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Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Sections
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
Body Centered Cubic Unit Cell
Face Centered Cubic Unit Cell

Phase Diagrams show what effect temperature and pressure have on a pure substance in a closed system without any air.

Phase Diagrams

Concept #1: States of Matter of Phase Diagrams

Example #1: At a temperature of 60ºC and 1.20 atm determine the physical state of the substance from the phase diagram shown above?

Practice: The critical point of this substance occurs at what temperature?

Concept #2: Phase Changes of Phase Diagrams

Example #2: A substance has a triple point -45.0 ºC and 500 mmHg. What is the most likely phase change to occur for a solid sample of this substance as it is heated from -60.0 ºC to 10 ºC at a pressure of 490 mmHg?

Practice: Arrow I corresponds to:

Practice: What is the normal freezing point of this unknown substance?

Practice: At what temperature can we no longer tell the difference between the liquid and gas phases?