Explain why the first ionization energy of aluminum is less than the first ionization energy of magnesium?

Answer 1

My answer: The 3p electron in aluminum is slightly more distant from the nucleus than the 3s, and partially screened by the 3s2 electrons as well as the inner electrons. Both of these factors offset the effect of the extra proton.

Answer 2

The crystal structure of aluminum is face centered cubic while the crystal structure of magnesium is hexagonal.

Its not the boiling point of aluminum is 2450 and the boiling point of mg is 1120

Answer 3

Chlorine exist as a diatomic molecule and between the molecules there are only weak intermolecular forces, called van der Waals. Magnesium chloride forms an ionic lattice, held by electrostatic attractions between oppositely charged ions. More energy is needed to break the ionic bonds.

Answer 4

Yes aluminum is less reactive than magnesium it is less reactive because as you read left to right on the Periodic Table the elements become less reactive because they get more electrons on their valence shells hope this helps you

Answer 5

The first ionization energy of aluminum is less than that of magnesium because aluminum has a higher effective nuclear charge, which means its electrons are held more tightly. Additionally, magnesium has a filled 3s subshell, which makes it easier to remove an electron compared to aluminum which has a partially filled 3p subshell.

Answer 6

I think that it has somthing to do with the fact that Mg doesn't have any electrons in the P sublevel in its outer enery level, but Al has one in the P sublevel in its outer energy level.

Answer 7

Aluminium is much lighter (less dense) than magnesium. That's why they use aluminum on aeroplanes.