(a(i))[2]
Complete the table by estimating: • the boiling point of chlorine • the density of fluorine at its melting point.
(a(ii))[1]
Describe the pattern in the melting points of the halogens down the group.
(a(iii))[2]
Deduce the state of matter of iodine at $130^\circ\text{C}$. Explain your answer.
(b(i))[1]
Give the electronic structure for a fluorine atom.
(b(ii))[1]
Explain why a fluoride ion carries a single negative charge.
(c)[1]
Magnesium reacts with excess fluorine to form magnesium fluoride. When $2.40\,\text{g}$ of magnesium is used, $6.20\,\text{g}$ of magnesium fluoride is formed. Calculate the mass of magnesium needed to make $1.24\,\text{g}$ of magnesium fluoride.