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NOMENCLATURE

NOMENCLATURE. Zumdahl – Ch 5 Holt – Ch 7. Monatomic Ions. Ions formed from a single atom Written as (E 2+ ) or (E 2- ). Binary Ionic Compounds. Metallic or positive element is named first ( cation ) Non-metallic or negative element is named second ( anion ) Cross over charges

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NOMENCLATURE

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  1. NOMENCLATURE Zumdahl – Ch 5 Holt – Ch 7

  2. Monatomic Ions Ions formed from a single atom Written as (E2+) or (E2-)

  3. Binary Ionic Compounds • Metallic or positive element is named first (cation) • Non-metallic or negative element is named second (anion) • Cross over charges • Metal doesn’t change • Non-metal suffix changes to -ide

  4. Oxidation Numbers • Pure element have an oxidation number of zero • Fluorine has an oxidation of -1 in all compounds • Oxygen has an oxidation number of -2 except when in a peroxide when its oxidation number is -1 • Hydrogen has an oxidation number of +1 except when bonded to a metal • The algebraic sum of the oxidation numbers of all atoms in a neutral compound is zero • The algebraic sum of the oxidation numbers of all atoms in a polyatomic ion is equal to the charge of the ion • These rules apply to covalently bonded atoms

  5. Balancing Charges

  6. Binary Ionic Compounds (Type II) • Many elements may form more than one type of positive ion EX – FeCl2 is named iron(II) chloride FeCl3 is named iron(III)chloride OLD SCHOOL NAMING • Higher oxidation number uses -ic ending (ferric chloride, Fe3+) • Lower oxidation number uses -ousending (ferrous chloride, Fe2+)

  7. Binary Ionic Compounds con’t • Stock System uses Roman numerals to indicate charge • Oxidation number in Roman numerals in parenthesis between cation and anion

  8. Binary Covalent Compounds • Formed between two non-metals • first element name doesn’t change • Second element ends with “-ide” • Don’t use “mono-” on first name • Use prefixes to indicate number of atoms of element

  9. Mono– 1 Di– 2 Tri- 3 Tetra- 4 Penta- 5 Hexa- 6 Hepta- 7 Octa- 8 Nona- 9 Deca- 10 Prefixes

  10. Binary Acids • Hydrogen takes place of metal ion • Use prefix -hydro in place of hydrogen • Use suffix -icon the root Examples – HCl – hydrochloric acid HF – hydroflouric acid H2S – hydrosulfuric acid

  11. Polyatomic Ions • Group of atoms with a shared charge • Most common form of ion ends with –ate • If one less oxygen, ending changes to –ite Ex – NO3- (nitrate) NO2- (nitrite)

  12. Common Polyatomic Ions

  13. Oxyacids • contain hydrogen, a non-metal, and oxygen • usually contain 3 or 4 oxygen atoms • add suffix -ic to the stem Examples – HBrO3 – bromic acid H2CO3 – carbonic acid HClO3 – chloric acid HNO3 – nitric acid H3PO4 – phosphoric acid H2SO4 – sulfuric acid

  14. Oxyacids con’t • Common name ends with -ate • One extra oxygen add per- to stem name Example – HClO3 – chloric acid HClO4 – perchloric acid • One less oxygen change -ic ending to -ous Example – HClO3 – chloric acid HClO2 – chlorous acid

  15. Oxyacids con’t • Two fewer oxygens change -ic ending to -ous AND add prefix hypo- Examples - HClO3 – chloric acid HClO – hypochlorous acid

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