Question

this energy diagram shows the allowed energy levels of an electron in a certain atom or molecule:
use this diagram to complete the table below.
which is the ground state?
how many excited states are there?
how many lines are in the absorption line spectrum?
which transition causes the absorption line at the shortest wavelength?
which transition causes the absorption line at the longest wavelength?

Explanation:

Step1: Determine excited states

Excited states are energy levels above the ground state. Here, ground state is A, so excited states are B and C. So number of excited states is 2.

Step2: Calculate absorption line spectrum lines

Absorption occurs when electron jumps from lower to higher energy level. From ground state A, it can jump to B and C. So number of lines in absorption line spectrum is 2.

Step3: Find transition for shortest - wavelength absorption

Using \(E = h\frac{c}{\lambda}\) (\(E\) - energy, \(h\) - Planck's constant, \(c\) - speed of light, \(\lambda\) - wavelength), shorter wavelength means higher energy. Transition \(A
ightarrow C\) has higher energy difference (as C is higher than B from A).

Step4: Find transition for longest - wavelength absorption

Longer wavelength means lower energy. Transition \(A
ightarrow B\) has lower energy difference.

Answer:

How many excited states are there? \(2\)
How many lines are in the absorption line spectrum? \(2\)
Which transition causes the absorption line at the shortest wavelength? \(A
ightarrow C\)
Which transition causes the absorption line at the longest wavelength? \(A
ightarrow B\)