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| - Covalent bonding is done between two non-metal elements. Here, the atoms share electrons so that they have a full outer shell, or a stable electronic configuration. Examples are: Water- H20 and Ethanol- C2H6O.
- Covalent bonds occur when two atoms of similar electronegativity, usually two organic elements, bond by sharing electrons. When this occurs electrons in the bond freely move between the orbitals of both atoms. A single bond occurs when a two electrons are shared between two nuclei/atoms. When this occurs, both electrons contribute their charges to both atoms. This happens because the electrons move within the orbitals of both atoms. Usually, each atom contributes one electron to the bond, but in some cases one atom contributes two electrons to the bond.
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| abstract
| - Covalent bonding is done between two non-metal elements. Here, the atoms share electrons so that they have a full outer shell, or a stable electronic configuration. Examples are: Water- H20 and Ethanol- C2H6O.
- Covalent bonds occur when two atoms of similar electronegativity, usually two organic elements, bond by sharing electrons. When this occurs electrons in the bond freely move between the orbitals of both atoms. A single bond occurs when a two electrons are shared between two nuclei/atoms. When this occurs, both electrons contribute their charges to both atoms. This happens because the electrons move within the orbitals of both atoms. Usually, each atom contributes one electron to the bond, but in some cases one atom contributes two electrons to the bond. In addition to single bonds, there are double and triple bonds. These are similar to single bonds by how electrons are shared between the two nuclei/atoms. However, they differ from single bonds by the number of electrons shared. In double bonds, four electrons are shared. In triple bonds, six are shared. One way to pictorially represent covalently-bonded molecules is with Lewis structures. These pictorially represent an atom's outer electron s and p-orbitals with dots or X's drawn in an octet around a chemical symbol. See below for an example. This is a Lewis dot representation of elemental nitrogen. Notice how the number of dots corresponds to the number of s and p-orbital electrons (2+3=5 total). In Lewis dot structures, the atoms form bonds when dots are shared between the atoms, as shown below. In this Lewis dot representation, the central carbon is bonded to three hydrogens and one oxygen. This one oxygen is subsequently bonded to one hydrogen. Notice how each bond is made up of two dots representing electrons. As previously stated, each atom contributes one electron to this bond.
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