chemical bonding

How to Understand Chemical Bonding

How to Understand Chemical Bonding: A Simple Guide

Introduction

Molecules are the smallest form of matter that can exist. An atom or a molecule can consist of a single nucleus and other basic building blocks such as electrons, nuclei, or atoms. However, these are simply parts of matter. If the number of atoms or nuclei are larger, the matter would be called a molecule. Molecules are composed of atoms, and every atom in a molecule has different kinds of electrons that can bond to each other. A chemical bond is one of the ways of holding the atoms together. This holds true for all kinds of bonds but is especially important for covalent bonds. The constant interplay of covalent bonds between atoms is responsible for the creation of the molecules in our bodies, and the ions in our ionized environment.

Covalent Bonding

Covalent bonds are very strong, because of the very high energy required to break them. The strongest chemical bond in the world is between two platinum atoms. Any covalent bond (or any bond that is attached to another compound) requires lots of energy to break. Covalent bonds are usually symmetric and very stable. Covalent bonds also don't move much, meaning that atoms don't move apart easily. This is why we can heat up our bodies and engines without any effect. Polar Covalent Bonding Polar covalent bonds are quite different. They are not very strong, and can often break even without the help of energy. The polar covalent bonds that exist between a metal and a nonmetal, however, will become unstable at high temperature.

Polar Covalent Bonding

The characteristics of a covalent bond include two or more atoms joining together. In the case of a covalent bond, the constituent atoms are bonded together like a circle is joined together by a line. The force applied on the two atoms is perpendicular to their relative positions. For example, the bond between carbon and hydrogen, called the carbon-hydrogen (CH 3 ) bond, is a polar covalent bond. The terms polar and covalent are used synonymously. Classical properties of a covalent bond include the fact that the bond tends to be more stable than the equivalent ionic bond. Furthermore, chemical bonds form very easily and are unlikely to break or slip. The decrease in risk is attributable to the fact that most covalent bonds are highly cohesive.

Ionic Bonding

Ionic bonds allow atoms to move around so they can react with each other. These bonds help molecules interact, either by pushing, pulling, or by reactivating an existing bond. Examples of Common Ionic Bonding: A water molecule, for example, bonds with an oxygen atom so the water molecule can absorb oxygen from the air. The hydrogen molecule bonds with the carbon atom in a carbonyl group to form a carboxylic acid. The oxygen in water bonds to nitrogen to create an ion (or nitrogen ion). Polar Covalent Bonding Polar covalent bonds are forces that hold atoms together. These bonds include van der Waals bonds, and Lewis bonds, in which atoms form single-letter bonds. Lewis-charged bonds are created by adding a single electron to an atom.

Conclusion

In the first section of this post we saw how different molecules are tied together by intermolecular forces. In the second part of this post we looked at chemical bonds and some of the intermolecular forces that form those bonds. In the third part of this post we will focus on covalent bonds and polar covalent bonds. Following the steps outlined in this post, when you understand what intermolecular forces are, then you can begin to understand how to apply the principles of chemistry to your life.

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