States of Matter Ch. 13.1-13.3.

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Presentation transcript:

States of Matter Ch. 13.1-13.3

Solids Have an orderly arrangement and fixed location of particles Particles “vibrate” in place, so they do not flow When heat (energy) is added, particles “vibrate” faster and begin to spread apart (melt) Most are crystalline (rigid), some are amorphous (lack an internal structure) Examples of amorphous solids: rubber, glass

Liquids Intermolecular attractions reduce movement of particles (more dense than gas) Vaporization: turning liquid to gas Evaporation: surface particles only Is a cooling process (sweat) Boiling: particles throughout liquid Vapor pressure = atmospheric pressure (BP) Higher altitudes=lower bp

Gases Kinetic Theory: Particles are small, hard spheres with an insignificant volume Most of particles is rapid, constant, and random All collisions are perfectly elastic (energy is transferred without loss) Gas Pressure: caused by collisions with an object SI unit: pascal (Pa) Standard Pressure: 1 atm = 760 mmHg = 101.3 kPa

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