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Nomenclature Review

Nomenclature Review. Because Every Student Loves Nomenclature. How do elements bond?. Ions. atoms or groups of atoms that have gained or lost electrons. cation -- positive ion anion -- negative ion. Ionic Compounds.

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Nomenclature Review

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  1. Nomenclature Review Because Every Student Loves Nomenclature

  2. How do elements bond?

  3. Ions • atoms or groups of atoms that have gained or lost electrons. • cation -- positive ion • anion -- negative ion

  4. Ionic Compounds • Neutral compounds which are formed when anions and cations come together in ratios that balance the positive and negative charges. (Form formula units)

  5. Cation Names = Element Name • Na+ sodium ion • Ca2+ calcium ion • Co3+ cobalt(III) ion • Co2+ cobalt(II) ion • for transition metals or other metals with variable oxidation states use roman numerals to designate charge.

  6. Anion Names = Elementide Ion • N3- nitrogen  nitride ion • O2- oxygen  oxide ion • S2- sulfur  sulfide ion • Cl- chlorine  chloride ion

  7. Compound Formation • Ions will combine in such a way as to neutralize charges

  8. Formula Unit • The smallest representative unit of an ionic compound

  9. NaCl

  10. Examples • Name the compound and write the formula formed from the following pairs of elements • magnesium and nitrogen • magnesium nitride, Mg3N2 • strontium and fluorine • strontium fluoride, SrF2 • iodine and cadmium • cadmium iodide, CdI2 • sulfur and cesium • cesium sulfide, Cs2S

  11. mercury(I) chloride cadmium nitride potassium bromide iron(III) oxide tin(II) fluoride Hg2Cl2 Cd3N2 KBr Fe2O3 SnF2 Examples

  12. magnesium chloride chromium(III) iodide lead(IV) oxide rubidium oxide silver sulfide MgCl2 CrI3 PbO2 Rb2O Ag2S Examples

  13. Polyatomic Ions • The polyatomic ion stays together as a charged unit • When two or more of the same polyatomic ion are present in the formula, that ion appears in parentheses with the subscript written outside • Parentheses and subscript are not used unless more than one of the polyatomic ions is present

  14. aluminum hydroxide barium acetate sodium nitrate lithium dichromate potassium permanganate Al(OH)3 Ba(C2H3O2)2 NaNO3 Li2Cr2O7 KMnO4 Examples

  15. Oxyanions – Groups of 4 Oxygens

  16. Oxyanions – Groups of 4 Oxygens • O4/O3/O2/O • These keep the same charge as the group 7A halogen anions • Ex: Cl- vs ClO4- • Use –ate and –ite endings and per- and hypo- prefixes to denote number of oxygens • per _____ate XO4- • Ex: perchlorate ion • _____ate XO3- • Ex: chlorate ion • _____ite XO2- • Ex: chlorite ion • hypo _____ite XO- • Ex: hypochlorite ion

  17. Oxyanions – Groups of 4/3 Oxygens

  18. Oxyanions – Groups of 4/3 Oxygens • O4/O3 • These also keep the charges of their respective groups • Ex: S2- vs SO42- and P3- vs PO43- • Use –ate and –ite endings to denote number of oxygens • ______ate EO42- or EO43- • Ex: sulfate ion, phosphate ion • ______ite EO32- or EO33- • Ex: sulfite ion, phosphite ion

  19. Oxyanions – Groups of 3/2 Oxygens

  20. Oxyanions – Groups of 3/2 Oxygens • O3/O2 • These do NOT keep the charge of their group • Starting with N, they take on -1, -2, -3 • Ex: N3- vs NO3- and C4- vs CO32- and BO33- • Use –ate and –ite endings to denote number of oxygens • _______ate EO3- • Ex: nitrate ion • _______ite EO2- • Ex: nitrite ion

  21. iron(II) chlorate cesium carbonate sodium sulfite sodium hypobromite lithium periodate Fe(ClO3)2 Cs2CO3 Na2SO3 NaBrO LiIO4 Examples

  22. vanadium(V) hypochlorite manganese(III) nitrite aluminum phosphate titanium(II) arsenate ammonium phosphate V(ClO)5 Mn(NO2)3 AlPO4 Ti3(AsO4)2 (NH4)3PO4 Examples

