Summary of Chemical Reactions Concepts chapter 5 notes

Introduction to Chemical Reactions

• Physical Change: Alters physical state without changing composition.

• Chemical Change: Converts substances into others through breaking/forming bonds.

Writing Chemical Equations

• Chemical Equation Format: Reactants (left) --> Products (right).

• Conservation of Mass: Atoms neither created nor destroyed.

• Balancing Equations: Coefficients ensure equal number of atoms on both sides.

• Symbols in Equations:

  • → : Reaction arrow

  • Δ : Heat

  • (s) : Solid

  • (l) : Liquid

  • (g) : Gas

  • (aq) : Aqueous solution

Types of Reactions

• Categories:

  • Combination

  • Decomposition

  • Single Replacement

  • Double Replacement

  • Oxidation-Reduction (Redox)

  • Acid-Base

• Combination Reaction: Multiple reactants form single product.

• Decomposition Reaction: Single reactant forms multiple products.

Oxidation and Reduction (Redox)

• Oxidation: Loss of electrons.

• Reduction: Gain of electrons.

• Redox Reaction: Involves both oxidation and reduction.

• Reducing Agent: Substance losing electrons.

• Oxidizing Agent: Substance gaining electrons.

The Mole and Avogadro's Number

• Definition of a Mole: 6.022 x 10²³ items.

• Molar Mass: Mass of 1 mole of a substance (g/mol).

• Formula Weight: Sum of atomic weights in amu, equivalent to molar mass in g/mol.

Mass to Mole Conversions

• Relating Grams to Moles: Molar mass as conversion factor.

• Find Number of Atoms/Molecules: Use Avogadro's number for conversions between moles and molecules.

Percent Yield and Limiting Reactants

• Theoretical Yield: Expected amount from reactants based on balanced equation.

• Actual Yield: Product formed in experiment.

• Percent Yield: (Actual Yield / Theoretical Yield) x 100.

• Limiting Reactant: Reactant completely consumed limits product formation.