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Chemistry 111

Chemistry 111. Chapter 6 - Nomenclature. Nomenclature – Main Tasks. Learn Specific Rule Sets Ionic Compounds Covalent Compounds Transition Metal Cations Learn Oxyanions & Oxyacids Memorize… Practice

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Chemistry 111

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  1. Chemistry 111 Chapter 6 - Nomenclature

  2. Nomenclature – Main Tasks • Learn Specific Rule Sets • Ionic Compounds • Covalent Compounds • Transition Metal Cations • Learn Oxyanions & Oxyacids • Memorize… • Practice • Flash Cards! Keep them in your pocket – pull them out when waiting in lines, during commercials. • Collate all of this information…

  3. Nomenclature • Rules / System of Rules (+ exceptions) • Elements • Covalent Compounds • Monatomic Ions • Regular • Super Sized (super ugly?) • Polyatomic Anions • 5 “normal” • more & less • Acids • Formulas of Ionic Compounds • Naming Ionic Compounds • Common Polyatomic Ions (other)

  4. Naming Elements • Very Simple – just their names. • Diatomic Elements • Remember H, O, N, Cl, Br, I, F all come as diatomic molecules in elemental form • “HONClBrIF” hon-cul-brif • H2, O2, …

  5. Covalent Compounds • 2 non-metals have covalent bonds. • Naming system needs to indicate how many of each: CO vs CO2 • Rules: • Use mono-, di-, tri- prefixes (1, 2, 3, …) • End with “-ide” • Exception: • Skip mono- prefix with 1st element • monocarbon dioxide?

  6. Monatomic Ions • We learned to figure out the charge of an ion formed by each element • except transition metals • How do we name them? • Cations: • just add “ion” • Ca2+ = “calcium ion” Al3+ = “aluminum ion” • Anions • Add “-ide” and “ion” • S2- = “sulfide ion” Cl- = “chloride ion”

  7. Transition Metal Ions • Many transition metals have multiple charges (all positive) • We have to memorize which are which! • (Naming them will be worse…)

  8. Common/Important Transition Metal Ions

  9. Common/Important Transition Metal Ions

  10. Stock System Use a roman numeral with the charge. Use English Name Fe3+ = iron (III) ion Fe2+ = iron (II) ion Sn4+ = tin (IV) ion Zn2+ = zinc ion Old System Use endings to indicate charge Higher “-ic” Lower “-ous” Use latin names Fe3+ = ferric ion Fe2+ = ferrous ion Sn4+ = stannic ion Naming Transition Metal Ions with Multiple Charges

  11. Naming Mercury • Hg22+ has +2 spread over 2 mercury atoms • mercury (I) ion, mercurous ion • Hg2+ has +2 on 1 mercury atom • mercury (II) ion, mercuric ion • Note that it’s a double exception – we don’t use the latin name!

  12. More Nomenclature • Polyatomic Anions • 5 “normal” • more & less • Acids • Formulas of Ionic Compounds • Naming Ionic Compounds • Common Polyatomic Ions (other)

  13. Polyatomic Anions • These are molecules with negative charge. • Inside the anion, bonding is covalent. • Outside they form ionic bonds. • Be sure to treat the poly-ions as a whole unit! shared electrons lost 1 electon - [ ] O Cl O Na+

  14. How do we learn all of these? • (Table 6.8) • Memorize the whole table. • Learn a system…(more of Herbelin’s propaganda)

  15. Oxyanion System • Learn (memorize) the 5 “normal” anions. • Element • Charge • # of oxygens • “-ate” • Learn how to add/subtract oxygens.

  16. 5 “Normal” Oxyanions

  17. Changing the Number of Oxygens • The ending shows how many oxygens are on an oxyanion:-ate = normal number-ite = 1 fewer oxygens • Nitrate NO3-, Nitrite NO2- • Anion keeps the same charge!

  18. What about other elements? • What is SeO42- ? • “selenate” • How do you know it’s “ate”? • Selenium is just below Sulfur. • Use the periodic trend. • Atoms below the five normal elements follow the ones above them. • Exception: What’s below N?

  19. Special Halogen Oxyanions • Halogens form 2 extra anions: • per-chlor-ate ClO4- per = 1 more • chlor-ate ClO3- “normal” • chlor-ite ClO2- -ite = 1 less • hypo-chlor-ite ClO1- hypo-ite = 2 less(ClO-) • Note: • charge stays the same. • No oxygens (Cl-) = chloride (easy rules)

  20. Naming Acids • Acids are poly anions with enough H+ to balance the charge: AnionNameAcid Name CO32- carbonate H2CO3 carbonic acid ClO3- chlorate HClO3 chloric acid ClO2- chlorite HClO2 chlorous acid ClO- hypochlorite HClO hypochlorous acid PO3- phosphite H3PO3 phosphorous acid

  21. Naming Acids • per-ate per-ic • -ate -ic • -ite -ous • hypo-ite -hypo-ous • None HCl hydrochloric acid

  22. Half-Way Hydrogens • You can put only some hydrogen (H+) on your polyatomic ions: • HSO4- hydrogen sulfate • HCO3- hydrogen carbonate (bicarbonate) • HPO42- monohydrogen phosphate • H2PO4- dihydrogen phosphate • Read your twinkies!

  23. Naming Ionic Compounds cation + Space + anion • Drop the word Ion • Anion will end with either:–ide or–ate/-ite • Note: we don’t use any number information on these.

  24. Examples • Na+ Cl- Sodium chloride, NaCl • Na+ NO3- Sodium nitrate, NaNO3 • K+ SO42- potassium sulfate, K2SO4 • Al3+ NO3- aluminum nitrate, Al(NO3)3

  25. Charge Balance • Ionic compounds have to be Neutral • Charge Balance gets them to the same number. • The math is “least common multiple” • We can also “cross” & simplify.Al3+ NO3-1 Al1(NO3)3 Al(NO3)3

  26. Other Polyatomic Ions • Cations: • NH4+ ammonium ion • H3O+ hydronium ion • Anions: • CH3COO- or C2H3O2- acetate ion • CN- cyanide ion • SCN- thiosyanate ion (thio = sulfur = smelly) • O22- peroxide ion (weird: oxygen = -1, not –2)

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