Don't really understand this question!

Question

Use the table to determine the energy in eV of the photon emitted when an electron jumps down from the n = 3 orbit to the n = 2 orbit of a hydrogen atom.

Allowed Values of the Hydrogen Electron's Radius and Energy for Low Values of n
1	0.053 nm	−13.60 eV
2	0.212 nm	−3.40 eV
3	0.477 nm	−1.51 eV
4	0.848 nm	−0.85 eV

Answer 1

When an electron goes from a higher energy orbital (higher n), to a lower energy orbital (lower n), it will emit a photon of energy equal to the difference in energy values between the two orbitals. My interpretation of the table is that the energy of the photon emitted when an electron moves from n = 3 orbital to n = 2 orbital is the difference between -1.51 eV and -3.40 eV; that is 1.89 eV.