Sure, here's an AP Physics 2 exam question on atomic structure:

Question: A hydrogen atom is in its ground state (n=1). If an electron in this hydrogen atom is excited to the n=3 level, calculate the energy required for this excitation.

Given:

• The energy of an electron in a hydrogen atom is given by the formula E = -13.6 eV/n^2, where E is the energy in electron volts (eV) and n is the principal quantum number of the electron's orbit.

Answer: We can start by finding the energy of the electron in the ground state (n=1). Plugging n=1 into the formula E = -13.6 eV/n^2 gives us: E_1 = -13.6 eV/1^2 = -13.6 eV

Next, we find the energy of the electron in the n=3 level: E_3 = -13.6 eV/3^2 = -13.6 eV/9 = -1.51 eV

The energy required for the excitation from n=1 to n=3 level is the difference between the energies of these two levels: ΔE = E_3 - E_1 ΔE = (-1.51 eV) - (-13.6 eV) ΔE = 12.09 eV

Therefore, the energy required for this excitation is 12.09 eV.

This question assesses the student's understanding of the energy levels of an electron in a hydrogen atom as described by the Bohr model. Students are expected to know the formula for the energy of an electron in a hydrogen atom, as well as how to calculate the energy difference between different energy levels.