Group 1: Alkali Metals
* Low ionization energy: They readily lose one electron to achieve a stable noble gas configuration. This makes them highly reactive, especially with water and oxygen.
* Strong reducing agents: Their tendency to lose electrons means they readily donate electrons to other elements, causing a reduction reaction.
Group 7: Halogens
* High electronegativity: They have a strong tendency to gain one electron to achieve a stable noble gas configuration.
* Strong oxidizing agents: They readily accept electrons from other elements, causing an oxidation reaction.
Why they exist as compounds:
* Stability: The compounds they form are more stable than their pure elemental forms because the atoms achieve a more stable electron configuration by bonding.
* Reactions with other elements: Alkali metals react vigorously with nonmetals like oxygen and halogens. Halogens react readily with metals and other nonmetals.
Examples:
* Sodium (Group 1): Sodium reacts violently with water to form sodium hydroxide (NaOH) and hydrogen gas. It also reacts with chlorine to form sodium chloride (NaCl) or table salt.
* Chlorine (Group 7): Chlorine reacts with sodium to form sodium chloride (NaCl) and with hydrogen to form hydrogen chloride (HCl), which is a strong acid.
In summary:
The highly reactive nature of group 1 and 7 elements makes them unstable in their pure forms. They readily react with other elements to form more stable compounds, which are more common in nature.
