High School Chemistry Fundamentals provides a comprehensive introduction to core chemistry concepts, equipping students with a solid foundation for advanced studies and practical applications. Students will master fundamental principles, explore chemical bonding and molecular structure, and learn to predict chemical behavior using periodic trends and electronic configurations. By the end of this course, students will be able to apply chemical principles to solve problems and understand the world around them.

Scientific Method and Core Principles

• Introduction to the scientific method — observation, question formulation, hypothesis creation
• Emphasis on chemistry fundamentals to build familiarity for future encounters
• Understanding the importance of accurate definitions and foundational knowledge

Quantum Numbers and Electronic Configuration

• Principal quantum number — energy level of an electron
• Angular momentum quantum number — shape of the electron's orbital (s, p, d, f)
• Magnetic quantum number — orientation of the orbital in space within a sub-level
• Spin quantum number — direction of electron spin
• Electron configuration — distribution of electrons within an atom's orbitals
• Utilizing URL links to access slides and recordings for review

Periodic Trends

• Effective nuclear charge (Zeff) — net positive charge experienced by an electron in a multi-electron atom, calculated using Z - S (atomic number minus shielded electrons)
• Trends in electronegativity, electron affinity, and atomic radius across the periodic table
• Understanding valence electrons and their role in chemical properties

VSEPR Theory and Molecular Geometry

• Valence Shell Electron Pair Repulsion (VSEPR) theory — predicting molecular shapes based on minimizing electron pair repulsion around a central atom
• Distinction between electronic geometry — arrangement of all electron regions (bonded and lone pairs) and molecular shape — 3D arrangement of atoms
• Regions of electron density — bonds and lone pairs around a central atom, influencing molecular shape

Chemical Bonding

• Explanation of how electrons are used in bonds around a central atom
• Understanding that it takes two electrons to create a bond

Molecular Shapes

• Tetrahedral — four regions of electron density
• Trigonal planar — three regions of electron density
• Bent — non-linear shape due to lone pair repulsion
• Recognition that if there are lone pairs as well as bonds, that will change the shape