Saturday
April 19, 2014

Search: Emission Spectrum of hydrogen ...CHEM

Number of results: 18,809

Physics
What type of spectrum is produced by a hydrogen gas when a high potential difference is applied to it? a visible spectrum emission spectrum absorption spectrum a continuous spectrum I've been all through my notes and cant figure this one out :/
Tuesday, March 6, 2012 at 12:33am by Bunny

Physics - Hydrogen Emission spectrum
a) Describe the emission spectrum of a hydrogen discharge tube b) Explain why different color lines appeared in different position in the spectrum. Use a suitable atomic model to help construct your answer. c) Explain how do you decide if the lines observed are of the first ...
Monday, November 8, 2010 at 7:10pm by Farah

Emission Spectrum of hydrogen ...CHEM
Can someone please explain the emissiom spectrum of hydrogen? THose lines represent the energy released by the electron when going from one orbital (energy level) to a lower orbital. The difference of energy levels exactly corresponds to the energy in the light photon.
Saturday, May 12, 2007 at 8:09pm by Pet

CHEMISTRY
In the emission spectrum of hydrogen what is the wavelength of the light emitted by the transition fro m n = 4 to n =2.
Wednesday, April 13, 2011 at 1:15am by HELP

Chemistry
What are the wavelengths, in nanometers, of the bright lines of the hydrogen emission spectrum corresponding to the transition: n=5 to n=2.
Saturday, October 22, 2011 at 10:13pm by Anonymous

Physics - Hydrogen discharge tube
a) Describe the emission spectrum of a hydrogen discharge tube b) Explain why different color lines appeared in different position in the spectrum. Use a suitable atomic model to help construct your answer. c) Explain how do you decide if the lines observed are of the first ...
Monday, November 8, 2010 at 5:22am by Farah

chemistry
What are emission spectra? Is it correct to say . The pattern of spectral emission lines produced by an element.Each element has his own unique emission spectrum. What do you think?
Thursday, November 10, 2011 at 7:08pm by mike

chem
what colored lines are expected in the atomic emission spectrum for mercury?
Monday, April 14, 2008 at 8:12pm by natash

physics
The ionisation potential of atomic hydrogen is 13.6 eV. A strong emission line in the spectrum of atomic hydrogen occurs at a wavelength of 121.6 nm. Deduce the initial and final values of the quantum number n for this spectral line.
Tuesday, May 17, 2011 at 11:25am by Olivia

Chemistry
Considering the emission of the hydrogen atom, a. what is the wavelength of the light emitted by the transition from n = 2 to n = 1. b. In what region of the electromagnetic spectrum does this radiation belong?
Thursday, May 19, 2011 at 12:20am by Shell

chemistry
The problem you posted doesn't say. If the original problem (the one from which you obtained your question) doesn't say, it doesn't matter. The only difference is that the emission spectrum is a photograph (negative) of dark lines against a white background. The absorption ...
Monday, November 9, 2009 at 8:08pm by DrBob222

Chemistry
Distinguish between an absorption spectrum and an emission spectrum.with which did bohr work?
Friday, June 8, 2012 at 2:53pm by Yeneta

Chemistry
I like part of it. I have bolded the change I would make. Feel free to change it to your writing style if you wish. By the way, the emitted spectrum MAY be in the visible spectrum but it may also be in the ultraviolet, infrared, x-ray region, etc etc. When the electrons in the...
Tuesday, November 6, 2007 at 9:25pm by DrBob222

chem
determine the wavelength of the line in the emission spectrum produced by an electron transition He+ from ni= 4 to nf= 2.
Wednesday, April 6, 2011 at 1:36am by james

Chem
What is the wavelength of the transition from n=4 to n=3 for Li2+? In what region of the spectrum does this emission occur? Li2+ is a hydrogen-like ion. Such an ion has a nucleus of charge +Ze and a single electron outside this nucleus. The energy levels of the ion are -Z^2RH/...
Saturday, November 3, 2007 at 9:08pm by Lauren

