Q6. For this question you should refer to the Periodic table at the back. These are the electronic structures of the atoms of three different elements. 28.1 2.8.8 2.8.8.1 element A element B element C (a) Identify elements A and B. Element A is __ Element B is __ (i) ) Why is element C more reactive than element A? __ (ii) Why is element B unreactive? __

## Step 1: Identify Elements A and BThe electronic structures given represent the number of electrons in each shell of an atom. The Periodic Table is arranged in such a way that the period (row) number corresponds to the number of electron shells an atom has. The group (column) number corresponds to the number of electrons in the outermost shell. ### represents an atom with 3 shells and 1 electron in its outermost shell. This corresponds to the element in Period 3, Group 1 of the Periodic Table, which is Sodium (Na).### represents an atom with 3 shells and 8 electrons in its outermost shell. This corresponds to the element in Period 3, Group 18 of the Periodic Table, which is Argon (Ar).## Step 2: Explain why Element C is more reactive than Element AReactivity of an element is determined by how easily it can lose or gain electrons to achieve a stable electron configuration, usually a full outer shell. ### Element C has the electron configuration , which means it has 1 electron in its outermost shell. This electron can be easily lost in a chemical reaction, making Element C highly reactive.### On the other hand, Element A has the electron configuration , which means it also has 1 electron in its outermost shell. However, since it has fewer electron shells than Element C, it is less likely to lose its outer electron and is therefore less reactive.## Step 3: Explain why Element B is unreactiveAn element is unreactive or inert when its outermost shell is full. ### Element B has the electron configuration , which means its outermost shell is full. Therefore, it does not need to lose or gain electrons to achieve stability, making it unreactive.