chapter 7 – chemical formulas and chemical compounds
TRANSCRIPT
Chapter 7 – Chemical Formulas and Chemical Compounds
7-1 Chemical Names and Formulas What’s so important about a chemical
formula?It indicates the relative # of atoms of
each kind in a chemical compoundMolecular Compound: chemical
formula reveals the # of atoms in a single molecule. C8H18
Ionic Compound: consists of a lattice of positive and negative ions held together by mutual attraction. Simplest ratio NaCl
Al2(SO4)3- How many atoms are there?
AlSO
2312
Monoatomic Ions
Ions formed from a single atom Ex. Na Na1+ , O O2-
Not all main-group elements form ions, C and Si form covalent bonds instead of ionic bonds
Sn and Pb are exceptions lose only 2 e-s instead of 4 or sometimes they keep all 4 electrons.
Naming Monoatomic Ions
Cations are identified by the elements name
Anions the ending of the element’s name is dropped. The ending –ide is added.Ex. Fluorine (F) = Fluoride ion (F-)Nitrogen (N) = Nitride (N3-)Flash Cards may be useful to
memorize these!!!!
Binary Ionic Compounds
Compounds composed of two different elements.
Ex. Magnesium and Bromine form Magnesium Bromide, MgBr2
Rules for Ionic Compounds
1. Write the symbols for the ions side by side. The cations go first. Al 3+ O 2-
2. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. Al2O3
3. Check subscript and divide them by their largest common factor to give the smallest possible whole-number ration.
4. Write the formula
Write the formula for the following:
Magnesium and iodine Potassium and sulfur Aluminum and chlorine Zinc and bromine Cesium and sulfur Strontium and oxygen Calcium and nitrogen
MgI2
K2S
AlCl3 ZnBr2
Cs2S SrO Ca3N2
Name the following:
BaF2
CaO AgF CdO K3N NaI AlBr3
Barium Fluoride Calcium Oxide Silver Fluoride Cadmium Oxide Potassium Nitride Sodium Iodide Aluminum Bromide
The Stock System of Nomenclature
Some elements form two or more ions such as Fe, with different charges.
This system uses Roman numerals to indicate an ions’ charge
Fe 2+ or Fe 3+ FeCl2 = iron (II) chloride
FeCl3 = iron (III) chloride
Write the formula and give the name for the following: Cu + and O 2-
Fe 3+ and S 2- Cu 2+ and Cl -
Sn 2+ and Cl -
Hg 2+ and O 2- Sn4+ and S 2- V 2+ and F -
V 4+ and Br -
Name the following:
CoI2
HgI2
PbS2
CuBr2
Compounds Containing Polyatomic ions
Oxyanions- polyatomic ions containing oxygen
Nitrate vs. Nitrite – (-ite less oxygen)NO3
- and NO2-
Sulfates, Nitrate, Chlorates
Write the formulas for:
Copper(II) nitrate Potassium iodide Sodium hydroxide Ammonium acetate Calcium carbonate Potassium permanganate Sodium sulfate Iron(III) nitrate
Name the following:
Ag2S NaMnO4
Ba(OH)2
NH4NO3
Fe(ClO)2
Ca(NO3)2
K2SO3
NaCH3COO
Naming Binary Molecular Compounds # 1 2 3 4 5 6 7 8 9 10
# Mono Di Tri Tetra Penta Hexa Hepta Octa Nona deca
Rules for Molecular Compounds 1. The least electronegative element
is first. It is given a prefix if it is more than one
2. the second element is named by combining a prefix, the root of the word, and –ide ending
3. the o or a at the end of the prfix is usually dropped when the word following begins with another vowel.
Examples.
As2O5 = diarsenic pentoxide PF5 = phosphorus pentafluoride XeF4 = Xenon tetrafluoride CCl4 = carbon tetrachloride Carbon dioxide = CO2
Dinitrogen pentoxide = N2O5
Sulfur hexafluoride = SF6
Dinitrogen monoxide = N2O
Acids and Salts
Acids can be binary acids or oxyacids Binary acids are acids that consist of
H and a halogen, HCl hydrochloric acid
Oxyacids, contain H, P and a third element, Sulfuric Acid, H2S
Pg 214