Why are emission and absorption spectra of molecules so much broader than atomic emission and absorption...
Why are emission and absorption spectra of molecules so much broader than atomic emission and absorption spectra? [HINT: Think about a molecular spectrum (like measuring the absorbance of quinine) vs analyzing calcium on an AAS.]
Homework Answers
Answer. Because in case of molecules the probalitiy distribution of electron density is larger in comparison to singly localized electronic distribution of a single element. The large electronic distribution lead to overlap the spectra coming from different electrons and gives a broader peak while in case of an element due to fixed location of electron density it gives much sharper peak.
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Why are emission and absorption spectra of molecules so much
broader than atomic emission and absorption...
Which of these might be responsible for why a moleculer metal salt spectra is broader than...
Which of these might be responsible for why a moleculer metal
salt spectra is broader than a hydrogen atomic spectra? More than
one may apply.
Overlapping bands caused by multiple transitions Additional ions formed in the flame More energy from the flame causing more emission Additional molecular species formed in the flame The electrons transition between levels faster in the hydrgen lamp Additional metals formed in the flame
why do molecular salts, (NaCl) for example, have broader bands of spectra compared to a simple...
why do molecular salts, (NaCl) for example, have broader bands of spectra compared to a simple atomic spectra like hydrogen??
in atomic spectroscopy the spectral absorption and emission lines are very narrow. why are they more...
in atomic spectroscopy the spectral absorption and emission lines are very narrow. why are they more narrow then in molecular spectroscopy?
1.explain why there are more lines in the hydrogen emission spectrum than in the absorption spectrum?...
1.explain why there are more lines in the hydrogen emission spectrum than in the absorption spectrum? 2. indicate asborption, from a lower energy level to a higher energy level. Then indicate emission for the same transition as through various pathways, which would then result in many more emission peaks than there was in the original absorption (transition).
I was having trouble with some lab question on atomic emission spectra. Also answer the following...
I was having trouble with some lab question on atomic emission
spectra.
Also answer the following questions about your observations: Are the lines present in the hydrogen spectrum the same lines predicted by the Bohr model the atom? Which lines, if any, are missing? Why might there be lines missing? Compare the spectral lines from your unknown substance to the other spectra you observed. Based on these comparisons, what is the identity of the unknown substance? Are there any general...
Number 2. Thank you 2. (2pt) Why do atomic emission spectra come in the form of...
Number 2. Thank you
2. (2pt) Why do atomic emission spectra come in the form of lines instead of broad bands that span whole regions of the electromagnetic spectrum? Atoms have quantized energy Tevels, they react to principal quantum numbers n=1,2,..
Would atomic emission spectroscopy be a useful technique for determining the oxidation state of arsenic in...
Would atomic emission spectroscopy be a useful technique for determining the oxidation state of arsenic in a water sample? Why or why not? (Bonus, what would an analyst have to do to determine oxidation state? (otherwise referred to as "speciation")) List two reasons why the excitation bandwidth using a hollow cathode lamp is much narrower than the emission bandwidth for atomic spectroscopy? Use an equation in your answer (hint, think Doppler).
Which one of the following atomic spectroscopy method gives the smallest detection limit for ion Flame...
Which one of the following atomic spectroscopy method gives the smallest detection limit for ion Flame absorption b) electrothermal absorption c) flame emission d) ICP torch emission What kinds of spectroscopy instruments currently employ Fourier transform for the most rapid acquisition of a spectrum UV-vis and NMR b) IR and NMR c) NMR and MS d) MS and UV-vis e) IR and AA Which type of mass analyzer is used in the MS analysis of large molecules like proteins True...
Why do you think that the enthalpy of vaporization for water is so much larger than...
Why do you think that the enthalpy of vaporization for water is so much larger than the enthalpy of fusion? Hint: Think about intermolecular forces.
a) Why is the Li+ radius so much smaller than the radius of the neutral Li...
a) Why is the Li+ radius so much smaller than the radius of the neutral Li atom? b) Why is the F- radius so much larger than the neutral F atom? b) Which transition involves the emission of less energy in the H atom, an electron moving from n=4 to n=3 or an electron moving from n=3 to n=2?
Which of these might be responsible for why a moleculer metal
salt spectra is broader than a hydrogen atomic spectra? More than
one may apply.
Overlapping bands caused by multiple transitions Additional ions formed in the flame More energy from the flame causing more emission Additional molecular species formed in the flame The electrons transition between levels faster in the hydrgen lamp Additional metals formed in the flame
I was having trouble with some lab question on atomic emission
spectra.
Also answer the following questions about your observations: Are the lines present in the hydrogen spectrum the same lines predicted by the Bohr model the atom? Which lines, if any, are missing? Why might there be lines missing? Compare the spectral lines from your unknown substance to the other spectra you observed. Based on these comparisons, what is the identity of the unknown substance? Are there any general...
Number 2. Thank you
2. (2pt) Why do atomic emission spectra come in the form of lines instead of broad bands that span whole regions of the electromagnetic spectrum? Atoms have quantized energy Tevels, they react to principal quantum numbers n=1,2,..
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