What is the ionization energy (in kJ/mol) of the atom in its first excited state?

The ionization energy of an atom refers to the amount of energy required to remove an electron from the atom in its gaseous state. When considering the ionization energy of an atom in its first excited state, we must account for the fact that the electron is at a higher energy level compared to the ground state. As a result, the ionization energy for the excited state is typically lower than that for the ground state, as the electron is further from the nucleus and experiences less effective nuclear charge.

To determine the exact value of the ionization energy for a specific atom in its first excited state, one would need experimental data or quantum mechanical calculations specific to that atom. Some common elements have well-documented ionization energies that can aid in your understanding.

For example, hydrogen has a first ionization energy of approximately 1312 kJ/mol in its ground state. When electrically excited, the energy required to ionize may vary due to factors like electron shielding and repulsion from other electrons.

In conclusion, to provide a specific numerical answer, please specify the atom of interest, as ionization energies differ for each element, and their excited states would need to be appropriately referenced from experimental data or calculated values.