Question

Question 8 An electron in an atom absorbs a photon with an energy of 3.07 eV and jumps from the n 2 to n = 4 energy level in the atom. Tries remaining: Calculate the wavelength of the photon absorbed by the electron. Marked out of 1.00 Answer m Flag question Check Question 9 4 level then jumps down to the n 3 level, emitting a photon with a wavelength of 2.14 um. The electron in the n Tries remaining: 3 Calculate the energy of the photon emitted. Marked out of 1.00 Answer Flag question Check Question 10 Calculate the difference in energy between the n 2 and the n 3 energy levels in this atom. Tries remaining: 3 Answer eV Marked out of 1.00 PFlag question Check Question 11 Calculate the frequency of the photon emitted when the electron jumps from the n = 3 to the n 2 energy level. Tries remaining: Answer: Hz Marked out of 1.00 PFlag question Check

Answer 1

04 photo へ EEner 97 F hC/ hv > Planck's Constant . 34 つ 6.626xlo E= 3.07 eV wavelength Speed of light 3 xL0 mns Avequeney CYv .6x101 S 4.91 x 1o T 34 x 3x103 hc 6. 6 26 x 10 E 4. 91x 19 7 4 O49 . W -6 2. 14m 214 h c 3106 6.626 I03t 17 4049 2.14 106 289 10 T -20 58 ev io7 9, 289x1o 3.07 e V. ns2 4 1 tran sition for $3 つ 、53ev

3 07ev .S2ev . (E)n-2-3 A 2 3.07-0.58ev 2-49 e v: 3. 989 x1o 2i49 ev E E 34 6.626 1o X 6 02 XI0 14 J 1