1. Chemistry I: The States of Matter

2. States of Matter:

4. 4 States of Matter All matter exists in one of the three following states: 1) solids-definite shape and volume 2) liquids-indefinite shape and definite volume 3) gases- indef. shape and indef. Volume 4) plasma- ionized gas particles (very rare)

5. All matter follows the KMT: Kinetic Molecular Theory KMT- the tiny particles in all forms of matter are in constant motion. (Kinetic Energy) The Avg. Velocity of the particles depends on the temperature of the gas. (The hotter the gas, the faster its particles vibrate, colder gas particles vibrate _____.

6. KMT for gas behavior KMT – as it applies to gases: A gas is composed of particles so tiny, that they have zero volume. (NOT REALLY!) All gas particles have zero attractive or repulsive forces on each other. (NOT REALLY!) All gas particles travel in straight lines, until they collide with each other or the walls of their containers. All collisions are perfectly elastic, that is during a collision, kinetic energy is transferred without loss from one particle to another.

7. Real vs. Ideal Real Gases- Do NOT follow KMT, because real gases: 1) Particles have volume 2) Particles have some attractive forces (Intermolecular Forces) Ideal Gases-Follow all the statements of KMT, they do NOT actually exist. Gases deviate from ideal behavior at ______ temperatures and _______ pressures.

8. Why do we have Ideal and Real Gases? Real Gases must follow the Van der Waals Equation: [P + a(n/V) 2 ] (V/n – b) = nRT Ideal Gases have a simpler equation: PV = nRT Since both measurements are so close, we will assume all gases are Ideal to simplify calculations.

9. Kinetic Molecular Theory

10. KMT

11. Allotropes-different forms of the same element, in the same physical state. Solid Carbon: Coal diamondgraphite C 60 (buckyballs) Amorphoustetrahedral hexagonal sheets soccer ball shape (Random)networknetwork network

12. Allotropes-different forms of the same element, in the same physical state. Oxygen gas: O 2 O 3 diatomic oxygenozone

13. Air Composition Air is approx.: 77% N 2 (inert) 21% O 2 1% Ar Rest is all other gases

14. Physical Properties of Gases Expansion/Compression- an increase or decrease to the volume of a gas in a container. Fluidity- the ability to flow. Viscosity- the resistance of a liquid to flow. Diffusion- the spontaneous mixing of gases in the same container. Effusion- the spontaneous escaping of a gas from its container through a pinhole opening.

15. Gas Pressure Gas Pressure- the force exerted by a gas per unit surface area. Pressure = force / area Barometer = an instrument which measures atmospheric pressure. Draw a barometer on the board

16. Torricelli’s Barometer The height of mercury in Torricelli’s Barometer = ________ mm Hg 1.00 atmosphere = 760 mm Hg = 760 Torricelli = 14.7 PSI = 101.3 KPa

17. Pressure Conversions 1 atm = 760 mmHg = 760 torr = 14.7 PSI = 101.3 KPa 455 mmHg = ____ atm = ____ KPa = ___ PSI = ___torr 18.3 PSI = ___ torr = ___mmHg = ___ KPa = ___ atm 675 torr = ___ atm = ___PSI = ___KPa = ____ mmHg

18. Volume Conversions

19. 1 Liter = 1 dm 3 = 1000 mL = 1000 cm 3 = 1000cc 285 mL = ____ cm 3 = ____L = ____ dm 3 = ___ cc.885 L = ___ mL = ___ dm 3 = ___ cc = ___ cm 3 68 cm 3 = ___ mL = ___ dm 3 = ___ L = ____cc

20. Temperature Conversions Kelvin = Celcius + 273 25 o C = ________ K85 K = ______ o C 218 K = _________- 62 o C = _____K

22. If you want to speed up the particles in matter, you must _________.

23. Liquids Liquid - the state of matter where particles are next to each other, but can move freely. Evaporation – a liquid converting to a gas, but not at its boiling point.

24. Vapor Pressure Vapor Pressure of a liquid – the pressure the vapor produced by a liquid in a sealed container, at equilibrium. Equilibrium – When the speed of evaporation equals the speed of condensation.

25. Vapor Pressure

26. TAKS Questions

30. Solids Solid – the state of matter where particles are next to each other and cannot move around. Most matter that is a solid has very strong(ionic) bonding. Most solids are crystalline(their atoms are arranged in a repeating pattern) Solids which have their atoms randomly arranged are amorphous solids.

31. Phase Changes Phase change – when matter changes its physical state. Examples: Melting(s  l), freezing(l  s), boiling(l  g), condensing(g  l), sublimation(s  g), deposition(g  s)

32. Phase Diagram(Draw on board)