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Electrochemistry - Menihek Home Page
Electrochemistry - Menihek Home Page

Organic Chemistry
Organic Chemistry

... Connect the atoms by single bonds. Arrange the remaining electrons so that each atom has a complete valence shell. • Show a bonding pair of electrons as a single line. • Show a nonbonding pair of electrons (a lone pair) as a pair of dots. • In a single bond atoms share one pair of electrons, in a do ...
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... 37. Which of the following is a correct interpretation of the results of Rutherford's experiments in which gold atoms were bombarded with alpha particles? (A) Atoms have equal numbers of positive and negative charges. (B) Electrons in atoms are arranged in shells. (C) Neutrons are at the center of a ...
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... This Unit has the Using Graphical Information component of Numeracy, and the Critical Thinking component of Problem Solving, embedded in it. This means that when candidates achieve the Unit, their Core Skills profile will also be updated to show that they have achieved Using Graphical Information an ...
Structure of Molecules and Compounds | Principles of Biology from
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... stable configuration. It can gain these electrons, for example, by combining with four hydrogen atoms. Each hydrogen atom has one electron in its outer shell and requires one electron to reach a stable configuration. The carbon atom shares one electron with each hydrogen atom, forming four covalent ...
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Chapter 19 Redox Reactions and Electrochemistry Notes (answers)

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Old Clusters with New Function: Oxidation Catalysis by High

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Oxidation state

The oxidation state, often called the oxidation number, is an indicator of the degree of oxidation (loss of electrons) of an atom in a chemical compound. Conceptually, the oxidation state, which may be positive, negative or zero, is the hypothetical charge that an atom would have if all bonds to atoms of different elements were 100% ionic, with no covalent component. This is never exactly true for real bonds.The term ""oxidation"" was first used by Lavoisier to mean reaction of a substance with oxygen. Much later, it was realized that the substance on being oxidized loses electrons, and the use of the term ""oxidation"" was extended to include other reactions in which electrons are lost.Oxidation states are typically represented by small integers. In some cases, the average oxidation state of an element is a fraction, such as 8/3 for iron in magnetite (Fe3O4). The highest known oxidation state is reported to be +9 in the cation IrO+4, while the lowest known oxidation state is −5 for boron, gallium, indium, and thallium. The possibility of +9 and +10 oxidation states in platinum group elements, especially iridium(IX) and platinum(X), has been discussed by Kiselev and Tretiyakov.The increase in oxidation state of an atom through a chemical reaction is known as an oxidation; a decrease in oxidation state is known as a reduction. Such reactions involve the formal transfer of electrons, a net gain in electrons being a reduction and a net loss of electrons being an oxidation. For pure elements, the oxidation state is zero.There are various methods for determining oxidation states/numbers.In inorganic nomenclature the oxidation state is determined and expressed as an oxidation number represented by a Roman numeral placed after the element name.In coordination chemistry, oxidation number is defined differently from oxidation state.
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