Chapter 1 Slide Deck

Matter

• Defined as anything that has mass and occupies space.

Types of Matter

• Elements: Pure substances that cannot be broken down.

  • Example: Copper (Cu), Hydrogen (H2).

• Compounds: Substances composed of two or more elements that are chemically combined.

  • Example: Water (H2O), Table sugar (C12H22O11).

• Mixtures:

  • Homogeneous: Uniform mixtures.

    • Example: Sugar water (H2O and C12H22O11).

  • Heterogeneous: Mixtures in which components can be seen and separated.

    • Example: Vegetable soup (H2O, various vegetables).

The Periodic Table of Elements

• Organized by groups (columns) and periods (rows).

  • Main-group elements: Include Alkali metals, Alkaline earth metals, Halogens, and Noble gases.

  • Each element has a unique elemental symbol, group number, and period.

Common Elements

• Main Elements in Living Things:

  • Macronutrients: Essential in larger quantities (O, C, N, etc.).

  • Micronutrients: Essential in trace amounts (Cu, Fe, F, I).

    • Roles:

      • Copper (Cu): Essential for enzymes, located in the liver.

      • Fluorine (F): Vital for teeth and bone integrity.

      • Iron (Fe): Key component of hemoglobin.

Chemical vs. Physical Changes

• Physical Change Examples:

  • Melting ice.

  • Mixing oil and water.

• Chemical Reaction Examples:

  • Burning wood.

  • Rusting of nails.

Forms of Water

• Liquid Water (H2O)

• Solid Water (Ice)

Significant Figures in Measurements

• Rules for counting significant figures:

  1. Non-zero digits are significant.

  2. Zeros between non-zero digits are significant.

  3. Leading zeros are not significant.

  4. Trailing zeros in a decimal number are significant.

Rules Examples:

• 15.3 m = 3 significant figures.

• 0.00024 g = 2 significant figures.

• 12,000 km = 2 significant figures (unless specified otherwise).

Scientific Notation

• Common powers of ten representation for large or small numbers.

  • Example: 1,000,000 = 1 × 10^6.

  • Example: 0.000001 = 1 × 10^-6.

Temperature Conversions

• Fahrenheit to Celsius and Kelvin:

  • Freezing point of water: 0 °C = 32 °F = 273 K.

  • Boiling point of water: 100 °C = 212 °F = 373 K.

Properties of States of Matter

• Solid: Definite shape and volume; particles tightly packed.

• Liquid: Definite volume but shape adapts to the container; particles less orderly.

• Gas: Fills the volume of its container; particles very far apart and in constant motion.

Comparing Different Substances

• Specific Heat Capacity: Water = 1.00 cal/g °C

• Values vary across substances, indicating how much heat is required to raise temperature.

Measurement Tools

• Common laboratory tools include:

  • Graduated cylinders for precise volume measurements.

  • Kings for weight measurements.

  • Thermometers for temperature readings.

Tables and Graphs

• Tables (e.g., micronutrients, blood chemistry results) help illustrate and summarize important data.

• Graphical representations may show trends in measurements or chemical reactions.