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Chapter 5 Nomenclature

Chemistry B2A. Chapter 5 Nomenclature. Binary Compounds. Ionic compounds ( a metal and a nonmetal ) 2. Covalent compounds ( two nonmetals ). Binary Compounds. Ionic compounds ( a metal and a nonmetal ). Cation (Y + ). Metals: lose 1, 2 or 3 e -. Ions. Nonmetals: gain 1, 2 or 3 e -.

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Chapter 5 Nomenclature

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  1. Chemistry B2A Chapter 5 Nomenclature

  2. Binary Compounds • Ionic compounds (a metal and a nonmetal) • 2. Covalent compounds (two nonmetals)

  3. Binary Compounds • Ionic compounds (a metal and a nonmetal)

  4. Cation (Y+) Metals: lose 1, 2 or 3 e- Ions Nonmetals: gain 1, 2 or 3 e- Anion (X-) Number of protons and neutrons in the nucleus remains unchanged. Cation (Y+): Na+ Li+ Ca2+ Al3+ Anion (X-): Cl- F- O-2

  5. 1A 2A 8A 4A 5A 6A 7A 3A Transition elements

  6. Ionic bonds Metal-Nonmetal Na  Na+ + e- Cl + e-  Cl- Opposite charges attract each other. Anion Cation

  7. Sodium (Na) NaCl Chlorine (Cl)

  8. Type I Monatomic Cations Metal has only one type of cation (main group elements) International Union of Pure and Applied Chemistry (IUPAC) systematic names Name of the metal + “ion” H+ Hydrogen ion Li+ Lithium ion Ca2+ Calcium ion Al3+ Aluminum ion

  9. Type II Monatomic Cations Metal has two (or more) type of cations (transition elements) IUPAC or Systematic names Co2+ Cobalt(II) ion Co3+ Cobalt(III) ion Fe2+ Iron(II) ion Fe3+ Iron(III) ion Cu1+ Copper(I) ion Cu2+ Copper(II) ion Hg+ Mercury(I) ion Hg2+ Mercury(II) ion Pb2+ Lead(II) ion Pb4+ Lead(IV) ion Sn2+ Tin(II) ion Sn4+ Tin(IV) ion

  10. Type II Monatomic Cations Common name (old name) “-ous” smaller charge Name of the metal + “-ic” larger charge Cu1+ Copper(I) ion Cuprous ion Cu2+ Copper(II) ion Cupric ion Hg+ Mercury(I) ion Mercurous ion Hg2+ Mercury(II) ion Mercuric ion Fe2+ Iron(II) ion Ferrous ion Fe3+ Iron(III) ion Ferric ion Sn2+ Tin(II) ion Stannous ion Sn4+ Tin(IV) ion Stannic ion

  11. Naming Monatomic Anions Stem part of name + “-ide”

  12. Molecule of NaCl Formula of NaCl matter are neutral (uncharged): total number of positive charges = total number of negative charges Na+ Cl- NaCl Ca2+ Cl- CaCl2 Al3+ S2- Al2S3 Ba2+ O2- Ba2O2 BaO

  13. Naming Binary Ionic compounds Name of metal (cation) + Name of anion NaCl Sodium chloride CaO Calcium oxide Cu2O Copper(I) oxide Cuprous oxide CuO Copper(II) oxide Cupric oxide CsBr Cesium bromide MgS Magnesium sulfide FeCl2 Iron(II) chloride Ferrous chloride FeCl3 Iron(III) chloride Ferric chloride

  14. Binary Compounds • Ionic compounds (a metal and a nonmetal) • 2. Covalent compounds (two nonmetals)

  15. Binary Compounds 2. Covalent compounds (two nonmetals)

  16. Naming Binary Covalent compounds (type III) 1 2 3 4 5 6 7 8 9 10 Mono – Di – Tri – Tetra – Penta – Hexa – Hepta – Octa – Nona – Deca prefix and full name of the first element in formula + prefix and the anion name of the second element + “ide” • Don’t use “mono” for the 1st element. • Drop the “a” when followed by a vowel. Rules:

  17. Naming Binary Covalent compounds (type III) NO2 Nitrogen dioxide N2O4 Dinitrogen tetroxide CCl4 Carbon tetrachloride S2O3 Disulfur trioxide PCl5Phosphorous pentachloride SF6 Sulfur hexafluoride

  18. No No Yes Yes Yes Binary Compounds Metal present? Type III Use prefixes Does the metal form more than one cation? Type II Find the charge of the cation Use a Roman number after the element name. Type I Use the element name for the cation

  19. Naming Polyatomic Ionic Compounds They contain more than two elements.

  20. Naming Polyatomic Ions Cation:NH4+ Ammonium MnO4- Permanganate CrO42- Chromate Cr2O72- Dichromate CO32- Carbonate HCO3- Hydrogen Carbonate (bicarbonate) PO33- Phosphite PO43- Phosphate HPO42- Hydrogen phosphate H2PO4- Dihydrogen phosphate Anion: OH- Hydroxide NO2- Nitrite NO3- Nitrate SO32- Sulfite SO42- Sulfate HSO3- Hydrogen Sulfite (bisulfite) HSO4- Hydrogen sulfate (bisulfate)

  21. Oxyanions Polyatomic anions with different numbers of oxygen atoms. When we have two oxyanions in a series: Smaller number of oxygen atoms ends with –ite. Larger number of oxygen atoms ends with –ate. NO2- Nitrite NO3- Nitrate SO32- Sulfite SO42- Sulfate HSO3- Hydrogen Sulfite (bisulfite) HSO4- Hydrogen sulfate (bisulfate) PO33- Phosphite PO43- Phosphate HPO42- Hydrogen phosphate H2PO4- Dihydrogen phosphate

  22. Oxyanions When we have more than two oxyanions in a series: (Fewest oxygen atoms) Prefix hypo- (Most oxygen atoms) Prefix per- ClO-hypochlorite ClO2- chlorite ClO3- chlorate ClO4-perchlorate

  23. matter are neutral (uncharged): total number of positive charges = total number of negative charges Na+ NO3- NaNO3 Ca2+ CO32- Ca2(CO3)2 Ca(CO3) Al3+ SO42- Al2(SO4)3 Mg2+ NO2- Mg(NO2)2

  24. Naming Polyatomic Ionic compounds Name of metal (cation) + Name of anion NaNO3 Sodium nitrate Calcium carbonate Ca(CO3) Al2(SO4)3 Aluminum sulfate Mg(NO2)2 Magnesium nitrite

  25. Naming Polyatomic Ionic compounds Name of metal (cation) + Name of anion FeCO3 Iron(II) carbonate Iron(III) carbonate Fe2(CO3)3

  26. Naming acids Acids: sour They produce H+ (proton) in water.

  27. Anion : -ide ion + Hydro -ic acid Naming binary acids HF F-: flouride ion Hydroflouric acid HCl Cl-: chloride ion Hydrochloric acid H2S S2-: sulfuride ion Hydrosulfuric acid

  28. Naming Polyatomic Acids -ite ion -ous acid Anion: -ate ion -ic acid HNO2 NO2-: Nitrite ion Nitrous acid HNO3 NO3-: Nitrate ion Nitric acid H2CO3 CO32-: Carbonate ion Carbonic acid H2SO3 SO32-: Sulfurite ion Sulfurous acid

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