(a(i))[2]
Define the term relative atomic mass.
(a(ii))[2]
Table 2.1 gives the abundances of two isotopes found in the iron sample. Use Table 2.1 to calculate the relative isotopic mass of the third isotope of iron in the sample. Show your working.
(b)[1]
Deduce how many pairs of electrons are present in the $3d$ sub-shell of an iron(II) ion.
(c)[1]
Sketch the shape of the lowest-energy orbital in the shell with principal quantum number $n = 2$.
(d)[2]
Complete Table 2.2 to give information about the particles in one ion of $^{56}\text{Fe}^{3+}$.
(e)[2]
The atomic radius of iron is $1.26 \times 10^{-10}\,\text{m}$. Suggest how the radius changes, if at all, after an iron atom reacts to form an $\text{Fe}^{3+}$ ion. Explain your answer.