Final answer:
The first six energy levels of a hydrogen atom are -13.6 eV, -3.4 eV, -1.51 eV, -0.85 eV, -0.54 eV, and -0.38 eV respectively, with -13.6 eV being the ground state energy.
Step-by-step explanation:
The energy levels of a hydrogen atom can be calculated using the Bohr model. The energy of the electron in the hydrogen atom is quantized, meaning it can only take on certain discrete values. According to the Bohr model, the energy of an electron in the first Bohr orbit of hydrogen (the ground state) is -13.6 eV. The energies for the first six orbits can be represented by the formula En = -13.6 eV / n2, where n is the principal quantum number corresponding to the different energy levels.
Here are the first six energy levels calculated using this formula:
- E1 = -13.6 eV (ground state)
- E2 = -3.4 eV (first excited state)
- E3 = -1.51 eV
- E4 = -0.85 eV
- E5 = -0.54 eV
- E6 = -0.38 eV
Note that each energy level is increasingly higher from the ground state, and the energy difference between successive levels decreases as n increases.