Liquids andsolids cheat sheet
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This document provides a summary of key chemistry concepts related to liquids and solids. It defines intermolecular forces like London dispersion forces, dipole-dipole forces, and hydrogen bonding. It also explains properties of solids like crystalline and amorphous structure. Phase changes between solid, liquid, and gas are discussed, including the energies involved in melting, vaporization, and sublimation. Vapor pressure equilibrium is defined as the state where the rate of evaporation equals the rate of condensation.
Liquids andsolids cheat sheet
- 1. AP Chemistry - Core Concept Cheat Sheet 17: Liquids and Solids Key Chemistry Terms Vapor Pressure Equilibrium • Intramolecular forces: chemical bonds within a molecule. • Intermolecular forces (IMF): physical attractions between separate molecules. • Dipole: Partial separation of charge. • London Dispersion Forces: temporary dipole due to electrons ganging up on one side of the molecule. • Dipole-Dipole Forces: Attractions between opposite charges in two polar molecules. • Ion Dipole Forces: Attraction between an ion and the opposite charge on a polar molecule. • Hydrogen bonding: Very strong dipole present when an H bonds to an N, O or F. The H can then “hydrogen bond” with the lone pairs on an N, O or F of a different molecule. • Vapor Pressure: Pressure caused by particles evaporating from a solid or liquid. • Equilibrium: The rate of change is equal to the rate of the opposite change. • Amorphous solid: No repeatable structural components. • Crystalline solid: Repeating unit cell of the components. • Lattice: Overall structure of crystalline solid. • Unit Cell: Repeating unit in lattice. • Atomic solids: Atoms are the components of the unit cells. • Molecular solids: Molecules are the components of the unit cell. • Phase change: Matter changes from one state to another. • Phase Diagram: Shows the state of matter at various temperature and pressures. • Enthalpy of fusion (Hfus): Energy needed to break enough intermolecular forces to melt. • Enthalpy of vaporization (Hvap): Energy needed to break remaining IMF’s to evaporate a liquid. Intermolecular Forces • Initially liquid particles escape resulting gas particles. The gas particles can collide with the liquid and re-join it. • The rate of gas evaporating remains the same. The rate of gas particles re-joining the liquids increases as more gas particles are made from evaporation. • Vapor Pressure equilibrium is established over time. Solid Properties of solids: • Definite shape and volume. • Particles are not free to move past one another. • Not compressible. Amorphous solid particles are “trapped” in place before they can arrange themselves into a repeating pattern. Three types of crystalline solids: • Atomic solids • Metallic solids—closest packing of metal atoms. Electrons are in a pool and are free to move throughout. • Network solids—one giant molecule. Each atom is covalently bonded to surrounding atoms. • Molecular solids—strong covalent bonds within the molecular, weaker physical attractions between them. • Ionic solids—electrostatic attraction between ions. Ions are stacked to minimize like-charge repulsions. Phase Changes • • • • • • • • IMF Happens with Relative strength • London Dispersion Forces • Dipole-Dipole Forces • Ion-Dipole Forces • Hydrogen Bonding • All molecules • Weakest IMF • 2 polar molecules • Ion and a polar molecule • H on an N, O or F with an N, O or F on another molecule • Medium strength • Medium strength • Strongest IMF • • • • Melting/freezing: solid liquid Boiling/condensing: liquid gas Sublimation/deposition: solid gas Melting: Requires energy to break some IMF. Boiling: Requires energy to break remaining IMF. Subliming: Requires energy to break all the IMF. Deposition, condensation and freezing: Energy is released as IMF’s formed. Boiling/Condensation Point: Temperature at which liquid and gas are at equilibrium. Vapor pressure of liquid = atmospheric pressure Melting/Freezing Point: Temperature at which solid and liquid are at equilibrium. Vapor pressure of solid = Vapor pressure of liquid Substances sublime when the IMF are so weak that all of them are broken at that temperature and pressure. Energy of Phase Changes Equations for energy change (ΔH) during a phase change: Melting: • London Dispersion Forces are temporary, and therefore weaker. The larger the molecule, the greater the London Dispersion Forces. Vapor Pressure Vapor Pressure • If a particle on the top surface of the liquid has enough energy, it can escape the intermolecular forces and evaporate—causing vapor pressure. • As temperature increases, more particles have the necessary energy to evaporate—vapor pressure increases. ΔH = m × H fus Evaporating: ΔH = m × H vap For freezing and condensing, use –Hfus and –Hvap since energy is released. Liquids Properties of liquids: • Definite volume but not shape. • Particles are free to move past one another. • Not very compressible. How to Use This Cheat Sheet: These are the keys related this topic. Try to read through it carefully twice then rewrite it out on a blank sheet of paper. Review it again before the exams. RapidLearningCenter.com ©Rapid Learning Inc. All Rights Reserved