🤓 Based on our data, we think this question is relevant for Professor McCrory's class at UMICH.
Distance = Energy
• lower-numbered shell there’s a bigger distance between them
• the distance between shells gets smaller the higher up you go
• the smaller the distance then the less energy is required for an electron to travel
↓ smaller distance, ↓ less energy required, ↑ wavelength
longest wavelength: n = 6 to n = 5
↑ bigger distance, ↑ higher energy required, ↓ wavelength
shortest wavelength: n = 6 to n = 1
We’re going to use the Balmer Equation which relates wavelengths to a photon’s electronic transitions.
λ = wavelength, m
R = Rydberg constant = 1.097x107 m-1
Z = atomic number of the element
ninitial = initial energy level
nfinal = final energy level
Calculate the wavelength of light (λ):
n = 6 to n = 5
Z = atomic number of Hydrogen = 1 (refer to the periodic table)
R = 1.097x107 m-1
ninitial = 1
nfinal = 3
λ = 7458 nm
n = 6 to n = 1
Calculate the longest and shortest wavelengths of light emitted by electrons in the hydrogen atom that begin in the n = 6 state and then fall to states with smaller values of n.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Bohr and Balmer Equations concept. If you need more Bohr and Balmer Equations practice, you can also practice Bohr and Balmer Equations practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor McCrory's class at UMICH.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.