38)
1/lambda = -R* (1/nf^2 - 1/ni^2)
R is Rydberg constant. R = 1.097*10^7
1/lambda = - R* (1/nf^2 - 1/ni^2)
1/lambda = - 1.097*10^7* (1/3^2 - 1/2^2)
lambda = 6.606*10^-7 m
lambda = 661 nm
Answer: 661 nm
39)
Electron is moving from lower energy state to higher energy state.
So, energy is being absorbed.
So, photon is being absorbed
Answer: absorbed
2 to n=3 in the hydrogen 38. (5 pts) Calculate the wavelength of light associated with the transition from n atom....
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calculate the wavelength of light emitted when an electron in a hydrogen atom makes from n=3 to n=2 transition
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Consider an electron transition from n 5 to n =3 of a hydrogen atom. 5. Use Bohr's H model to calculate the energy required to for this electron transition. Will the hydrogen atom absorb or emit energy during this transition? a) What wavelength of light will the hydrogen atom absorb or emit in this electron transition? b) A rifle bullet (mass-4.20 g) has a velocity of 2160 mph. What is the wavelength associated with this bullet? (1 km 0.62137 mil)...
Calculate the wavelength of light emitted when an electron in the hydrogen atom makes a transition from an orbital with 5to an orbital with n = 2 3.14 x 10m 4.34 x 10-7m 4.58 x 10 2.28 x 10 m m Submit Request Answer
Example Determine the wavelength of light emitted when a hydrogen atom makes a transition from the n 6 to the n -2 energy level according to the Bohr model