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Naming Chemicals

Naming Chemicals. AP Chemistry. Classes of Chemicals. Elements Ionic Compounds Covalent Compounds Organic Compounds. Gold. Elements. All elements on the periodic table All just one word: iron, sodium, neon, etc. All neutrally charged Mostly monatomic: Fe, Na, Ne

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Naming Chemicals

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  1. Naming Chemicals AP Chemistry

  2. Classes of Chemicals • Elements • Ionic Compounds • Covalent Compounds • Organic Compounds

  3. Gold Elements • All elements on the periodic table • All just one word: iron, sodium, neon, etc. • All neutrally charged • Mostly monatomic: Fe, Na, Ne • Some diatomic: H2 O2 N2 Cl2 Br2 I2 F2 • Some polyatomic: S8, P4

  4. Ionic Compounds • Made of one metal positive ion (cation) and one non-metal negative ion (anion) • Always two words starting with the cation and ending with the anion • Cation is same name as element • Anion always has a different suffix Sodium chloride

  5. Anion Suffixes • Monatomic atoms end with –ide • Oxygen atom = O • Oxide ion = O-2 • Sulfur atom = S • Sulfide ion = S-2 • Chlorine atom = Cl • Chloride ion = Cl-1

  6. Oxy-Anions • Oxy-anions end in –ate • Sulfate = SO4-2 Chlorate = ClO3-1 • Chromate = CrO4-2 Nitrate = NO3-1 • If the anion is further oxidized then add the prefix per- • ClO3-1 = chlorate ClO4-1 = perchlorate

  7. Less Oxidation • If the anion is less oxidized by 1 then change the –ate suffix to an –ite suffix • SO4-2 = sulfate SO3-2 = sulfite • ClO3-1 = chlorate ClO2-1 = chlorite • If the anion is less oxidized again then add the prefix hypo- • ClO-1 = hypochlorite SO2-2 = hyposulfite

  8. Summary

  9. Sulfur Replacement • If one of the oxygens in an oxy-anion is replaced with a sulfur then add the prefix thio- • SO4-2 = sulfate S2O3-2 = thiosulfate • SO3-2 = sulfite S2O2-2 = thiosulfite • CNO-1 = cyanate CNS-1 = thiocyanate

  10. Anion Summary • Mon-atomic anions end in –ide • Oxy-anions end in –ate or –ite • Add prefixes per- and hypo- when necessary • Add thio- prefix when a sulfur replaces and oxygen

  11. Combining Ions • Ionic compounds are always neutrally charged so the number of each ion within the compound is fixed • Sodium oxide: Na+1 O-2 Since the compound must be neutral we need another positive charge Na+1 Now we have two sodium atoms to balance out the oxide so the final formula is: Na2O

  12. Parenthesis • Use parenthesis for multiple polyatomic ions Aluminum chromate Al+3 CrO4-2 Al2(CrO4)3

  13. Be careful of Hydroxides! Calcium hydroxide Ca+2 OH-1 Ca(OH)2 CaOH2

  14. Transition Metals

  15. Transition Metals • Transition Metals often have more than one charge • Examples: Fe+2 and Fe+3 • This makes a difference in formulae: • Iron chloride could be: • FeCl2 or FeCl3

  16. So what do we do? • Since FeCl2 and FeCl3 are obviously not the same compound, they can’t both have the same name. • We differentiate them by using a Roman Numeral to indicate the charge on the transition metal • Fe+2 and Cl-1 FeCl2 = iron (II) chloride • Fe+3 and Cl-1 FeCl3 = iron (III) chloride • Be sure to note that the roman numeral indicates charge and not number.

  17. Sodium bromide NaBr Quick practice • Calcium oxide • CaO • Aluminum nitrate • Al(NO3)3 • Ammonium phosphate • (NH4)3PO4 • Barium hydroxide • Ba(OH)2 • Copper (I) sulfide • Cu2S • Copper (II) sulfate • CuSO4 • Iron (III) dichromate • Fe2(Cr2O7)3

  18. Potassium hypochlorite KClO More practice • Sodium sulfite • Na2SO3 • Aluminum bromate • Al(BrO3)3 • Ammonium phosphite • (NH4)3PO3 • Magnesium nitrite • Mg(NO2)2 • Iron (III) perchlorate • Fe(ClO4)3 • Strontium cyanate • Sr(CNO)2 • Copper (I) thiosulfate • Cu2S2O3

  19. Covalent Compounds • Comprised of two or more non-metals covalently bonded • Start with less electronegative and end with more electronegative • Name as normal except that all compounds change the second element to an –ide ending

  20. Covalent Examples • CO = carbon oxide • CS2 = carbon sulfide • NF3 = nitrogen fluoride • Notice in each example the more electronegative atom is second and ends in -ide

  21. Problem • Covalent compounds can combine in multiple proportions- that is there can be more than one ratio of atoms in a compound • CO vs. CO2 • They can’t both be carbon oxide • NO2 vs. N2O4 • They can’t both be nitrogen oxide

  22. Solution? • Use prefixes to indicate the number of covalently bonded atoms present in the molecule • CO vs. CO2 • Carbon monoxide Carbon dioxide

  23. 1 2 3 4 5 6 7 8 9 10 Mono- Prefixes • Di- • Tri- • Tetra- • Penta- • Hexa- • Hepta- • Octa- • Nona- • Deca-

  24. Overall Covalent Rules • Comprised of two or more non-metals covalently bonded • Start with less electronegative and end with more electronegative • Name as normal except that all compounds change the second element to an –ide ending • Add a prefix to indicate number of atoms in the compound • The second atom ALWAYS gets a prefix • The first atom can ignore MONO-

  25. CO Carbon monoxide Practice • N2O5 • Dinitrogen pentoxide • PCl5 • Phosphorus pentachloride • SO3 • Sulfur trioxide • N2O • Dinitrogen monoxide

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