The Alkali metals, the Halogens and the noble gases
The alkali metals are a group of elements in the periodic table that
includes lithium, sodium, potassium, rubidium, cesium, and
francium. They are all highly reactive, which means they readily
lose electrons to form positive ions. As a result, alkali metals are
typically found in nature in the form of compounds, rather than as
pure elements. They are also highly reducing, which means they can
donate electrons to other elements and reduce them to their
elemental form.
The halogens are a group of elements that includes fluorine,
chlorine, bromine, iodine, and astatine. Like the alkali metals, the
halogens are highly reactive and can gain electrons to form negative
ions. They are known for their strong oxidising properties, which
means they can accept electrons from other elements and oxidise
them to their elemental form. The halogens are also highly
electrophilic, which means they are attracted to electrons and can
readily participate in chemical reactions with other elements.
When an alkali metal reacts with a halogen, the result is a
compound known as a salt. The alkali metal donates an electron to
the halogen, which gains the electron and becomes negatively
charged. The alkali metal then becomes positively charged and
forms an ion. The positive and negative ions are attracted to each
other and form an ionic bond, resulting in the formation of a salt.
