What wavelength should the astrophysicist look for to detect a transition of an electron from the n equals 7 to the n equals 3 level?

Answer 1

,

Use Rydberg's Equation to solve for this problem, which is as follows:

1/wavelength = R((1/n2x )-(1/ny2 ))

Where R is Rydberg's constant, 1.0974 * 107 m-1

And where nx is the lower energy state (n=1), and ny is the higher energy state (n=3).

So, plugging in those values gives us the following calculations to be made:

1/(12)=1, and 1/(32)= 1/9, so (1) - (1/9) = 8/9.

So, we get:

1/wavelength = (1.0974* 107 m-1)(8/9)

=

1/wavelength = (.9754666667 m-1)

=

wavelength = 1/(.9754666667 m-1)

=

Wavelength = 1.025150355 * 10-7 m

And, since wavelength is typically given in nanometers (1 nm = 1 * 10-9 m) when looking at hydrogren emission spectra, convert the 10-7to 10-9 by moving the decimal back two more places.

So,

The wavelength expected for light composed of photons produced by an n=3 to n=1 transition in a hydrogen atom is:

102.5150355 nm

or, to three significant figures,

103 nm

Hope I helped!

I am an engineering student at the University of Arizona.

Answer 2

The astrophysicist should look for a wavelength corresponding to the energy difference between the n=7 and n=3 energy levels in the hydrogen atom. This can be calculated using the Rydberg formula: 1/λ = R (1/n_initial^2 - 1/n_final^2), where n_initial=7, n_final=3, and R is the Rydberg constant. Solving for λ would give the wavelength to look for.

Answer 3

What wavelength should the astrophysicist look for to detect a transition of an electron from the to the level?

Answer 4

1.00*10^-6 m

Answer 5

In what atom? Need a Z number.

Answer 6

1.00*10^-6