Ionic Bonds

Electron arrangement and trends in properties shielding the other electrons from the charge of the nucleus. As a result of this the other electrons are more strongly attracted to the nucleus, and the radius of the atom gets smaller. When an electron is added to an atom, forming an anion, the added electron repels other electrons, resulting in an increase in the size of the atom. In regards to the trend size of ionic radii is due to shielding of the outermost electrons by the inner-shell electrons so that the outer shell electrons does not get the positive charge of the nucleus. (Chemguide, 2016)

 Electronegativity

Electronegativity is a measure of the attraction an atom has for the electrons in the bond that are involved in a bond. An atom which has a high electronegativity would attract bonded electrons towards it, bringing them closer where as an atom which has a low electronegativity will have an extremely weak attraction for electrons. On a periodic table, electronegativity values increases from left to right and decrease on a descending group. (Clark, 2016)

 Type of bonding in the element

Ionic bonds form when a non-metal and a metal exchange electrons, while covalent bonds form when electrons are shared between two non-metals. There are two bonds known as Ionic Bonds and Covalent Bonds. Ionic bonds form between metals and non-metals whereas covalent bonds are formed when electron are shared between two non-metals. An ionic bond is formed though an electrostatic attraction between two positively charged ions. Bonds between a partly ionic ion and a partly covalent ion is known as a polar covalent bond. A covalent bond is when electrons are shared between atoms and the most stable state is when the valence electron shell is full. Then, atoms form a covalent bonds share their valence electrons to get a more stable state. (Janet Rae-Dupree,