* Atomic Radius: Sodium has a larger atomic radius than magnesium. This means its outermost electron is further from the nucleus and experiences weaker attraction. As a result, it's easier to remove this electron, making sodium more readily oxidized.
* Ionization Energy: Sodium has a lower ionization energy than magnesium. This means it requires less energy to remove an electron from a sodium atom, making it more likely to lose an electron and become a cation.
* Electronegativity: Sodium has a lower electronegativity than magnesium. This means it has a weaker attraction for electrons and is more likely to donate electrons in a chemical reaction.
In simpler terms: Sodium's larger size and weaker hold on its outermost electron make it more reactive than magnesium. It's easier for sodium to lose an electron and form a positive ion, which is the basis of its reactivity.
Here's a helpful analogy: Imagine a balloon. A larger balloon (sodium) is easier to burst than a smaller balloon (magnesium) because the pressure on its surface is less. Similarly, sodium's larger size means its outermost electron is less tightly bound, making it easier to "burst" and become reactive.
