if electron transition from n=7 to n=4 principal energy level
then En= - 2,18*10-18 j( 1/n2 )
E=E7 - E4
= -2.18 * 10-18 ( 1 / 42 - 1 / 72 )
=-2.18 * 10-18 * 33 /784
=- 9,18 *10-20
=2.1 *10-6 m
the value of wavelength is =2.1 *10-6 m
6) Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its...
5..Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by E --2.18 x 10-18 (1/n) 18 10-20 nm 216x 103 nm 45 x 10-20 nm 16x 10-6 nm 1.38 x 1014 nm
Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n 4 to the n=1 principal energy level. Recall that for hydrogen En-2.18x 10-18 J(1/n2). (h 6.63 x 10 34 J s) Select one: a. 3.08 x 1015s' b. 1.03x 108 s1 c. 2.06 x 1014s O d. 1.35 x 10-51 s1 e. 8.22 x 1014g
calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n=4 to the n=1 principal energy level. E=-2.18x10^-18 J(1/n^2) Constants (c = 2.9979 | 109 m/s; h = 6.626 | 10 " J[s) 1. What is the energy in joules of a mole of photons with visible light of wavelength 486 nm? (246 kJ) 2. Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its...
What is the wavelength of light emitted when the electron in a hydrogen atom undergoes a transition from level n = 9 to level n = 4? (c = 3.00 × 108 m/s, h = 6.63 × 10-34 J • s), RH = 2.179 × 10-18 J) a) 5.49 × 105 m b) 1.09 × 10–19 m c) 1.65 × 1014 m d) 3.64 × 10–28 m e) 1.82 × 10–6 m
Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level.
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Calculate frequency Calculate the frequency of light emitted from a hydrogen atom when a transition is made from n = 7 to n = 5. h = 6.63 x 10^-34 Js c = 2.9979 x 10^8 m/s R_H = 2.18 x 10^-18 J 7.151 x 10^13 s^-1 5.991 x 10^13 s^-1 5.347 x 10^13 s^-1 6.442 x 10^13 s^-1 4.703 x 10^13 s^-1
JW 18) What is the wavelength of light emitted when the electron in a hydrogen atom undergoes a transition from level n 8 to level n 2? (c 3.00 x 108 m/s, h= 6.63 x 104 J.s, RH 2.179 x 10-18
What is the wavelength of the photon emitted when an electron in a hydrogen atom which is in the initial state n = 8 jumps to the final state n = 2? How do you solve to get C as the correct answer? 2) What is the wavelength of the photon emitted when an electron in a hydrogen atom which is in the initial state n 8 jumps to the final staten 2? (c J 3.00 x 108 m/s, h...
What wavelength (in nanometers) of light is emitted when an electron in a hydrogen atom falls from the n=4 to the n=3 energy level? What wavelength (in nanometers) of light is emitted when an electron in a hydrogen atom falls from the n=4 to the n=3 energy level? nm Check