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AP CHEM CHAPTER 3

AP CHEM CHAPTER 3 . A REVIEW OF NOMENCLATURE. MONATOMIC IONS. MONATOMIC IONS. METALS FORM POSITIVE IONS NON METALS FORM NEGATIVE IONS POSITIVE IONS: ELEMENT NAME+ ION NEGATIVE IONS: ELEMENT ROOT + “IDE” ENDING Examples: Mg 2+ magnesium ion F - fluor ide ion.

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AP CHEM CHAPTER 3

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  1. AP CHEMCHAPTER 3 A REVIEW OF NOMENCLATURE

  2. MONATOMIC IONS

  3. MONATOMIC IONS • METALS FORM POSITIVE IONS • NON METALS FORM NEGATIVE IONS • POSITIVE IONS: ELEMENT NAME+ ION • NEGATIVE IONS: ELEMENT ROOT + “IDE” ENDING • Examples: • Mg 2+ magnesium ion • F- fluoride ion

  4. MONATOMIC IONS (cont) • TRANSITION ELEMENTS (GROUPS 3-12) • All are metals and form positive ions • Can form ions with more than one charge, so they must have a Roman numeral • Transition elements that do not require a Roman numeral: Zn, Cd, and Ag. • Non transition elements that do require a Roman numeral: Pb and Sn

  5. POLYATOMIC IONS “ate” and “ite” ions contain oxygen • “per”____ “ate” ions- one more oxygen than the ate ion • “ate” ions- memorize • “ite” ions- one less oxygen that the “ate” ion • “hypo”____ “ite” ions- one less oxygen than the “ite” ion

  6. POLYATOMIC IONS- EXAMPLES* some of the examples are ions that do not exist, but are used for practice purposes

  7. OTHER POLYATOMIC IONS • Adding a hydrogen (H+) ion to the beginning of a polyatomic ion : • CO3 2- carbonate ion • HCO3 - hydrogen carbonate or bicarbonate • SO4 2- sulfate ion • HSO4 - hydrogen sulfate or bisulfate • PO4 3- phosphate ion • HPO4 2- hydrogen phosphate ion • H2PO4 - dihydrogen phosphate ion

  8. NOMENCLATURE OF IONIC COMPOUNDS • GENERAL RULE: Ionic compound are made up of: • A metal + a non metal • A metal + a polyatomic ion

  9. NOMENCLATURE OF IONIC COMPOUNDS (CONT) To write the formula: cross charges Calcium chloride Ca 2+ Cl - CaCl2

  10. NOMENCLATURE OF MOLECULAR COMPOUNDS ( 2 NON METALS) • binary (2 elements) • 1st element: prefix + element name (except do not use “mono” on the first element) • 2nd element: prefix + element name + “ide” ending • Example: CCl4 carbon tetrachloride N2O dinitrogen monoxide

  11. Prefixes for molecular compounds 1- mono 6- hexa 2- di 7- hepta 3- tri 8- hexa 4- tetra 9- nona 5- penta 10- deca

  12. Binary acids • H + a halogen, or sulfur, or tellurium • Hydo _________ ic acid • HCl: hydrochloric acid • HF: hydrofluoric acid • H2S: hydrosulfuric acid

  13. Oxyacids • H+ element + oxygen • Aka: H + polyatomic ion • “ate” ions  “ic” acids • “ite” ions  “ous” acids HNO3= nitric acid H2SO3= sulfurous acid

  14. Hydrocarbons • Contain C and H • Alkanes: CnH(2n+2) • Alkenes: CnH 2n • Alkynes: CnH 2n-2 • Alcohols: alkane – H + OH

  15. Alkanes • Methane: CH4 • Ethane: C2H6 • Propane: C3H8 • Butane: C4H10 • Pentane: C5H12 • Hexane: C6H14 • Heptane: C7H16 • Octane: C8H18 • Nonane: C9H20 • Decane: C10H22

  16. alkenes • Methene xxxxxxx • Ethene: C2H4 • Propene: C3H6 • Butene: C4H8 • Pentene: C5H10 • Hexene: C6H12 • Heptene: C7H14 • Octene: C8 H16 • Nonene: C9H 18 • Decene: C10H20

  17. Alkynes • Methynexxxxxxxxxxxxxx • Ethyne C2H2 • Propyne C3H4 • Butyne C4H6 • Pentyne C5H8 • Hexyne C6H10 • Heptyne C7H12 • Octyne C8H14 • Nonyne C9H16 • Decyne C10H18

  18. Alcohols • Methanol CH3OH • Ethanol C2H5OH • Propanol C3H7OH • Butanol C4H9OH • Pentanol C5H11OH • Hexane C6H13OH • Heptane C7H15OH • Octane C8H17OH • Nonane C9H19OH • Decane C10H21OH

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