Week 7B Intro to Bonding and Ionic Bonds

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Molecule

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A group of atoms bonded together, representing the smallest fundamental unit of a chemical compound that can participate in a chemical reaction.

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Covalent bond

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A type of chemical bond where two atoms share one or more pairs of electrons to achieve a full outer shell.

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Lewis diagram

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A representation of a molecule showing how valence electrons are arranged among the atoms, with dots for electrons and lines for bonds.

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Electron dot structure

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Another term for a Lewis diagram; it displays valence electrons around atoms to show bonding and lone pairs.

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Valence electrons

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Electrons in the outermost energy level of an atom that participate in chemical bonding.

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Molecular orbital

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A region of space where electrons are likely to be found in a molecule; formed by the overlap of atomic orbitals when atoms bond.

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Octet rule

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A rule stating that atoms tend to gain, lose, or share electrons to have a full set of eight valence electrons, achieving a stable electron configuration similar to noble gases.

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Lone pair

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A pair of valence electrons that are not involved in bonding and belong exclusively to one atom.

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Double bond

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A covalent bond in which two pairs of electrons are shared between two atoms.

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Triple bond

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A covalent bond where three pairs of electrons are shared between two atoms.