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Naming compounds
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- 2. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 2 5.1 Naming Compounds 5.2 Naming Binary Compounds That Contain a Metal and a No 5.3 Naming Binary Compounds That Contain Only Nonmetals 5.4 Naming Binary Compounds: A Review 5.5 Naming Compounds That Contain Polyatomic Ions 5.6 Naming Acids 5.7 Writing Formulas from Names
- 3. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 3 • Binary Compounds Composed of two elements • Binary Ionic Compounds Metal—nonmetal • Binary Covalent Compounds Nonmetal—nonmetal
- 4. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 4 • Binary ionic compounds contain positive cations and negative anions. Type I compounds • Metal present forms only one cation. Type II compounds • Metal present can form 2 or more cations with different charges.
- 5. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 5 Metals (Groups I, II, and III) and Non-Metals Metal _________ + Non-Metal _________ideSodium Chlorine Sodium Chloride NaCl Type I Compounds
- 6. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 6 Common Simple Cations and Anions
- 7. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 7 1. The cation is always named first and the anion second. 2. A simple cation takes its name from the name of the element. 3. A simple anion is named by taking the first part of the element name (the root) and adding –ide. Rules for Naming Type I Ionic Compounds
- 8. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 8 • Examples: KCl Potassium chloride MgBr2 Magnesium bromide CaO Calcium oxide Binary Ionic Compounds (Type I)
- 9. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 9 Exercise What is the name of the compound SrBr2? a) strontium bromine b) sulfur bromide c) strontium dibromide d) strontium bromide
- 10. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 10 Binary Ionic Compounds (Type II) • Metals in these compounds can form more than one type of positive charge. • Charge on the metal ion must be specified. • Roman numeral indicates the charge of the metal cation. • Transition metal cations usually require a Roman numeral.
- 11. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 11 Metals (Transition Metals) and Non-Metals Metal ______ +Roman Numeral (__) + Non-Metal ________ideIron III Bromine Iron (III) Bromide FeBr3 Compare with Iron (II) Bromide FeBr2 Metals (Transition Metals) and Non-Metals Older System Metal (Latin) _______ + ous or ic + Non-Metal ________ideFerrous Bromine Ferrous Bromide FeBr2 Compare with Ferric Bromide FeBr3 Type II Compounds
- 12. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 12 Common Type II Cations
- 13. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 13 1. The cation is always named first and the anion second. 2. Because the cation can assume more than one charge, the charge is specified by a Roman numeral in parentheses. Rules for Naming Type II Ionic Compounds
- 14. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 14 • Examples: CuBr Copper(I) bromide FeS Iron(II) sulfide PbO2 Lead(IV) oxide Binary Ionic Compounds (Type II)
- 15. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 15 Exercise What is the name of the compound CrO2? a) chromium oxide b) chromium(II) oxide c) chromium(IV) oxide d) chromium dioxide
- 16. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 16 Exercise What is the correct name of the compound that results from the most stable ion for sulfur and the metal ion that contains 24 electrons? a) iron(III) sulfide b) chromium(II) sulfide c) nickel(III) sulfate d) iron(II) sulfide
- 17. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 17 • Formed between two nonmetals. 1. The first element in the formula is named first, and the full element name is used. 2. The second element is named as though it were an anion. 3. Prefixes are used to denote the numbers of atoms present. 4. The prefix mono- is never used for naming the first element. Rules for Naming Type III Binary Compounds
- 18. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 18 Type III Compounds Non-Metals and Non-Metals Use Prefixes such as mono, di, tri, tetra, penta, hexa, hepta, etc. CO2 Carbon dioxide CO Carbon monoxide PCl3 Phosphorus trichloride CCl4 Carbon tetrachloride N2O5 Dinitrogen pentoxide CS2 Carbon disulfide
- 19. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 19 Prefixes Used to Indicate Numbers in Chemical Names 9 nona- 10 deca- 11 undeca- 12 dodeca- 13 trideca- 14 tetradeca- 15 pentadeca- 16 hexadeca- 17 heptadeca- 18 octadeca- 19 nonadeca- 20 icosa Additional Prefixes
- 20. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 20 • Examples: CO2 Carbon dioxide SF6 Sulfur hexafluoride N2O4 Dinitrogen tetroxide Binary Covalent Compounds (Type III)
- 21. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 21 Exercise What is the name of the compound SeO2? a) selenium oxide b) selenium dioxide c) selenium(II) oxide d) selenium(IV) dioxide
- 22. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 22 Flow Chart for Naming Binary Compounds
- 23. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 23 Let’s Practice! Name the following. CaF2 K2S CoI2 SnF2 SnF4 OF2 CuI2 CuI SO2 SrS LiBr Strontium Sulfide Lithium Bromide Copper (I) Iodide or Cuprous Iodide Sulfur dioxide Copper (II) Iodide or Cupric Iodide Oxygen diflouride Tin (IV) Fluoride or Stannic Fluoride Tin (II) Fluoride or Stannous Fluoride Cobalt (II) Iodide or Cobaltous Iodide Potassium Sulfide Calcium Flouride
- 24. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 24 • Polyatomic ions are charged entities composed of several atoms bound together. • They have special names and must be memorized.
