16. The problems below may prioritize rote fundamentals, but facility with conversion between frequency, wavelength, and energy is one of the more useful tools you can take with you from a spectroscopy class. Determine the energy (in kJ/mol) of the following: (a) light having a frequency of 250 MHz (b) light having a wavelength of 810 nm (c) light having a wavenumber of 3000 cm³¹
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- 1. (a) Briefly explain why IR spectroscopic data is reported in wavenumbers and not absorbance or transmittance? (b) True or False: The energy released by an excited fluorescent material is immediately released after exposure to the light source.7. What is the wavenumber of an infrared photon whose wavelength is 100 μm? a) 1 cm¹ b) 10 cm-¹ c) 100 cm-¹ d) 100 cm-¹ e) 1000 cm¹ 8. Consider the energy level diagram shown at the right, which represents several light absorption and emission transitions. Which arrow represents the transition emitting light with the greater frequency? a) A b) B c) C d) D e) E 9. Consider the energy level diagram shown at the right, which represents several light absorption and emission transitions. Which arrow represents the transition absorbing light with the lowest frequency? a) A b) B c) C d) D e) E 10. Photoluminescence is a term describing the emission of light by atoms or molecules that have been excited by energy. a) chemical b) electrical c) electromagnetic d) thermal e) any of these 11. Which of the equalities below is the definition of the property "absorbance"? a) A = abc b) A = Ebc c) A = -log T d) all of these e) none of these 12. Under certain conditions the transmittance of a sample is…(1) Why don't we observe the transition from na > ni for the hydrogen atom in the line spectrum? Be specific. 4000 300 3000 2500 2000 1500 1000 s00 300 350 400 450 800 550 700 750 800 Wavelength anometera) (2) An emission spectrum for a red laser pointer is shown above. Calculate the energy associated with the red laser pointer. (3) Draw an emission spectrum to represent light emitted by a blue laser. (qunao Ag
- Calculate the frequency of visible light having a wavelength of 486 nm. ( Answer in s-1, to 3 sig figs. )(a) Prove the relationship between the absorbance and concentration in Beer Lambert's law. What is the absorbance (A) of a sample if the transmittance (T) is 0.347?Wave [Select] has the shortest wavelength. This means that in relation to the other waves, it has the: [Select] associated with it. [Select] frequency. [Select] B [ Select] wavenumber. ♦ î energy period.
- 5) Given the absorbance spectrum shown below, what wavelength of light would you use for nickel(II) ion? Explain your answer. Absorbance 0.8 0.6 0.4 1 0.2 0 350 400 Absorbance vs. Wavelength for Nickel(II) ion 450 500 550 600 650 Wavelength (nm) 700 750 800 850Q/ An electron in a hydrogen atom undergoes the transitiondepicted to the right. Calculate the wavelength (in nm),frequency (in Hz), and energy (in J) of the photon emitteddue to the relaxation of the electron. Report each value tothree significant figures. Show all work.Atomic absorption spectrophotometry is a method for the quantitative determination of metal ions. a) Describe in detail the AAS instrument and especially the parts that differ from a normal spectrophotometer. b) What light source is used in this technology and how does it work? c) What interferences can occur with this equipment? d) What is the theoretical basis of the AAS method?
- (1)Draw a ground state energy level diagram for a silicon atom that shows where all of the electrons would be (n, L, ml and show spin up or spin down with an arrow). (2) Determine the values of L and S for the ground state using Hund's rule. (3) For chlorine, repeat steps 1 and 2.Which of the following statements concerning spectroscopy is correct? A) Concentration of a solution is directly proportional to the % of photons transmitted. B) Salt plates are often used in IR spectroscopic measurements because they are transparent in that region. C) Molar absorptivity is a constant for given species, regardless of concentration or wavelength. D) Fluorescence excitation is usually red-shifted from emission wavelength. E) 2 or more statements are correct. The absorbed energy to enable vibrational level transition falls within which wavelength range A) radio wave B) microwave C) IR D) X-ray E) UV and visibleGive typed full explanation not a single word hand written otherwise leave it Which of the following statements are 'correct' regarding the fluorescence and phosphorescence emission processes commonly used in spectroscopy? I- Fluorescence and phosphorescence events are important emission processes that occur after the excitation of atoms or molecules with a thermal or chemical energy. II. In the photoluminescence processes called fluorescence and phosphorescence, a ray-excited species returns to its ground state by releasing its extra energy in the form of photons. III-If gaseous atoms are excited with any energy, the atom emits a beam with the wavelength that characterizes it, and makes fluorescent radiation. IV. It is possible for a light-excited atom or molecule to return to a lower energy level or ground state by heat transfer by collisions without emitting any rays. A. IandIII B. IandII C. II and IV D. Il and III