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Ionic Nomenclature

Ionic Nomenclature. Cation. Defn: A positively charged particle. Name of metal+ the word “ion”. Ex. Potassium Potassium Ion. Anion. Defn: a negatively charged particle. Name of non-metal w/ ending changed to “ide” Ex. Chlorine Chlor ide. Binary Ionic Compounds.

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Ionic Nomenclature

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  1. Ionic Nomenclature

  2. Cation • Defn: A positively charged particle. • Name of metal+ the word “ion”. • Ex. Potassium • Potassium Ion

  3. Anion • Defn: a negatively charged particle. • Name of non-metal w/ ending changed to “ide” • Ex. Chlorine • Chloride

  4. Binary Ionic Compounds • Contains only 2 different elements in the compound • Naming the Compounds • Name of metal + Name of non-metal with “ide” ending. • Ex NaCl • Sodium Chloride

  5. More Examples • MgO • Magnesium Oxide • MgCl2 • Magnesium Chloride • LiBr • Lithium Bromide • Ca3P2 • Calcium Phosphide

  6. Transition Metals • Transition metals can give up different numbers of electrons • Therefore they can have multiple charges (This applies to lead and tin, too.) • Ex. If Titanium loses 3e- • Ti3+

  7. Roman Numerals • Tells the charge of the ion preceding it. When an ion can have more than one charge, you need to use a roman numeral to specify the charge. • Ex Lead • Pb2+ • Lead (II) ion • Pb4+ • Lead (IV) ion

  8. Exceptions • If the transition metal only has one charge, then DO NOT use a roman numeral! • Ex. Zinc • Zn2+ Zinc ion • What are other examples of a transition metal with only one charge? • Ag+, Cd2+, Sc3+

  9. Reminder • Roman numerals tell the charge of an ion, NOT HOW MANY! • Ex. Gold (III) chloride • What is the charge of the gold ion in gold (III) chloride? • 3+

  10. Example: • Tin (II) bromide • What is the charge of the tin ion in tin (II) bromide? • 2+

  11. Writing Formulas • The positive and negative charges must equal ZERO in the compound. • Write the symbol and charge for each individual ion • Use the least common denominator (LCD) to determine how many of each ion is needed in order to make a zero net charge. • Write the formula, using a subscript(s) to indicate the number of each ion in the compound

  12. Example • Zinc sulfide • Zn2+ S2- • ZnS

  13. Example • Sodium Oxide • Na+ O2- • Na2O

  14. Example • Scandium bromide • Sc3+ Br – • ScBr3

  15. Naming ionic compounds with polyatomic ions (tertiary ionic compounds): • Name of cation first • Name of anion second • Remember roman numerals, if necessary • Enclose polyatomic ions in parenthesis when it requires a subscript

  16. Example • Zn2+ SO42- • Balanced Formula? • ZnSO4 • Name? • Zinc sulfate

  17. Calcium Phosphate • Ca2+ PO43- • Balanced Formula? • Ca3(PO4)2 • Name? • Calcium Phosphate

  18. Manganese (IV) Nitrite • Mn4+ NO2- • Balanced Formula? • Mn(NO2)4 • Name? • Manganese(IV) Nitrite

  19. MgCl2

  20. CuSO4

  21. Example: Copper (I) Chlorate • Cu+ ClO3- • Balanced Formula? • CuClO3 • Name? • Copper (I) Chlorate

  22. Chromium (III) Hydroxide • Cr3+ OH- • Balanced Formula? • Cr(OH)3 • Name? • Chromium(III) hydroxide

  23. NaNO3

  24. Al(OH)3

  25. Cu3PO4

  26. Covalent Nomenclature aka Molecular Compounds

  27. To Name Covalent Compounds: • Translate the subscript of the first element into a prefix + the name of the element • Translate the subscript of the 2nd element into a prefix + root name of element with the “ide” ending

  28. NOTE • If there is only 1 of the 1st element, do not use a prefix • Ex. CO • carbon monoxide

  29. Name the Following Compounds • N2O • Dinitrogen monoxide • PCl3 • Phosphorus trichloride • SF6 • Sulfur hexafluoride

  30. Name the Following Compounds • CO2 • Carbon dioxide • NO • nitrogen monoxide • CCl4 • carbon tetrachloride

  31. To Write Formulas for Covalent Compounds: • Correlate the prefix of the 1st element to its numerical value…write it as the subscript • Correlate the prefix of the 2nd element to its numerical value…write it as the subscript • Prefix should match the subscript written for each element *Remember, if there is not a prefix, then it’s just 1.

  32. Write the formula for each • Tetraiodine nonoxide • I4O9 • Sulfur trioxide • Phosphorus pentafluoride

  33. Write the formula for each • Nitrogen dioxide • NO2 • Dichlorine heptoxide • Cl2O7 • Carbon disulfide • CS2

  34. Acid Nomenclature

  35. Naming Acids • Acids always have hydrogen. • Binary Acids • Hydrogen + 1 other element • Oxy Acids • Hydrogen + oxygen (from a polyatomic ion)

  36. Binary Acids • Use “hydro” for hydrogen • Root of 2nd element + ic (take off the ending) • add “acid” to the end • Ex : HCl • Hydrochloric acid

  37. Name the Binary Acids • H2S • Hydrosulfuric acid • (notice here that it is sulfuric, not sulfic) • HF • Hydrofluoric acid • HBr • Hydrobromic acid

  38. Oxy Acids “ite” • The name of the acid comes from the name of the polyatomic ion. • If the polyatomic ion ended in “–ite”, then the ending for the acid is “–ous” • Take off the “ite” ending of the polyatomic ion and add –”ous” • Add the word “acid” • Ex. HNO2 • Nitrous Acid

  39. Name the oxy acids • H2SO3 • Sulfite Ion • Sulfurous acid • H3PO3 • Phosphite Ion • Phosphorous acid

  40. Oxy Acids “ate” • If the polyatomic ion ended in “–ate”, then the ending for the acid is “–ic” • Take off the “ate” ending of the polyatomic ion and add –”ic” • Add acid • Ex. HNO3 • nitrate ion • Nitric acid

  41. Name the oxy acids • H2SO4 • Sulfate ion • Sulfuric Acid • H3PO4 • Phosphate ion • Phosphoric Acid

  42. Writing formulas for binary acids • Determine what kind of acid it is; binary or oxy • Does it have hydro at the front? • If yes, then it is binary • Determine the charges for the individual ions • Write the formula so that the overall charge equals zero

  43. Example • Hydroiodic acid • H+ I- • HI • Hydroselenic acid • H+ Se2- • H2Se

  44. Writing formulas for oxy acids • Determine what kind of acid it is; binary or oxy • Does it have -ous or –ic at the end? • If yes, then it is an oxy acid • Determine the charges for the individual ions • Write the formula so that the overall charge equals zero

  45. Example • Chlorous acid • from chlorite ion • ClO2- HClO2 • Boric acid • From borate ion • BO33- H3BO3 • Chloric acid • from chlorate ion • ClO3-  HClO3

  46. Examples • Sulfurous acid • from sulfite ion, • SO32- H2SO3 • Carbonic acid • from carbonate ion, • CO32- H2CO3

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