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CHAPTER 5 - NOMENCLATURE IONIC COMPOUNDS NAMING Name the cation first, then name the anion second

CHAPTER 5 - NOMENCLATURE IONIC COMPOUNDS NAMING Name the cation first, then name the anion second CATIONS 1) Metals that form only one monatomic cation Name as the elemental name. 4A-1 (of 32). Al 3+ Zn 2+ Ag +. Group 1 (1+) Group 2 (2+). 4A-2. Ca 2+ calcium. K + potassium.

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CHAPTER 5 - NOMENCLATURE IONIC COMPOUNDS NAMING Name the cation first, then name the anion second

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  1. CHAPTER 5 - NOMENCLATURE IONIC COMPOUNDS NAMING Name the cation first, then name the anion second CATIONS 1) Metals that form only one monatomic cation Name as the elemental name 4A-1 (of 32)

  2. Al3+ Zn2+ Ag+ Group 1 (1+) Group 2 (2+) 4A-2

  3. Ca2+ calcium K+ potassium Al3+ aluminum 4A-3

  4. 2) Metals that form more than one monatomic cation Name as the elemental name, followed by their charge as a roman numeral in parenthesis 4A-4

  5. Mn2+ manganese Mn3+ manganese Sn4+ tin (IV) (II) (III) George Foreman George Foreman George Foreman George Foreman George Foreman 4A-5

  6. 3) Cations that are polyatomic NH4+ ammonium UO22+ uranyl Hg22+ mercury (I) 4A-6

  7. ANIONS 1) Nonmetals that form a monatomic anion Name as the root of the elemental name, ending in -ide 4A-7

  8. H (1-) Group 17 (1-) Group 16 (2-) Group 15 (3-) 4A-8

  9. O2- oxide Cl- chloride N3- nitride S2- P3- H- 4A-9

  10. 2) Anions that are polyatomic Name polyatomic anions that contain oxygen as the root of the elemental name, ending in –ate or –ite CO32- carbonate NO3- nitrate NO2- nitrite PO43- phosphate SO42- sulfate SO32- sulfite 4A-10

  11. Some elements can make 4 oxyions ClO4- perchlorate ClO3- chlorate ClO2- chlorite ClO- hypochlorite 4A-11

  12. Name the following: CaCl2 calcium chloride Na2O sodium oxide MgS 4A-12

  13. AuI3 1- 1- 1- PbBr2 1- 1- Cu2O 3+ 2+ gold (III) iodide lead (II) bromide 4A-13

  14. Cr2S3 2- 2- 2- K2SO4 SnCO3 3+ 3+ chromium (III) sulfide potassium sulfate 4A-14

  15. FORMULAS Base formulas on charge balance barium fluoride Ba2+ F- (2+) + (1-) + (1-) = 0 potassium oxide K+ O2- (1+) + (1+) + (2-) = 0 Need 2 to make total charge 0 Need 2 to make total charge 0 K2O BaF2 4A-15

  16. Makes 6+ Makes 6- lithium nitride aluminum sulfide Al3+ S2- (3+) + (3+) + (2-) + (2-) + (2-) = 0 Al2S3 4A-16

  17. cobalt (III) chloride Co3+ Cl- (3+) + (1-) + (1-) + (1-) = 0 lithium nitrate Li+ NO3- (1+) + (1-) = 0 Need 3 to make total charge 0 CoCl3 LiNO3 4A-17

  18. barium hydroxide Ba2+ OH- (2+) + (1-) + (1-) = 0 Sodium bicarbonate Na+ HCO3- (1+) + (1-) = 0 Need 2 to make total charge 0 NaHCO3 BaOH2 NO! Ba(OH)2 4A-18

  19. iron (III) nitrate Fe3+ NO3- (3+) + (1-) + (1-) + (1-) = 0 zinc phosphate Need 3 to make total charge 0 Fe(NO3)2 4A-19

  20. HYDRATES Compounds with water molecules trapped in their crystals Name ionic compound first, then a prefix for the number of waters, followed by -hydrate 1 mono 2 di 3 tri 4 tetra 5 penta 6 hexa 7 hepta 8 octa 9 nona 10 deca 4A-20

  21. CuCl2.6H2O copper (II) chloride hexahydrate iron (III) nitrate nonahydrate Fe(NO3)3.9H2O 4A-21

  22. COVALENT COMPOUNDS NAMING BINARY COMPOUNDS Name the 1st nonmetal as element name, using prefix if more than 1 atom Name the 2nd nonmetal with –ide, always use a prefix CO2 carbon dioxide CO carbon monoxide N2O dinitrogen monoxide 4A-22

  23. FORMULAS OF BINARY COMPOUNDS Base formulas on prefixes Phosphorus triiodide PI3 diarsenic pentasulfide 4A-23

  24. NAMING ACIDS ARRHENIUS ACID – A compound that loses hydrogen ions in solution ARRHENIUS BASE – A compound that loses hydroxide ions in solution Out of water – named as an ionic compound HCl (g) hydrogen chloride Dissolved in water – name based on name of the acid’s anion 4A-24

  25. Anion in acid ends in –ide hydro–root–ic acid Anion in acid ends in –ate root–ic acid Anion in acid ends in –ite root–ous acid HBr Br- bromide ion hydrobromic acid 4A-25

  26. Anion in acid ends in –ide hydro–root–ic acid Anion in acid ends in –ate root–ic acid Anion in acid ends in –ite root–ous acid H2S S2- sulfide ion hydrosulfuric acid 4A-26

  27. Anion in acid ends in –ide hydro–root–ic acid Anion in acid ends in –ate root–ic acid Anion in acid ends in –ite root–ous acid HNO3 NO3- nitrate ion nitric acid 4A-27

  28. Anion in acid ends in –ide hydro–root–ic acid Anion in acid ends in –ate root–ic acid Anion in acid ends in –ite root–ous acid H2SO4 SO42- sulfate ion sulfuric acid 4A-28

  29. Anion in acid ends in –ide hydro–root–ic acid Anion in acid ends in –ate root–ic acid Anion in acid ends in –ite root–ous acid H3PO3 PO33- phosphite ion phosphorous acid 4A-29

  30. FORMULAS OF ACIDS Anion in acid ends in –ide hydro–root–ic acid Anion in acid ends in –ate root–ic acid Anion in acid ends in –ite root–ous acid hydrofluoric acid fluoride ion F- HF 4A-30

  31. FORMULAS OF ACIDS Anion in acid ends in –ide hydro–root–ic acid Anion in acid ends in –ate root–ic acid Anion in acid ends in –ite root–ous acid carbonic acid carbonate ion CO32- H2CO3 4A-31

  32. FORMULAS OF ACIDS Anion in acid ends in –ide hydro–root–ic acid Anion in acid ends in –ate root–ic acid Anion in acid ends in –ite root–ous acid nitrous acid nitrite ion NO2- HNO2 4A-32

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