Chemistry
calculate the wavelength of the second line in the Brackett series (nf=4) of the hydrogen emission spectrum. Rh= 2.180e-18 any help please? i know its energy levels 4 to 6... but that is all.
Monday, September 24, 2007 at 2:18pm by Lily

chem
The hydrogen emission spectrum has four series (or sets) of lines named Balmer, Brackett, Paschen, and Lyman. Indicate the energy (infrared, ultraviolet, or visible), the nf value for each series, and all possible ni values up to 7. ( Separate the values with commas from ...
Thursday, January 14, 2010 at 7:13pm by Sunny

chemistry
In the emission spectrum of hydrogen, some lines are in the infra red range. h l Suggest an electron transition (specify n and n) that is in this range and calculate its corresponding wavelength and delta E.
Monday, November 15, 2010 at 11:33am by help

CHEMISTRY
Why is the atomic emission spectrum of hydrogen composed of lines? What does each line indicate? Why do the lines become closer together from left to right in a typical diagram?
Tuesday, November 5, 2013 at 8:47pm by michelle

chemistry
Is it correct to say . The pattern of spectral emission lines produced by an element.Each element has his own unique emission spectrum. What do you think?
Thursday, November 10, 2011 at 6:25pm by mike

Chemistry
A gas in a discharge tube consists entirely of ions of the same element, of the same charge. Each ion has only one remaining electron. The voltage between the electrodes of the gas discharge tube is increased from zero. Electrons are accelerated across the potential, and then ...
Friday, March 22, 2013 at 7:38pm by Sam Chem

physics
What difference does an astronomer see between the emission spectrum of an element in a receding star and a spectrum of the same element in the lab?
Saturday, May 3, 2008 at 10:49pm by Kim

Chemistry
what is the emission spectrum of the sun and what does this spectrum reveal about the types of elements in the sun?
Saturday, October 27, 2007 at 12:55pm by Alison

11th grade Physics
Difference between Atomic spectrum and emission spectrum. First give me the clear cut definition of both and then the difference!!!
Saturday, July 24, 2010 at 2:28pm by Akashdeep Singh

chemistry
A gas in a discharge tube consists entirely of ions of the same element, of the same charge. Each ion has only one remaining electron. The voltage between the electrodes of the gas discharge tube is increased from zero. Electrons are accelerated across the potential, and then ...
Saturday, March 23, 2013 at 3:07pm by schoolgirl

inorganic chermistry
a large number of hydrogen atoms have electrons excited to the n_h=4 state.How many possible spectral lines can appear in the emission spectrum as a results of the electron reaching the ground state(n_1=1)?
Monday, August 30, 2010 at 4:23am by kabelo

chemistry
The hydrogen emission spectrum has four series (or sets) of lines named Balmer, Brackett, Paschen, and Lyman. Indicate the energy (infrared, ultraviolet, or visible), the nf value for each series, and all possible ni values up to 7
Monday, January 11, 2010 at 8:31pm by tea

science
Why is the helium spectrum have so many more lines than the hydrogen spectrum?
Wednesday, November 30, 2011 at 7:10am by hewitt

Chemistry
The hydrogen atomic emission spectrum includes a UV line with a wavelength of 92.3 nm. Is this line associated with a transition between different excited states or between an excited state and the ground state? What is the value of n1 of this transition? What is the ...
Saturday, October 22, 2011 at 10:28pm by Anonymous

Chemistry
I found this but wasn't sure how accurate is was: 4.) There is a major effect of the nitrate ion in solution on the color emission because the nitrate ion is the oxidizing agent in the compound without it you could not produce a spectrum so there would not be an emission of ...
Tuesday, December 16, 2008 at 8:34pm by Steff

astronomy
on a domestic gas cooker the temperture in the hottest part of the flame is about 2200k.if salty eater is spilled in the flame then it becomes yellow-orange.measurements with a spectrometer show the presence of an emission line at 589n. 1) the solar spectrum shows an ...
Monday, March 3, 2008 at 4:11pm by amy21

chemistry ------ flame test-------------
Did the nitrate ion effect the color emission of the solution ? how did you decide ? my answer: No , because The nitrate ion is the oxidizing agent in the compound without it you could not burn the chemicals and you could not produce a spectrum so there would be no emission ...
Thursday, October 11, 2012 at 12:12am by Maria

Cosmology
Which type of emission closely traces the star-forming regions of a galaxy? none of these coronal X-ray emission 21 cm emission molecular CO emission
Friday, March 1, 2013 at 7:54am by C

