UV-Visible (UV-Vis) is often called a general technique because most molecules will absorb in the UV-Vis wavelength range. The UV extends from 100-400 nm and the visible spectrum from 400–700 nm. The 100-200 nm range is called the deep UV. Light sources are more difficult to find for this range, so it is not routinely used for UV-Vis measurements. Typical UV-Vis spectrometers use a deuterium lamp for the UV that produces light from 170-375 nm and a tungsten filament lamp for visible, which produces light from 350-2,500 nm.
When a photon hits a molecule and is
absorbed, the molecule is promoted into a more excited energetic
state. UV-visible light has enough energy to promote electrons to a
higher electronic state, from the highest occupied molecular
orbital (HOMO) to the lowest unoccupied molecular orbital (LUMO).
The energy difference between the HOMO and the LUMO is called the
band gap. Typically, these orbitals are called bonding and
anti-bonding. The energy of the photon must exactly match the band
gap for the photon to be absorbed. Thus, molecules with different
chemical structures have different energy band gaps and different
absorption spectra. The most common transitions that fall in the
UV-Vis range are -
* and n-
*.
-orbitals arise due
to double bonds, and n-orbitals are for non-bonding electrons.
*
is anti-bonding
-orbitals. Thus, the
best UV-Vis absorption is by molecules that contain double bonds.
-orbitals adjacent
to each other that are connected, called conjugation, typically
increases absorption.
-
*
transitions, associated with single bonds, are higher energy and
fall in the deep UV, so they are less useful for routine use. The
appearance of broad bands or shoulders on the UV-Vis structure is
due to the numerous vibrational and rotational states of a
molecule, which lead to separate energy band gaps of slightly
different energies.
Hence, one will be able to use a UV absorption wavelength of 280 nm to quantitatively measure the amount of protein in a sample.
Why are we able to use a UV aborption wavelength of 280 nm to quantitatively measure the amount o...
Atmospheric ozone plays a UV-A (320-400 nm), UV-B (280-320 nm), and UV-C (200-280 nm). Unfortunately, human-caused pollution has eroded the ozone layer in the stratosphere, allowing a greater amount of ultraviolet radiation to reach the Earth's surface. The damaging effects of the radiation can be related to it's photon energy. Arrange the regions of UV radiation from overall lowest to highest photon energy. role in absorbing high-energy and damaging UV radiation, including Lowest Photon Energy Highest Photon Energy. Which region of...
(c) Tryptophan can absorb UV light around 280 nm and fluoresces around 355 nm. Explain why the fluoresced light is of a longer wavelength than the light absorbed. Include an energy level diagram to illustrate your answer. 14 marks
4. The H2 molecule absorbs UV radiation of wavelength 109 nm. What is the origin of this absorption, i.e. what transition does this absorption correspond to and what eneray (in kJ mol-1) is involved? Why does absorbing ultraviolet radiation of this wavelength cause H2 to sp respective atoms? lit into its
2. A wavelength of 650 nm was selected to measure the absorbance of CuSO4. Aqueous KMnO4, a purple solution, requires a wavelength of approximately 565 nm. Explain why different wavelengths of light are selected to measure the absorbance of KMnO4 and CuSO4 solutions.
The hydrogen atomic emission spectrum includes a UV line with a wavelength of 92.323 nm. Photons of this wavelength are emitted when the electron transitions to n_t = 1 as the final energy state. Is this line associated with a transition between different excited states or between an excited state and the ground state? different excited states between an excited state and the ground state What is the energy of the emitted photon with wavelength 92.323 nm? What was the...
1. (a) Why does buta-1,3-diene (max 217 nm) have a longer-wavelength (lower-energy) UV-Vis absorption peak as compared to ethene (max 171 nm)? Include an energy level diagram with your answer. (b) What would you expect to happen as you add on to this structure with additional double bonds? Hint: consider the total number of p atomic orbitals contributing to each molecule, as depicted below. ?-? Ethene Butadiene
The red light (wavelength = 630 nm) illuminates a cuvette at an incident angle of 30° with respect to the normal. The cuvette is made of glass (refractive index = 1.515) and some protein solution is inside the cuvette. At a specific protein solution, the refractive index of the solution is 1.34. If the protein concentration is increased, the refractive index of the solution gets higher. What physical parameter (e.g., angular change, distance change) can you measure to detect the...
I forgot to put down that the observance (=OD) at 280nm is
0.679A
Experiment 8: Bradford assay and UV-method for determination of protein concentrations Materials - An ice bucket with ice, your purified sample, three visible plastic cuvettes for Bradford assay, one UV plastic cuvette for UV-method, a piece of parafilm, a Vis-spec, a Lab Quest, Bradford reagent, white tape (share), a sharpie. Bradford assay (reference 21) 1. Add 990 uk Bradford assay reagent to a plastic cuvette 2. Blank...
Why is it a bad idea to use polystyrene cuvettes when making UV absorbance measurements in the 200-300 nm range? Choose one. a. Polystyrene will be attached by acid. b. Polystyrene absorbs a lot of light in this range. c. Polystyrene might react with some species in the sample. d. Polystyrene fluoresces in this range. e. Polystyrene will be attacked by some organic solvents.
Please answer and explain thoroughly
Suppose we were able to measure the amount of oxygen gas formed in units of moles/L, and the rate of formation of oxygen was found to be 0.0125 M/s. Using the rate law for this reaction and the units associated with each variable, show what the derived units for the rate law constant would be. What would be the rate of decomposition of the hydrogen peroxide? Explain your answer.