trends down group 2

Why dos atomic radii increase down group 2

Outer electron is less tightlly held due to an increase in sheilding (electrons repel due to an increase in nuclear charge)

Outer electron becomes further away from nucleus so atomic radii increases

Explain why the atomic radius of calcium is smaller than that of strontium

Fewer shells of electrons

Fewer sheilding so stronger attraction

in calcium so outer electrons are closer to the nucleus

Why does ionisation energy decrease don group 2

Atomic radius increases

Outer electron is less tightly held due to the increase in sheilding and repulsion

Easier to remove

Less ionisation energy

State and explain the general trend in melting point of the group 2 metas

It decreases

Going down group the size of the positive ions increases

Metalllic bonding between ions and delocalised electrons is weaker

Compare the strength of metallic bond in the group 2 metal and the transition metals

Metallic b in transition metals is stronger than that of group 2 metals

Transition metals have more electrons which can be delocalised than group 2 metals