Exam 40: Atomic Structure

An s state (l = 0) energy level is split into two levels by an applied magnetic field. A photon of microwave radiation having frequency 60 GHz induces a transition between the two levels. What is the magnitude of the applied magnetic field? (h = 6.626 × 10^-34 J ∙ s, Bohr magneton = μB = 9.27 × 10^-24 J/T)

An electron in a hydrogen atom has orbital quantum number l = 7. How many possible values of the magnetic quantum number ml could it have?

An electron in a hydrogen atom has orbital quantum number l = 4. How many possible values of the magnetic quantum number ml could it have?

What is the minimum speed needed by a ground-state hydrogen atom for its kinetic energy to be enough to ionize the atom in a collision? (1 eV = 1.60 × 10^-19 J, ^mH ≈ mproton = 1.67 × 10^-27 kg)

An atom in a state with its orbital quantum number l = 1 decays to its ground state (with l = 0). A photon of wavelength 630.000 nm is emitted in the process. When the same process takes place in the presence of an intense magnetic field, the following change in the spectrum is observed. With the magnetic field present, one of the emitted lines observed now has a wavelength of 630.030 nm. Which of the following wavelengths would you expect to be also present?

If an electron has spin quantum number ms = - what is the possible value for the orbital quantum number l of the electron?

Consider the n = 9 shell. (a) What is the largest value of the orbital quantum number, l, in this shell? (b) How many electrons can be placed in this shell?

In the ground state, the quantum numbers (n, l, ml, ms) for hydrogen are, respectively

If two electrons in an atom have the same energy, then they must have the same four quantum numbers.

What is the correct electronic configuration for ground state carbon, which has 6 electrons?

The correct ground state electron configuration of boron, which has 5 electrons, is

If the orbital quantum number is l = 4, which one of the following is a possible value for the principal quantum number n?

An atom has completely filled inner shells and a single valence electron in an excited p state. The filled inner shells have an orbital momentum equal to zero. A magnetic field is applied, defining the z-axis along the field. Which of the following sets of angles are possible angles between the magnetic field and the orbital angular momentum?

If two electrons in the same atom have the same four quantum numbers, then they must have the same energy.

The energy of an electron in the p-level of an atom is changed in the presence of a magnetic field of magnitude 4.6 T. What is the difference between the largest and smallest possible energies? (Bohr magneton = μB = 9.27 × 10^-24 J/T)

The magnitude of the orbital angular momentum L of an electron in a certain atom is equal to 3.464ħ. Which one of the following numbers could be the principal quantum number n of the electron?

What is the greatest total angular momentum J for an electron in the n = 2 shell?

What is the correct electronic configuration for the ground state sodium atom, which has 11 electrons?

What is the energy of an incident photon that is just enough to excite a hydrogen atom from its ground state to its n = 4 state?

For each value of the principal quantum number n, what are the possible values of the electron spin quantum number m_s? (There may be more than one correct choice.)