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- 2. Molecules absorb IR radiation consistent with vibrational energy and rotational energy. Which of these is present in condensed phases (liquid, solution, solid)?9) The vibrational frequency of gaseous HCl occurs at 2885 cm¹ in the IR spectrum. What is the energy E, of this radiation in joules? a) 5.73 x 10-20 J b) 8.24 x 10-19 J c) 6.48 x 10-21 J d) 1.80 x 10-19 JSpectroscopy measures the interaction of molecules with electrical current. * O True False O O
- 5. The fundamental vibrational frequencies for 1H19F and 2D19F are 4138.52 and 2998.25 cm-1, respectively, and De for both molecules is 5.86 eV. What is the difference in the bond energy (bond dissociation energy) of the two molecules? A) 0.567 eV B) 0.15 eV C) 0.0707 eV D) 0.254 eV9. 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 of4G I 5:53 2.30 O Yo 40 52% KB/s 1. The C-C stretch in allene (H,C-C=CH,) is about 1650 cm'; the C-H stretch is about 3,100 cm". Calculate the corresponding wavelengths (in nm) and energies (in kJ/mol) of these vibrations. () II
- Which of the statements is CORRECT regarding the Beer-Lambert Law? There is an inverse relationship between the concentration and the absorbance of the solution. It describes the relationship between the number of protons absorbed and the number of absorbing molecules in a sample. It describes the relationship between the number of electrons absorbed and the number of absorbing molecules in a sample. It describes the relationship between the number of photons absorbed and the number of absorbing molecules in a sample.1B. Explain how a vibrationally excited molecule is able to withstand up a billion of collisions without losing its excitation.Calculate the number of possible vibrational modes for each of the following molecules and assign frequency ranges to each. i) NH3 ii) C2H4 iii) CCl2F2 iv) CH3CH2OH b) Which of the above molecules will absorb IR radiations most strongly? Explain your answer.
- Emission 0.26 0.24 0.22 0.20 0.18 0.16 0.14 0.12 0.10 0.08 0.06 0.04 300 350 400 450 Wavelength (nm) 500 550 According to the spectrum, the most intense light emitted results from the following types of transition in it's molecules. Electronic transitions from high to low energy states O Vibrational transitions from low to high energy states Vibrational transitions from high to low energy states Electronic transitions from low to high energy statesCovalent bonds in a molecule absorb radiation in the IR region and vibrate at characteristic frequencies. (a) The C---O bond absorbs radiation of wavelength 9.6 mm. What frequency (in s-1) corresponds to that wavelength? (b) The H---Cl bond has a frequency of vibration of 8.652x1013 Hz. What wavelength (in mm) corresponds to that frequency?Riboflavin absorbs UV-visible light making the electrons in the molecule more energetic. As a result, the more energetic electrons move from the 'ground state' electronic energy level to higher electronic energy levels known as 'excited states’. Which of the following statements is NOT true regarding how the ‘excited state’ molecule loses energy and returns to the 'ground state'? a) non-radiative losses via bond vibration and rotation within the molecule b) non-radiative losses via phosphorescence c) non-radiative losses via collisions with other molecules d) radiative losses via fluorescence emission of light