We obtain the Raman spectrum of Cl2(l) vibration by excitation with radiation from a Hg lamp with a wavelength of 4358.25 Å. In this way we obtain a Stokes line at 4466.5 Å which is very intense. Calculate the wave number of the fundamental vibration of the chlorine molecule and the bond strength constant (we will assume that it is a harmonic vibration).Data: h = 6.626x10-34J s; c = 2.998x108 m s-1, NA = 6.022x1023 mol-1; relative atomic mass of Cl = 35.45.

We obtain the Raman spectrum of Cl2 (l) vibration by excitation with radiation from a Hg lamp with a wavelength of 4358.25 Å. In this way we obtain a Stokes line at 4466.5 Å which is very intense. The wave number of the fundamental vibration of the chlorine molecule is 540 cm-1 and the bond force constant is 482 N/m.Calculate the wave number at which the first anti-Stokes line of vibration will appear.Data: h = 6.626x10-34J s; c = 2.998x108 m s-1, NA = 6.022x1023 mol-1; relative atomic mass of Cl = 35.45.

Calculate the standard deviation of the bond length ox of the diatomic molecule 'H1°F when it is in the ground state and first excited state using the quantum harmonic oscillator wavefunctions. The fundamental harmonic vibrational frequency of HF is 4,460 cm-1 and the equilibrium bond length is 0.091nm. How do you interpret the change in the ratio of average bond length to ox as a function of energy in the vibration?

The 14 N160 molecule undergoes a transition between its rotational ground state and its rotational first excited state. Approximating the diatomic molecule as a rigid rotor, and given that the bond length of NO is 1.152 Angstroms, calculate the energy of the transition. As your final answer, calculate the temperature T in Kelvin, such that Ethermal = kBT equals the %3D energy of the transition between NO's rotational ground state and fırst excited state.

Explain the importance of the quantization of vibrational, rotational, and translational energy as it relates to the behavior of atoms and molecules.

The vibrational frequency of the ICl molecule is 1.15 ×1013 s-1. For every million (1.00 × 106) molecules in the ground vibrational state, how many will be in the first excited vibrational state at a temperature of 300 K?

A standard sample of Argon gas is 22.4L, 1.00atm, 1.00mol, 273.15K.   In the right setups excited gas can be tricked into using heat and giving away photons of light.  If the sample gave off 0.01mol of 3,634nm light by converting thermal energy into those photons find the new final temp of the gas. SAr = 0.52J/gK

The force constant of the hydroxide anion, ¹ H ¹6 O is 2500 N/m. Assume it is a harmonic oscillator. Use the constants in the che302r library: 1 ΝΑ = N.A (number of particles) ħ hb (Js). c = cl (m/s). = a. Compute w for the fundamental vibration. w = 1.26e15 S-1 b. Compute the energy corresponding to the fundamental vibration. E = 4.17e-19 X J

But molecules combine both vibrational and rotational states in such a way that both selection rules must be satisfied if we are only talking about absorption or emission of electromagnetic radiation (i.e. photons). 5 1 images from Krane Ch 9. Relative absorption : 0.330 L=3 to L=2 L=2 to L = 1 Electronic excited state. Electronic ground state L→ L-1 L = 1 to L = 0 Ť 0.340 0.350 SE Energy (eV) 2B 0.360 : hf L=0 L=1 L=2 to to to L = 1 L = 2 L = 3 Photo 4 1 3 1 2 1 1 0 1 1 5 0 4 0 30 20 1 0 0 0 LN L→ L+1 0.370 0.380 no emission here because AL # 0, AL = +1 AN = ±1, HCI spectra. In the middle of the gap is the energy hf that would correspond to a pure vibrational transition, which would violate the rotational selection rule. What is the value of hf for the HCI spectra?

The first five vibrational energy levels of ¹H¹27 I are at 1144.83, 3374.90, 5525.51, 7596.66, and 9588.35 cm¹. Treating the molecule as an anharmonic oscillator, estimate the dissociation energy of the molecule in units of reciprocal centimetres (cm-¹). [Note: m(¹H) = 1.0078 u, m(¹271) = 126.9045 u; assume the second order anharmonicity constant, Ye, to be zero.] [Note: Use graph paper in your answer.]