**Properties of Matter**
- **Physical vs Chemical Properties**
- *Physical Properties:* Can be observed without changing the substance (e.g., color, density, melting point, boiling point)
- *Chemical Properties:* Describe a substance’s ability to undergo chemical changes (e.g., flammability, reactivity with acid)
- **Examples of Each**
- Physical: Ice melting, water boiling, density, solubility
- Chemical: Rusting iron, burning wood, tarnishing silver
- **Intensive vs Extensive Properties**
- *Intensive:* Do not depend on the amount of matter (e.g., density, boiling point, color)
- *Extensive:* Depend on the amount of matter (e.g., mass, volume, length)
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**Density**
- **Definition, Units, and Formula**
- Density (ρ) = Mass (m) / Volume (V)
- Units: g/cm³ (solids), g/mL (liquids), kg/m³ (gases)
- **Comparison of Densities**
- Solids: Generally highest density
- Liquids: Lower density than solids but higher than gases
- Gases: Lowest density
- **Solid: Regular vs Irregular Shape**
- *Regular Shape:* Use geometric formulas to find volume
- *Irregular Shape:* Use water displacement method
- **Factors Affecting Density**
- Temperature (increase decreases density for most substances)
- Pressure (affects gases significantly)
- Composition (different materials have different densities)
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**Elements, Compounds, and Mixtures**
- **Matter: Definition and Examples**
- Anything that has mass and takes up space (e.g., air, water, rocks)
- **Pure vs Impure Matter**
- *Pure:* Elements and compounds (e.g., oxygen, water)
- *Impure:* Mixtures (e.g., saltwater, air)
- **Atom vs Element**
- *Atom:* Smallest unit of an element
- *Element:* Substance made of one type of atom
- **Compounds vs Mixtures**
- *Compounds:* Chemically bonded elements (e.g., H2O, CO2)
- *Mixtures:* Physically combined substances (e.g., salad, air)
- **Types of Mixtures**
- Homogeneous (solutions, uniform throughout)
- Heterogeneous (distinct parts, not uniform)
- **Examples of Mixtures**
- Homogeneous: Saltwater, air
- Heterogeneous: Salad, granite
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**Solubility**
- **Solutions**
- *Parts:* Solute (dissolved substance) + Solvent (dissolving substance)
- *Examples:* Saltwater (solute: salt, solvent: water)
- **Effect of Temperature and Pressure**
- Higher temperature increases solubility of solids in liquids
- Higher pressure increases solubility of gases in liquids
- **Gases vs Liquids**
- Gases dissolve better in cold liquids under high pressure
- Liquids dissolve better at higher temperatures
- **Gaseous, Liquid, and Solid Solutions**
- Gaseous: Air (oxygen in nitrogen)
- Liquid: Saltwater (NaCl in H2O)
- Solid: Alloys (brass, steel)
- **Concentrations**
- Unsaturated: Can dissolve more solute
- Saturated: Maximum solute dissolved
- Supersaturated: Holds more than normally possible
- **Solubility Curve**
- Shows solubility vs temperature
- Higher points indicate higher solubility
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**The Mole**
- **Avogadro’s Number**
- 6.022 x 10^23 particles per mole
- **Molar Mass**
- Mass of one mole of a substance (g/mol)
- **Particle, Mass, and Mole Calculations**
- Particle calculations: Using Avogadro’s number
- Mass calculations: Converting between grams and moles
- Mole calculations: Determining amount of substance
- **Moles at STP (Standard Temperature and Pressure)**
- 1 mole of gas = 22.4 L at STP
- **Atomic Mass Units (AMU)**
- Unit for atomic/molecular mass
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**Labs**
- **Density Lab**
- Measure mass and volume, calculate density
- Compare densities of different materials
- **Elements, Compounds, and Mixtures Lab**
- Classify substances based on their properties
- **Mystery Powder Lab**
- Identify unknown substances using solubility and reactions
- **Cornstarch Lab**
- Explore properties of non-Newtonian fluids
This guide covers essential concepts in matter, density, solubility, and the mole, along with relevant lab activities
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