1. Chapter 13-States of Matter Chem 311

2. Kinetic Theory All mater consists of tiny particles that are in constant motion Specifically, the particles in gas are considered to be small hard spheres with an insignificant volume The particles in gas are spread out leaving a lot of open space

3. Gas Particles The motion of particles in a gas is rapid, constant, and random As a result gases will always spread out and fill the area they are contained in The particles travel in a straight line but change course after collisions with other gas molecules During collisions kinetic energy is transferred from one particle to the other without loss as the collisions are characterized as elastic

4. Kinetic Theory of Gases A gas is composed of a large number of molecules that are very small relative to the distance between molecules. The molecules of a gas are in constant, random motion and frequently collide with each other and with their container.

5. Measuring Air Pressure A Barometer is a device used to measure atmospheric pressure and can be read the same way as a thermometer. The height of the mercury in a barometer depends on weather and altitude. The higher the altitude, the lower the pressure. The atmospheric pressure pushes the mercury from the reservoir into the glass tube. The pressure at sea level is 760mm, or 29.2 inches. The tip of the tube is a vacuum- an empty space with no pressure or particles.

6. Gas Pressure Gas Pressure is the result of simultaneous collisions of billions of rapidly moving gas particles against an object. The more collisions, the higher the pressure. The collision / movement of these gas particles can be explained with the Kinetic theory (which states that matter consists of tiny particles in constant motion). The Pascal (Pa) is the SI unit of pressure, another unit of measurement is millimeters of mercury (mm Hg) and standard atmospheres (atm).

7. Kinetic Theory + Distribution Curve Increase in kinetic energy= increase in temperature Higher temperature has wider range of kinetic energies Increase in avg kinetic energy causes a rise of the temperature

8. Kelvin At absolute zero (0 K) particles have no kinetic energy/no motion. There is no lower temperature than absolute zero Kelvin. Kelvin temperature is directly proportional to the avg kinetic energy of a substance  For example, particles of helium at 200K have 2x the avg kinetic energy as helium at 100K

9. A Model for Liquids Both the particles in gases and the particles in liquids have kinetic energy. This energy allows the particles in gases and liquids to flow past each other. Substances that can flow are known as fluids. Since fluids flow the way they do, they conform to the shape of their containers.

10. Pt. II Unlike the particles of gases, inter-molecular attractions reduce the amount of space between the particles in liquids. Since the particles of liquids are close together, liquids have a definite volume. Liquids are consequently much more dense than gases Changing the amount of pressure on a liquid hardly effects its volume. Since liquids and solids are mostly incondensable, they are known as condensed states of matter.

11. Solid Organization and Properties Closely packed ions, atoms, or molecules, well organized Closely packed ions, atoms, or molecules, well organized Particles have fixed location and vibrate around fixed points, strong attractions Particles have fixed location and vibrate around fixed points, strong attractions  Solids do not flow Dense (not easily compressed) Dense (not easily compressed) Melting points Melting points  Ionic solids- high melting point  Molecular solids- low melting point

12. Melting Point of Solids melting point-temperature where solid changes into a liquid melting point-temperature where solid changes into a liquid  When melted, solid particles have high vibrations that allow them to move out of fixed positions and into liquid form  Equilibrium- temperature where melting point of solid and freezing point of liquid are at same temperature  Melting point is determined by particle organization  Solid melting point exceptions Cane sugar and wood Cane sugar and wood

13. Crystal Structures and Systems Crystal- three dimensional pattern arrangement of solid particles Crystal- three dimensional pattern arrangement of solid particles Crystal shape describes solid particle arrangement Crystal shape describes solid particle arrangement Crystal properties Crystal properties  Has sides or face Labeled a, b, c Labeled a, b, c  Has angles that intersect at faces Labeled β, Υ, α Labeled β, Υ, α  Seven groups of crystals- cubic, tetragonal, rhombic, monoclinic, triclinic, hexagonal, and rhombohedra

14. Liquid Organization and Properties Contain kinetic energy Contain kinetic energy Fluids- particles that flow Fluids- particles that flow  Allows liquids to take shape of container Particles have relatively strong attractions Particles have relatively strong attractions  Keep particles together  Create definite volume  Keeps particles close together Denser than gases, less dense then solids Denser than gases, less dense then solids Not effected by pressure Not effected by pressure

15. Gas Organization and Properties Particles have kinetic energy (like liquids) Particles have kinetic energy (like liquids)  Keeps particles in constant motion Particles are small hard spheres with insignificant volume Particles are small hard spheres with insignificant volume  Spacing is high  No attractive forces to hold them together Particles are in constant motion Particles are in constant motion  Fill container regardless of shape

16. Attractive forces Organizati on of particles GasesNoParticles in constant motion LiquidsYes, slightly strong Takes shape of container SolidsYes, very strong In crystal structures

17. Solid Liquid Gas Organization and Attraction

18. Distinguishing Between Crystal and Glass Properties of Crystal Properties of Crystal  Particles are arranged in an orderly, 3-D pattern called a crystal lattice  Has sides, or faces  In general, have high melting points (unless molecular)  When shattered, fragments have the same surface angles as the original solid Properties of Glass Properties of Glass  Also called amorphous solid  Crystallization does not occur  The structures of glasses are intermediate between those of crystalline and those of free-flowing liquids  Do not melt at a definite temp.  When shattered, fragments have irregular angles and jagged edges

19. Crystal vs. Glass Structures Crystal Crystal  The shape of a crystal reflects the arrangement of particles within the solid  The smallest group of particles that retains its geometric shape is the unit cell The unit cell may be simple cubic, body-centered cubic, or face-centered cubic The unit cell may be simple cubic, body-centered cubic, or face-centered cubic Glass Glass  Glasses or, amorphous solids, are transparent fusion products of inorganic substances that have cooled to a rigid state WITHOUT crystallizing

20. Different Shapes of Crystal Systems

21. Sublimation When a solid becomes a gas without passes through the liquid state. Occurs when a solid has a vapor pressure higher than the pressure at or near room temperature. Vapor pressure: the measure of a force exerted by a gas above a liquid (true for solids too)

23. Deposition When a gas becomes a solid without passes through the liquid state.

25. Phase diagram -shows the conditions and pressure at which a substance exists as a solid, liquid, and gas Triple point- the only set of conditions where all three states can exist. Critical point- beyond this region the physical and chemical properties of water and steam converge to the point where they are identical. Thus, beyond the critical point, we refer to this single phase as a "supercritical fluid". Boiling, melting, and subliming curves

26. Plasma: What is it? Most common state of matter Electrically charged particles at high energy that collect around electromagnetic fields and form gas-like clouds It is made of extremely hot ions and electrons in space, but on Earth, it cools into atoms and molecules The particles are affected by electromagnetic, electric, and magnetic signals but are hardly affected by gravity.

27. Plasma: What is it? (cont.) The full range of plasma’s density, temperature, and spatial scales is nearly incomprehensible as it is so wide and varied. Without sufficient energy, the plasma reverts back to a neutral gas Energy being thermal, electrical, or light (i.e. ultraviolet) Ions and electrons move independently in large spaces Plasmas are still being studied and understood today

29. Plasma Examples Flames neon signs Nebulae (Clouds in space) solar wind Auroras Galaxies dense solid state of matter Stars Space Lightning florescent lights