In the figure above we see a partial energy level diagram for a hypothetical ato

Question

In the figure above we see a partial energy level diagram for a hypothetical atom. In our picture we are looking at 4 possible electron transitions that could result when the atom is given sufficient energy. What is the energy required for each of the electron transitions shown in the diagram Transition 1 = Transition 2 = Transition 3 = Transition 4 = Imagine that we irradiate the atom with light having wavelengths of between 150 nm and 700 nm (to provide the energy). Select all of the transitions that are possible when this atom is exposed to this light.

Explanation / Answer

Solution :-

Calculation of energy for the each transitions using the change in the energy values of the each energy levels

transition 1 = E2-E1 = (-9.00E-19 J ) – (-1.33E-18 J ) = 5.897E-19 J

trantion 2 = E3- E1 = (-6.38E-19)-(-1.33E-18) = 6.92E-19 J

ransition 3 = E4-E1 = (-5.33E-19)-(-1.33E-18) = 7.97 E-19 J

transition 4 = E5-E1 = (-3.34E-19)-(-1.33E-18) = 9.96E-19 J

Now lets calculate the energy obtained from the radiation with wavelength between 150 nm to 700 nm

Calculating energy for 150 nm = 1.50*10^-7 m

E= hc/l

= 6.626E-34 J .s * 3E8 m s-1 / 1.50E-7 m

= 1.32*10^-18 J

So the enrgy obtained from 150 nm radiation is higher than energy needed for the tranations

So all the transitions can takes place using the 150 nm wavelength raidtion.

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.