1st Semester Review
Chemistry I
Chapter 1: The Science of Chemistry
1.1 What Chemistry is About
- Measurements & Units: Mass & weight; Volume; Density; Pressure
- Accuracy & precision
- Significant figures
- Scientific notation
- Dimensional analysis
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
- phases
- energy def
- Law of Conservation of Energy
Chapter 2: Matter and Atoms
2.1 Matter and the Elements
- substance vs. mixture
- element
- physical properties & physical change
- chemical properties & chemical change
- Periodic Table
- mole
- Avogadro's number
- calculations
2.2 Molecules and Compounds
- defs
- chemical formula
- molecular compound
- ionic compound
- formula mass
2.3 Mixtures and Solutions
- homogeneous vs. heterogeneous
- solution
- solute
- solvent
- dissolved
- concentration
- concentrated vs. dilute
- solubility
- molarity
- calculations
- percent by mass
- molarity
- mixtures of gases
- molar volume
- STP
Chapter 5: The Structure of the Atom
5.1 The Atom Has a Structure
- Historical development of atomic theory
- Democritus, Dalton, Thomson, Rutherford
- atom interior
- nucleus
- electron cloud
- properties of subatomic particles
- atomic number, atomic mass
- isotope
- average atomic mass
- ions
5.2 The Quantum Atom
- quantum theory
- quantum state
- 5 statements
- waves & particles
- frequency
- wavelength
- photon
- Planck's constant
- relationship btwn frequency & wavelength, energy & frequency; wavelength & energy
- electrons as waves
- allowed wavelengths
- orbitals
- energy levels
- 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
- emission spectrum
- 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
- alpha radiation = alpha particle
- parent nuclide
- daughter nuclide
- beta decay
- beta radiation = beta particle
- gamma decay
- positron emission
- positron
Chapter 6: Elements and the Periodic Table
6.1 The Periodic Table
- periodic properties
- Mendeleev
- atomic level periodic properties
- atomic radius
- electronegativity
- 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 4: Physical and Chemical Change
4.1 Understanding Chemical Changes
- def
- irreversible
- interatomic forces vs intermolecular forces
- chemical bonds
- covalent bond – molecule
- ionic bonds
- enthalpy of formation
- reactivity
4.2 Chemical Reactions
- chemical reaction
- reactants & products
- balance equation
- coefficient
- endothermic vs. exothermic
- activation energy
4.3 Chemical Reactions in the Lab
- symbols for states of matter
- precipitate
- salt
- oxidation vs. reduction
- acid-base reaction
- pH scale
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:
- binary ionic compounds
- compounds with polyatomic ions
- 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:
- 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:
- 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
- parent compound
- R group
- structural isomer
- alkene
- alkyne
17.2 Functional Groups
- alcohol
- ether
- aldehyde
- ketone
- carboxylic acid
- amine
- ester