The graph displays the first ionisation energies for some Group 2 elements.
(a)[1]
Give an equation for the first ionisation energy of Mg. Include state symbols.
(b)[3]
Explain the pattern seen in first ionisation energies as you go down Group 2.
(c)[2]
The second ionisation energy of Be is $1757\\ \text{kJ mol}^{-1}$. Explain why the second ionisation energy of Be is greater than the first ionisation energy of Be.
Worked solution & mark scheme
This 6-mark question has a full step-by-step worked solution and mark scheme. One marking point: “A gaseous magnesium atom loses one electron to form a gaseous magnesium ion: $\\mathrm{Mg(g) \\to Mg^+(g) + e^-}$” …