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How are covalent bonds represented in Lewis structures?
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covalent bond
In polar covalent bonds, such as that between hydrogen and oxygen atoms, the electrons are not transferred from one atom to the other as they are in an ionic bond. Instead, some outer electrons merely spend more time in the vicinity of the other atom. The effect of this orbital distortion is to induce regional net charges that hold the atoms together, such as in water molecules.
In Lewis structures, a covalent bond is represented by a line (or dash) connecting two atoms, which signifies a shared electron pair known as a bonding pair.12
The representation of these bonds follows specific conventions:
- Single bonds: Indicated by a single line, representing one shared electron pair.2
- Multiple bonds: Indicated by multiple lines, such as double lines (=) for a double bond (two shared pairs) and triple lines (β‘) for a triple bond (three shared pairs).2
- Lone pairs: Electrons that are not involved in bonding are typically represented as pairs of dots on the individual atoms.12
It is important to note that while these structures effectively illustrate the topological pattern of bonds and the distribution of valence electrons, they do not necessarily represent the actual three-dimensional shape of the molecule.12