Chemistry Advance

Chemistry Advance

This course will dive into the foundations of chemistry and apply science to aspects of everyday life. A way to prepare for the final exam with an introduction to key concepts.


Chemistry Advance Outline

I. Atomic and Molecular Structure/ Periodic Table

1. Identify molecular weight, group names (alkaline metals, halogens, noble gases, etc.) and their properties
2. Recognize trends of periodic table: ionization energy, atomic radii, electronegativity
3. Be able to find number of valence electrons
i. electron configuration
ii. orbital notation
4. Atomic structure (protons, electron, neutrons)

II. Chemical Bonds

1. Covalent bonding, ionic bonding, and metallic bonding
i. review important covalent bonds/salts
2. Nomenclature
3. Lewis dot structures
i. determining shape/geometry and polarity

III. Stoichiometry

1. Conversion calculations (mass -> mole -> atom)/ Dimensional Analysis
2. Relationship between molar mass, moles, particles
i. Avogadros number
ii. defining mole
3. Mole to mole ratio
4. Writing balanced equations
5. Empirical/ molecular Formula

IV. Gases 

1. Boyle’s Law
2. Charles’s Law
3. Gay-Lussac’s Law
4. Ideal Gas Law PV=nRT
5. STP
6. Converting temperature from fahrenheit, celsius, and kelvin

V. Equilibrium/ Reaction Rates  

1. Writing and solving equilibrium laws and equilibrium constant problems
2. Predicting direction of equilibrium ( Q=K, Q>K, Q<K)
3. Equilibrium calculations (ICE Table)
4. Le Chatelier’s Principle
5. Factors that affect reaction rates
6. Writing rate laws and solving
7. Order of reactions (Zero, First, Second Order)

VI. Acids and Bases 

1. Arrhenius Acids: add H+ ions to solution/ Bases: Add OH- to solution
2. Bronsted Lowry Acids: proton donor/ Bases: proton acceptor
3. Lewis Acid: electron pair acceptor/ Bases: electron pair donor
4. Naming acids and bases
5. Properties of Strong Acids/ Strong bases/ Weak Acids/Weak bases
6. pH scale; calculating pH from [H+]
7. Kw= [H+][OH-]

VII. Thermodynamics 

1. Exo/endothermic reactions
2. When something (melts -> heat is absorbed) (freezes -> heat is absorbed)
3. Specific heat, phase changes
4. Hess’s Law and Enthalpy change and heats of formation

VIII. Solutions

1. Solute vs. solvent
2. Likes dissolve likes
3. Strong, weak, non electrolytes
4. Calculating molarity, molality, mole fraction, parts per million, % composition
5. Freezing point/ boiling point depression