Oxides Oxides across a period The acid-base character of the oxides provides evidence of chemical trends in the periodic table The broad trend is that oxides change from basic through amphoteric to...
Metallic & Non-metallic Periodic trends can also be seen in the typical properties of metals and non-metals which are summarised below: The typical properties of metals and non-metals The typic...
Electronegativity: Definition Electronegativity is the ability of an atom to attract a pair of electrons towards itself in a covalent bond This phenomenon arises from the positive nucleus’s ability...
Electron Affinity When atoms gain electrons they become negative ions or anions Electron affinity (EA) can be thought of as the opposite process of ionisation energy and is defined as The amount of...
First Ionisation Energy The ionisation energy (IE) of an element is the amount of energy required to remove one mole of electrons from one mole of atoms of an element in the gaseous state to form o...
Atomic & Ionic Radius Atomic radius The atomic radius of an element is a measure of the size of an atom It is the distance between the nucleus of an atom and the outermost electron shell It can...
Structure of the Periodic Table The periodic table is a list of all known elements arranged in order of increasing atomic number, from 1 to 118. In addition to this, the elements are arranged in su...
Electron Configurations: Basics The electron configuration gives information about the number of electrons in each shell, subshell and orbital of an atom The subshells are filled in order of increa...
Electron Orbitals Each shell can be divided further into subshells, labelled s, p, d and f Each subshell can hold a specific number of orbitals: s subshell : 1 orbital p subshell : 3 orbitals label...
