Chapter 2: Measurement and Problem Solving

Measurements

• Scientific Notation: A method for expressing very large or very small numbers using powers of ten.

  • Rewrite a number in standard (decimal) notation to scientific notation.

  • Rewrite a number in scientific notation to standard notation.

  • Example:

• Significant Figures: Digits in a measurement that are known with certainty plus one estimated digit.

  • Identify the value as an exact or inexact quantity.

  • Read a volume or length measurement and estimate to the correct decimal place.

  • Identify the number of significant figures in a number.

  • Round a number to a given number of significant figures.

  • Use correct rules for multiplication/division and addition/subtraction.

  • Example: has five significant figures.

• Calculate volume from length

  • l x w x h

• Unit Conversions: Changing from one unit to another using conversion factors.

  • Calculate volume with metric units and prefixes.

  • Metric system prefixes for conversion: mega, kilo, deci, centi, milli, micro, nano, pico

  • Use single and multiple conversion factors.

Density

• Density as a Conversion Factor: Use density to convert between mass and volume.

• Identify metals based on their densities

• Use the displacement of water to calculate the volume of a liquid

Chapter 3: Matter

Classification and Properties of Matter

• Definition of Matter: Anything that has mass and takes up space.

• States of Matter:

  • Solid: Definite shape and volume.

  • Liquid: Definite volume, takes shape of container.

  • Gas: No definite shape or volume.

• Solids:

  • Crystalline: atoms or molecules that are arranged in a geometric pattern

  • Amorphous: atoms or molecules have no distinct pattern/ no long range order

• Compressibility:

• Classification:

  • Pure Substances: made of one or more atom or molecule with fixed composition that can't be separated by physical means

  • Mixtures: Physical combinations of substances; can be homogeneous (solutions) or heterogeneous;

    • Homogeneous : same composition throughout

    • Heterogeneous : composition varies throughout

• Physical and Chemical Properties:

  • Physical Properties: Observed without changing the substance (e.g., melting point, density).

  • Chemical Properties: Describe how a substance reacts (e.g., flammability, reactivity).

• Physical and Chemical Changes:

  • Physical Change: Change in state or appearance without altering composition.

  • Chemical Change: Produces new substances with different properties.

• Examples: Melting ice (physical change), burning wood (chemical change).

Chapter 6: Moles and Mole Conversions

The Mole Concept

The mole is a fundamental unit in chemistry for counting particles such as atoms, molecules, or ions. It allows chemists to relate mass to number of particles.

• Definition of Mole: One mole contains particles (Avogadro's number).

• Molar Mass: The mass of one mole of a substance, expressed in grams per mole ().

• Conversions:

  • Use molar mass to convert between moles and grams. Formula:

  • Use Avogadro's number to convert between moles and number of atoms/molecules. Formula:

• Example: of water () is mole.