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Chemical Bonding

Chemical Bonding. Chapter 7 Section 1 Pages 219-231. Chemical Formulas. Chemical formulas indicate the elements involved and how many of each type are in the molecule. C 8 H 18 Al 2 (SO 4 ) 3 subscripts. Types of Ions. Monatomic Ions – one element. Criss-Cross Method.

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Chemical Bonding

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  1. Chemical Bonding Chapter 7 Section 1 Pages 219-231

  2. Chemical Formulas • Chemical formulas indicate the elements involved and how many of each type are in the molecule. C8H18 Al2(SO4)3 subscripts

  3. Types of Ions • Monatomic Ions – one element

  4. Criss-Cross Method Used to write formulas of ionic compounds (salts) Step 1: List Charges of each ion Step 2: Criss-Cross the # of the Charge only! Step 3: Simplify (Never write a subscript of 1)

  5. Criss-Cross means: • # of the Charge of cation subscript of the anion. • # of the Charge of anion subscript of the cation.

  6. Types of Ions • Polyatomic – more than one element

  7. Example: Calcium Phosphate Use parentheses for a polyatomic ion. PO4 = 3- Ca = 2+ (PO4) Ca 3 2

  8. Empirical Formula Lowest Whole Number Ratio of Elements CaSO4 = 1 calcium ion for every 1 sulfate ion Na2SO4 = 2 sodium ions for every 1 sulfate ion

  9. *Stock System of Naming Compounds Roman numeral matching the charge is used. Ex: Cu +1, copper I Cu +2, copper II Cu+2 N03-: Cu(N03)2 copper II nitrate Cu+ NO3- : CuNO3 copper I nitrate

  10. Naming Binary Ionic Compounds • Cation: Name the Metal (use Roman numerals for transition metals) • Anion: nonmetal Change the ending to –ide. Calcium Chloride Barium Oxide Potassium Sulfide Iron (III) Bromide Chromium (III) Oxide

  11. Traditional Naming of Ionic Compounds Traditional naming of ionic compounds used the Latin names or some common names and a suffix corresponding to the charge as follows. Copper: Cuprum Cu+1: cuprous Cu+2: cupric The ous ending was used with the lower charged ion. The ic ending was used with the higher charged ion.

  12. Tradition Names Ferrous Nitrate : Iron +2, nitrate: Fe(NO3)2 Plumbic Chloride: Lead +4, chlorine: PbCl4 Latin Names: Ferrum – Iron, Cuprum – Copper, Stannum – Tin, Mercurum – Mercury Common Names: Any element with more than one possible charge: lead, mercury, tin, etc.

  13. *Examples of Naming for Polyatomic Ions Calcium Sulfite Barium Phosphate Ammonium Sulfide Iron (III) Sulfite

  14. Naming Molecular Compounds Same rules EXCEPTinclude prefixes NEVER start a compound name with mono- (drop the prefix)

  15. Naming Molecular Compounds = nitrogen dioxide NO2 = boron trifluoride BF3 = diphosphorus pentoxide P2O5

  16. *Molecular Formula Indicates how many atoms are in a single molecule of the compound. C6H12O6 = glucose 6 carbon atoms 12 hydrogen atoms 6 oxygen atoms

  17. Naming of Acids & Salts • Binary Acids: Contain only two elements. • Hydrogen & a nonmetal • Hydro- ____________ -ic acid. Ex: HCl = Hydrochloric Acid H2S = Hydrosulfuric Acid

  18. Naming of Acids & Salts • Binary Salts: Contain only two elements. • A metal & a nonmetal • Name the metal & change the ending on the non-metal to –ide. Ex: NaCl = Sodium Chloride MgBr2 = Magnesium Bromide

  19. Naming of Acids & Salts • Ternary Acids: Prefix & Suffix • X could be any element other than (Sulfur, Phosphorus, Nitrogen or Carbon) • HXO = hypo-________-ous • HXO2 = __________-ous • HXO3 = __________-ic • HXO4 = per-_________-ic

  20. Naming of Acids & Salts • Example: • HClO = hypochlorous acid • HClO2 = chlorous acid • HClO3 = chloric acid • HClO4 = perchloric

  21. Naming of Acids & Salts • Ternary Salts: Prefix & Suffix • X could be any element other than (Sulfur, Phosphorus, Nitrogen or Carbon) • XO- = hypo-________-ite • XO2 - = __________-ite • XO3 - = __________-ate • XO4 - = per-_________-ate

  22. Naming of Acids & Salts • Example; Chlorine (X represents any metal) • XClO- = hypochlorite • XClO2 - = chlorite • XClO3 - = chlorate • XClO4 - = perchlorate

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