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Discover the kinetic theory, phase changes, vaporization, and equilibrium in gases, liquids, and solids. Learn about the properties, pressure, and behavior of matter in different states. Convert units, measure pressure, and explore the unique characteristics of each state. Gain insights into the relationship between particles, temperature, and energy in this comprehensive overview of the four states of matter.
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Starter S-137 List and describe the four states of matter.
States of Matter Chapter 13
13.1 The Nature of Gases Chapter 13
13.1 The Nature of Gases Kinetic Theory – all matter consists of tiny particles that are in constant motion • Particles of a gas are considered to be small hard spheres with an insignificant volume (too small to matter) • Motion of the particles in a gas is rapid, constant, and random
13.1 The Nature of Gases • Collisions between particles in a gas are perfectly elastic. -no energy is lost in collisions
13.1 The Nature of Gases Gas pressure is caused by the collision of particles with the container Atmospheric Pressure – caused by the collision of atoms and molecules in air with objects
13.1 The Nature of Gases Barometer – a device to measure atmospheric pressure The pressure depends on Temperature Altitude Measured in pascal (Pa) very small unit
13.1 The Nature of Gases Units must be converted for problems to work out These are equalities, so they can be used to create conversion factors
13.1 The Nature of Gases The Kelvin temperature of a substance is directly proportional to the average kinetic energy of the particles of the substance PhET Gas
13.1 The Nature of Gases Notice - the average shifts, but there are particles with very different temperatures - the hotter one has particles with almost no energy, just like the colder one
Starter S-139 Convert each of the following to kilopascals • 450 mmHg • 1045 torr • 1.29 atm • 95,000 pa
13.2 The Nature of Liquids Chapter 13
13.2 The Nature of Liquids Fluids – substances that can flow gases liquids Unlike gases, liquids particles attracted to each other
13.2 The Nature of Liquids Physical properties of a liquid are determined by • Motion of the particles (due to temperature) • Attraction among the particles • The particles are closer together due to these forces Phase Change
13.2 The Nature of Liquids Vaporization – conversion of a liquid to a gas or vapor Evaporation – vaporization on the surface of a liquid that is not boiling
13.2 The Nature of Liquids During evaporation – only molecules with a certain minimum kinetic energy escape from the liquid Evaporation takes away the hot (faster) particles and is a cooling process
13.2 The Nature of Liquids Vapor Pressure – the force exerted by a gas above a liquid Gas produced by evaporation Eventually rate of particles leaving the liquid equal the particles reentering the liquid Vapor Pressure Equilibrium
13.2 The Nature of Liquids The container only reaches equilibrium if it is sealed Vapor pressure depends on temperature at higher temperature the average kinetic energy is higher
13.2 The Nature of Liquids The vapor pressure shows of volatile a liquid is How easily it evaporates
13.2 The Nature of Liquids Boiling – when the temperature is high enough, that particles throughout the liquid have the kinetic energy to vaporize Bubbles of vapor form throughout the liquid Boiling point – the point where the vapor pressure of the liquid is equal to the external pressure on the liquid
Starter S-140 1. What is • Vaporization • Boiling • Evaporation • Vapor Pressure 2. What is the relationship between vapor pressure and boiling?
13.3 The Nature of Solids Chapter 13
13.3 The Nature of Solids Properties of solids are determined by • Orderly arrangement of their particles • Fixed locations of their particles Melting point – temperature at which a solid changes into a liquid
13.3 The Nature of Solids The melting point and freezing point are the same temperature The states are at equilibrium Crystalline Solids – the particles are arranged in crystals Crystal – orderly 3D pattern
13.3 The Nature of Solids Crystal Systems Defined by 6 Values
13.3 The Nature of Solids Seven Basic Shapes Unit Cell – the smallest group of particles that has the geometric shape of the crystal
13.3 The Nature of Solids Allotropes – two or more different molecular forms of the same element in the same physical state Carbon Diamond Graphite Soot (buckminsterfullerene)
13.3 The Nature of Solids Amorphous Solid – lacks an internal structure Rubber Plastics Glass Do not have a specific melting point Shatter into random shapes
Starter S-141 1. Define • Crystalline Solid • Amorphous Solid 2. What are the three allotropes of carbon?
13.4 Changes of State Chapter 13
13.4 Change of State Solid – molecules vibrate in place Melting – Particles increase speed start to move Liquid – molecules move, but still attracted to each other Evaporation – particles move fast enough to that intermolecular forces do not matter Melting Phase Change
13.4 Change of State Sublimation – solid goes directly to a gas Vapor pressure of the solid is greater than atmospheric pressure Carbon Dioxide (Dry Ice) Iodine
13.4 Change of State Phase Diagram – shows states (solid, liquid, gas) in relation to pressure and temperature
13.4 Change of State Triple Point – the point where a solid, liquid, and gas state can all exist For water that would be 0.61 kPa and 0.016 oC Notice – An increase in pressure drives most substances toward a solid An increase in temperature drives substances toward a gas
