 x 10-8 m 1.7 x 10-8

Solution: According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 x 103 m/s, the uncertainty in its position (in m) is at least.66 m 17 m 6.6 x 10-8 m 1.7 x 10-8

According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 x 10^{3} m/s, the uncertainty in its position (in m) is at least.

- 66 m

- 17 m

- 6.6 x 10
^{-8}m

- 1.7 x 10
^{-8 }m

- 2.1 x 10
^{-10}m

We’re being asked to **determine the uncertainty in the position** of an electron with **uncertainty in the speed of 3.5 × 10 ^{3} m/s**.

Recall that ** Heisenberg’s Uncertainty Principle** states that we cannot accurately determine both the position and velocity of an electron. This means we can only know either one at any given time.

Mathematically, this is expressed as:

$\overline{){\mathbf{\Delta x}}{\mathbf{\xb7}}{\mathbf{\Delta p}}{\mathbf{\ge}}\frac{\mathbf{h}}{\mathbf{4}\mathbf{\pi}}}$

where:

**h** = Planck’s constant (6.626 × 10^{–34} kg • m^{2}/s)

**Δx** = uncertainty in position (in m)

**Δp** = uncertainty in momentum (in kg • m/s)