Chemistry
Atoms of ionized lithium gas (Li2+) are struck by neutrons moving at a velocity of 1.46e5 m/s. Calculate the shortest wavelength in the emission spectrum of Li2+ under these circumstances. You can assume that all electrons start in the ground state.
Friday, March 22, 2013 at 7:48pm by Sam Chem

Astronomy
Which type of emission closely traces the star-forming regions of a galaxy? - molecular CO emission - coronal X-ray emission - 21 cm emission - none of these
Friday, March 1, 2013 at 2:18am by qwerty

Chemistry
What is the wavelength of the transition from n=4 to n=3 for Li2+? In what region of the spectrum does this emission occur? Li2+ is a hydrogen-like ion. Such an ion has a nucleus of charge +Ze and a single electron outside this nucleus. The energy levels of the ion are -Z^2RH/...
Saturday, November 3, 2007 at 6:33pm by Lauren

chemistry
yes, it's all about emission spectrum..
Thursday, September 15, 2011 at 4:52pm by grace

Chemistry
What is the wavelength of the transition from n=4 to n=3 for Li2+? In what region of the spectrum does this emission occur? Li2+ is a hydrogen-like ion. Such an ion has a nucleus of charge +Ze and a single electron outside this nucleus. The energy levels of the ion are -Z^2RH/...
Sunday, November 4, 2007 at 11:22am by Lauren

Chem
A line in the hydrogen atomic line spectrum has a wavelength of 486 nm. What is the frequency of this light (in Hz)?
Sunday, July 17, 2011 at 9:31pm by Sam

Physics
If the electron in a hydrogen atom obeyed classical mechanics instead of quantum mechanics, would it emit a continuous spectrum or a line spectrum?
Thursday, April 10, 2008 at 8:59pm by Kara

chemistry
The hydrogen emission spectrum has four series (or sets) of lines named Balmer, Brackett, Paschen, and Lyman. Indicate the energy (infrared, ultraviolet, or visible), the nf value for each series, and all possible ni values up to 7. ( Separate the values with commas from ...
Thursday, January 14, 2010 at 7:14pm by Sunny

chemistry
According to the Bohr model of the hydrogen atom, how is hydrogen's bright line spectrum produced?
Tuesday, October 27, 2009 at 7:39pm by ryan

Physics
An emission spectrum will be produced. Some, but not all, of the radiation emitted will be visible.
Tuesday, March 6, 2012 at 12:33am by drwls

CHEM 1LB
Complete the table below: The hydrogen emission spectrum has four series (or sets) of lines named Balmer, Brackett, Paschen, and Lyman. Indicate the energy (infrared, ultraviolet, or visible), the nf value for each series, and all possible ni values up to 7. ( Separate the ...
Sunday, January 17, 2010 at 4:51pm by Anonymous

Chemistry
A gas in a discharge tube consists entirely of ions of the same element, of the same charge. Each ion has only one remaining electron. The voltage between the electrodes of the gas discharge tube is increased from zero. Electrons are accelerated across the potential, and then ...
Monday, March 25, 2013 at 1:46am by Chemq

science
What happens is that a single electron changes its orbit. In an emission spectrum, an electron makes a transition from a higher to a lower energy state, causing a photon to be emitted at a particular frequency. In a very hot gas, many transitions of this type are going on ...
Thursday, June 9, 2011 at 7:37pm by drwls

Chem.
λ for one line of the hydrogen spectrum is .4118 x 10-4 cm. Use this value in the Rydberg equation to calculate the RH value using n1 = 2, and n2 = 6.
Tuesday, October 26, 2010 at 9:26pm by Toni

chemistry
The spectrum of an element consists of a series of wavelengths (colors in the visible spectrum but there are wavelengths in the ultraviolet and infrared regions, also) that are emitted by the excited atom(s) of the element. In practice, the wavelengths are sent through an ...
Monday, November 9, 2009 at 8:08pm by DrBob222

Chemistry
Explain the production of an emission spectrum in terms of the energy states of an electron. what does that mean someone help me please.
Tuesday, November 6, 2007 at 9:25pm by John

chem
λ for one line of the hydrogen spectrum is .4118 x 10-4 cm. Use this value in the Rydberg equation to calculate the RH value using n1 = 2, and n2 = 5. change the line spectrum to meters you know the equation is Et= Ef-Ei (i think is the equation they want you to use, i ...
Monday, October 2, 2006 at 8:12pm by Mary

chemistry
A-alpha emission B-Positron emission C-electron capture D-beta emission
Sunday, June 26, 2011 at 7:43pm by mali

