Group 2

Question 1

How does melting point change going down the group?

Answer 1

• decreases
• metallic bonding weakens as atomic size increases
• distance between positive ions and delocalised electrons increases
• electrostatic forces of attraction weaken

Question 2

Why do first and second ionisation energies decrease going down the group?

Answer 2

• outer shell electrons have weaker attraction to nucleus as they are further distance from it
• repulsive force of innershtell electrons also decreases attraction

Question 3

What is second ionisation energy defined as?

Answer 3

enthalpy change when one mole of gaseous ions with a single positive charge forms one mole of gaseous ions with a double positive charge

Question 4

how does reactivity change going down group 2?

Answer 4

Reactivity increases going down group 2, as atomic radii increase there is more shielding. Nuclear attraction decreases and its easier to remove outer shell electrons. Cations form more easily