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  2. Aluminium oxide (data page) - Wikipedia

    en.wikipedia.org/wiki/Aluminium_oxide_(data_page)

    Phase behavior Triple point? K (? °C), ? Pa Critical point? K (? °C), ? Pa Std enthalpy change of fusion, Δ fus H o? kJ/mol Std entropy change of fusion, Δ fus S oJ/(mol·K)

  3. Aluminium oxide - Wikipedia

    en.wikipedia.org/wiki/Aluminium_oxide

    Aluminium oxide (or aluminium(III) oxide) is a chemical compound of aluminium and oxygen with the chemical formula Al 2 O 3. It is the most commonly occurring of several aluminium oxides, and specifically identified as aluminium oxide. It is commonly called alumina and may also be called aloxide, aloxite, or alundum in various forms and ...

  4. Bond length - Wikipedia

    en.wikipedia.org/wiki/Bond_length

    It is generally considered the average length for a carbon–carbon single bond, but is also the largest bond length that exists for ordinary carbon covalent bonds. Since one atomic unit of length (i.e., a Bohr radius) is 52.9177 pm, the C–C bond length is 2.91 atomic units, or approximately three Bohr radii long.

  5. Aluminium oxides - Wikipedia

    en.wikipedia.org/wiki/Aluminium_oxides

    Aluminium oxides or aluminum oxides are a group of inorganic compounds with formulas including aluminium (Al) and oxygen (O). Aluminium(I) oxide ( Al 2 O ) Aluminium(II) oxide ( AlO ) (aluminium monoxide)

  6. Molecular geometry - Wikipedia

    en.wikipedia.org/wiki/Molecular_geometry

    Molecular geometries can be specified in terms of 'bond lengths', 'bond angles' and 'torsional angles'. The bond length is defined to be the average distance between the nuclei of two atoms bonded together in any given molecule. A bond angle is the angle formed between three atoms across at least two bonds.

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  8. Metallic bonding - Wikipedia

    en.wikipedia.org/wiki/Metallic_bonding

    The strong bonding of metals in liquid form demonstrates that the energy of a metallic bond is not highly dependent on the direction of the bond; this lack of bond directionality is a direct consequence of electron delocalization, and is best understood in contrast to the directional bonding of covalent bonds.

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