AS-Level The Periodic Table
The Periodic Table
The periodic table is a fundamental tool used by chemists (and chemistry students!) all over the world. Elements are arranged based on their atomic number (number of protons).
The periodic table is a visual way of representing the atomic structures of all elements. The structure of atoms shows us that as elements get bigger, their properties change. Certain characteristics of an element can be predicted based on its atomic structure.
For s and p-block elements (see below), atoms can only have eight electrons in their outermost electron shell (octet rule). Part of the reactivity of an atom comes from how many electrons are in its outer shell (valence number). Atoms with the same number of electrons in their outer shells behave in similar ways.
There are only eight possibilities for the number of outermost electrons for s and p-block elements, these are shown as ‘groups’ in the periodic table. All the elements in a particular group have the same number of outer electrons (valency).
As there are only eight possibilities for outermost electrons in an element, there are only eight groups in the periodic table. Once an element has a full outer shell the element that follows next (in the order of number of protons) must be a group 1 element, so a new row in the table is formed. Each row in the periodic table is called a period.
It’s not just the number of outermost electrons that can be different between elements, but also the type of orbital shell that the electrons exist in. As we move across a period in the table, we are adding a proton (and an electron) to each element. This means we fill the orbitals as follows for period 3:
The shape of orbital that the outermost electron exists in is known as the element’s ‘block’.