Things to know for the Chem 100, Fall 2000 Final
(C) - Copyright, 2000 F.W. Boyle, Jr., Ph.D.
Useful information:
1 yd = 3 ft 1 ft = 12 in 1 in = 2.54 cm
1 m = 1000 mm 1 gal = 3.785 L 1 m = 1.0936 yd
1 g = 0.0022 lb 1 L = 1.0567 qts 1 qt = 2 pints
1 pint = 2 cups 1 cup = 8 oz 1 fl oz = 31.25 ml
1 mile = 1.6093 km 1 J = 0.23901 cal Q = s*m*T
| The following set of rules is by no means complete but it
provides sufficient information for many ionic
compounds. |
|---|
| General Rules of Solubility of Ionic/Inorganic
Compounds |
|
1. All common compounds of Group I Elements and NH4+ (ammonium ion) are soluble.
|
|
2. All compounds containing nitrates NO3-, acetates C2H3O2-,
and chlorates ClO3- are soluble.
|
|
3. Compounds of Cl-, Br-, and I- with metals are soluble, except those of Ag, Hg(I), and Pb.
|
|
4. All sulfates SO42- are soluble, except those of barium, strontium, calcium, lead, silver, and mercury (I).
|
|
5. Except for compounds listed under Rule 1, all other carbonates
CO32-, hydroxides OH-, oxides
O2-, silicates SiO44-, and
phosphates PO43- are insoluble.
|
|
6. Sulfides S2- are insoluble except for those of calcium, barium, strontium, magnesium, sodium, potassium, and ammonium.
|
Specific Items to study
1) scientific method P.8
2) measurement - quantitative and qualitative
3) SI base units and power values of prefixes P. 19 & 20
4) conversion (equivalence) factors - your card
5) significant figures P. 25 & 26
6) scientific notation (at least how to get you calculator to do it!)
7) know how to use a linear factor to calculate area and volume
factors
8) Temperatures scales for C and K and conversion P. 36 - 44
9) Density = volume/mass P. 44
10) matter and its three states P. 60
11) physical change versus chemical change P. 63
12) Elements, compounds, mixtures, pure substances P. 64 - 66,
Figure 3.10 also
13) Units for energy - calories & joules, converting P. 70
14) specific heat P. 73
15) Major elements P. 89
16) Dalton's Atomic Theory P. 93
17) Rules for writing formulas P. 95
18) The structure of the atom P. 96 including formation of atoms,
ions P. 110-114, and isotopes P. 100-103
19) Makeup of the Periodic Table, metals, nonmetals, metalloids,
groups, natural states Pp. 103 - 110
20) Properties of metals P. 105, nonmetals from knowledge of
metals
21) ionic compounds and molecular compounds, net charge of
compounds, Polyatomic ions P. 142
22) binary compounds P. 127, type I, II, & II compounds Pp. 128-
139, Figure 5.1 P. 139
23) Naming acids P. 145
24) Evidence of chemical reactions P. 160 Table 6.1
25) Balancing reactions. Law of Conservation of Matter Chp. 6,
Rules for P. 169
26) Predicting reactions using solubility rules. Chp. 7,
especially yellow box, P. 187.
27) Types of reactions Chp. 7, note: P206 Figure 7.12
28) Types of equations (VERY IMPORTANT) Yellow box P. 191
29) Strong acids and bases P. 195 yellow box
30) Know what happens:
precipitation reaction
oxidation-reduction reaction
synthesis/combination
decomposition
formation
31) Atomic mass, molar mass, Avogadro's Number, mole
32) molecular formula (actual formula based upon mass of 1 mole),
empirical formula (simplest formula such as CH2O
used for ALL carbohydrates eventhough molecular formulas
differ) P. 239 yellow box P. 242
33) Calculating mole ratios to determine formulas from %
composition or from masses of elements in a compound.
34) mole-mole relationships in BALANCED chemical equations
P. 261 including yellow box
35) Mass-mole and mole-mass conversions Chp. 9 Yellow box P. 268
36) mass to molecule, molecule to mass, mole to molecule,
molecule to mole conversions Chp. 9 and my new papers
37) limiting reactant and calculations involving. Use balanced
reaction to determine "perfect" or "correct" ratios.
Understand that all of one reactant will not react if other
reactant is not used at the correct ratio. P. 272-277 yellow
box P. 277
38) Percent yield, actual yield, theoretical yield Chp. 9