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Phase

Bob Jones PPT Notes -- Chapter 2c

Subject: 
Chemistry
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Physics
Chemical engineering
Condensed matter physics
thermodynamics
State functions
State of matter
Gas
Kinetic theory
matter
energy
Plasma
Phase
Environment

Section 2C States of Matter Kinetic-Molecular Theory All particles are in motion. Add energy = increase motion. Motion tries to tear apart matter. Attractive forces hold matter together. Attractive ? electrical, between particles Disruptive ? caused by kinetic energy (motion) Balance between these forces determines state. Kinetic-Molecular Theory Two Forces Solid Low energy Touching Locked in place Only vibrate (The inter-molecular forces are higher in energy than the kinetic energy.) 4 p. 41 of Chem. textbook Liquid More kinetic energy Still touching Not locked in place Can roll around (The intermolecular forces are almost equal to the kinetic energy.) 5 p. 41 of Chem. textbook Atoms are touching. Attractions are greater than repulsions. Atoms roll around. Atoms are small.

Chapter 10

Subject: 
Chemistry
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Chemistry
Thermodynamic properties
Chemical engineering
Materials science
Phase transitions
Enthalpy
Enthalpy of vaporization
Vapor pressure
Phase
Enthalpy of fusion
Dipole
Evaporation

Chapter 10 notes Claire Rafson 10.1-10.2 Intermolecular forces- occur b/w not in molecules. From solid to liquid to gas molecules remain in tact Forces: Dipole-dipole forces are forces that act between polar molecules Hydrogen bonding- strong form of dipole dipole with H and NOF London Dispersion- Present in all but ionic . noble gas and nonpolar and Polar. Big atom with a lot electrons LD can be stronger than dipole dipole Higher IMF = higher: surface tension, boiling/meltin point. Lower: vapor pressure Capillary action- polar liquids typically exhibit it 10.3- crystalline solids- highly regular arrangement of their components ionic and molecular amorphous solids- considerable disorder 10.5- Network atomic Solids- giant molecule Strong covalent bonds Silica- SiO2

bio

Subject: 
Biology
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Chemistry
Mixture
Chemical substance
Physical change
Homogeneous
Chemical compound
Homogeneity and heterogeneity
Chemical element
Solution
matter
Phase
Chemical change
Environment

Warm-Up Your car's gas tank holds 18.6 gallons and is one quarter full. Your car gets 16 miles/gal. You see a sign saying, "Next gas 73 miles." Your often-wrong brother, who is driving, is sure you'll make it without running out of gas. You're not so sure and do some quick figuring: Matter and Change Matter: Anything that has mass and takes up space. Mass: measure of the amount of matter. Matter and Change Atoms: Smallest unit of an element that maintains the properties of that element Elements: pure substance made of one atom. Compounds: made of atoms of two or more elements that are chemically bonded Physical properties and changes Physical properties: quality or condition of a substance that can be observed or measured without changing the substance
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