May you explain this for me please? **The reactivity of group 1 metals INCREASES down a group but the reactivity of group 17 nonmetals DECREASES down a group. Explain**In the periodic table, elements are arranged in a way that demonstrates periodic trends. Two notable groups are group 1 metals (alkali metals) and group 17 nonmetals (halogens). These groups show opposite trends in reactivity as you move down the group.**Group 1 Metals (Alkali Metals):**- **Reactivity Increases Down the Group:** As you move down group 1, from lithium to cesium, the atomic size increases. This is because additional electron shells are added, which increases the distance between the outermost electron and the nucleus. The increased distance and shielding effect from inner electrons reduce the effective nuclear charge felt by the outermost electron. Consequently, it becomes easier for the atom to lose its valence electron, thereby increasing reactivity.**Group 17 Nonmetals (Halogens):**- **Reactivity Decreases Down the Group:** Halogens need to gain an electron to achieve a stable electronic configuration. As you move down group 17, from fluorine to iodine, the atomic size increases, making the nucleus less able to attract additional electrons due to the increased distance and electron shielding effect. This makes it progressively harder for these elements to gain an electron, resulting in decreased reactivity.Understanding these trends is crucial for predicting the chemical behavior of elements in these groups.

Interpretation- Reason, why the reactivity of group 1 metals increases down a group but the reactivity of group 17 non-metals decreases down a group is to be explained. Periodic trends of atomic radius- Atomic radius increases form left to right across a period. Atomic radius decreases form top to bottom down the group. Metals and non-metals Metals have tendency to loose electrons and acquire positive charge. Non-metals tend to gain electrons and acquire negative charge.Answer- Effective nuclear charge is constant but number of shells increases top to bottom in a group. Thus, attraction between valence electron and nucleus decreases. Thus, size increases as we go from top to bottom in a group. Hence, it is easy to loose to electron but difficult to gain electron for large size elements. Group 1 elements are alkali metals. Group 2 elements are halogen and are non-metals. Metals which readily loose electrons are reactive and non-metals which readily gain electron are reactive. Hence, due to all the above reasons the reactivity of group 1 metals increases down a group but the reactivity of group 17 non-metals decreases down a group