O chem
comment on suitability of running infared spectrum under the following conditions: A neat spectrum of liquid with a boiling point of 150 C is determined with salt plates. and same question but at 35 C
Tuesday, September 18, 2012 at 10:06pm by MELISSA

chemistry
What is the wavelength of the transition from n = 2 to n = 1 for Li2+? Li2+ is a hydrogen-like ion. Such an ion has a nucleus of charge +Ze and a single electron outside this nucleus. The energy levels of the ion are -Z2RH/n2, where Z is the atomic number. nm In what region of...
Sunday, November 7, 2010 at 6:03pm by Emily

chemistry
The red line in the Helium spectrum is longer than the red line in the hydrogen spectrum. What does that tell us about the distance between n2 and n3 in helium as compared with the distance between n2 and n3 in hydrogen?
Monday, November 15, 2010 at 11:34am by help

Science
What type of spectrum are you talking about? Reflection from the solid? Intrared transmission? Visible or ultraviolet transmission of aqueous solution? Flame emission spectroscopy? Atomic absorption spectrometry? What do you mean by "reacted with fire?" In the flame emission ...
Wednesday, May 28, 2008 at 12:08am by drwls

Physics-Astronomy
Hello, I have no idea how to do the following question. Any help would be appreciated: An energy of at least 13.6 electron-volts is required to ionise a hydrogen atom. What is the longest wavelength of electromagnetic wave capable of ionising hydrogen? And which regions of the...
Monday, November 16, 2009 at 10:51am by Mark

Physics
A transmission diffraction grating with 600 lines/mm is used to study the line spectrum of the light produced by a hydrogen discharge tube with the setup shown above. The grating is 1.0 m from the source (a hole at the center of the meter stick). An observer sees the first-...
Friday, September 16, 2011 at 8:05am by AfterLife

science
for the emission spectrum of Be3+, calculate the lowest wavenumber νˉ (in inverse meters) of light produced by electron transitions between n=2, n=3, and n=4.
Friday, November 16, 2012 at 6:35am by lef

chemistry
For the emission spectrum of Be3+, calculate the lowest wavenumber νˉ (in inverse meters) of light produced by electron transitions between n=2, n=3, and n=4.
Saturday, November 17, 2012 at 5:44am by Anonymous

chemistry
For the emission spectrum of Be3+, calculate the lowest wavenumber νˉ (in inverse meters) of light produced by electron transitions between n=2, n=3, and n=4.
Saturday, November 17, 2012 at 8:30am by amar chauhan

chem
can anyone help me with this question what is the advantages and disadvantages of hydrogen power as opposed to hydrogen fuel, also what is the equation for hydrogen feul? I do not understand your first question. Hydrogen power REQUIRES hydrogen fuel. Hydrogen fuel is H2; ...
Saturday, March 3, 2007 at 12:41pm by ana

college-- chemistry
I got stuck on this problem and I cannot figure out what to do or explain this problem. Please help me with this problem. The emission lines of one-electron atoms and ions can all be fit to the equation describing the spectrum of the hydrogen atom: E= -(2.18X10^-18J)Z^2(1/n^...
Monday, February 16, 2009 at 3:26am by shylo

chemistry 1
How do you write balanced equations A. Neutron emission by 88Br B. Electron absorption by 116Sb C. Positron emission by 184Hg D. Alpha emission by 229Th E. Neutron capture by 200Hg
Friday, October 25, 2013 at 10:56am by Alexus

Chemistry
1. If all you are doing is identifying meal ions, the contamination of the HCl with Al will not affect the results at all UNLESS the Al energy overlaps one of those from the unknown. Why? Because it takes a certain amount of energy for the Al lines to appear and it takes A ...
Sunday, February 16, 2014 at 9:25pm by DrBob222

chem lab
ok I'm having trouble with graphing this chemistry lab. It's on atomic emission spectra. In this experiment we observed the line spectrum of first helium, and here is the data: color: distance: wavelenght: violet 20.35cm light blue 21.70cm green 23.08cm light green 22.75cm ...
Monday, April 28, 2008 at 12:46am by natash

chemistry
An electron of wavelength 1.74*10-10m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
Saturday, March 23, 2013 at 6:01am by Maikol

chemistry
An electron of wavelength 1.74*10-10m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
Monday, March 25, 2013 at 1:01am by James

chemistry
An electron of wavelength 1.74*10-10m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
Monday, March 25, 2013 at 1:01am by James

chemistry
in emission spectrum which one has a highest frequency and highest energy is it blue red or violet? which one is the lowest?
Thursday, September 15, 2011 at 5:02pm by grace

