2. The atomic radius increases down Group 2.

5. There are more filled energy levels between the nucleus and the outer electrons, which are more shielded from its attraction.

6. There are more filled energy levels between the nucleus and the outer electrons, which are more shielded from its attraction.

7. There are more filled energy levels between the nucleus and the outer electrons, which are more shielded from its attraction.

8. The attraction between the outer electron and the nucleus decreases down group 2, so the first ionisation enthalpy decreases.

9. The attraction between the outer electron and the nucleus decreases down group 2, so the first ionisation enthalpy decreases.

10. The attraction between the outer electron and the nucleus decreases down group 2, so the first ionisation enthalpy decreases.

11. The atomic radius increases, there are more filled energy levels between the nucleus and the outer electron, and more shielding.

12. The atomic radius increases, there are more filled energy levels between the nucleus and the outer electron, and more shielding.

13. The atomic radius increases, there are more filled energy levels between the nucleus and the outer electron, and more shielding.

14. Proton number Electronegativity decreases down Group 2.

15. Proton number Electronegativity decreases down Group 2.

16. Proton number Electronegativity decreases down Group 2.

17. Proton number The atomic radius increases, the outer electrons are more shielded, and so bonding electrons are less strongly attracted to the nucleus.

18. Proton number The atomic radius increases, the outer electrons are more shielded, and so bonding electrons are less strongly attracted to the nucleus.

19. Proton number The atomic radius increases, the outer electrons are more shielded, and so bonding electrons are less strongly attracted to the nucleus.

20. In general, the melting point decreases down Group 2.

23. The strength of the metallic bonding decreases because the radius of the metal ions increases.

24. The strength of the metallic bonding decreases because the radius of the metal ions increases.