1st Semester Review
Chemistry I
Chapter 1: The Science of Chemistry
Chapter 2: Matter and Atoms
1.1 What Chemistry is About
 Measurements & Units: Mass & weight;
Volume; Density; Pressure
 Accuracy & precision
 Significant figures
 Scientific notation
 Dimensional analysis
2.1 Matter and the Elements
 substance vs. mixture
o element
 physical properties & physical change
 chemical properties & chemical change
 Periodic Table
 mole
o Avogadro's number
o calculations
1.2 Scientific Inquiry
 natural laws
 inquiry
 theory
 hypothesis
 experiment
 variable
 experimental variable
 control variables
 error
 average
 conclusion
 significant difference
 objective
 repeatable
 procedure
 scientific method
1.3 Matter and Energy
 matter def
o phases
 energy def
o Law of Conservation of Energy
2.2 Molecules and Compounds
 defs
 chemical formula
 molecular compound
 ionic compound
 formula mass
2.3 Mixtures and Solutions
 homogeneous vs. heterogeneous
 solution
o solute
o solvent
o dissolved
 concentration
o concentrated vs. dilute
o solubility
o molarity
o calculations
 percent by mass
 molarity
 mixtures of gases
o molar volume
o STP
Chapter 5: The Structure of the Atom
5.1 The Atom Has a Structure
 Historical development of atomic theory
o Democritus, Dalton, Thomson,
Rutherford
 atom interior
o nucleus
o electron cloud
o properties of subatomic particles
 atomic number, atomic mass
o isotope
o average atomic mass
 ions
5.2 The Quantum Atom
 quantum theory
o quantum state
o 5 statements
 waves & particles
o frequency
o wavelength
o photon
o Planck's constant
o relationship btwn frequency &
wavelength, energy & frequency;
wavelength & energy
 electrons as waves
o allowed wavelengths
 orbitals
 energy levels
o Pauli exclusion principle
 Periodic Table & energy levels
5.3 Electron Configurations
 def
 writing electron configurations
5.4 Light and Spectroscopy
 spectrum
 spectrometer
 electromagnetic spectrum
 interactions between light and matter
o emission spectrum
o absorption spectrum
Ch 20: Radioactivity
20.1 Nuclear Equations
 atomic number (Z)
 mass number (A)
 neutron number (N)
 chemical reactions vs. nuclear reactions
20.2 Nuclear Reactions
 nuclear reactions-def
 radioactivity-def
 radiation
 alpha decay
o alpha radiation = alpha particle
o parent nuclide
o daughter nuclide
 beta decay
o beta radiation = beta particle
 gamma decay
 positron emission
o positron
Chapter 6: Elements and the Periodic Table
6.1 The Periodic Table
 periodic properties
 Mendeleev
 atomic level periodic properties
o atomic radius
o electronegativity
o ionization energy
 historical development
 orbitals & atomic radius
6.2 Properties of Groups of Elements
 alkali metals
 alkaline earth metals
 transition metals
 C, N & O
 halogens
 noble gases
 why compounds form: filled vs. partially
filled energy levels
6.3 Valence
 valence electrons
 determining valence electrons
 main group elements
 Lewis dot diagram
Chapter 7: Bonding
7.1 What is a Chemical Bond?
- polarization
 Forming Bonds: overlapping orbitals,
attractive force, equilibrium distance,
two bond types
 Bond Models & Diagrams


Predicting Bond Type: electronegativity
difference
- electronegativity
- ionization energy
 Covalent Bonds:
- covalent bond
- nonpolar covalent
- polar covalent
 Ionic & Metallic Bonds: ionic crystals
-ionic bond
-metallic bond
 Polar Molecules: polarity & physical
properties
7.2 Valence Electrons & Bonding Patterns
 Bonding: unpaired valence electrons
form bonds
 The Octet Rule
-octet rule
 Valence electrons & Ion Formation: ion
patterns
 Electron Configuration of Ions – same
as noble gases
 Simple Ionic Formulas – formulas must
be neutral
 Covalent Bonds – number of covalent
bonds possible = number of unpaired
electrons
7.3 Molecular Geometry & Lewis Structures
 drawing Lewis dot diagrams
- isomer
 Double & Triple bonds
 Molecular Geometry
- VSEPR
- region of electron density
Review Problems - #s 21, 22, 26, 29, 30, 31,
33, 34
Chapter 8: Compounds & Molecules
8.1 Ionic Compounds
 Properties
 charges cancel
 Polyatomic ions
 Writing Formulas: total positive charge
must balance total negative charge
 Formulas with Polyatomic ions: use
parentheses
 Names:
o binary ionic compounds
o compounds with polyatomic ions
o compounds with transition metals
8.2 Covalent Compounds
 Properties
- molecule
 Small molecules
 Medium-sized molecules
- lipid
- steroid
- hydrocarbon
 Polymers
- polymer
- monomer
- homopolymer
- copolymer
 Network covalent
 Formulas
- empirical formula
- molecular formula
 Naming:
o binary covalent compounds,
prefixes
8.3 Intermolecular Forces
- intermolecular forces
- van der Waals attractions
 Dipole-dipole attractions
- dipole-dipole attractions
- hydrogen bonding
-surface tension (p. 247 & 264)
 Water - special properties
 London dispersion attraction:
o factors that affect London
dispersion attraction
- London dispersion attraction
8.4 Formula Masses
 calculation of molar mass
 Percent Composition: formula
 Calculating Empirical Formulas
 Calculating Molecular Formulas
Review Problems - #s 22, 24, 26, 27, 28, 30,
37, 38, 39, 42, 45, 46, 47, 48, 51
Ch 17: Organic Chemistry
17.1 Carbon Molecules
 saturated
 unsaturated
 alkane
o parent compound
o R group
 structural isomer
 alkene
 alkyne
17.2 Functional Groups
 alcohol
 ether
 aldehyde
 ketone
 carboxylic acid
 amine
 ester
Ch 11: Stoichiometry
11.1 Analyzing a Chemical Reaction
- stoichiometry
 Interpreting the chemical equation - coefficients
 Determining mole-to-mole relationships
- stoichiometric equivalent
 Using the Mole Ratio
- mole ratio
 Practicing with mole ratios: mole to mole conversions
 Gram to gram conversions
11.2 Percent Yield & Concentration:
- percent yield
- actual yield
- theoretical yield
 Percent yield: formula
 Calculating percent yield: calculate theoretical yield, measure actual yield
 Stoichiometry with solutions: use molarity or percent mass to calculate moles
11.3 Limiting Reactants
- limiting reactant
- excess reactant
 Determining the limiting reactant: never compare reactant masses in grams, always convert to
moles of each reactant
 Using the limiting reactant: limiting reactant determines how much product can form
11.4 Solving Stoichiometric Problems
 Key ideas – p. 353
Review Problems - #s 11, 17, 24, 32, 33