The elements in group 2 are known as the alkaline earth metals. As you move down the group of the periodic table, additional shells of electrons are added that increase the atomic radius.

As the atomic radius decreases, the nucleus has a tighter hold on its electrons, so more energy is required to remove them. Therefore, the ionisation energy of alkaline earth metals decreases going down a group.

Melting point decreases going down group 2 of the periodic table as metallic bonds are weaker for larger elements and less energy is required to break them. Magnesium is an exception, with an unusually low melting point.

1

Would calcium, strontium or barium have the lowest melting point out of these metals?

2

Would magnesium, calcium or strontium have the lowest ionisation energy out of these metals?

3

Why does the atomic radius increase as you go down group 2 of the periodic table?

4

Which alkaline earth metal has the largest ionisation energy?

5

Which alkaline earth metal has the largest atomic radius?