Chemistry 20

Unit 1: Diversity of Matter & Chemical Bonding

Why atoms join at all — from the transfer of electrons that makes ionic compounds to the sharing that makes molecules — and how the bonding inside and between particles explains the properties we can see, feel and measure.

• Naming ionic compounds
• Ionic formulas as lowest whole-number ratios
• Valence electrons, electronegativity and ionic bonds

• Periodic table and electron dot diagrams for ionic bonding
• Ionic bonds from attraction of opposite charges
• Ionic lattices and properties

• Naming molecular substances
• Molecular formulas count atoms
• Electron pairing and covalent bonds
• Electron dot diagrams and Lewis structures

• VSEPR theory and molecular shapes
• Illustrating molecular structure
• Polarity from shape and charge distribution

• London, dipole-dipole and hydrogen bonding
• Intermolecular forces and physical properties
• Bonding as a continuum

Unit 2: Forms of Matter: Gases

The state of matter that fills its container, presses on its walls and answers to a single tidy equation — how the motion of unseen particles produces the pressure, volume and temperature we can measure, and the gas laws that connect them.

• Real and ideal gases
• Celsius and Kelvin temperature scales
• Law of combining volumes
• Boyle's, Charles's and the ideal gas law

Unit 3: Matter as Solutions, Acids & Bases

Most chemistry happens in water. This unit builds from what a solution is and how concentrated it is, through solubility and equilibrium, to the special solutions we call acids and bases — how strong they are, and how we measure them with pH.

• Pure substances, mixtures and homogeneous mixtures
• Dissolving as a prerequisite for reactions
• Dissolving as endothermic or exothermic
• Electrolytes and nonelectrolytes

• Ways of expressing concentration
• Calculating molar concentration
• Dilution calculations
• Concentration of ions in solution

• Solubility and its factors
• Saturation as a dynamic equilibrium
• Preparing and diluting solutions

• IUPAC naming of acids and bases
• Empirical definitions of acidic, basic and neutral
• Arrhenius acids
• Arrhenius bases
• Neutralization

• Calculating pH and pOH
• SI units and significant digits in pH
• How pH and pOH change with concentration
• Indicators, pH paper and pH meters

• Strong vs weak acids and bases
• Monoprotic and polyprotic acids and bases

Unit 4: Quantitative Relationships in Chemical Changes

Chemistry with numbers attached — predicting products, balancing equations, and using the mole to calculate exactly how much reacts and how much is made, then testing those predictions against real yields and titration data.

• Predicting reaction products by type
• Balancing chemical equations
• Quantitative vs qualitative analysis
• Ionic and net ionic equations

• Gravimetric, solution and gas stoichiometry
• Conservation of mass in quantitative analysis
• Limiting and excess reagents

• Theoretical and actual yields
• Why actual yield differs from theoretical

• Drawing and interpreting titration curves
• Function and choice of indicators
• Equivalence point vs indicator end point