IIIIIIIV Chemical Bonding Chapter 7 Section 1 Pages 219-231.
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I II III IV
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.
C8H18 Al2(SO4)3
subscripts
Types of Ions
Monatomic Ions – one element
Criss-Cross Method
Used to write formulas of ionic compounds (salts)
Step 1: List Charges of each ionStep 2: Criss-Cross the # of the Charge only!
Step 3: Simplify (Never write a subscript of 1)
Criss-Cross means: • # of the Charge of cation subscript of the anion.• # of the Charge of anion subscript of the cation.
Types of Ions
Polyatomic – more than one element
Example: Calcium Phosphate
Ca = PO4 = 2+ 3-
Use parentheses for a polyatomic ion.
Ca (PO4)
23
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
*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
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
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.
Tradition Names
Ferrous Nitrate : Iron +2, nitrate: Fe(NO3)2
Plumbic Chloride: Lead +4, chlorine: PbCl4Latin Names:
Ferrum – Iron, Cuprum – Copper,
Stannum – Tin, Mercurum – Mercury
Common Names: Any element with more than one possible charge: lead, mercury, tin, etc.
*Examples of Naming for Polyatomic Ions
Calcium Sulfite
Barium Phosphate
Ammonium Sulfide
Iron (III) Sulfite
Naming Molecular Compounds
Same rules
EXCEPT
include prefixes
NEVER start a
compound name
with mono-
(drop the prefix)
1 = mono 2 = di
3 = tri 4 = tetra
5 = penta 6 = hexa
7 = hepta 8 = octa
9 = nona 10 = deca
Naming Molecular Compounds
NO2= nitrogen dioxide
BF3= boron trifluoride
P2O5= diphosphorus pentoxide
*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
Naming of Acids & Salts
Binary Acids: Contain only two elements. Hydrogen & a nonmetal Hydro- ____________ -ic acid.
Ex: HCl = Hydrochloric Acid
H2S = Hydrosulfuric Acid
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
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
Naming of Acids & Salts
Example:
HClO = hypochlorous acid HClO2 = chlorous acid
HClO3 = chloric acid
HClO4 = perchloric
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
Naming of Acids & Salts
Example; Chlorine (X represents any
metal) XClO- = hypochlorite XClO2
- = chlorite
XClO3 - = chlorate
XClO4 - = perchlorate
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