Chemistry Help! Looked all through the book and cant find anything that relates!!?

Question

For the following electronic transitions in the hydrogen atom, calculate the energy, frequency, and wavelength of the associated radiation and determine whether the radiation is emitted or absorbed during the transition.
(a) from n = 3 to n = 6
____ J (energy)

____ s-1 (frequency)

____m (wavelength)



(b) from n = 9 to n = 3
____J (energy)

____ s-1 (frequency)

_____m (wavelength)



(c) from n = 7 to n = 4
____J (energy)

_____s-1 (frequency)

_____m (wavelength)

I tried that source already, and searched google..cant find nothing on this topic! GRR!

Answer 1

Try going to this site wich has free encycopedia it's called: www.wikipedia.com

Answer 2

I would like you to learn how to solve your questions by providing you the necessary formulas..please study the attached and this will guide you...I am a Prof. in Chemistry and I do hope this helps.
Please take close attention to the formulas. You can find this whole explanation by going to this site

Hydrogen Schrodinger Equation
... field associated with the transitions resembles an oscillating electric dipole. ... change by one unit in a electronic transition, j=0 -> 0 can't happen because ...hyperphysics.phy-astr.gsu.edu/hbase/quantum/hydazi.html

where it is more on PHYSICS...the concept is in Chemistry but the computations are in PHYSICS ...so that is the catch..or should I say the rub of studying ? always remember..Chemistry and Physics entertwine each other...

by the way..as you click the site..it will open up to the page
THE AZIMUTHAL EQUATION....

To the right side column of this page you will read

INDEX

Schrodinger equation concepts

Hydrogen Concepts


you must click the Hydrogen concept which will lead you to a page

HYDROGEN SCHEMATIC DIAGRAM

click each icon that will led you to all the mathematical formulas you need to solve your problems...below is the overview of the explanation to guide you if you were in the right page...

happy computing..enjoy the wonders of Physics embraced by Chemistry...



you must follow thru each page until you reach an illustration of
.Electron Transitions
The Bohr model for an electron transition in hydrogen between quantized energy levels with different quantum numbers n yields a photon by emission with quantum energy:

take note that a downward transition involves emission of a photon of energy
___________________________E
n o 2
2 \
\ E
___________V________________ 1
n
1

where :
E =hv = E - E
photon 2 1

Given the expression for the energies of the HYDROGEN electron states:
_ 2 4
hv = 2 II me [ 1 -- 1]
--------------- --- ---
2 2 2
h n n
1 2

( please take note that the formula above may not appear as I have typed so check on the proper location of each variable at the site.)
This is often expressed in terms of the inverse wavelength or "wave number" as follows:


Index

Atomic structure concepts
HyperPhysics***** Quantum Physics R Nave
Go Back





Hydrogen Energy Levels
The basic hydrogen energy level structure is in agreement with the Bohr model. Common pictures are those of a shell structure with each main shell associated with a value of the principal quantum number n.




This Bohr model picture of the orbits has some usefulness for visualization so long as it is realized that the "orbits" and the "orbit radius" just represent the most probable values of a considerable range of values. If the radial probabilities for the states are used to make sure you understand the distributions of the probability, then the Bohr picture can be superimposed on that as a kind of conceptual skeleton.

Energy level plot Energies in eV Hydrogen spectrum

Electron energy level diagrams
Index

Hydrogen concepts

Atomic structure concepts
HyperPhysics***** Quantum Physics R Nave
Go Back





Hydrogen Energy Level Plot
The basic structure of the hydrogen energy levels can be calculated from the Schrodinger equation. The energy levels agree with the earlier Bohr model, and agree with experiment within a small fraction of an electron volt.




If you look at the hydrogen energy levels at extremely high resolution, you do find evidence of some other small effects on the energy. The 2p level is split into a pair of lines by the spin-orbit effect. The 2s and 2p states are found to differ a small amount in what is called the Lamb shift. And even the 1s ground state is split by the interaction of electron spin and nuclear spin in what is called hyperfine structure.


Electron level calculation Energies in eV
Index

Hydrogen concepts

Atomic structure concepts
HyperPhysics***** Quantum Physics R Nave
Go Back





Hydrogen Spectrum



This spectrum was produced by exciting a glass tube of hydrogen gas with about 5000 volts from a transformer. It was viewed through a diffraction grating with 600 lines/mm. The colors cannot be expected to be accurate because of differences in display devices.

For atomic number Z = ,

a transition from n2 = to n1 =

will have wavelength l = nm

and quantum energy hn = eV

At left is a hydrogen spectral tube excited by a 5000 volt transformer. The three prominent hydrogen lines are shown at the right of the image through a 600 lines/mm diffraction grating.

An approximate classification of spectral colors:

Violet (380-435nm)
Blue(435-500 nm)
Cyan (500-520 nm)
Green (520-565 nm)
Yellow (565- 590 nm)
Orange (590-625 nm)
Red (625-740 nm)


Radiation of all the types in the electromagnetic spectrum can come from the atoms of different elements. A rough classification of some of the types of radiation by wavelength is:

Infrared > 750 nm
Visible 400 - 750 nm
Ultraviolet 10-400 nm
Xrays < 10 nm
Bohr model Measured hydrogen spectrum Other spectra
Index

Great experiments of physics

Hydrogen concepts

Atomic structure concepts
HyperPhysics***** Quantum Physics R Nave
Go Back





Measured Hydrogen Spectrum
The measured lines of the Balmer series of hydrogen in the nominal visible region are:


Wavelength
(nm) Relative
Intensity Transition Color
383.5384 5 9 -> 2 Violet
388.9049 6 8 -> 2 Violet
397.0072 8 7 -> 2 Violet
410.174 15 6 -> 2 Violet
434.047 30 5 -> 2 Violet
486.133 80 4 -> 2 Bluegreen (cyan)
656.272 120 3 -> 2 Red
656.2852 180 3 -> 2 Red


The red line of deuterium is measurably different at 656.1065 ( .1787 nm difference).
Illustration of transitions




Hydrogen fine structure (3->2 transition)

More extensive table of spectral lines

Answer 3

ok i dont feel like doing the calculations for you but heres what you have to use:
v=wavelength
R=rydberg constant =10 973 731.6 m^-1
c=speed of light=2.998 x 10^8 m/s
f=frequency
e=energy
h=plank's constant
=6.626068 × 10^-34 m2 kg / s
ni=initial orbital of the electron
nf=final orbital of the electron
first formula: v=R(1/(ni)^2-1/(nf)^2)
that gets you the wavelength
then use: f=c/v
that gets you the frequency
and finally use e=fv to get the energy