- 25. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 25 Names of Common Polyatomic Ions (page 130)
- 26. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 26 • Naming ionic compounds containing polyatomic ions follows rules similar to those for binary compounds. Ammonium acetate
- 27. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 27 NaOH Sodium hydroxide Mg(NO3)2 Magnesium nitrate (NH4)2SO4 Ammonium sulfate FePO4 Iron(III) phosphate Examples
- 28. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 28 Overall Strategy for Naming Chemical Compounds
- 29. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 29 Exercise What is the name of the compound KClO3? a) potassium chlorite b) potassium chlorate c) potassium perchlorate d) potassium carbonate
- 30. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 30 Exercise Examine the following table of formulas and names. Which of the compounds are named correctly? a) I, II b) I, III, IV c) I, IV d) I only Formula Name I P2 O5 Diphosphorus pentoxide II ClO2 Chlorine oxide III PbI4 Lead iodide IV CuSO4 Copper(I) sulfate
- 31. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 31 • Acids can be recognized by the hydrogen that appears first in the formula—HCl. • Molecule with one or more H+ ions attached to an anion. Acids
- 32. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 32 • If the anion does not contain oxygen, the acid is named with the prefix hydro– and the suffix –ic attached to the root name for the element. • Examples: HCl Hydrochloric acid HCN Hydrocyanic acid H2S Hydrosulfuric acid Rules for Naming Acids
- 33. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 33 Acids That Do Not Contain Oxygen
- 34. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 34 • If the anion contains oxygen: The suffix –ic is added to the root name if the anion name ends in –ate. • Examples: HNO3 Nitric acid H2SO4Sulfuric acid HC2H3O2 Acetic acid Rules for Naming Acids
- 35. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 35 • If the anion contains oxygen: The suffix –ous is added to the root name if the anion name ends in –ite. • Examples: HNO2 Nitrous acid H2SO3Sulfurous acid HClO2 Chlorous acid Rules for Naming Acids
- 36. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 36 Some Oxygen-Containing Acids
- 37. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 37 Flowchart for Naming Acids
- 38. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 38 Exercise Which of the following compounds is named incorrectly? a) KNO3 potassium nitrate b) TiO2 titanium(II) oxide c) Sn(OH)4tin(IV) hydroxide d) PBr5 phosphorus pentabromide e) H2SO3 sulfurous acid
- 39. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 39 • Sodium hydroxide NaOH • Potassium carbonate K2 CO3 • Sulfuric acid H2 SO4 • Dinitrogen pentoxide N2 O5 • Cobalt(III) nitrate Co(NO3 )3 Examples
- 40. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 40 Exercise A compound has the formula XCl3 where X could represent a metal or nonmetal. What could the name of this compound be? a) phosphorus trichloride b) carbon monochloride c) tin(IV) chloride d) magnesium chloride
- 41. Naming Compounds Return toTOC Copyright © Cengage Learning. All rights reserved 41 Lets Practice Some More! HF Na2CO3 H2CO3 KMnO4 HClO4 H2S NaOH CuSO4 PbCrO4 H2O NH3 Hydrooxic acid (no……just water) Nitrogen trihydride (no..just ammonia) Copper (II) sulfate or Cupric sulfate Lead (II) chromate or Plubous chromate Sodium hydroxide Hyrdogen sulfuric acid Perchloric acid Potassium permanganate Sodium carbonate Hydroflouric acid Carbonic acid
Editor's Notes
- #10 Strontium bromide. Sr is the symbol for strontium. Br is the symbol for bromine, but t ake the first part of the element name (the root) and add – ide to get the name bromide.
- #16 Chromium(IV) oxide. Cr is the symbol for chromium. O is the symbol for oxygen, but t ake the first part of the element name (the root) and add – ide to get the name oxide. Since chromium can have more than one charge, a Roman numeral must be used to identify that charge. There are two oxygen ions each with a 2– charge, giving an overall charge of –4. Therefore, the charge on chromium must be +4.
- #17 Iron(II) sulfide. For sulfur, t ake the first part of the element name (the root) and add – ide to get the name sulfide. Iron with a +2 charge (as the Roman numeral indicates) contains 24 electrons (26p – 24e = +2 charge).
- #22 Selenium dioxide. Se is the symbol for selenium. O is the symbol for oxygen, but t ake the first part of the element name (the root) and add – ide to get the name oxide. Since they are both nonmetals, prefixes are used to identify the elements (except mono- is not used for the first element). Two oxygen atoms require the use of the prefix di-, making the name dioxide.
- #30 ClO 3 – is the polyatomic ion chlorate.
- #31 Only Formula I is named correctly. Formula II is chlorine dioxide. Formula III is lead(IV) iodide. Formula IV is copper(II) sulfate.
- #39 The correct answer is “b”. The charge on oxygen is 2–. Since there are two oxygen atoms, the overall charge is 4–. Therefore, the charge on titanium must be 4+ (not 2+ as the Roman numeral indicates).
- #41 Phosphorus trichloride. Carbon monochloride has the formula CCl. Tin(IV) chloride has the formula SnCl 4 . Magnesium chloride has the formula MgCl 2 . Phosphorus trichloride has the formula PCl 3 and is therefore the correct answer.