A 5f electron in a 6P orbital 1 electron is a hydrogenic atom and make a spectroscopic transition because of an outer orbital electron.
PS6.4 To what orbitals may a 5f electron in a hydrogenic atom make spectroscopic transitions?
To what orbitals may a 2p electron in H atom make electric-dipole allowed radiative transitions and explain.
To what orbitals may a 3p electron make electron-dipole allowed radiative transitions? Construct a Grotrian diagram which shows the allowed transitions just for cases where Δn= + or - 1.
Locate the radial nodes of each of the 3d orbitals of a hydrogenic atom of atomic number Z
2. Define fermion and boson AND give examples of each. 3. To what orbitals may electrons in a 4d orbital make spectroscopic transitions in a hydrogen atom? 4. Calculate wavelength of the n=6 transition in the Paschen series for a hydrogen atom 5. What terms and levels arise from the ground-state configuration of carbon? Which term has the lowest energy? 6. List and simplify the complete wavefunction for a 2s orbital.
Locate the radial and angular nodes for each of the 3p orbitals of a hydrogenic atom of atomic number Z. Give the angular nodes for the angular functions Y1,1(Θ,Φ) and Y1,–1(Θ,Φ) “by themselves” and when they are combined to give the 3px and 3py orbitals.
Selection rules and allowed transitions: Electron in a hydrogen atom is in 4p state. The energy level diagram is shown below. Note the energies are given to first decimal place only. (a) Draw arrows showing all the allowed transitions the 4p electron can make that lead to the emission of photon. Include all the transitions until the electron reaches the ground state. (b) What are the kinetic and potential energies of the electron in the 4p state? (c) Calculate the wavelengths (in nm)...
3. In the ground electronic state of Li atom, the electron configuration is 1s 2s'. If we neglect all the electron-electron repulsion, and assume all Li atomic orbitals follow those in hydrogenic atoms. Determine the energy (in eV) of the electron ground state: 1s2 2s1. Namely, the total energy of the 3 electrons in 1s 2s'. Check the end of chapter problem: E8C.2(a). 3. In the ground electronic state of Li atom, the electron configuration is 1s 2s1. If we...
Using spectroscopic notation write the complete electron configuration for the carbon atom.
1. The figure below illustrates two electron transitions for a hydrogen atom. The transitions are labeled (a) and (b) in the figure. Energy n = 3 - n = 2 1 n = 1 Based on the figure alone (without performing any calculations) decide which of the transitions is associated with a lower wavelength. Briefly explain your reasoning.
Determine the wavelength of light emitted or absorbed by a hydrogen atom when an electron transitions from n = 6 to n = 9. Give your answer in units of nm. An electron in a hydrogen atom absorbs 2.66 x 10 -20 J of energy. If the electron originated at energy level 5, to what level was it excited?