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Chemistry Inorganic Nomenclature Transition Metals and Oxidation States

Chemistry Inorganic Nomenclature Transition Metals and Oxidation States. Do Now: Take out HW to check. CALCULATORS NOT REQUIRED PERIODIC TABLES REQUIRED. Transition Metals. Elements in the d-block are referred to as the transition metals .

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Chemistry Inorganic Nomenclature Transition Metals and Oxidation States

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  1. ChemistryInorganic NomenclatureTransition Metals and Oxidation States Do Now: Take out HW to check. CALCULATORS NOT REQUIRED PERIODIC TABLES REQUIRED

  2. Transition Metals • Elements in the d-block are referred to as the transition metals. • This is because they can have multiple different charges. • In a compound’s name, we need to find a way to distinguish between different d-block charges. • This also applies to p-block metals, like lead and tin.

  3. Transition Metals • Example: Iron can either be +2 or +3 • Fe2++ O2-= FeO • Fe3++ O2-= Fe2O3 • A Roman numeral is used to show the charge on the transition metal: • FeO = iron (II) oxide • Fe2O3 = iron (III) oxide

  4. Transition Metals Without Roman Numerals • Zinc and silver are transition metals that only have one charge, and do not require Roman numerals. • Silver: Ag+ • Zinc: Zn2+

  5. More Practice • Name the following compounds: • Fe(NO3)3 • Na2SO4 • Zn(ClO3)2 • Give the formula for the following compounds: • Sodium chlorate (aka bleach) • Silver nitrate • Copper (II) phosphate

  6. Oxidation States • The oxidation state of an element is an integer value that indicates the degree of oxidation of an element in a compound. • More specifically, it is a hypothetical charge on an atom, pretending that all of the bonds are 100% ionic. • Oxidation refers to lack of electrons. The higher the value of the oxidation state, the less electron density on that atom.

  7. Rules for Calculating Oxidation States • The oxidation number of any uncombined element is zero. Fe, Cl2, O2 • The oxidation number of a monatomic ion equals the charge on the ion. H+ O2-NaCl • The more electronegative element in a binary compound is assigned the number equal to the charge it would have as an ion. NH3 N2O

  8. Rules for Calculating Oxidation States 4. Fluorine always has an oxidation state of -1. 5. Oxygen has an oxidation state of -2 unless it is combined with F (when it is +2), or is in a peroxide (such as H2O2 or Na2O2) 6. The oxidation state of hydrogen is most of its compounds is +1 unless it is combined with a metal, in which case it is -1. H2O NaH (sodium hydride)

  9. Rules for Calculating Oxidation States 7. In compounds, the elements of groups 1A and 2A as well as aluminum have oxidation states of +1, +2, and +3 respectively. 8. The sum of the oxidation numbers of all atoms in a neutral compound is 0. H2SO4 H2SO3 9. The sum of the oxidation numbers of all atoms in a polyatomic ions equals the charge on the ion. Cr2O72- CrO42-

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