【People's Education Edition】High School Chemistry Elective Compulsory Volume 2

📚 Content Summary

This textbook is an elective compulsory module of the high school chemistry curriculum, delving into the intrinsic connections between microscopic structures (atoms, molecules, crystals) and their macroscopic properties.

Explore the mysteries of the microscopic world and reveal the chemical essence of material properties.

Author: People's Education Press Curriculum Textbook Research Institute Chemistry Curriculum Textbook Research and Development Center

Acknowledgments: Approved by the National Textbook Committee Expert Committee in 2019

🎯 Learning Objectives

1. Describe the motion states of electrons outside atomic nuclei, and master concepts such as energy levels, sublevels, atomic orbitals, and electron spin.
2. Accurately write electron configurations and orbital diagrams for ground-state atoms of common elements.
3. Apply electron configuration rules to explain trends in elemental properties (e.g., ionization energy variations, atomic spectral line formation).
4. Understand bonding nature: distinguish the formation characteristics (axial symmetry vs. mirror symmetry) of \sigma bonds and \pi bonds, and their distribution in single, double, and triple bonds.
5. Predict molecular geometry: proficiently use the Valence Shell Electron Pair Repulsion (VSEPR) model to calculate lone pair counts, and combine it with hybrid orbital theory (sp, sp^2, sp^3) to deduce molecular spatial configurations.
6. Explain physical properties: determine molecular polarity based on bond polarity vectors, and use intermolecular forces and the "like dissolves like" principle to explain trends in melting/boiling points and solubility.
7. Explain the characteristics of plasmas and liquid crystals, and clarify differences between crystals and amorphous materials in terms of microscopic structure and macroscopic properties (self-forming ability, anisotropy).
8. Master the concept of the unit cell; skillfully apply the "sharing method" to calculate the number of atoms within a unit cell, and understand the role of X-ray diffraction in determining crystal structures.
9. Distinguish and describe the microscopic particles and interparticle interactions in molecular crystals, covalent crystals, metallic crystals (electron gas theory), and ionic crystals; understand the existence of transitional and mixed-type crystals.

🔹 Lesson 1: Atomic Structure and Periodic Law

Overview: This lesson covers core theories of atomic structure in the microscopic world, focusing on the distribution patterns of electrons outside the nucleus. Students will progress from qualitative concepts of energy levels and sublevels to quantum mechanical models involving electron clouds and atomic orbitals, and gain deep understanding of the three fundamental principles governing electron arrangements (Aufbau principle, Pauli exclusion principle, Hund’s rule). Ultimately, through analysis of valence electron configurations and ionization energies, the essence of the periodic law is revealed.

Learning Outcomes:

• Describe the motion states of electrons outside atomic nuclei, and master concepts such as energy levels, sublevels, atomic orbitals, and electron spin.
• Accurately write electron configurations and orbital diagrams for ground-state atoms of common elements.
• Apply electron configuration rules to explain trends in elemental properties (e.g., ionization energy variations, atomic spectral line formation).

🔹 Lesson 2: Molecular Structure and Nature of Chemical Bonds

Overview: This course module explores the structural organization of matter at the molecular level, covering the microscopic mechanisms of covalent bond formation (\sigma and \pi bonds) to predicting molecular geometries (VSEPR model and hybrid orbital theory). Additionally, the course extends to how intermolecular forces (van der Waals forces, hydrogen bonding) determine physical properties (polarity, solubility, boiling point), and briefly introduces molecular chirality and coordination compound fundamentals, establishing a complete logical framework where “structure determines properties.”

Learning Outcomes:

• Understand bonding nature: distinguish the formation characteristics (axial symmetry vs. mirror symmetry) of \sigma bonds and \pi bonds, and their distribution in single, double, and triple bonds.
• Predict spatial structure: proficiently use the Valence Shell Electron Pair Repulsion (VSEPR) model to calculate lone pair counts, and combine it with hybrid orbital theory (sp, sp^2, sp^3) to deduce molecular spatial configurations.
• Explain physical properties: determine molecular polarity based on bond polarity vectors, and use intermolecular forces and the "like dissolves like" principle to explain trends in melting/boiling points and solubility.

🔹 Lesson 3: Crystal Structure and States of Matter

Overview: This course aims to guide students toward a deeper understanding of the states of matter by linking microscopic structures with macroscopic properties. It covers not only solid, liquid, and gaseous states but also plasma and liquid crystal phases. The focus lies on the essential differences between crystals and amorphous materials (self-forming ability, anisotropy, and X-ray diffraction experiments), and provides detailed analysis of the structural features and properties of four typical crystal types (molecular, covalent, metallic, ionic) and transitional crystal forms. Finally, introductions to coordination compounds and supramolecular chemistry expand students’ understanding of intermolecular interactions and molecular self-assembly.

Learning Outcomes:

• Explain the characteristics of plasmas and liquid crystals, and clarify differences between crystals and amorphous materials in terms of microscopic structure and macroscopic properties (self-forming ability, anisotropy).
• Master the concept of the unit cell; skillfully apply the "sharing method" to calculate the number of atoms within a unit cell, and understand the role of X-ray diffraction in determining crystal structures.
• Distinguish and describe the microscopic particles and interparticle interactions in molecular crystals, covalent crystals, metallic crystals (electron gas theory), and ionic crystals; understand the existence of transitional and mixed-type crystals.