Friedel Crafts

What is the wavelength (in cm) of the waves emitted by an NMR spectrometer that operates at a radio frequency of 700 MHz?

Write the electron configuration for atoms of chlorine Cl in their ground state and use it to predict which of the following PES spectra would be generated by these atoms. II 347 29.1 2.38 2.05 37.1 3.93 0,42 239 16.05 100 10 100 10 lonization Energy (MJ/mol) lonization Energy (MJ/mol) II IV 273 20.2 2.44 24.1 2.82 26.8 1.25 31.5 1.52 100 10 100 10 lonization Energy (MJ/mol) lonization Energy (MJ/mol) Number of Electrons Number of Electrons Number of Electrons Number of Electrons

Spectroscopy relies on the excitation and relaxation of electrons. Which of the following statements about spectroscopy is true? Phosphorescence is the emission of a photon of light as an electron transitions from the excited singlet state to ground state. Collisional deactivation of an excited molecule decreases the absorbance response. Molecular absorption spectrometry measures the change in light intensity as light passes through a sample. Fluorescence is the absorption of a photon of light as an electron transitions from the ground state to an excited triplet state.

Explain the concept of Infrared spectroscopy ?

The spectra that you observe are for approximately 1 x 1012 atoms. So it is likely, that with electronic excitation, many of the electronic energy levels will be readily populated. However, the higher energy levels will be less populated, so what does say about the intensity of the higher energy peaks? Is that observation consistent with the spectrum we measured with the spectrometer?

Food dye spectroscopy  2. At what wavelengths should the readings be taken? What instrumentation will you utilize with a solution of a known dye to determine the wavelength for your analysis?

[References] Photosynthesis uses 650-nm light to convert CO2 and H2 into glucose and O2. Calculate the frequency of this light. Frequency = Hz %3D

Which of the following describes visible light spectroscopy?   Group of answer choices A method of measuring the amount of energy 400 nm - 700 nm due to absorption by electrons in the sample. A method of measuring the amount of energy 400 nm - 700 nm due to emission by electrons in the sample. A method of measuring the amount of energy 0.8 ?μm - 2.5 ?μm due to absorption by electrons in the sample. A method of measuring the amount of energy 0.8 ?μm - 2.5 ?μm due to emission by electrons in the sample. A method of measuring the amount of energy 100 nm - 400 nm due to absorption by electrons in the sample. A method of measuring the amount of energy 100 nm - 400 nm due to emission by electrons in the sample.

Here is an energy level diagram that illustrates the absorption process. Energy ES (n=5) E4 (n=4) E3 (n=3) E2 (n=2) E1 (n=1)

If a sample is placed in a magnetic field of applied field strength = 1.1 Tesla, the spin-up and spin-down 1H nuclei show an energy difference that corresponds to a photon with frequency = 60 MHz.  If this same sample is moved into the vicinity of a magnetic field of strength = 5.5 Tesla, what will be the frequency of a photon that could match the energy difference of the spin-up and spin-down states?

. Atomic Absorption Spectroscopy (AAs) and Atomic Emission Spectroscopy (AEs) have many uses including in forensic science and choice of colors for fireworks. Explain in not more than six (6) sentences how this is so.

QUES Which of the following is the reason that a more concentrated dye solution absorbs more light than a les concentrated solution? There are more molecules of dye in solution that can absorb photons, meaning fewer photons reach the detector, increasing absorbance. O There are fewer molecules of dye in solution that can absorb photons, meaning more photons reach the detector, increasing absorbance. O There are more molecules of dye in solution that can absorb isotopes. O There are fewer molecules of dye in solution that can absorb electrons, meaning more electrons reach the detector, increasing absorbance. O There are more molecules of dye in solution that can absorb electrons.

Which transition will correspond to the absorption of the greatest amount of energy in a hydrogen atom?

1) Whose law is utilized in this lab with regards to solution concentration and absorbance? 2) How many possible energy releasing electron transitions are possible for a single electron in a hydrogen atom if there are 7 orbits available to the electron? 3) An electron in a hydrogen atom transitioning from orbit n = 7 releases a photon whose frequency equals 6.44196  1013 Hz. Determine the orbit to which the electron transitioned.

9. Absorption spectra for molecules are more complex than atomic spectra because: C (a) Molecular species have side reactions C (b) Atomic species do not absorb light C (c) The number of energy states of molecules is enormous when compared with the number of energy states for isolated atoms. 10 absorption / emission of light by a molecule and describe the processes in terms of energy levels. How this information can be used for obtaining analytical information on an analyte of interest? Explain the phenomenon of