Unit I Study Guide: Matter and Reactions
Chapters 1-4
To Memorize:
1. Definitions of the following terms:
a. Matter
ll. Diatomic molecule
b. Property
mm.
Molecular compounds
c. Elements
nn. Molecular formulas
d. Atoms
oo. Empirical formulas
e. Molecules
pp. Ion
f. Gas
qq. Cation
g. Liquid
rr. Anion
h. Solid
ss. Reactants
i. Pure substance
tt. Products
j. Elements
uu. Stoichiometry
k. Compounds
vv. Molar mass
l. Mixtures
ww.
Formula weight
m. Law of constant composition
xx. Molecular weight
n. Solutions
yy. Limiting reactant
o. Physical properties
zz. Excess reactant
p. Chemical properties
aaa. Theoretical yield
q. Intensive properties
bbb.
Percent yield
r. Extensive properties
ccc. Solubility
s. Physical change
ddd.
Molecular equation
t. Chemical change
eee. Complete ionic equation
u. Filtration
fff. Net ionic equation
v. Distillation
ggg.
Spectator ion
w. SI units
hhh.
Acids
x. Mass
iii. Bases
y. Conversion factor
jjj. Strong bases
z. Subatomic particles
kkk.
Weak Bases
aa. Atomic mass unit
lll. Neutralization reaction
bb. Angstrom
mmm.
Oxidation
cc. Mass number
nnn.
Reduction
dd. Atomic number
ooo.
Redox reactions
ee. Isotopes
ppp.
Oxidation numbers
ff. Periods
qqq.
Activity series
gg. Groups
rrr. Molarity
hh. Metals
sss. Dilution
ii. Nonmetals
ttt. Titration
jj. Metalloids
uuu.
Equivalence point
kk. Chemical formula
vvv.
Standard solution
2. Characteristics of the three states of matter (page 7)
3. Metric prefixes: Kilo, milli, micro, nano, and pico (table 1.5 on page 16)
4. Celsius to Kelvin formula (1.1 on page 17)
5. Density formula (1.3 on page 19)
6. Rules for identifying a significant figure
7. Rules for rounding to the appropriate place or number of significant figures following calculations
involving measurements
8. Subatomic particles (table 2.1 on page 45)
9. Groups on periodic table (table 2.3 on page 51)
10. Patterns for charge on periodic table (figure 2.20 on page 56)
11. Polyatomic ions
12. Nomenclature handout
13. The structure of a chemical equation
14.
15.
16.
17.
The major types of chemical reactions
The difference between ionic and molecular compounds when they dissolve
The concept of chemical equilibrium
Major concepts and calculations from all labs done during the unit
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Distinguish between the three states of matter.
Classify an example of matter as a pure substance or a mixture.
Classify a pure substance as an element or compound.
Classify mixtures as heterogeneous or homogeneous.
Classify a property as a chemical or physical property.
Classify a property as intensive or extensive property.
Classify a change as physical or chemical.
Convert between Celsius and Kelvin.
Calculate density or use density to determine mass or volume of a sample.
Determine the number of significant figures in a number.
Record measurements with the appropriate significant figures.
Round answers to calculations to the appropriate place or number of significant figures.
Convert from one unit to another using dimensional analysis.
Determine the chemical symbol, number of protons, electrons or neutrons, atomic number, mass number
and charge when given partial information.
Calculate the weighted average atomic mass of a given element.
Identify information about an element based on its location on periodic table, including its group, period,
metallic character, and charge.
Distinguish between an empirical formula and a molecular formula.
Predict the ionic character of a given compound.
Name cations and anions.
Name acids, ionic and binary molecular compounds.
Determine the chemical formula of acids, ionic, and binary molecular compounds.
Balance chemical equations.
Classify reactions into their general categories.
Write combustion reactions, combination reactions between metal oxides and water and decomposition
reactions of metal hydroxides or metal hydroxides.
Calculate the formula/molecular weight or molar mass of an element or compound.
Calculate percentage composition from formulas and vice versa.
Use Avogadro’s number to convert from mole to number of atoms/things and vice versa.
Convert between moles and mass.
Calculate empirical formulas using combustion analysis.
Calculate molecular formulas from molar masses and empirical formulas.
Use balanced chemical equations to convert from moles of a substance to moles or another substance (in
solutions as well).
Determine the limiting and excess reactant.
Calculate theoretical yield and percent yield.
Write both complete and net ionic equations.
Apply solubility rules to predict precipitates.
Write neutralization reactions.
Assign oxidation numbers.
Use the activity series to predict if one metal is able to reduce another.
Calculate the molarity of a solution and use it to convert to volume, moles, and mass.
Solve dilution problems.
Determine unknown concentrations using titrations and related calculations.