In 1916, Kossel and Lewis succeeded in giving a successful explanation based upon the concept of an electronic configuration of noble gases about why atoms combine to form molecules. Atoms of\u00a0noble gases\u00a0have little or no tendency to combine with each other or with atoms of other elements. This means that these atoms must have stable electronic configurations.<\/p>\n\n\n\n
Due to the stable configuration, the noble gas atoms neither have any tendency to gain nor lose electrons and, therefore, their combining capacity or valency is zero. They are so inert that they do not even form diatomic molecules and exist as monoatomic gaseous atoms.<\/p>\n\n\n\n
When substances participate in chemical bonding and yield compounds, the stability of the resulting compound can be gauged by the type of chemical bonds it contains.<\/p>\n\n\n\n
The type of chemical bonds formed varies in strength and properties. There are 4 primary types of chemical bonds which are formed by\u00a0atoms or molecules\u00a0to yield compounds. These types of chemical bonds include<\/p>\n\n\n\n
These types of bonds in chemical bonding are formed from the loss, gain or sharing of electrons between two atoms\/molecules.<\/p>\n\n\n\n
Ionic bonding is a type of chemical bonding which involves a transfer of electrons from one atom or molecule to another. Here, an atom loses an electron, which is, in turn, gained by another atom. When such an electron transfer takes place, one of the atoms develops a negative charge and is now called the anion.<\/p>\n\n\n\n
The other atom develops a positive charge and is called the cation. The\u00a0ionic bond\u00a0gains strength from the difference in charge between the two atoms, i.e., the greater the charge disparity between the cation and the anion, the stronger the ionic bond.<\/p>\n\n\n\n
Types of Chemical Bonds \u2013 Ionic bonding<\/p>\n\n\n\n
A\u00a0covalent bond\u00a0indicates the sharing of electrons between atoms. Compounds that contain carbon (also called organic compounds) commonly exhibit this type of chemical bonding. The pair of electrons which are shared by the two atoms now extend around the nuclei of atoms, leading to the creation of a molecule.<\/p>\n\n\n\n
Covalent bonds can be either polar or non-polar in nature. In polar covalent chemical bonding, electrons are shared unequally since the more electronegative atom pulls the electron pair closer to itself and away from the less electronegative atom. Water is an example of such a polar molecule.<\/p>\n\n\n\n
A difference in charge arises in different areas of the atom due to the uneven spacing of the electrons between the atoms. One end of the molecule tends to be partially positively charged, and the other end tends to be partially negatively charged.<\/p>\n\n\n\n
Compared to ionic and covalent bonding, Hydrogen bonding is a weaker form of chemical bonding. It is a type of polar covalent bonding between oxygen and hydrogen, wherein the hydrogen develops a partial positive charge. This implies that the electrons are pulled closer to the more electronegative oxygen atom.<\/p>\n\n\n\n
This creates a tendency for the hydrogen to be attracted towards the negative charges of any neighbouring atom. This type of chemical bonding is called a\u00a0hydrogen bond\u00a0and is responsible for many of the properties exhibited by water.<\/p>\n\n\n\n
The bond formed as a result of strong electrostatic forces of attraction between a positively and negatively charged species is called an\u00a0electrovalent or ionic bond. The positively and negatively charged ions are aggregated in an ordered arrangement called the crystal lattice, which is stabilised by the energy called the Lattice enthalpy.<\/p>\n\n\n\n
Generally, the ionic bond is formed between a metal cation and a non-metal anion.<\/p>\n","protected":false},"excerpt":{"rendered":"
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