Physical Chemistry
An electron of wavelength 1.74*10-10m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
Saturday, March 23, 2013 at 9:04am by Echoes

chemistry
E = h*frequency. High frequency means high energy. I don't know how that fits into a discussion of elements unless you are talking about their emission spectrum.
Thursday, September 15, 2011 at 4:52pm by DrBob222

Chemistry
For the emission spectrum of Be3+, calculate the lowest wavenumber νˉ (in inverse meters) of light produced by electron transitions between n=2, n=3, and n=4. I don't want to know the answer, just tell me wat method I need to use to get there... Pls x
Sunday, November 18, 2012 at 9:06am by Anonymous

Chemistry NMR
the spectrum didn't turn out but peak one 2 hydrogen approx 4.10 ppm peak two 1 hydrogen approx 2.00 ppm peak three 3 hydrogen approx 1.10 ppm
Monday, March 29, 2010 at 4:19pm by Andy

chemistry
An emission spectrum is formed when electrons from an excited atom move to lower energy levels. That energy they absorbed in the first place (to become excited) is emitted.
Thursday, November 10, 2011 at 6:25pm by DrBob222

chemistry
For all deexcitations that result in the visible spectrum of hydrogen, what is n ?
Monday, November 15, 2010 at 1:18pm by help

CHEMISTRY
I don't think it's a matter of which ions are excited versus those that are not as much as it is the color. Atoms/ions that are used in flame emission are there primarily for three reasons: 1. They are easily volatilized in a flame and 2. They emit energy that places the ...
Sunday, October 27, 2013 at 1:41pm by DrBob222

Chemistry hW
For the emission spectrum of Be3+, calculate the lowest wavenumber νˉ (in inverse meters) of light produced by electron transitions between n=2, n=3, and n=4. I don't want to know the answer... Just tell me what I would need to do to work it out :) pls?? X
Sunday, November 18, 2012 at 9:01am by Anonymous

Physics
You cannot get the flame temperature from that observation. You do not have blackbody continuum emission, which would be required to get a temperature from the spectrum. The wavelengths that you observe depends upon the emitting species, which happen to be trace amounts of C2 ...
Friday, October 21, 2011 at 3:11pm by drwls

Chemistry
How do I calculate the wavelength of the emission line when electrons drop from the 4th to the 3rd energy level in the hydrogen atom?
Wednesday, February 9, 2011 at 12:29am by Lis

Chemistry
A line in the Lyman series of the hydrogen atom emission results from the transition of an electron from the n=3 level to the ground state level. a) What n level (#) is the ground state level for the hydrogen atom? b) What is the energy of this photon in Joules?
Sunday, July 17, 2011 at 9:32pm by Ashley

Chemistry
is this a good answer? When the electrons in the element are excited they jump to higher energy level and as the electrons fall back down it leave the excited state energy which is re-emitted, the wavelength of which is the emission spectrum.
Tuesday, November 6, 2007 at 9:25pm by John

Chemistry 151
Of the following transitions in the Bohr hydrogen atom, the ____ transition results in the emission of the highest-energy photon. a.n=1, n=6 b.n=6, n=1 c.n=6,n=3 d.n=3,n=6 e.n=1,n=4
Monday, November 8, 2010 at 6:49pm by Jessica

chemistry
Atoms of ionized lithium gas (Li2+) are struck by neutrons moving at a velocity of 1.46e5 m/s. Calculate the shortest wavelength in the emission spectrum of Li2+ under these circumstances. You can assume that all electrons start in the ground state. Enter the wavelength in m:
Saturday, March 23, 2013 at 3:58pm by schoolgirl

physics
The wave theory also does not sccount for spontaneous emission and induced emission (which are needed to explain gaseous emission and laser amplification). The wave theory also cannot explain "shot noise" in light measurements, which is caused by statistcal fluctuations in ...
Sunday, February 1, 2009 at 6:39am by drwls

