Take a look at the location of sodium (Na) and chlorine (Cl) on the Periodic Table. Use these elements to explain how the Periodic Table arranges elements according to similar properties and reactivities.
Sodium (Na) and chlorine (Cl) are both located in Group 1 and Group 17 of the Periodic Table, respectively.
The Periodic Table arranges elements according to their atomic number (number of protons) and organizes them into periods (rows) and groups (columns). Elements in the same group, like sodium and chlorine, share similar properties and reactivities.
Sodium, located in Group 1, is a highly reactive metal. It is characterized by having one valence electron in its outermost energy level. This electron configuration makes sodium tend to lose that electron and form a positively charged ion (Na+). Sodium reacts vigorously with water and oxygen, and it is highly reactive with most non-metals.
Chlorine, situated in Group 17 (also called Group 7 or the halogens), is a highly reactive non-metal. It has seven valence electrons in its outermost energy level, just one short of a stable octet. To achieve this stability, chlorine tends to gain an electron and form a negatively charged ion (Cl-). Chlorine is particularly reactive with metals, and it can form compounds with a wide range of elements.
The fact that sodium and chlorine are located in different groups of the Periodic Table indicates that they have distinct properties and reactivities. However, when combined, they undergo a chemical reaction known as ionic bonding. The electronegativity difference between sodium and chlorine causes sodium to easily transfer its valence electron to chlorine, resulting in the formation of sodium chloride (NaCl), which is a stable compound commonly known as table salt.
The arrangement of sodium and chlorine on the Periodic Table demonstrates how elements with similar properties and reactivities are grouped together. In this case, sodium and chlorine belong to different groups but have complementary reactivities, enabling them to form stable compounds through chemical reactions that fulfill their electron configurations and achieve greater stability.