I. Student Learning Outcomes (SLOs):

• State formulae of common elements and compounds
• Define molecular formula
• Define empirical formula
• Deduce formula and name of binary compounds from ions
• Deduce formula of molecular substances from given structures
• Use relationship: amount of substance = mass/molar mass
• Define mole and Avogadro's number
• Explain relationship between mole and Avogadro's constant
• Construct chemical and ionic equations
• Deduce symbol equations with state symbols

II. Introduction:

• Historical context: Ancient Greek philosophers' beliefs about elemental substances
• John Dalton's atomic theory in the 19th century
• 20th century developments in atomic structure
• Chapter goal: Understand fundamental concepts about matter

III. Empirical and Molecular Formulas:

A. Empirical Formula:

Definition: Simplest integer ratio of atoms of each element in a compound.
Example: Hydrogen peroxide (HO)
Exercise: Empirical formula of glucose

B. Molecular Formula:

Definition: Specifies the actual number of atoms of each element in one molecule.
Example: Hydrogen peroxide (H₂O₂), Glucose (C₆H₁₂O₆)
Relationship to empirical formula: Molecular formula is a multiple of the empirical formula.
Examples where empirical and molecular formulas are the same: H₂O (water), NH₃ (ammonia)

IV. Common Formulas:

Table of common elements and compounds with their formulas:

• Elements: Hydrogen (H₂), Oxygen (O₂), Nitrogen (N₂), etc.
• Compounds: Water (H₂O), Carbon dioxide (CO₂), Hydrochloric acid (HCl), etc.