define covalent bond. Illustrate covalent bond formation with Lewis electron period diagrams.

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Ionic bonding commonly occurs once it is straightforward for one atom to lose one or much more electrons and also another atom to obtain one or much more electrons. However, part atoms won’t offer up or gain electrons easily. Yet they still take part in compound formation. How? over there is an additional mechanism for obtaining a finish valence shell: sharing electrons. When electrons are shared in between two atoms, they make a bond referred to as a covalent bond.

Let us show a covalent link by utilizing H atoms, with the knowledge that H atoms need only 2 electrons to to fill the 1s subshell. Every H atom starts through a solitary electron in that valence shell:

\<\mathbfH\, \cdot \; \; \; \; \; \mathbf\cdot \: H\>

The two H atoms can share your electrons:

\<\mathbfH\: \mathbf: H\>

We can use one to display that every H atom has actually two electrons about the nucleus, fully filling each atom’s valence shell:


Because every H atom has a filled valence shell, this link is stable, and also we have actually made a diatomic hydrogen molecule. (This defines why hydrogen is just one of the diatomic elements.) because that simplicity’s sake, the is not inexplicable to stand for the covalent bond through a dash, instead of v two dots:


Because 2 atoms are sharing one pair that electrons, this covalent bond is called a single bond. As an additional example, think about fluorine. F atoms have seven electrons in your valence shell:


These 2 atoms deserve to do the exact same thing that the H atoms did; they share their unpaired electrons to do a covalent bond.

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Note that each F atom has actually a finish octet roughly it now:


We can likewise write this utilizing a dash to stand for the shared electron pair:


There are two different species of electrons in the fluorine diatomic molecule. The bonding electron pair makes the covalent bond. Each F atom has three other pairs of electron that execute not get involved in the bonding; castle are called lone pair electrons. Every F atom has one bonding pair and also three lone pairs of electrons.

Covalent bonds have the right to be made between different facets as well. One example is HF. Every atom beginning out with an odd variety of electrons in that valence shell: