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Chemical Naming: Covalent and Ionic Compounds

Learn how to name chemical compounds, including vocabulary, covalent and ionic bonds, formulas, and the nomenclature for molecular and ionic compounds. Also covers hydrates and acid naming.

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Chemical Naming: Covalent and Ionic Compounds

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  1. Chapter 2 II. Naming Compounds

  2. A. Vocabulary CHEMICAL BONDS IONIC COVALENT 2 nonmetals M etal + Nonmetal e- transferred e- shared CO2 NaCl

  3. A. Vocabulary CHEMICAL FORMULA IONIC COVALENT Formula Unit Molecular Formula NaCl CO2

  4. A. Vocabulary COMPOUND more than 2 elements 2 elements Binary Compound Ternary Compound NaCl NaNO3

  5. A. Vocabulary ION 2 or more atoms 1 atom Monatomic Ion Polyatomic Ion Cation Anion Na+ NO3-

  6. B. Covalent Nomenclature • Prefix System (binary compounds) 1. Less e-neg atom comes first. Ex. CO2 2. Add prefixes to indicate # of atoms. Omit mono- prefix on first element. Ex.Carbon Dioxide 3. Change the ending of the second element to -ide.

  7. PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 B. Molecular Nomenclature

  8. B. Molecular Nomenclature • CCl4 • H2O • SF6 • carbon tetrachloride • dihydrogen monoxide • sulfur hexafluoride

  9. B. Molecular Nomenclature • arsenic trichloride • dinitrogen pentoxide • tetraphosphorus decoxide • AsCl3 • N2O5 • P4O10

  10. C. Ionic Nomenclature Ionic Formulas • Write each ion, cation (+) first. Don’t show charges in the final formula. • Overall charge must equal zero. • If charges cancel, just write symbols. • If not, use subscripts to balance charges. Sodium Iodide: Na+ I - NaI Calcium Bromide: Ca+2Br - CaBr2

  11. C. Ionic Nomenclature Ionic Names • Write the names of both ions, cation (+) first. • Change ending of monatomic ions to -ide. • Polyatomic ions have special names. Use parentheses to show more than one polyatomic ion in a formula. (See Handout!) • Stock System - Use Romannumerals to show the ion’s charge if more than one is possible for the transition metals.

  12. C. Ionic Nomenclature • Consider the following: • Does it contain a polyatomic ion? • -ide, 2 elements  no • -ate, -ite, 3+ elements  yes • Does it contain a Roman numeral? • Check the table for metals not in Groups 1 or 2. • No prefixes!

  13. C. Ionic Nomenclature Common Ion Charges • potassium chloride • magnesium nitrate • copper(II) chloride  KCl • K+ Cl- • Mg2+ NO3-  Mg(NO3)2  CuCl2 • Cu2+ Cl-

  14. C. Ionic Nomenclature • MgBr2 • Na2CO3 • FeCl3 • magnesium bromide • sodium carbonate • iron(III) chloride

  15. D. Hydrates – Day 2 • Hydrates - Ionic compounds that absorb water into their solid structure • Water can be removed by heating • Anhydrous is the opposite and means “without water”.

  16. D. Hydrates • Formula and name of a hydrate: CuSO4o 5H20 Copper (II) Sulfate PentaHydrate CoCl2o 6H20 Cobalt (II) Chloride HexaHydrate

  17. E. Determining Charge • Find the charge of each ion and the total number of atoms: • Na3PO4: Chg: Na+1 PO4-3 • Na – 3 atoms; P – 1; O – 4 atoms • Fe(OH)3: Chg: Fe+3 OH-1 • Fe – 1 atom; O – 3; H – 3 atoms • Cu(NO3)2 : Chg: Cu+2 NO3-1 • Cu – 1 atom; N – 2; O – 6 atoms

  18. F. Naming Acids • Acids, p. 64-67 • Compounds that form H+ in water. • Formulas usually begin with ‘H’. • Examples: • HCl – hydrochloric acid (stomach acid) • HNO3 – nitric acid • H2SO4 – sulfuric acid (car battery acid)

  19. Naming acids p.65 • If the formula has oxygen in it • write the name of the anion, but change • ate to -ic acid • ite to -ous acid • Watch out for sulfuric and sulfurous • H2CrO4 • HNO3 • HNO2

  20. Naming acids • If the acid doesn’t have oxygen • add the prefix hydro- • change the suffix -ide to -ic acid • HCl • H2S

  21. Acid Nomenclature

  22. Acid Nomenclature

  23. Acid Nomenclature • HBr • H2CO3 • H2SO3 hydrobromic acid 2 elements, -ide 3 elements, -ate  carbonic acid  sulfurous acid 3 elements, -ite

  24. Acid Nomenclature • hydrofluoric acid • sulfuric acid • nitrous acid 2 elements  H+ F-  HF 3 elements, -ic  H+ SO42-  H2SO4  H+ NO2-  HNO2 3 elements, -ous

  25. Formulas for acids • Backwards from names. • If it has hydro- in the name it has no oxygen • Anion ends in -ide • No hydro, anion ends in -ate or -ite • Write anion and add enough H to balance the charges.

  26. Formulas for acids • hydrofluoric acid • dichromic acid • carbonic acid • hydrophosphoric acid • hypofluorous acid • perchloric acid • phosphorous acid

  27. Read and take notes: • Chp. #2 – Sec. 2.4 and pp.64-67, Naming acids. • Skip Sec. 2.8 (we will do this later) • 1st half of problems: (1-27) already assigned* • 2nd half of problems: (35, 46, 50, 58, 60, 63, 64, 68, 69, 73, 79, 87).

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