chemistry

Chapter 1: States of Matter

1.1 The 3 States of Matter

  • Matter: Physical substance that has mass and occupies space; composed of particles (atoms, molecules, ions).

  • 3 States of Matter:

    • Solid:

      • Shape: Fixed

      • Volume: Fixed

      • Particle Arrangement: Regular

      • Separation: Tightly packed

      • Forces of Attraction: Strong

      • Motion: Vibrates in fixed positions

      • Compressibility: Not compressible

    • Liquid:

      • Shape: Not fixed (takes shape of container)

      • Volume: Fixed

      • Particle Arrangement: Random

      • Separation: Loosely packed

      • Forces of Attraction: Less than solids

      • Motion: Slide over each other

      • Compressibility: Not compressible

    • Gas:

      • Shape: Not fixed (takes shape of container)

      • Volume: Not fixed

      • Particle Arrangement: Random

      • Separation: Far apart

      • Forces of Attraction: Very little

      • Motion: Randomly moving

      • Compressibility: Compressible

1.2 Kinetic Theory

  • Particles constantly move.

  • Higher temperatures increase particle speed.

  • Larger particles move slower.

  • State Changes:

    • Melting: solid to liquid (endothermic)

    • Boiling: liquid to gas (endothermic)

    • Condensation: gas to liquid (exothermic)

    • Freezing: liquid to solid (exothermic)

  • Expansion/Contraction:

    • Solids expand/slightly contract with temperature changes.

    • Gases expand greatly with temperature.

1.3 Pressure Changes

  • Pressure Increase:

    • Decrease volume, increase temperature, add gas.

    • Decreasing volume increases collision frequency, thus increasing pressure.

    • Increasing temperature gives particles more kinetic energy, leading to more frequent collisions.

1.4 Changes of State

  • Heating Curve: Temperature constant during phase changes (melting/boiling).

  • Melting Point: Temperature where solid converts to liquid.

  • Boiling Point: Temperature where liquid converts to gas.

  • Keywords:

    • Melting: Gain energy, overcome forces, become liquid.

    • Boiling: Gain enough energy to escape as gas.

    • Condensation: Lose energy, regain attractive forces, become liquid.

    • Freezing: Lose energy, regain attractive forces, become solid.

Chapter 2: Experimental Techniques

2.1 Apparatus and Uses

  • Balances: Measure mass (top pan balance).

  • Thermometer: Measure temperature (°C).

  • Beakers: Measure/easy use.

  • Pipettes and Burettes: Accurate volume measurement.

2.2 Collecting Gases

  • Gas syringe: For measuring gas volumes (heavy/lighter gases).

  • The process: Using different methods for gases such as downward/upward delivery.

2.3 Safety Hazards and Precautions

  • Safety Signs: Indicate hazards (flammable, corrosive, etc.).

  • Wearing PPE: Lab coats, gloves, and goggles for protection.

2.4 Separating Techniques

  • Filtration: Obtain solids from liquids.

  • Evaporation: Obtain soluble solids from a solution.

  • Crystallization: Formation of solid crystals.

  • Distillation: Obtain pure solvents from solutions.

  • Chromatography: Separate mixtures of colors.

Chapter 3: Atoms, Elements, & Compounds

3.1 Atomic Structure

  • Atoms: Smallest unit of matter; composed of protons, neutrons, and electrons.

  • Electrons: Orbit nucleus in shells. 1st shell (2E), 2nd shell (8E), 3rd shell (18E).

  • Mass: Protons + Neutrons = Atomic Mass (Ar).

3.2 Elements and Compounds

  • Elements: Pure substances of one type of atom (e.g., O).

  • Compounds: Made of two or more types of atoms (e.g., H2O).

  • Mixture: Combination of two or more substances physically combined.

For further chapters and concepts (like Stoichiometry, Electrochemistry, etc.), please refer to specific sections based on your syllabus needs.