1 / 39

NOMENCLATURE

NOMENCLATURE. COVALENT COMPOUNDS IONIC COMPOUNDS (SALTS) HYDRATES ACIDS + OXY ACIDS BASES PEROXIDES. COVALENT COMPOUNDS Formulas. IUPAC name: International Union of Pure and Applied Chemistry Name using Prefixes b/c elements can combine in DIFFERENT ratios

jorn
Download Presentation

NOMENCLATURE

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. NOMENCLATURE COVALENT COMPOUNDS IONIC COMPOUNDS (SALTS) HYDRATES ACIDS + OXY ACIDS BASES PEROXIDES

  2. COVALENT COMPOUNDS Formulas • IUPAC name: International Union of Pure and Applied Chemistry • Name using Prefixes b/c elements can combine in DIFFERENT ratios • 1- Mono 6- Hexa • 2- Di 7- Hepta • 3- Tri 8- Octa • 4- Tetra 9- Nona • 5- Penta 10- Deca

  3. COVALENT COMPOUNDS Naming • NAME tells you formula (pre-fixes) • Prefix depends on number of individual atoms • ENDING: "ide“ • “mono” in first atom is not neccesary

  4. no MONO for C COVALENT COMPOUNDS • N2O • Dinitrogen monoxide • N2O5 • Dinitrogen pentoxide • CO • Carbon monoxide • CO2 • Carbon dioxide • C2O2 • Dicarbon dioxide

  5. IONIC COMPOUNDS or SALTS: Naming • IUPAC name • Metal, then non-metal • 1 Metal + 1 Non-metal OR BINARY compound • ENDING: "ide“ • NO PREFIXES!

  6. IONIC COMPOUNDS or Salts: Formula • CRISSCROSS tells you formula • Ex 1: K and O Ex 2: Ca and O K1+ O2- Ca2+ O2- K2O CaO • CaO is reduced to its lowestform • Formula must be in LOWEST ratio

  7. POLYATOMIC IONS(IONIC: 1 metal + more than 1 NM) • Metal + group of non-metals • Non-metal group has overall charge • Ex: (CO3)2-is Carbonate • The CO3group likes to gain 2 electrons so, overall charge of -2 • Page 66 Table 2.4: Polyatomic Ions

  8. POLYATOMIC IONS • (NO31-) Nitrate • (ClO31- ) Chlorate • (HCO31-)Bicarbonate • (OH1-) Hydroxide • (CO32-) Carbonate • (SO42- )Sulphate /Sulfate • (PO43- )Phosphate • (NH41+) Ammonium

  9. POLYATOMIC IONS • Try: Sodium Chlorate • Na1+ ClO31- Na(ClO3) • Try: Calcium Carbonate • Ca2+ CO32- Ca(CO3)

  10. MULTIVALENT ELEMENTS • Elements with varying numbers of valence electrons can form more than one type of ion • Ex: Cu can form a Cu2+ or Cu1+ VS Cl: always forms a Cl1- • Use ROMAN NUMERALS to identify differences (I, II, III, IV)

  11. MULTIVALENT ELEMENTS

  12. MULTIVALENT ELEMENTS • Copper (I) Chloride • CuCl • Copper (II) Chloride • CuCl2 • Lead (II) Nitride • Pb3N2 • Gold (III) Nitride • AuN has been Reduced to lowest terms • Gold (I) Nitride • Au3N

  13. ALTERNATE NAMING FOR MULTIVALENT ELEMENTS • Alternate LATIN naming system for multivalent elements • “ous” ending used with LOWER Valence • “ic” ending used with HIGHER Valence • Table 3.6 page 103 • CuCl2 is Copper(II)chloride or Cupric chloride

  14. ALTERNATE NAMING FOR MULTIVALENT ELEMENTS • CuCl2  Copper(II)chloride • Cupric Chloride • CuCl  Copper (I) chloride • Cuprous chloride

  15. ALTERNATE NAMING FOR MULTIVALENT ELEMENTS

  16. TEXTBOOK QUESTIONS: • Pg 70 • 7-9 (skip e,f), 10, 12 • Pg 73 • 1-10 • Pg 75 • 1-5 (skip g,h), 6 (skip c), 7-10 (skip g,h)

  17. HYDRATES • Are examples of Ionic Compounds • Crystallize from a water solution such that water molecules stick to the crystals • Called “Hydrates” • Exist in specific ratio of compound : water

  18. HYDRATES • A dot expresses how many water molecules are attached to the compound • Na2SO4 • 6H2O • 6 molecules of water attach to 1 unit of Sodium Sulphate

  19. NAMING HYDRATES • Name the compound before the dot • Name the water using prefix (# of water molecules) followed by the word “hydrate” • Na2SO4 • 6H2O • Sodium sulphatehexahydrate

