HO2 Hydroperoxyl Radical

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Railsback's Some Fundamentals of Mineralogy and Geochemistry The multiple forms of oxygen Fully-reduced Not-fully-reduced oxygen; oxygen unstable at some time scale Mineralogists think of oxygen in Nominal its 2- oxidation state in minerals, oxidation and geochemists additionally think number -2 -1 0 about it as elemental diatomic Name of Elemental oxygen (O2) in redox geochemistry. Oxide However, that's just a beginning if state oxygen one additionally considers chemical processes in the atmosphere. As Oxide minerals Diatomic the table at right shows with its blue e.g., MgO oxygen region, atmospheric chemistry additionally deals with ozone, with Oxysalt minerals peroxide, and with oxide gases. O2 The interaction of the less-reduced e.g., CaCO3 Hydroxyl forms of oxygen with the not-fully- & MgFeSiO4 radical Ozone oxidized gases (SO2, NO, NO2, Examples 0 etc.) provides much entertainment Hydroxide minerals OH O3 in atmospheric chemistry. e.g., Al(OH) 3 Hydrogen Atomic One very important point to note here is the difference between OH, ology Hydroxide ion peroxide oxygen the highly reactive hydroxyl radical, Minera - and the hydroxide ion OH-, the OH H2O2 O entity found in water that we can Hydroperoxyl Significant think of as dissociated H2O. In the Water & its vapor in the upper table at right, the OH representing radical atmosphere the peroxide radical has a "0" H2O (>85 km) superscript to remind readers of its HO2 overall neutral charge, but most Aqueous/redox Oxide gases One O0 & authors and printers leave it simply geochemistry e.g., CO, CO , SO one O- as an unadorned "OH". Thus the 2 2 names and chemical symbols for N2O, NO, & NO2 C N OFNe OH and OH- look much alike, but Atmospheric Si P S Cl Ar the two chemical entities are very chemstry different. As Se Br Kr LBR OxygenForms04 3/2008.

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Oxidation State Slides.Key
Oxidation States Dr. Sobers’ Lecture Slides The Oxidation State Also known as the oxidation number The oxidation state is used to determine whether an element has been oxidized or reduced. The oxidation state is not always a real, quantitative, physical constant. The oxidation state can be the charge on an atom: 2+ - MgCl2 Mg Cl Oxidation State: +2 -1 2 The Oxidation State For covalently bonded substances, it is not as simple as an ionic charge. A covalent bond is a sharing of electrons. The electrons are associated with more than one atomic nuclei. This holds the nuclei together. The electrons may not be equally shared. This creates a polar bond. The electronegativity of a covalently bonded atom is its ability to attract electrons towards itself. 3 Example: Chlorine Sodium chloride is an ionic compound. In sodium chloride, the chloride ion has a charge and an oxidation state of -1. The oxidation state of sodium is +1. 4 Example: Chlorine In a chlorine molecule, the chlorine atoms are covalently bonded. The two atoms share electrons equally and the oxidation state is 0. 5 Example: Chlorine The two atoms of a hydrogen chloride molecule are covalently bonded. The electrons are not shared equally because chlorine is more electronegative than hydrogen. There are no ions but the oxidation state of chlorine in HCl is -1 and the oxidation state of hydrogen is +1. 6 7 Assigning Oxidation States See the handout for the list of rules. Rule 1: Free Elements Free elements have an oxidation state of zero Example Oxidation State O2(g) 0 Fe(s) 0 O3(g) 0 C(graphite) 0 C(diamond) 0 9 Rule 2: Monatomic Ions The oxidation state of monatomic ions is the charge of the ion Example Oxidation State O2- -2 Fe3+ +3 Na+ +1 I- -1 V4+ +4 10 Rule 3: Fluorine in Compounds Fluorine in a compound always has an oxidation state of -1 Example Comments and Oxidation States NaF These are monatomic ions.
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Plutonium Is a Physicist's Dream but an Engineer's Nightmare. with Little
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