Posted on April 12.
From the information below, identify element X.
a. The wavelength of the radio waves sent by an FM station
broadcasting at 97.1 MHz is 30.0 million (3.00 e7) times
greater than the wavelength corresponding to the energy difference
between a particular excited state of the hydrogen
atom and the ground state.
b. Let V represent the principal quantum number for the valence
shell of element X. If an electron in the hydrogen atom
falls from shell V to the inner shell corresponding to the excited
state mentioned above in part a, the wavelength of light
emitted is the same as the wavelength of an electron moving
at a speed of 570. m/s.
c. The number of unpaired electrons for element X in the ground
state is the same as the maximum number of electrons in an
atom that can have the quantum number designations n = 2,
mL = 1, and mS = 1/ 2.
d. Let A equal the charge of the stable ion that would form when
the undiscovered element 120 forms ionic compounds. This
value of A also represents the angular momentum quantum
number for the subshell containing the unpaired electron(s)
for element X.
a.
i used lambda= nu/c
97.1Mhz*10^6s^1=97,100,000s^1
lambda= 97,100,000/2.998e8= 0.324m
0.324m/30,000,000 = 1.08e8m
I then found the energy for n=1 through n=5
n=1 E= 2.18e18J/atom
n=2 5.45e19
n=3 2.42e19
n=4 1.36e19
n=5 8.72e20
DrBob222 said:
The difference between the energy of the orbits (the N values) will be the energy of the electron when it makes the transition between any one of them to any other below it. Convert energy difference to wavelength, delta E = hc/lambda and compare with the wavelength of the radio station divided by 30 million. That will tell you N for the excited state.
How do I do that. Do I do each difference. I really don't understand any of this please help! I understand about getting the difference and the converting to wavelength but the difference of which n's and why.
Thanks for posting again on page 1. I hardly ever go back to page 8 or 9 where your original post is by now.
First, you need to correct the first piece of data you have.
c = nu*lambda, not what you have.
3E8 meters = 97.1E6Hz*lambda
lambda = 3E8/97.1E6 = ?? lambda of the radio wave;
and ??/30,000,000 = xx = lambda of the wavelength when the electron makes the transition in the hydrogen atom discussed in part a of the problem.
Then Energy of the electron = E = hc/lambda = hc/xx.
All of your E values for N=1 through N=5 are correct. I would add another one for N=6 just for good measure.
Here is the scoop. An electron falls from one of those upper levels to the ground state (look at the problemit says it falls to th ground state and the ground state is N=1). The energy it gives off is the difference between the upper state energy and the lower state energy; so, just subtract E2E1 = energy when electron falls from N=2 to N=1. Then E3E1 = energy when the electron falls from N=3 to N=1 etc. Convert each of these energies to lambda and compare with lambda from part a of the problem OR compare the energy difference to the energy in part a of the problem. E2E1 or E3E1 or E4E1 or E5E1 or E6E1 will match. All of this is for the purpose of identifying the excited state (the upper level or N = ??) because the next part of the problem has the electron falling from some higher level to the excited state so you much know what the excited state is.
Post your work if you get stuck. That helps, you see, for I could tell you that your initial calculation was not correct. Good luck.
now I have:
38e8/97.1e6 = 3.089m
3.09m/30,000,000 = 1.029e7
E= 6.626e34*3e8/1.029e7
= 1.932e18J
E2E1=1.635e18
E3E1=1.938e18
E4E1= 2.044e18
E5E1= 2.093e18
E6E1= 2.119e18
so it would be N=3
Absolutely right. The electron is in the N=3 level, the excited state, and falls to the ground state where N=1. Now you are ready to determine V, the principal quantum number in part b.
Remember the De Broglie wavelength, lambda = h/mv.
don't you need a mass to used the de broglie equation or is that what we are solving for?
You have a mass. It's the mass of the electron that is traveling at whatever? its velocity. So you have h, m, and v and you can calculate lambda. And from that you can calculate E = hc/lambda if you wish.
sorry.. i still don't understand the mass... do you use the mass of hydrogen 1.008? In class everything is more clear, but I just don't understand these problems.
b. Let V represent the principal quantum number for the valence
shell of element X. If an electron in the hydrogen atom
falls from shell V to the inner shell corresponding to the excited
state mentioned above in part a, the wavelength of light
emitted is the same as the wavelength of an ELECTRON moving
at a speed of 570. m/s.
The secret is there. An electron moving at a speed of 570 m/s has what wavelength? The De Broglie equation is
lambda = h/mv.
You know h, you know mass of the ELECTRON (I made it all caps from your original question), and you know v. Calculate lambda. And from that, if you wish, you may calculate Energy = E = hc/lambda.
These railroad problem CAN be a little confusing because we are overwhelmed (innundated) with information and it is coming at us from all directions. This particularly problem is more confusing than most because it goes from talking about one thing to another; that is, from 97.1 MHz on the radio to a electron in a hydrogen atom and from a principal quantum number to the same "system" in a hydrogen atom. It gets even worse for part c. Part d is a little better.
well the mass of an electron is 9.109e31kg, right?
yes
lambda= 6.626e3/(9.109e31)(570)= 1.276e25m
E= (6.626e34)(3e8)/1.276e25
=1.558e50J
I think h = 6.626E34 J*s and not E3. That will make a difference in lambda.
E= ?? also is wrong. I have lambda = 1.276E6 m for lambda and 1.558E19 J for energy. Your number is ok but the exponent is wrong. After you have done that, then start subracting the energy of one level from Energy of level 3 (that's the excited state in part a) of the H atom. Just like the process you did in part a. You will find one of those (E6E3 or E5E3 or E4E3) match the speed of the electron's energy when it is moving 570 m/s. If that doesn't do it, you will need to go back and calculate energy for N=7, N=8 etc but I think one of these will do it.
Check my last post for the A,B, and C problem. I don't buy the final pressure being 1 atm.
yes you're right it wrote it wrong.. now i get what you have
for E5E3 i get 1.548e19
for the A,B,C problem I used V=18.60L, maybe I gave the wrong moles
OK. So now you know the principal quantum number of element X is N=5 (or in their terms, V=5). Reread part b of the question so you will understand what we have just done.
i used the 1.4L of A to calc new moles? should i have done that?
I understand the v=5 and part b.
I have class now so I will be gone for a while. Thank you for all of your help. hopefully you will still be available when I come back. Thank you!
p = nRT/V= 0.446*0.08205*273/18.60 = ??. Check my thinking. I don't get 1 atm using either mol A remaining or mols dichloroethane (mols B)formed. The only way I can obtain 1 atm is by using 10.0 L for volume. p = 0.446*0.08205*273/10 = 0.999 which we would round to 1. Also, I don't know how you got p1v1 = p2v2 to come out, either.
ok. Glad you understand part b.
Yes, you should have converted 1.4 L to mols. Also convert 8.6 L of compound B to mols. Add them together for total n. Use 18.60 for volume.
now i get P=0.537 atm
1 answer

What's the answer to this problem?
I got molybdenum...