  20. HYDRATES • Cu(SO4)• 5H2O • Copper (II) sulphate pentahydrate • Cu2(SO4)• 5H2O • Copper (I) sulphate pentahydrate • Barium chloride dihydrate • BaCl2• 2H2O

  21. Last words on Hydrates • The water can be removed from some hydrates • Called ANHYDROUS compounds • Anhydrous Barium Chloride • BaCl2 • Barium chloride dihydrate • BaCl2• 2H2O

  22. BASES • Generally end in OH • OH1- = Hydroxide • Metal Hydroxides = Bases • Ex: NaOH = Sodium Hydroxide • Ex: KOH = Potassium Hydroxide

  23. PEROXIDES • Contains O-O single bond (O2) • O2 has a 2- charge • H2O2is Hydrogen peroxide • MgO2 is Magnesium peroxide • CaO2 is Calcium peroxide • NOTE: Mg + O usually makes MgO • Ca + O usually makes CaO

  24. Hydrogen + Single ion ACIDS • Compounds that give away Hydrogen in water • Two types of Acids One or more hydrogen + Polyatomic ion

  25. ACIDS (Hydrogen and Single Ion) • Acids are dissolved in water so (aq) is written to denote aqueous • HF (aq): Hydrofluoric Acid HF : Hydrogen fluoride • HCl(aq):Hydrochloric Acid HCl : Hydrogen chloride • HBr(aq):Hydrobromic Acid HBr :Hydrogen bromide • HI(aq): Hydroiodic Acid HI : Hydrogen iodide

  26. ACIDS (One or more H + Polyatomic Ion) • Called Oxy-Acids • Polyatomic Ion has Oxygen

  27. These acids have morethan1H STANDARD OXY- ACIDS • HClO3(aq) Chloric Acid • HFO3(aq) Fluoric Acid • HBrO3(aq) Bromic Acid • HIO3(aq) Iodic Acid • HNO3(aq) Nitric Acid • H2CO3(aq) Carbonic Acid • H2SO4(aq) Sulphuric Acid • H3PO4(aq) Phosphoric Acid

  28. FORMS OF OXY- ACIDS • Recall: All oxy acids have Oxygen • Can change the number of Oxygen • This changes the NAME of the Oxy-acid • Prefix or suffix or BOTH added to acid name

  29. FORMS OF OXY-ACIDS • Regular formula: “ic” ending • 1 more Oxygen: “per” prefix; “ic” suffix • 1 less Oxygen: “ous” suffix • 2 less Oxygens: “hypo” prefix; “ous” suffix

  30. EX: CHLORIC ACID • HClO4(aq) :Perchloric Acid (1 more O) • HClO3(aq) :Chloric Acid (REGULAR) • HClO2(aq) : Chlorous Acid (1 less O) • HClO(aq) : HypoChlorous Acid (2 less O)

  31. Name the following Oxy-Acids • HClO4(aq) • HFO2(aq) • HBrO2(aq) • HBrO(aq) • HNO3(aq) • H2CO2(aq) • H2SO5(aq) • H3PO5(aq)

  32. Name the following Oxy-Acids • HClO4(aq) Perchloric Acid • HFO2(aq) Fluorous Acid • HBrO2(aq) Bromous Acid • HBrO(aq) Hypobromous Acid • HNO3(aq) Nitric Acid • H2CO2(aq) Carbonous Acid • H2SO5(aq) Persulphuric Acid • H3PO5(aq) Perphosphoric Acid

  33. OXY- ACID SALTS • Formed by bumping out Hydrogen from Oxy-acids • Formed when oxy-acids react with a metal • Na + H3PO4(aq) H2 + Na3PO4 • Sodium + Phosphoric Acid Hydrogen + Sodium Phosphate • RULE: “ic” acid “ate” salt

  34. OXY- ACID SALTS • Na + H2SO3(aq) H2 + Na2SO3 • Sodium + Sulphurous Acid Hydrogen + Sodium Sulphite • RULE: “ous” acid “ite” salt • Na + H2SO2(aq) H2 + Na2SO2 • Sodium + Hyposulphurous Acid Hydrogen + Sodium Hyposulphite • RULE: “hypo” “ous” acid “hypo” “ite” salt

  35. SUMMARY: OXY-ACIDS

  36. PRACTICE: OXY-ACIDS • HBrO4(aq) • Perbromic Acid • HFO(aq) • Hypofluorous Acid • HIO2(aq) • Iodous Acid • HClO(aq) • Hypochlorous Acid

  37. PRACTICE: OXY-ACID SALTS • Mg(NO4)2(aq) • Magnesium pernitrate • Na2(CO2)(aq) • Sodium carbonite • K2(SO5)(aq) • Potassium persulphate • Ba3(PO2)3(aq) • Barium hypophosphite

  38. Homework • REVIEWALL Nomenclature rules • Friday/ Monday: Review • BIG QUEST: TUESDAY

More Related