Consider an electron in the N shell. (c) What is the largest orbital angular momentum this electron could have in any chosen direction? Express your answers in terms of U and in SI units.

Model a hydrogen atom as an electron in a cubical box with side length L. Set the value of L so that the volume of the box equals the volume of a sphere of radius a = 5.29 * 10-11 m, the Bohr radius. Calculate the energy separation between the ground and first excited levels, and compare the result to this energy separation calculated from the Bohr model.

A photon is emitted when an electron in a threedimensional cubical box of side length 8.00 * 10-11 m makes a transition from the nX = 2, nY = 2, nZ = 1 state to the nX = 1, nY = 1, nZ = 1 state. What is the wavelength of this photon?

Consider an electron in the N shell. (a) What is the smallest orbital angular momentum it could have?

Consider an electron in the N shell. (b) What is the largest orbital angular momentum it could have? Express your answers in terms of U and in SI units

Consider an electron in the N shell. (d) What is the largest spin angular momentum this electron could have in any chosen direction? Express your answers in terms of U and in SI units.

The orbital angular momentum of an electron has a magnitude of 4.716 * 10-34 kg # m2>s. What is the angular momentum quantum number l for this electron?

Calculate, in units of U, the magnitude of the maximum orbital angular momentum for an electron in a hydrogen atom for states with a principal quantum number of 2, 20, and 200. Compare each with the value of nU postulated in the Bohr model. What trend do you see?

A hydrogen atom is in a d state. In the absence of an external magnetic field, the states with different ml values have (approximately) the same energy. Consider the interaction of the magnetic field with the atom's orbital magnetic dipole moment. (a) Calculate the splitting (in electron volts) of the ml levels when the atom is put in a 0.800-T magnetic field that is in the +z@direction