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Review for final exam:
Chapter 1
Definitions - chemistry, matter, mass, energy, kinetic energy, potential energy
Conservation of mass, conservation of energy
States of matter (solid, liquid, gas) and their general properties; condensed phase, fluid
Crystalline and amorphous solids
Pure substances and mixtures, homogeneous mixtures (solutions), heterogeneous mixtures
Elements and compounds; atoms and molecules
Scientific notation
The metric system, metric prefixes, their size and symbol
SI units; fundamental and derived units
Volume units, m3, cm3, L, mL
Temperature scales (Celsius, Fahrenheit, Kelvin); conversion among these scales
Chemical and physical properties; chemical and physical changes
Precision and accuracy; intensive and extensive properties
Rules for counting significant figures
Significant figures for addition/subtraction and multiplication/division, and combinations of these
Rounding off numbers
Conversion factors and dimensional analysis
Chapter 2
Early theories of matter - continuous or discrete
Conservation of mass, law of definite proportion, law of multiple proportion
Dalton's atomic theory - main ideas, use in explaining observations, shortcomings
Electrons - discovery and properties
The plum pudding model and the nuclear model; Rutherford experiment and explanation
Protons, neutrons, electrons and their general properties
Atomic structure, the nucleus, electron cloud charge
Redefinition of an element
Atomic number, mass number, isotopes, notation for isotopes of atoms
Atomic mass units (amu); definition and use
Mass spectrometry and its use to find atomic and molecular mass
Atomic mass for unstable elements; average atomic mass for stable elements and its calculation
The periodic table
general organization of the table, rows (periods) and columns (groups)
main group, transition metals, lanthanides, actinides
alkali metals, alkali earth metals, halogens, noble gases
metals, nonmetals, metalloids (semimetals); general properties and location
Ions; cations and anions; formation of ions from atoms
Ion charges for main group elements
Ion charges for transition metals (know they can usually form several different ions)
Chemical formula; molecular formula and formula unit; molecular compounds and ionic
compounds
Empirical formula
Finding the ion charge and formula for binary ionic compounds of main group elements
Finding the charge of the metal ions for binary ionic compounds with transition metals
Polyatomic ions; cation groups, anion groups; hydrates
Naming rules for simple substances (see Handout 1)
Organic compounds - definition; hydrocarbons; functional groups (alcohols, amines, carboxylic
acids, aldehydes)
Chapter 3
Molecular mass and formula mass; calculation of molecular and formula mass
Percent by mass; calculation of percent by mass and its use as a conversion factor
Balanced chemical equations; procedure for balancing equations
The mole; definition, Avogadro’s number
Use of the mole concept in calculations; conversion from moles to numbers of atoms or molecules
Determination of empirical formulas from experimental data
Combustion analysis for hydrocarbons and for compounds containing C, H, and O
Finding the molecular formula from the empirical formula and molecular mass
Interpretation of balanced chemical equations; use of chemical equations in calculations
Calculations of mass of products and reactants
Theoretical yield, actual yield, percent yield
Limiting reactant; calculation of theoretical yield
Types of chemical reactions; combination, decomposition, combustion