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AP CHEM CHAPTER 3

This resource provides a detailed overview of nomenclature for both monatomic and polyatomic ions, crucial for understanding chemical compounds. It covers how metals form positive ions and non-metals form negative ions, along with examples of common ions such as magnesium and fluoride. Transition elements and their unique nomenclature requirements are also discussed. The guide outlines the rules for naming ionic and molecular compounds, including binary acids and hydrocarbons, and details for constructing formulas by crossing charges.

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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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