Final answer:
The correct answer for the first ionization energy of neon is 2081, which represents the energy needed to remove one electron from a neon atom in its gaseous state.
Step-by-step explanation:
The first ionization energy of neon is the energy required to remove the outermost electron from a neutral neon atom in its gaseous state. Given the choices provided, the correct answer is the third option, '2081'. This value is typically represented in units of kilojoules per mole (kJ/mol). If we compare it with the provided data, it is clear that option '280' is too low and '28010' is excessively high for a first ionization energy value.
The first ionization energy is an indicator of how strongly an atom holds onto its electrons, and for neon, which has a filled valence shell of electrons, this energy is relatively high. Due to neon's electron configuration of [He]2s²2p⁶, the first ionization involves removing an electron from a stable, noble gas electron configuration, which requires a significant amount of energy.
The first ionization energy is a key concept in understanding atomic structure and chemical reactivity, and it reflects the stability of an atom's electron configuration.