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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

MO Theory: Homonuclear Diatomic Molecules

MO Theory: Heteronuclear Diatomic Molecules

MO Theory: Bond Order

Molecular Polarity

Intermolecular Forces

Intermolecular Forces and Physical Properties

Clausius-Clapeyron Equation

Phase Diagrams

Heating and Cooling Curves

Atomic, Ionic, and Molecular Solids

Crystalline Solids

Simple Cubic Unit Cell

Face Centered Cubic Unit Cell

Solutions: Solubility and Intermolecular Forces

Molality

Parts per Million (ppm)

Mole Fraction of Solutions

Solutions: Mass Percent

Types of Aqueous Solutions

Intro to Henry's Law

Henry's Law Calculations

The Colligative Properties

Boiling Point Elevation

Freezing Point Depression

Osmosis

Osmotic Pressure

Vapor Pressure Lowering (Raoult's Law)

General Chemistry 1 Final - Part 3 of 3

Calculate the energy required to melt 7.23 kg of ice at 0°C if it was placed on the ground with a temperature of 26.0°C. ΔHf,H2O = 80.0 cal/g

Calculate the energy required to melt 7.23 kg of ice at 0°C if it was placed on the ground with a temperature of 26.0°C.
ΔH_f,H2O = 80.0 cal/g