Chemical bonds are produced nearly exclusively as a result of interactions between valence electrons in atoms. Valence electrons should be depicted in a simple manner so that we can better understand how they interact with each other.

This type of diagram (also known as an electron dot diagram, or a Lewis structure) depicts the valence electrons for a certain element in the form of a series of dots encircling the element’s symbol. The number of valence electrons in an atom is represented by the number of dots on a graph. Arrangement: The dots are arranged to the right and left of the symbol, as well as above and below it, with no more than two dots on either side. (It makes no difference which positions are used in which order.)

Brief note on how to draw a Lewis structure: 

In a Lewis structure, the electron density surrounding atoms is visually displayed. Understanding Lewis structures enables you to predict the number and type of bonds that will surround an atom. It is also possible to utilise a Lewis structure to forecast a molecule’s geometry. Chemistry students are typically baffled by the models, however they can easily sketch Lewis structures provided the proper procedures are followed. Lewis constructions can be built in a multitude of ways, so keep that in mind. In these instructions, the Kelter method for drawing Lewis structures for molecules is explained.

The first step is to figure out how many valence electrons there are in the atom.

Counting the number of valence electrons in each molecule is now complete.

Make sure that the atoms are stable with the number of electrons they require.

To put it another way, full outer electron shells are thought of as “happy” atoms. Eight electrons are required for the outer electron shell of elements in the periodic table up to period four. The term “octet rule” is used to describe this phenomenon.

Work out the number of bonds in the molecule.

Covalent bonds are formed when two electrons from each atom form an electron pair. For example, Step 2 tells you how many electrons are required, and you can use this information to determine how many electrons you already possess. In order to arrive at the final octets’ number of electrons, subtract Step 1’s value from Step 2’s value and multiply the result by 8. This means that the number of bonds is half of what it would have been if all electrons had been used to make them.

A Centre Atom must be chosen at this point.

Most molecules have a single, central atom that is the least electronegative atom in the molecular chain. Use the periodic table trends or an electronegativity table to determine the electronegativity of a substance. Electronegativity drops as one moves down a group of the periodic table, but it increases as one moves across a period. Atoms of hydrogen and halogen are almost never present at the centre of a molecule.

In Step 5, draw a Skeletal Structure.

Atoms are connected to the central atom by an unbroken line suggesting the presence of a link between them. Any number of extra atoms can be connected to the main one.

In Step 6, Add Electrons to the Outside Atoms.

Make sure you fill in all of the octets surrounding each of the outer atoms with zeros. If there aren’t enough electrons to complete the octets, the skeletal structure from Step 5 is incorrect. Try out a different set-up. It may take some trial and error to get the hang of this at first. The ability to predict bone forms improves with practice.

Step 7 requires the final electrons to be placed around the centre atom.

The remaining electrons must be used to complete the octet surrounding the central atom. Using lone pairs on the outside atoms of any remaining bonds from Step 3, form additional double bonds. A double bond is depicted by painting two solid lines in between two atoms. If the central atom contains more than eight electrons and is not an exception, the first step may have been incorrectly counted. It’s for this reason. The molecule’s Lewis dot structure will be complete after this step.

Lewis dot structure for Carbon :

 When an element or molecule has an electron dot diagram, this is referred to as Lewis structure; it shows the distribution of valence electrons around the element or molecule.

Due to the fact that carbon possesses four valence electrons, they are depicted as if they were drawn on the four sides of a carbon atom as shown in the drawings below.

Lewis structure of CO : 

Carbon monoxide (CO) is a toxic gas that has no odour or colour and can be detected with the naked eye. Because of the way it is constructed, it has two unique atoms: carbon and hydrogen. It’s a polar molecule with bond angles that are 180 degrees. There is a triple bond between the carbon and oxygen atoms in this compound. The carbon monoxide molecule has a total of ten valence electrons in its structure.

Octet configuration of Carbon : 

When it comes to stabilising an atom’s outermost energy level, the octet rule says that eight electrons are required. This is the understanding that most atoms try to achieve by filling the outermost energy level’s electron s and p orbitals with eight electrons. Carbon has an electron configuration of 1s22s22p2, which means that it has four valence electrons, which is the same as the configuration of 1s22s22p2.

Conclusion : 

Chemical bonds are produced nearly exclusively as a result of interactions between valence electrons in atoms. It would be beneficial to have a simple manner of depicting valence electrons in order to better understand how they interact with one another.When an element or molecule has an electron dot diagram, this is referred to as Lewis structure; it shows the distribution of valence electrons around the element or molecule.