Chemistry Fall Semester Exam Review
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Chapter 1 Review questions: pg 34; 34, 36 – 38, 40 – 47, 50 – 51, 53 – 62, 70 – 71
- Vocabulary
- Experiment
- Scientific law
- Scientific theory
- Technology
- Hypothesis
- Scientific Method
- 5 branches of chemistry
Chapter 2 review questions: pg 58; 35 – 39, 41 – 46, 48 – 50, 52 – 56, 60 – 63, 76
- Vocabulary
- Extensive Property
- Intensive Property
- Homogeneous
- Heterogeneous
- Reactant
- Product
- Phase
- Chemical Change
- Physical Change
- Precipitate
- Homogeneous mixture
- Heterogeneous mixture
- Physical change
- Chemical change
- Mixture vs. compound vs. element
- Know how to separate mixtures by physical means
Chapter 3 review questions: pg 96; 57 – 61, 63, 66 – 67, 71 – 72, 74, 76 – 77, 79, 80, 82, 84 – 89, 92, 94, 97
- Metric conversions
- Standard notation
- Scientific notation
- Precision vs. accuracy
- Significant figures
Chapter 4 review questions: pg 122, 34, 37, 39 – 41, 43 – 51, 65, 69, 71, 81
- Vocabulary
- Proton
- Atom
- Electron
- Isotopes
- Atomic number
- Atomic mass
- Neutron
- Dalton’s Atomic Theory
- Isotopes
- Average Mass calculation
- Know how to find atomic number, mass number, #protons, #electrons, # neutrons.
- Know the anatomy of an atom and the particle charges
Chapter 5review questions: pg 149; 23, 25 – 27, 29 – 32, 34 – 37, 39, 50, 52, 68
- Vocabulary
- Atomic orbital
- Energy levels
- Quantum
- Quantum mechanical model
- Aufbau principle
- Hund’s rule
- Electron configurations
- Pauli exclusion principle
- Electronic Configuration (long and short)
- Number of orbitals for each sublevel
- Number of electrons per orbital, or sublevel
- Electron configuration rules
- Bohr’s model
- Formula for finding maximum number of electrons per energy level
Chapter 6 review questions: pg 181; 24 – 30, 33, 36 – 39, 42, 43, 45, 47 – 49
- Vocabulary
- Electronegativity
- Groups
- Atomic radius
- Ionization energy
- Periodic law
- Metalloids
- Ions
- Metals
- Anion
- Cation
- Periodic table group names / numbers
- Periodic group similarities
- Anion/cation
- Ionization energy
- Electronegativity
- Atomic Size
- Mendeleev’s periodic table organization vs. modern periodic table
Chapter 7review questions: pg 207; 31 – 36, 40 – 45, 48, 51, 55, 56, 60, 64, 67, 73, 80
- Vocabulary
- Alloy
- Chemical formula
- Electron dot structure
- Ionic bond
- Ionic compound
- Metallic bond
- Octet rule
- Valence electron
- How to determine valence electrons
- Ionic compound properties
- Ionic bonding metal (cation) bonding with non metal (anion)
- How to write the ionic chemical formula for a given compound
- How to name an ionic compound
- How to determine the ionic compound when given the cation and anion
- Draw Electron Dot Structures
- Metals give away electrons, have positive charges, aka cations
- Non metals accept electrons, have negative charges, aka anions
- Know that ionic compounds are electrically neutral, but can conduct electricity when in solution or melted.
Chapter 8 Review questions: pg 247; 39 – 46, 50, 57 – 59, 61, 64
- Vocabulary
- Coordinate covalent bond
- Covalent bond
- Diatomic molecule
- Dipole
- Molecular compound
- Molecular formula
- Molecule
- Resonance structure
- Structural formula
- Distinguish the differences between ionic and molecular (covalent) compounds
- Know how many electrons form the following bonds
- Single = 2 electrons
- Double = 4 electrons
- Triple = 6 electrons
- Recognize diatomic molecules, (magnificent 7, CO, NO, etc.)
- Be able to name and write molecular formulas for given compounds
- Carbon monoxide = CO
- Be able to draw Bohr’s model and Electron Dot Structures for molecular compounds