Types of Chemical Bonds

Chemical bonding is the attraction between atoms. The bond between two atoms is what causes a molecule to be a substance. The bond between atoms also gives a substance its chemical properties. The strength of a material and its ability to resist breaking is determined by its chemical bonds. These bonds hold the molecules of a material together and determine its strength and hardness. 

Types of chemical bonds

There are mainly five types of chemical bonds: ionic, covalent, coordinate or dative, metallic, and hydrogen.

Ionic bond

Ionic bonding is one of the most important types of chemical bonding. It is responsible for the very existence of the solid state, which is the basis of all physical and chemical properties. The ionic bond consists of the transfer of polar covalent bonding electrons from one atom to another. This leads to the formation of oppositely charged ions in the molecule. Ionic compounds are formed by the attraction between oppositely charged ions.

It is impossible to separate the metallic ions in an ionic compound by heating or applying electrical current because they have strong electrostatic bonds. The strength of an ionic bond depends on the number of electrons transferred. It also depends on the difference in electronegativity; if the difference between electronegativity values is significant, the bond formed is strong. Ionic compounds have a high melting and boiling point compared to other compounds formed by covalent or metallic bonds.

Covalent bond 

A covalent bond is formed by an attractive force between atoms, in which the electrons are shared. This type of bonding occurs between two atoms of an equivalent element. This bond is usually found among non-metals, but it also occurs between metals and nonmetals. Metals by themselves never form covalent bonds.

Molecules with covalent bonds include inorganic substances such as hydrogen, nitrogen, chlorine, water, and ammonia, along with all organic compounds.

In the structural representation of compounds, the bonds are shown with the help of lines between the atoms. A single line indicates a single covalent bond between two atoms; two lines indicate a double covalent bond between two atoms; three lines mean a triple covalent bond.

Coordinate or dative bond

Coordinate bonds are formed between objects or features with coordinates. Coordinates are specified by a set of numbers that indicate the location of an object or feature in a 2D or 3D space. The coordinates of an object or feature can be thought of as its position or location on a coordinate plane or grid. The location of one object or feature on the coordinate plane or grid can be represented by a pair of coordinates.

Metallic bond

Metallic bonds are chemical bonds that form when one atom is attached to another through a permanent sharing of electrons. This means that unlike ionic bonds, where one atom gains or loses electrons, metallic bonds are not affected by other atoms or ions. This also means that unlike covalent bonds, where two or more atoms share a pair of electrons to form a chemical bond, metallic bonds only involve sharing a single electron or pair of electrons to form a strong bond. Metallic bonds are the most common type found in nature. The most common example of a metallic bond is when iron forms a bond with oxygen to create rust. Rust is a solid form of iron that is highly reactive and is used for various purposes, such as making paper and paint.

Hydrogen bond

A hydrogen bond is a weak bond created between a hydrogen atom and an electronegative element that has a lone pair to share with the hydrogen atom to create an electrostatic attraction between portions of the molecule of the two atoms.

The nature of a hydrogen bond is either dipole-dipole type, ion-dipole type, or dipole-induced dipole type.

The hydrogen atom mainly forms a bond with the chemical elements of fluorine, nitrogen, and oxygen. In the context of organic chemistry, it forms a bond with the elements of carbon and chlorine.

There are certain prerequisites for forming a hydrogen bond; for example, the element forming a bond with the hydrogen atom must be electronegative. Also, the atom’s electronegativity must be equal to or greater than 3. Finally, the atom must have a lone pair to share with the hydrogen atom, which must be smaller in size.

Conclusion

The molecules and compounds that make up our world are held together by chemical bonds. The stronger the bonds, the stronger the material. However, not all bonds are equal. Some are stronger than others, and some are stronger in certain circumstances than others.

There are five types of chemical bonds: ionic, covalent, hydrogen, coordinate/dative, and metallic. We have also discussed the electronic theory of chemical bonding, in which a chemical bond is formed between atoms to get the nearest inert gas configuration. This can be achieved by either losing or gaining/sharing electrons.