Explanation:

When an electron jumps from a lower energy level to a higher energy level, it is said to be excited. The first excited state in a hydrogen atom is the state in which the electron is in the n=2 energy level. The energy of this state is given by the formula:

E₂ = -13.6/n² eV

where n is the principal quantum number and has a value of 2 for the first excited state. Substituting the value of n, we get:

E₂ = -13.6/2² eV
E₂ = -13.6/4 eV
E₂ = -3.4 eV

Therefore, the energy in the first excited state in a hydrogen atom is -3.4 eV.


The ground state in a hydrogen atom is the state in which the electron is in the n=1 energy level. The potential energy of a hydrogen atom in the ground state can be calculated using the formula:

E₁ = -13.6/n² eV

where n is the principal quantum number and has a value of 1 for the ground state. Substituting the value of n, we get:

E₁ = -13.6/1² eV
E₁ = -13.6 eV

Therefore, the potential energy of a hydrogen atom in the ground state is -13.6 eV.


The energy in the first excited state in a hydrogen atom is -3.4 eV, while the potential energy of a hydrogen atom in the ground state is -13.6 eV. This means that a hydrogen atom in the ground state has a greater potential energy than a hydrogen atom in the first excited state.