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Ozone synthesis from oxygen in dielectric barrier discharges

In theory, sulfur can react with oxygen to form either SO2or SO3, whose Lewis structures are given in the figurebelow.

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Oxygen chiral phosphodiesters. 2. Enzymatic synthesis …

Sulfuric acid and sulfurous acid are both examples of a classof compounds known as oxyacids, because they areliterally acids that contain oxygen. Because they are negativeions (or anions) that contain oxygen, the SO32-and SO42- ions are known as oxyanions.The Lewis structures of some of the oxides of sulfur that formoxyacids or oxyanions are given in the table below.

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Because sulfur is directly below oxygen in the periodic table,these elements have similar electron configurations. As a result,sulfur forms many compounds that are analogs of oxygen compounds,as shown in the table below. Examples in this table show how theprefix thio- can be used to indicate compounds in whichsulfur replaces an oxygen atom. The thiocyanate (SCN-)ion, for instance, is the sulfur-containing analog of the cyanate(OCN-) ion.

Oxygen is a chemical element with symbol O and atomic number 8

The VSEPR theory predicts that the geometry around each oxygenatom in H2O2 should be bent. But thistheory cannot predict whether the four atoms should lie in thesame plane or whether the molecule should be visualized as lyingin two intersecting planes. The experimentally determinedstructure of H2O2 is shown in the figurebelow.

Double bonds between sulfur and oxygen or carbon atoms can befound in compounds such as SO2 and CS2 (seefigure below). But these double bonds are much weaker than theequivalent double bonds to oxygen atoms in O3 or CO2.The bond dissociation enthalpy for a C=S double bond is 477kJ/mol, for example, whereas the bond dissociation enthalpy for aC=O double bond is 745 kJ/mol.

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Fluorine is the only element that is more electronegative thanoxygen. As a result, oxygen gains electrons in virtually all itschemical reactions. Each O2 molecule must gain fourelectrons to satisfy the octets of the two oxygen atoms withoutsharing electrons, as shown in the figure below.

Elemental oxygen consists of O2 molecules in whicheach atom completes its octet of valence electrons by sharing twopairs of electrons with a single neighboring atom. Because sulfurdoes not form strong S=S double bonds, elemental sulfur usuallyconsists of cyclic S8 molecules in which each atomcompletes its octet by forming single bonds to two neighboringatoms, as shown in the figure below.

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The gas is approximately 1.1 times heavier than air and is slightly soluble in water and alcohol. Below its boiling point, oxygen is a pale blue liquid slightly heavier than water.

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Oxygen (O2) and ozone (O3) are examplesof allotropes (from the Greek meaning "inanother manner"). By definition, allotropes are differentforms of an element. Because they have different structures,allotropes have different chemical and physical properties (seetable below).

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Because sulfur is much less electronegative than oxygen, it ismore likely to form compounds in which it has a positiveoxidation number (see table below).

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The electron configuration of an oxygen atom [He] 2s22p4 suggests that neutral oxygen atoms canachieve an octet of valence electrons by sharing two pairs ofelectrons to form an O=O double bond, as shown in the figurebelow.

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