2/ Please explain the answer in detail The J = 0 to j = 1 transition for carbon monoxide (12C160) occurs at 1.153 × 105 MHz. Calculate the value of the bond length in carbon monoxide.
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- 6. The NaH molecule undergoes a rotational transition from J=0 to J=1 when it absorbs a photon of frequency 2.94×10' Hz. What is the equilibrium bond length of the molecule?A molecule can have various types of energies (translational, rotational, vibrational, and electronic), the sum of which is the molecule's total energy. E trans = (n +n + n²) Erot = J (J + 1) h² 87²1 Evib = (U+ 1 ) h hv h² 8mV (2/3) In the equations, nx, ny, nz, J, and u are quantum numbers, h is Planck's constant, m is the mass of the molecule, V is the volume of the container, I is the moment of inertia of the molecule, and v is the fundamental vibration frequency. For carbon monoxide, CO, the moment of inertia is I = 1.45 x 10-46 kg-m², and the fundamental vibration frequency is v = 2130 cm-¹. Let V = 12.5 L, and let all the quantum numbers be equal to 1. Calculate the translational, rotational, and vibrational energies per mole of CO for these conditions.When β-carotene is oxidized in vivo, it breaks in half and forms two molecules of retinal (vitamin A), which is a precursor to the pigment in the retina responsible for vision. The conjugated system of retinal consists of 11 C atoms and 1 O atom. In the ground state of retinal, each level up to n = 6 is occupied by two electrons. Assuming an average internuclear distance of 140 pm, calculate (a) the separation in energy between the ground and first exciteted state in which one electron occupies the state with n = 7, and (b) the frequency of radiation required to produce a transition between these two states. From your results, correct the following sentence (from the options in brackets). The absorption spectrum of a linear polyene shifts to (higher/lower) frequency as the number of conjugated atoms (increases/decreases).
- 问题3 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 Eshermal = kBT equals the energy of the transition between NO's rotational ground state and first excited state.Determine the electronic configration of transition metal ion: TiO2.The Morse potential energy is very useful as a simple representation of the actual molecular potential energy. When 85Rb1H was studied, it was found that ˜ν = 936.8 cm−1 and x_eν˜ = 14.15 cm−1. Plot the potential energy curve from 50 pm to 800 pm aroundRe = 236.7 pm. Then go on to explore how the rotation of a molecule may weaken its bond by allowing for the kinetic energy of rotation of a molecule and plotting V∗ = V + hcBJ˜ (J + 1) with B˜. Plot these curves on the same diagram for J = 40, 80, and 100, and observe how the dissociation energy is affected by the rotations. Hints: Taking B˜ = 3.020 cm−1 as the equilibrium bond length will greatly simplify the calculation. The mass of 85Rb is 84.9118mu
- A microwave using 18.99cm IR radiation is used to heat 18.2g water from 18.8C to 71.2C. Find the number of MOLES of photons required to accomplish this task.2. What are the term symbols for the microstates possible for the 1s 2s2p' electronic configuration of boron?5. Sketch the Radial Distribution Function 4xr³R² vs. r for 4s . ● . ● 5s 4p • • 5p • 6s бр 4d,²-²
- Consider the molecules: CH2=CH-CH=CH-CH=CH-CH=CH-CH=CH2. let’s assume that the 10 electrons that make up the double bonds can exist everywhere along the carbon chains. The electrons can then be considered as particles in a box; the ends of the molecule correspond to the boundaries of the box with a finite or zero potential energy inside. In this “molecular box”, 2 electrons can occupy an energy level. What are quantum states that the electrons from this molecule can occupy in the ground state? What’s the smallest frequency of light that can excite the electron? Briefly explain why. Note that the length of a C-C bond is about 1.54A and the length of a C=C bond is 1.34A to allow you to estimate the length of the “molecular box”Consider the molecules: CH2=CH-CH=CH-CH=CH-CH=CH-CH=CH2. Let’s assume that the 10 electrons that make up the double bonds can exist everywhere along the carbon chains. The electrons can then be considered as particles in a box; the ends of the molecule correspond to the boundaries of the box with a finite or zero potential energy inside. In this “molecular box”, 2 electrons can occupy an energy level. What’s the smallest frequency of light that can excite the electron? Briefly explain why.Consider the molecules: CH2=CH-CH=CH-CH=CH-CH=CH-CH=CH2. Let’s assume that the 10 electrons that make up the double bonds can exist everywhere along the carbon chains. The electrons can then be considered as particles in a box; the ends of the molecule correspond to the boundaries of the box with a finite or zero potential energy inside. In this “molecular box”, 2 electrons can occupy an energy level. What are quantum states that the electrons from this molecule can occupy in the ground state? Note that the length of a C-C bond is about 1.54A and the length of a C=C bond is 1.34A to allow you to estimate the length of the “molecular box”