Final answer:
The statement is likely referring to the first ionization energy (IE₁), which is the energy required to remove the most loosely bound electron from an atom in its gaseous state. Ionization energies increase with the removal of additional electrons, and the atomic radius affects the ease of removal.
Step-by-step explanation:
The question asks whether the statement provided is true or false, regarding the energy needed to remove the most loosely held electron from an atom (valence electron). This is not actually stated in the provided information; however, we can infer that the statement is concerning the first ionization energy (IE₁), which indeed refers to the energy required to remove the most loosely bound electron from a gaseous atom in its ground state. The information provided primarily discusses the concept of ionization energy, including the first ionization energy and subsequent energies required to remove additional electrons from an atom.
Moreover, the information explains that as the atomic radius increases, the electrons are located farther from the nucleus and can be removed more easily, suggesting that IE₁ is typically lower for larger atoms. Additionally, the second ionization energy (IE₂) and further ionization energies involve removing electrons beyond the first one, which subsequently requires more energy as those electrons are more tightly bound to the nucleus.