  23. Sulfur compounds • When an oxygen atom in an ion is replaced by a sulfur atom the prefix thio is added to the name. • OCN- cyanate SCN- thiocyanate • SO4-2 sulfate S2O3-2 thiosulfate

  24. Acids • Two Types • Binary Acids • Oxoacids

  25. Acids

  26. Binary Acids • Formed when certain gaseous compounds dissolve in water • Example: • When gaseous hydrogen chloride dissolves in water it forms a solution called hydrochloric acid • Name: Prefix hydro- + nonmetal root + suffix –ic + separate word acid • Pattern holds for many compounds in which hydrogen combines with an anion that has an –ide suffix

  27. Acid Nomenclature • Binary Acids • HX hydrogen _____ide becomeshydro______ ic acid

  28. Examples • HCl(g) hydrogen chloride • HCl (aq) hydrochloric acid • H2S(g) hydrogen sulfide • H2S(aq) hydrosulfuric acid • HCN(g) hydrogen cyanide • HCN(aq) hydrocyanic acid

  29. Oxyacids • Similar to oxyanions, except two suffix changes • -ate in the anion becomes –ic in the acid • -ite in the anion becomes –ous in the acid • hypo- and per- prefixes are kept • Examples: • BrO4- - perbromate HBrO4 – perbromic acid • IO2- - iodite HIO2 – iodous acid

  30. Oxyacid Nomenclature • Hydrogen ___ate  ___ic acid • Hydrogen ___ite  ___ous acid • Hydrogen per __ate  per__ic acid • Hydrogen hypo__ite hypo__ous acid

  31. Examples • Name the following anions and give the names and formulas of the acids derived from them: • Br- • bromide; hydrobromic acid, HBr • IO3- • iodate; iodic acid, HIO3 • CN- • cyanide; hydrocyanic acid, HCN • SO42- • sulfate; sulfuric acid, H2SO4 • NO2- • nitrite; nitrous acid, HNO2

  32. Acid Salt Nomenclature • HX- Hydrogen anion name • H2X- Dihydrogen anion name • Sometimes use the prefix bi to indicate the presence of one H attached to an anion

  33. Examples • HCO3-1 hydrogen carbonate or bicarbonate • HS-1 hydrogen sulfide or bisulfide • HSO4-1 hydrogen sulfate or bisulfate

  34. Examples • HPO4-2 hydrogen phosphate • H2PO3-1 dihydrogen phosphite

  35. Hydrates • Some salts precipitate with water molecules in the crystal lattice. These are called hydrates. • Name as compound name ___hydrate • Where the prefix tells the number of water molecules in the crystal

  36. Hydrates • Compounds with a specific number of water molecules associated with each formula unit • Formula is written with the hydrate after a centered dot • Systematic names use a Greek numeral prefix before the word hydrate • Examples: • Epsom salt: MgSO4l 7H2O is magnesium sulfate heptahydrate • Gypsum: CaSO4l 2H2O is calcium sulfate dihydrate

  37. sodium nitrate tetrahydrate potassium phosphate heptahydrate magnesium oxide pentahydrate NaNO3·4H2O K3PO4·7H2O MgO·5H2O Examples

  38. Binary Covalent Compounds • Formed by the combination of two elements, usually nonmetals

  39. Binary Covalent Compounds • Element with lower group number is first • Exception: if it is oxygen with a halogen, the halogen goes first and oxygen second • If both elements are in the same group, the one with the higher period is named first • The second element is named with its root and the suffix –ide • Covalent compounds have Greek numerical prefixes to indicate the number of atoms of each element in the compound • The first element has a prefix only when more than one atom of the element is present • The second element always has a prefix

  40. Binary Covalent Compounds

  41. mono 1 di 2 tri 3 tetra 4 penta 5 hexa 6 hepta7 octa 8 nona 9 deca 10 Prefixes

  42. sulfur tetrafluoride dichlorine heptoxide dinitrogen trioxide nitrogen triiodide xenon hexafluoride SF4 Cl2O7 N2O3 NI3 XeF6 Examples

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