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== Introduction ==

Electron sharing is a fundamental concept in [[Chemistry|chemistry]], particularly in the study of [[Chemical Bonding|chemical bonding]]. It refers to the process where atoms share electrons to achieve a stable [[Electron Configuration|electron configuration]], typically a full outer shell, which is often referred to as the [[Octet Rule|octet rule]]. This sharing of electrons results in the formation of a [[Covalent Bond|covalent bond]], a strong chemical bond that holds atoms together in a molecule.

[[Image:Detail-71919.jpg|thumb|center|A close-up view of two atoms sharing electrons.|class=only_on_mobile]]
[[Image:Detail-71920.jpg|thumb|center|A close-up view of two atoms sharing electrons.|class=only_on_desktop]]

== Understanding Electron Sharing ==

The concept of electron sharing is rooted in the principles of [[Quantum Mechanics|quantum mechanics]]. According to the [[Quantum Theory|quantum theory]], electrons exist in regions around the nucleus of an atom known as [[Atomic Orbital|atomic orbitals]]. These orbitals can be visualized as a cloud-like region where there is a high probability of finding an electron. Each orbital can hold a maximum of two electrons, which must have opposite spins according to the [[Pauli Exclusion Principle|Pauli Exclusion Principle]].

When an atom has an incomplete outer shell, it tends to react with other atoms to achieve stability. This can be achieved in two ways: by transferring electrons, leading to the formation of [[Ionic Bond|ionic bonds]], or by sharing electrons, leading to the formation of covalent bonds. Electron sharing is the mechanism behind the latter.

== Covalent Bonding and Electron Sharing ==

In a covalent bond, two atoms share one or more pairs of electrons. This allows both atoms to reach a stable electron configuration. The shared electrons are counted as part of the electron configuration of both atoms. This type of bond is common in nonmetals and is characterized by the sharing of electron pairs between atoms.

For example, in a molecule of [[Hydrogen|hydrogen]] (H2), each hydrogen atom shares its single electron with the other, forming a covalent bond. This allows each hydrogen atom to achieve the stable electron configuration of the nearest noble gas, helium.

== Types of Covalent Bonds ==

There are three types of covalent bonds: single, double, and triple. These are distinguished by the number of electron pairs that are shared between two atoms.

- Single Covalent Bond: A single covalent bond involves the sharing of one pair of electrons. This is seen in a hydrogen molecule (H2), where two hydrogen atoms share one pair of electrons.

- Double Covalent Bond: A double covalent bond involves the sharing of two pairs of electrons. This is seen in an oxygen molecule (O2), where two oxygen atoms share two pairs of electrons.

- Triple Covalent Bond: A triple covalent bond involves the sharing of three pairs of electrons. This is seen in a nitrogen molecule (N2), where two nitrogen atoms share three pairs of electrons.

== Factors Influencing Electron Sharing ==

There are several factors that influence the sharing of electrons between atoms. These include the [[Electronegativity|electronegativity]] of the atoms involved, the atomic size, and the energy required to form the bond.

- Electronegativity: Electronegativity is a measure of an atom's ability to attract shared electrons. In a covalent bond, if one atom is more electronegative than the other, the shared electrons will be more attracted to the more electronegative atom. This can lead to a polar covalent bond, where the electrons are not shared equally.

- Atomic Size: The size of an atom can also influence electron sharing. Larger atoms have their valence electrons further from the nucleus, making them less tightly held and more likely to be shared.

- Energy: The formation of a covalent bond involves a balance between the energy required to bring two atoms close together and the energy released when the bond is formed. The bond forms if the energy released is greater than the energy required.

== Conclusion ==

Electron sharing is a fundamental concept in chemistry that explains the formation of covalent bonds. It is a process where atoms share electrons to achieve a stable electron configuration. The understanding of electron sharing is crucial for the study of molecular structures and chemical reactions.

== See Also ==

- [[Ionic Bonding]]
- [[Molecular Orbital Theory]]
- [[Valence Bond Theory]]

[[Category:Chemistry]]
[[Category:Physical Chemistry]]
[[Category:Chemical Bonding]]