Molecular and Ionic Compounds

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Molecular compounds

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Involve the sharing of electrons between atoms, unlike ionic compounds which involve the transfer of electrons.

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A molecule is defined as

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a neutral group of atoms held together by covalent bonds, which can vary in size and complexity.

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Diatomic molecules

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consist of only two atoms, such as O2 (oxygen) or H2 (hydrogen).

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The molecular formula

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indicates the number of each type of atom in a molecule, omitting the subscript '1' for single atoms.

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Molecular compound characteristics

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Low melting and boiling points are characteristic of molecular compounds, often making them gases or liquids at room temperature.

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Molecular compound conductivity

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poor conductors of electricity due to the lack of free-moving charged particles.

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Molecular compounds at room temp (typically)

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Molecular compounds are often gases or liquids.

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The representative unit for ionic compounds vs molecular compounds

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Formula units represent ionic compounds, while molecules represent molecular compounds.

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Diatomic molecules

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Covalent compound consisting of 2 atoms of the same element. Examples: H2, N2, O2, and Cl2

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Covalent bonds can be classified as single, double, or triple based on the number of shared electron pairs

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Single covalent bonds involve one shared pair of electrons, double bonds involve two shared pairs, and triple bonds involve three shared pairs of electrons.