Atoms and Electromagnetic Spectra

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Questions

• Question #ce8f3
• Question #a7afa
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• Question #f270b
• Why do elements emit colors when heated?
• Why is the electromagnetic spectrum continuous?
• Why is the electromagnetic spectrum a transverse wave?
• Why are atomic spectra of an element discontinuous?
• Why is the electromagnetic spectrum important?
• Why do atomic spectra appear as lines?
• What is the electromagnetic spectrum used for?
• What can I see on the electromagnetic spectrum?
• How is atomic emission spectrum related to flame tests?
• How does electromagnetic spectrum work?
• How does the electromagnetic spectrum affect humans?
• How does the electromagnetic spectrum affect photosynthesis?
• How do atomic spectra work?
• How do I get atomic emission spectra?
• How do scientists use atomic spectra?
• How could atomic spectra be useful to an astronomer?
• How can atomic spectra be used to identify elements?
• How can atomic emission spectra be useful?
• How are atomic spectra used?
• What is an example of converging energy?
• What are some examples of atomic spectra?
• Why is spectroscopy important to astronomers?
• Question #97b7c
• You can identify a gas by passing electricity through it. True or false?
• Question #2be7f
• What are the spectral series we see in the Hydrogen atom emission spectrum?
• Question #83c0d
• What is Balmer Series ???
• What causes the emission of radiant energy that produces characteristics spectral lines?
• Using Rydberg's equation for the energy levels (E = -R/n^2) and the wavelength and the c=(lambda)v, E=hv equations, SHOW/ PROVE how E(red band in H-spectrum, lambda = 656 nm) = (Delta or change/ difference) E (3 --> 2)?
• A photon on a hydrogen atom excited an electron from #n = 1# to make a transition to #n=3#. What is the wavelength (in run) pertaining to this transition and was the transition emitting or absorbing in nature?
• What happens to an electron during an absorption process?
• Question #506c8
• Question #20ecb
• How would you compare and contrast the continuous spectrum and emission spectrum?
• What is emission line spectrum?
• What is line emission spectrum?
• What is the reason behind hydrogen's line emission spectrum?
• How do colored spectral emission lines relate to frequency?
• How do electrons create colors in a line-emission spectrum?
• How does line emission spectrum work?
• How does the line emission spectrum of an element relate to these flame tests?
• How is a line emission spectrum created?
• How is line emission spectrum produced?
• Why is line emission spectrum so special?
• How would you explain the hydrogen spectrum?
• Why is there a hydrogen emission spectrum?
• Why is hydrogen atomic spectrum a line spectrum?
• How are the lines in a hydrogen spectrum obtained?
• How do you read the hydrogen NMR spectrum?
• Why does the hydrogen spectrum have four lines?
• Why is the spectrum of helium different from that of hydrogen?
• What are the wavelengths of x-rays and gamma rays?
• Question #aa1e9
• Question #d0cfc
• When an electron jumps from a high energy state to a lower state, what form does the emitted energy take?
• How does an atomic spectrum get affected by external electromagnetic fields?
• How many silver atoms are there in 3.84 g of silver?
• What wavelength of light will be emitted from a hydrogen atom for an electron that falls from n = 5 to n = 2 ?
• Question #19476
• Question #1ecbb
• Why does hydrogen give large number of spectral lines despite having only one electron?
• What type of compounds cannot be detected using infrared spectroscopy and why?
• What does the spectra of atoms reveal?
• If light of frequency #6.90 xx 10^14 "s"^(-1)# is emitted when an electron in hydrogen atom relaxes from #n_1 = 5#, what is #n_2#?
• Where is visible light located on the electromagnetic spectrum?
• Question #90211
• What is the difference between the Rydberg constants #R_H = "109678.77 cm"^(-1)# and #R_(oo) = "109737.32 cm"^(-1)#?
• Light is a mixture of all visible wavelengths of what spectrum?
• What is the difference between the Rydberg constants #R_H = "109678.77 cm"^(-1)# and #R_(H) = 2.18 xx 10^(-18) "J"#?
• Which Rydberg constant should be used for hydrogen atom? #"109737.32 cm"^(-1)# or #"109678.77 cm"^(-1)#?
• Is the energy of the photon coming in greater than or less than the energy of the electronic transition?
• What is #"AAS"#....?
• What transition energy corresponds to an absorption line at 460 nm?
• How do you determine which of these hydrogen atom energy transitions has the highest energy difference? Isn't it #(4)# since it is the odd one out?
• Question #3f808
• Balmer series says transitions from n ≥ 3 to n = 2 as n= 2 is the ground state ? how Hydrogen atom electron gain energy from level 2 to higher levels as normally H electrons in level n = 1 ?
• Question #0d50a
• Question #827e8
• Question #eb892
• Do helium and lithium both give emission spectra?
• Question #27e1c
• Only we can calculate the energy emitted when #n_x rarr n_t#only in the hydrogen atom not in any other atom. When will be the new equation which can apply to all atoms found in the future?????
• Question #db2ec
• Question #7cbdc
• What is an EM spectrum?
• What is the total energy needed to see all 15 spectral lines for the electronic transitions involving #n = 1# up to and including #n = 6#, assuming every transition occurs only once? What wavelength is needed to cause this in angstroms?
• The line spectrum for element X includes a band of green light of wavelength 522 nm. This band corresponds to what energy transition within an atom of element X? Let Planck’s constant h = 4.136 × 10−15 eV ∙ s, and the speed of light c = 3.00 × 108 m/s.
• Hot objects with temperatures of 10 million Kelvin give off most of their radiation in which part of the electromagnetic spectrum?
• How do you calculate the ionization energy of a hydrogen atom in its ground state?
• What is the ionization potential for an electron going from #n = 2# to #n = 3# in #"eV"# for hydrogen atom?
• A stationary #He^+# ion emitted a photon corresponding to a first line of the Lyman series. The photon liberated a photoelectron from a stationary H atom in the ground state. What is the velocity of the photoelectron?
• Question #2ab5b
• Question #d1d52
• What is the wavelength of light that causes an electronic transition for #"Li"^(2+)# if #n_f - n_i = 2# and #n_i + n_f = 4#?
• Explain why #Gd^(3+)# is colorless?
• What is the frequency of limiting line in Balmer series?
• How much energy is released when #"1 mol"# of hydrogen atoms transition from #n=3# to #n=2#?
• Question #fc63c
• Question #2e787
• What will be the ratio of the wavelength of the first line to that of the second line of paschen series of H atom? A)256:175 B)175:256 C)15:16 D)24:27
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• Question #db4d1
• In a sample of excited hydrogen atoms electrons make transition from n = 3 to n = 1 and emitted photons strike on a metal of work function 6.08 eV. The maximum kinetic energy of the ejected electron in the process will be?
• Question #03297
• Question #79130
• For the Lyman series, #n_f = 1#. How can we calculate the #E_"photon"# for the bandhead of the Lyman series (the transition #n = oo -> n = 1# for emission) in joules and in eV?
• Question #5da42
• An electron changes from an #n = 2# to an #n = 6# energy state. What is the energy of the photon in joules?