Chemistry Lab
Complete the table below: The hydrogen emission spectrum has four series (or sets) of lines named Balmer, Brackett, Paschen, and Lyman. Indicate the energy (infrared, ultraviolet, or visible), the nf value for each series, and all possible ni values up to 7. ( Separate the ...
Monday, January 17, 2011 at 6:29pm by Shawn Tabrizi

Chemistry
In the spectrum of a specific element, there is a line with a wavelength of 656 nm. Use the Rydberg equation to calculate the value of n for the higher energy Bohr orbit involved in the emission of this light. Assume the value for the lower energy orbit equals 2.
Monday, March 31, 2014 at 2:35am by James

Chemistry
What is the frequency of the photons emitted by the hydrogen atoms when they undergo transitions from n=5 to n=3? In which region of the electromagnetic spectrum does this radiation occur?
Saturday, October 22, 2011 at 10:14pm by Anonymous

chem
why are the atomic emission line spectra different for each element?
Monday, April 14, 2008 at 8:11pm by natash

chem
Im not sure what your question is but are you wondering the concentation of Hydrogen in a polyatomic ion of Hydrogen?
Thursday, December 18, 2008 at 8:39pm by Tom from Mississippi

Chemistry
Atoms usually exist in their "so-called" ground state; i.e., the lowest energy. When an atom is placed in a flame, the energy from the flame is enough to make an outer electron (say from a Na atom) move from the 3s level to a higher energy level. After a short period of time ...
Tuesday, September 17, 2013 at 8:52pm by DrBob222

Chemistry
A line in the Lyman series of the hydrogen atom emission results from the transition of an electron from the n=3 level to the ground state level. a) What n level (#) is the ground state level for the hydrogen atom? b) What is the energy of this photon in Joules? c) What is the...
Monday, July 18, 2011 at 12:49am by Ashley

Chemistry
What is the wavelength of the electromagnetic radiation emitted from a hydrogen atom when the electron undergoes the transition n = 5 to n = 3?((Broken Link Removed) is a spectrum m In what region of the spectrum does the line occur? near ultraviolet far ultraviolet near ...
Friday, June 10, 2011 at 8:17pm by Lance

chemistry
Calulate the wavelengths (in nm) of the visible lines in the line spectrum of hydrogen using the Rydberg equation (nf = 2; ni = 3, 4, 5, and 6).
Tuesday, November 10, 2009 at 1:03pm by Jim

Chemisty
Consider a hydrogen atom that goes from the n = 2 to the n = 1 state. (a) Calculate the wavelength, in nm, of the photon emitted. (b) What part of the electromagnetic spectrum is it?
Tuesday, September 20, 2011 at 8:28pm by Pamela

chem lab
I'm doing a lab on helium and hydrogen emission spectra. so I got violet 20.35cm blue/green 21.70cm green 22.75 light green 23.08 yellow 27.70 red 31.70 faint red 33.95 and I also have the wavelenghts for helium spectra, its given. like for ex. violet is 380-420, my question ...
Monday, April 28, 2008 at 7:16pm by natash

chem
In the explosion of a hydrogen-filled balloon, 0.54 g of hydrogen reacted with 6.6 g of oxygen to form how many grams of water vapor?
Monday, October 4, 2010 at 7:32pm by jeff

Chemistry
We did a flame test today to see what substances produce what colors when burned. Can you please explain... Why each of the different elements have a different atomic emission spectrum? Would the flame tests be useful for detecting individual elements present in a mixture of ...
Tuesday, September 17, 2013 at 8:52pm by Sarah

general chemistry
The red line in the hydrogen line spectrum corresponds to to which electron transition?
Thursday, March 11, 2010 at 10:39am by Max

Physical Science Question 2
What is the electromagnetic spectrum? Give examples of each kind of wave and relate each example to its relative position in the spectrum. I will be happy to critique your thinking on this. The following 2 sites will answer all your questions. http://www.geo.mtu.edu/rs/back/...
Tuesday, June 20, 2006 at 10:14am by Liz

chem
λ for one line of the hydrogen spectrum is .4118 x 10-4 cm. Use this value in the Rydberg equation to calculate the RH value using n1 = 2, and n2 = 5. I am not certain of your difficulty here. Can you amplify? How did you make the symbol for lamda? (1/lambda) = R(1/n1^2...
Monday, October 2, 2006 at 8:12pm by Mary

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