Unlike ionic bonds, covalent binding are frequently formed in between atoms where one of the atoms cannot easily acquire a noble gas electron shell configuration v the lose or acquire of one or 2 electrons. In together cases, it is simpler to ‘share’ valence electrons.

Electron ‘sharing’ occurs when the electrons in the outermost electron shell, or valence shell electrons, native one atom deserve to be supplied to finish the outermost electron shell of one more atom without being permanently transferred, together occurs in the development of an ion. Electrons deserve to only be so much from an atom prior to they are no longer associated with it; therefore, share electrons and forming covalent bond restricts the preferably distance in between two external inspection atoms.

A finish outermost electron covering is the most stable state. As such atoms the bond covalently share your electrons to finish their valence shell. Let’s an initial use the example of Hydrogen (H). Hydrogen has actually one electron and requires one added electron to have actually the very same valence shell configuration as the noble gas Helium (He). The simplest way to attain this is for two hydrogen atoms to share their single electron v one another. Shown below, every Hydrogen atom (H) and also its single electron are portrayed in one of two people red or blue. Once the two atoms share their single electrons (shown in ~ the oval), the beginnings of the electrons are tantamount from one another. Therefore it appears that there are two electron in the valence shells of both the red H and also the blue H.

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What about more facility examples? Carbon (C) has four valence electrons, and requires four added electrons to have the very same valence covering configuration together Neon (Ne). Developing a solitary covalent bond through a 2nd carbon atom will certainly not complete either atom’s valence shell. Because of this a Carbon atom can instead share each of its electrons with four separate Hydrogen atoms. This completes the valence shells for four Hydrogen atoms and also one Carbon atom. In this example, one pair of electron is shared between two atoms. The covalent bond shown listed below are all called single covalent bonds.

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As one can surmise, there room a range of methods of arranging electrons in covalent bonds. Different atoms linked by a covalent bond carry out not necessarily add equal numbers of electrons. In addition an individual atom might contribute much more than one electron come a covalent bond. Making use of Carbon and also Hydrogen as examples again, take into consideration the construction of electron sharing required to produce C2H6, C2H4, and also C2H2.

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The bonds developed by common electrons are frequently simplified right into lines in between the external inspection atoms. Each line represents one pair the electrons. As such the three compounds over can it is in redrawn as presented below.

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Using mutual electrons to finish valence shells has actually some straight implications to the compounds. The valence shells will just be finish so long as the electrons room shared, which calls for that the bonded atoms stay close to one another. Atoms within covalent bonds would shed their finish valence shells if they to be separated. This is in contrast to ionic bonds; the valence shells of ions space not impacted when ionic bonds are disrupted. Thus, covalent binding are frequently very strong regardless of environment since the after-effects to the valence shells would certainly be the very same in every situations.