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Chapter 7: Inorganic Nomenclature

Chapter 7: Inorganic Nomenclature. cation. anion. Inorganic branch of chemistry dealing with metals and nonmetals . Nomenclature naming system used to identify compounds. Binary compounds simplest compounds contain only two elements .

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Chapter 7: Inorganic Nomenclature

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  1. Chapter 7: Inorganic Nomenclature cation anion • Inorganic • branch of chemistry dealing with metals and nonmetals. • Nomenclature • naming system used to identify compounds. • Binary compounds • simplest compounds • contain only two elements. • Remember: the cation is placed first, then the anion. cation anion

  2. Naming Binary Compounds • Begin with the positive ion • the first element in the compound. • The cation’s name  first part of the compound’s name. • The anion has its name truncated (shortened) and “–ide” is added. • The correct name is then… Magnesium Chloride Magnesium Chlorine Name Chloride

  3. Common anions • O – oxygen, = “oxide” • H – hydrogen, = “hydride” • S – sulfur, = “sulfide” • Cl – chlorine, = “chloride” • F – fluorine, = “fluoride” • I – iodine, = “iodide” • N – nitrogen, = “nitride” • C – carbon, = “carbide” • Br – bromine, = “bromide” • P – phosphorus, = “phosphide” Some atoms can be positive or negative: Carbon: -4 or +4 Nitrogen: -3 or +5 Sulfur: -2 or +6

  4. Multiple Nonmetal Anions • When both elements are nonmetals. • we add a latin-based prefix to the anion. • One anion: “mono-” • Two anions: “di-” • Three anions: “tri-” • Four anions: “tetra-” Carbon monoxide Mono in front of a single anion is optional (older) Carbon dioxide Boron trifluoride Carbon tetrachloride

  5. Special Cations :d-block metals • Transition metals (d-block): • d-block electrons can migrate into the s and p orbitals. • d-block (and p-block with d-electrons) metals can have several charges when bonding. • Use a Roman Numeral to show the cation’s charge: • Fe2+ Co3+ Sn4+ Cr6+ • Iron(II) Cobalt(III) Tin(IV) Chromium(VI) • Identify the ions and charges on: • V4+ Cu2+ Tin (II) Nickel(IV) D-block metals do not follow the octet rule when bonding

  6. Oxidation number • charge that an atom would have when it bonds. • The oxidation number of hydrogen in H2O is +1. • The oxidation number of oxygen in H2O is -2. • Rule 1: The total oxidation numbers of all the atoms in a compound must be zero. (NaCl) • Rule 2: Oxidation of a free element is zero. (H2) • Can you figure the oxidation numbers of the following atoms? • Li+ Mg2+CaS AgCl AlF3 O2 • +1 +2 -2 -1 +3 0 You need to predict the oxidation based on the location in the p-table Some elements can change their oxidation numbers in chemical reactions.

  7. Oxidation Practice • Use rules for oxidation to determine the names of these compounds: • Write the formulas for these compounds: Lithium Fluoride Barium Chloride Cobalt (II) Bromide Iron (III) Oxide Chromium (VI) Phosphide Sodium Oxide Copper (II) Fluoride Nickel (VI) Nitride Titanium (IV) Oxide Manganese (VII) Sulfide

  8. Polyatomic ions • Polyatomic ion: • Ion composed of more than one element. (big) • stable units that bond like individual atoms. • Polyatomic ions used in class are: • NO3- “nitrate” charge of -1 • OH- “hydroxide” charge of -1 • C2H3O2- “acetate” charge of -1 • SO42- “sulfate” charge of -2 • CO32- “carbonate” charge of -2 • PO43-“phosphate”charge of -3 • NH4+ “ammonium” charge of +1

  9. Naming With Polyatomic Ions • Use the cation as normal…. • Add the name of the polyatomic anion. • Here, the compound is Copper (II)sulfate. Copper (II) sulfate Lithium nitrate Lead (II) nitrate (II) for Lead is optional

  10. Nomenclature Practice… • Name the following: • Identify the following compounds: • Notice how the NO3- polyatomic is placed in ( ) Calcium chloride Barium sulfate Silver (I) nitrate Tin (IV) fluoride Carbon tetraiodide Lithium nitrate Boron trichloride Potassium iodide Copper (II) nitrate (careful)

  11. Empirical Formula / Molecular Formula • Molecular Formula • shows the actual numbers of atoms in a molecule • Empirical Formula • reduced form • shows only the ratio of atoms in a molecule: ( 1:2 or 1:2:1 ) • Can use fractions of moles (.33mol : .66mol) End of chapter 7 - % comp removed

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