Matches in DBpedia 2016-04 for { ?s ?p "In chemistry, the linear molecular geometry describes the geometry around a central-atom bonded to two other atoms (or ligands) placed at a bond-angle of 180°. Linear=organic molecules, such as acetylene (HC≡CH), are often described by invoking sp orbital hybridization for their carbon-centers.According to the VSEPR model, linear-geometry occurs at central-atoms with two bonded-atoms and zero or three lone-pairs (AX2 or AX2E3) in the AXE notation. Neutral AX2 molecules with linear-geometry include beryllium fluoride (F—Be—F) with two single-bonds, carbon dioxide (O=C=O) with two double-bonds, hydrogen cyanide (H—C≡N) with one single and one triple-bond. The most important linear-molecule with more than three atoms is acetylene (H—C≡C—H), in which each of its carbon atoms is considered to be a central-atom with a single-bond to one hydrogen and a triple=bond to the other carbon atom. Linear-anions include azide (N3−) and thiocyanate (SCN−), and a linear-cation is nitronium ion (NO2+).Linear-geometry also occurs in AX2E3 molecules, such as xenon difluoride (XeF2) and the triiodide-ion (I3−) with one iodide bonded to the two others. As described by the VSEPR model, the five-valence, electron-pairs on a central-atom form a trigonal bipyramid in which the three lone-pairs occupy the less crowded, equatorial-positions and the two bonded-atoms occupy the two axial-positions at the opposite-ends of an axis, forming a linear-molecule."@en }
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- Linear_molecular_geometry abstract "In chemistry, the linear molecular geometry describes the geometry around a central-atom bonded to two other atoms (or ligands) placed at a bond-angle of 180°. Linear=organic molecules, such as acetylene (HC≡CH), are often described by invoking sp orbital hybridization for their carbon-centers.According to the VSEPR model, linear-geometry occurs at central-atoms with two bonded-atoms and zero or three lone-pairs (AX2 or AX2E3) in the AXE notation. Neutral AX2 molecules with linear-geometry include beryllium fluoride (F—Be—F) with two single-bonds, carbon dioxide (O=C=O) with two double-bonds, hydrogen cyanide (H—C≡N) with one single and one triple-bond. The most important linear-molecule with more than three atoms is acetylene (H—C≡C—H), in which each of its carbon atoms is considered to be a central-atom with a single-bond to one hydrogen and a triple=bond to the other carbon atom. Linear-anions include azide (N3−) and thiocyanate (SCN−), and a linear-cation is nitronium ion (NO2+).Linear-geometry also occurs in AX2E3 molecules, such as xenon difluoride (XeF2) and the triiodide-ion (I3−) with one iodide bonded to the two others. As described by the VSEPR model, the five-valence, electron-pairs on a central-atom form a trigonal bipyramid in which the three lone-pairs occupy the less crowded, equatorial-positions and the two bonded-atoms occupy the two axial-positions at the opposite-ends of an axis, forming a linear-molecule.".
- Q2226179 abstract "In chemistry, the linear molecular geometry describes the geometry around a central-atom bonded to two other atoms (or ligands) placed at a bond-angle of 180°. Linear=organic molecules, such as acetylene (HC≡CH), are often described by invoking sp orbital hybridization for their carbon-centers.According to the VSEPR model, linear-geometry occurs at central-atoms with two bonded-atoms and zero or three lone-pairs (AX2 or AX2E3) in the AXE notation. Neutral AX2 molecules with linear-geometry include beryllium fluoride (F—Be—F) with two single-bonds, carbon dioxide (O=C=O) with two double-bonds, hydrogen cyanide (H—C≡N) with one single and one triple-bond. The most important linear-molecule with more than three atoms is acetylene (H—C≡C—H), in which each of its carbon atoms is considered to be a central-atom with a single-bond to one hydrogen and a triple=bond to the other carbon atom. Linear-anions include azide (N3−) and thiocyanate (SCN−), and a linear-cation is nitronium ion (NO2+).Linear-geometry also occurs in AX2E3 molecules, such as xenon difluoride (XeF2) and the triiodide-ion (I3−) with one iodide bonded to the two others. As described by the VSEPR model, the five-valence, electron-pairs on a central-atom form a trigonal bipyramid in which the three lone-pairs occupy the less crowded, equatorial-positions and the two bonded-atoms occupy the two axial-positions at the opposite-ends of an axis, forming a linear-molecule.".