Final answer:
Ionization energy is related to the energy needed to remove an electron from an atom. Mg's higher ionization energy compared to Al is attributed to its full s-orbital, leading to a stable configuration that requires more energy to disrupt. Ionization energy generally increases as we move across the periodic table due to higher nuclear charge.
Step-by-step explanation:
The query revolves around the concept of ionization energy, which is defined as the amount of energy required to remove an electron from an atom in its gaseous state. The ionization energies for elements can vary based on their position in the periodic table. Ionic spectrometry is a common technique used to measure various properties of atoms, including ionization energy.
The first ionization energies of Mg and Al provided—738 kJ/mol for Mg and 578 kJ/mol for Al—reflect their different atomic structures. Magnesium (Mg) has a higher ionization energy than Aluminum (Al) because Mg has a full s-orbital, which results in a stable electron configuration that requires more energy to remove an electron. In contrast, Al, which is to the right of Mg in the periodic table, has a partially filled p-orbital, making it easier to remove an electron and hence has a lower ionization energy.
As one moves from left to right across the periodic table, the ionization energy generally increases due to the increase in nuclear charge, which tightens the grip on the valence electrons. However, there can be exceptions due to factors such as subshell completion and electron shielding, which is why Mg has a higher ionization energy than Al.