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Understanding Acids and Bases Behavior: Naming and Writing Guide

Learn how acids and bases behave and how to name and write their formulas in this comprehensive guide. Discover the Arrhenius definitions, naming principles for acids, and how bases produce the hydroxide ion. Practice examples included.

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Understanding Acids and Bases Behavior: Naming and Writing Guide

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  1. Section 2.4—Defining, Naming & Writing Acids & Bases We need to know how acids and bases behave when talking about ant-acids!

  2. Acids

  3. H +1 +1 H water O O H H H H Acids – Arrhenius Definition • A compound that has a H+ cation that it can donate to water to produce the hydronium ion (H3O+1) hydronium ion By this definition, if an acid is to give a H+1 to water, then all acids will have hydrogen as the cation (first element written).

  4. - H O H H How do Acids produce Hydronium? water acid Hydrogen cation with some anion

  5. - H O H H How do Acids produce Hydronium? +1

  6. - H O H H How do Acids produce Hydronium? +1 Hydronium ion Anion

  7. Naming Acids

  8. Naming Non-oxygen Acids • These compounds : • Start with “H” (more than 1 “H” is OK, too). • Have only 2 elements in total (One of them is hydrogen the other is NOT oxygen.) • Examples: HCl H2S • To name these compounds: • Use “hydro____ic acid” • Fill in the blank with the anion’s name without the last syllable

  9. Example #1 HBr

  10. Example #1 It’s an acid Hydrogen cation HBr Hydrobromic acid Bromine No oxygen Use “hydro___ic”

  11. Naming Oxygen Acids • These compounds have: • Start with “H” (more than 1 “H” is OK, too). • Contain a polyatomic ion that has oxygen in it. • To name these compounds: • Use “___ic acid” for “-ate” anions; the blank is filled in with the polyatomic ions name without the suffix. • Use “___ous acid” for “-ite” anions; the blank is filled in with the polyatomic ions name without the suffix. Examples: HNO2 is . . . HNO3 is . . .

  12. Example #2 H2SO3

  13. Example #2 It’s an acid Hydrogen cation H2SO3 Sulfite ion “-ite” ion Use “___ous” acid Sulfurous acid

  14. Example #3 H2SO4

  15. Example #3 It’s an acid Hydrogen cation H2SO4 Sulfate ion “-ate” ion Use “___ic” Sulfuric acid

  16. Let’s Practice HI H2CO3 HC2H3O2 H3PO3 Example: Write the name for the following compounds

  17. Let’s Practice HI H2CO3 HC2H3O2 H3PO3 hydroiodic acid carbonic acid acetic acid phosphorous acid Example: Write the name for the following compounds

  18. Writing Acid Formulas

  19. “Hydro-” acids • To write these formulas: • The cation is H+1 • Write the anion and charge • Balance the charges by adding the appropriate subscript to the hydrogen cation

  20. Example #4 Hydrofluoric acid

  21. Example #4 H+1 Hydrogen cation Hydrofluoric acid Only one other element F-1

  22. Example #4 H+1 Hydrogen cation Hydrofluoric acid Does not contain oxygen H+1F-1 F-1 HF

  23. NON “Hydro-” acids • To write these formulas: • The cation is H+1 • If it is an “-ic” acid, the anion is the “-ate” polyatomic ion • If it is an “-ous” acid, the anion is the “-ite” polyatomic ion • Add subscript to the hydrogen cation to balance charges

  24. Example #5 Carbonic acid

  25. Example #5 H+1 Hydrogen cation Carbonic acid From the “___ate” anion CO3-2

  26. Example #5 H+1 Hydrogen cation Carbonic acid H+CO32- From the “___ate” anion CO3-2 H2CO3

  27. Example #6 Nitrous acid

  28. Example #6 H+1 Hydrogen cation Nitrous acid From the “___ite” anion NO2-1

  29. Example #6 H+1 Hydrogen cation Nitrous acid H+NO2- From the “___ite” anion HNO2 NO2-1

  30. Let’s Practice Phosphoric acid Hydroiodic acid Acetic acid Perchloric acid Example: Write the formula for the following acids

  31. Let’s Practice Phosphoric acid Hydroiodic acid Acetic acid Perchloric acid H3PO4 HI HC2H3O2 HClO4 Example: Write the formula for the following acids

  32. Bases • Objective: • Define and distinguish between acids & bases • Explain and use nomenclature rules for naming and writing formulas for bases

  33. -1 O H Bases – Arrhenius Definition • Bases produce the hydroxide ion in water • MOST bases will be ionic compounds with the OH-1 anion. (Ex. NaOH or Ca(OH)2) • MOST IMPORTANT EXCEPTION is NH3 (ammonia). • NH3 + H2O  NH4+1 + OH-1 Hydroxide Ion

  34. Naming & Writing Bases

  35. Naming Bases • Most bases are just ionic compounds with “hydroxide” as their anion • The most common exception to this is ammonia. NH3 is a base even though it doesn’t contain “-OH” as the anion.

  36. Example #7 NaOH

  37. Example #7 Sodium NaOH Sodium Hydroxide Hydroxide

  38. Example #8 Iron (III)hydroxide Fe+3 OH-1 criss –cross the number of the charges Fe(OH)3

  39. Let’s Practice Ca(OH)2 KOH Sr(OH)2 Copper (II) hydroxide Magnesium hydroxide Example: Write the formula or name for each

  40. Let’s Practice Ca(OH)2 KOH Sr(OH)2 Copper (II) hydroxide Magnesium hydroxide Calcium hydroxide Potassium hydroxide Strontium hydroxide Cu(OH)2 Mg(OH)2 Example: Write the formula or name for each

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