Course title

Pre-requisite

Course description

Course Prefix:
Pre-AP Chemistry
Pre-requisite:
Biology; Algebra I
Course Description:
This course provides a rigorous foundation in chemistry in order to prepare the student for college-level studies. The course covers significant figures; units; scientific investigation; the mole concept; stoichiometry; thermochemistry; thermodynamics; kinetics; acids and bases; solutions; atomic structure and theory; Lewis structures; ionic and covalent bonding; nuclear chemistry; and equilibrium. The strong lab component in this course includes the following laboratory experiments which can be found below in the scope and sequence of the course.
Pre-AP Chemistry - Scope and Sequence

What is matter?

Scientific Investigation
• Candle Observation Lab 1
• Data Collection
• Communicating Data
• Chemical vs Physical Change
• Reactants and Products
• Writing a Chemical Reaction
Melting Behavior
• Lab 2 – Melting Behaviors
• Modeling
Solids; Liquids; and Gasses
• Behavior of solids in heat – demo bimetals
• Thermometer – make our own!
o Precision and Accuracy!
• Eureka Videos (Solids; Liquids and Gasses – episodes 16-20)
Density
• Find density of solid and liquid
Modeling Particle Motion/KMT
• Kinetic Molecular Theory – particles do what?
• Energy of phases – which has more energy?
Melting Point/Boiling Point
• Lab 3 – Melting Point
• Difference between pure and impure substances (mixtures)
• Energy Transfer – Heat (quantity) - Eureka Video (episode 21)
• Calorimetry - Lab 4

How does matter behave?

Gas Laws
• Gasses take up space (volume)
• Density of a gas lab?
• Pressure vs Volume – Lab 5
• Pressure vs Temperature – bulb demo and class data collection
o Absolute Zero – Kelvin Scale
• Volume vs Temperature – capillary tubes and volume changes
Avogadro’s Hypothesis
• Masses of equal volumes of gasses – Lab 6
• Avogadro’s hypothesis powerpoint (equal volumes of gases at standard conditions have same number of molecules)
Moles
• Avogadro’s #
• Dimensional analysis
• Conversion of moles; grams; volume (density)
Conservation of Mass and Matter
• Chemical change and mass relationship – Lab 7
• Einstein’s Big Idea - LaVoisier clip
Balancing Chemical Reactions
• Conserving matter/atoms
• Moles are not conserved
Stoichiometry
• Dimensional analysis and balancing chemical reactions
• Expense of chemicals and real world applications

Why do things react in the first place?

Atomic Theory – Periodic Table
• Atoms - Democritus; Aristotle; Boyle; LaVoisier; Dalton; Mendeleev
• Trends – atomic radius; electronegativity
• Electrons – Stoney; Crookes; and JJ Thomson (Plum Pudding Model)
• Protons – Thomson and Rutherford (Gold Foil Experiment)
Atomic Theory – Waves and Energy
• Electric and Magnetic Fields - Maxwell
• Electromagnetic Radiation - Waves and frequency
• Lab 9 – Spectra Lab
• Lab 10 – Identification of Ions using Line Spectra
• Energy of EM Spectrum – Planck (Planck’s Constant – father of Quantum Theory)
Atomic Theory – Model
• Line Spectra – Neils Bohr
• Atomic “Planetary” Model - Orbitals
• Electron Configuration
• Periodic Table and Electron Configuration

From what we know; can we predict how things will react together?

Bonding - Ionic
• Empirical Formulas
o Magnesium Ribbon Lab 11
• Octet Rule
• Ionic Bonds – writing ionic chemical formulas
• Polyatomic Ions
• Solution Chemistry
o Water as polar molecule
o Ionic Bonds in water
o Molarity
o Precipitates
o Lab 12 Identify Ions in Solution through Precipitates
Bonding – Covalent
• Electronegativity and Octet Rule
• Electron Dot Diagrams – Lewis Structures
• Molecular Structures/Models
• Pipet Rocket Lab – Chemical reaction of H2 and O2 - Lab 13
• Reactions and Bond Energy
Bonding –
• Comparison Lab – Covalent; Ionic; and Metallic - Lab 14
• Metallic – delocalized electrons (conductivity)
• Strength comparison – ions; molecules; and network covalent
Reaction Rates - Kinetics
• Factors that affect reaction rates: Concentration; Heat; Catalysts; Surface Area
• Study of Alka Seltzer in Varying Conditions Lab – Lab 15
• Potential Energy Diagrams
• Kinetic Molecular Theory in Reactions
Equilibrium
• Define equilibrium – reaction rates of forward and reverse reactions are equal
• Le Chatelier’s Principle – Stressing a system at equilibrium
• Le Chatelier’s Lab – Lab 16
• Important Case: Equilibrium of Water
• Acids and Bases
o Identify acid or base by pH
o Calculate pH; pOH; [H+]; [OH-]
o Le Chatelier’s Principle in accordance with acid and bases
o Titration Lab – Lab 17
o Calculate molecular mass of unknown acid/base – Lab 18
Nuclear Chem
• Isotopes vs Ions
• Radioactivity
o Alpha; beta; and gamma decay
• Half-Life
• Ethics and Science – atomic bomb

School Country

School state

School city

School Address

School zip code

Requested competency code

Date submitted

Approved

Approved competency code

• LCHM
• Chemistry

Approved date

Online / Virtual