You will find in Chapter $39$ that electrons cannot move in definite orbits within atoms, like the planets in our solar system. To see why, let us try to "observe" such an orbiting electron by using a light microscope to measure the electron's presumed orbital position with a precision of$,$ say, $10$ pm $($a typical atom has a radius of about $100$ pm $).$ The wavelength of the light used in the microscope must then be about $10$ pm $.$

Your answer is partially correct.

$($a$)$ What would be the photon energy of this light?

Number

Units

$($b$)$ How much energy would such a photon impart to an electron in a head$-$on collision?

Number

Units

Correct.

$($c$)$ What do these results tell you about the possibility of "viewing" an atomic electron at two or more points along its presumed orbital path? $($Hint: The outer electrons of atoms are bound to the atom by energies of only a few electron$-$volts.$)$

It is possible to "view" an atomic electron.

It is impossible to "view" an atomic electron.