Phases of Matter

1. Phases of Matter

2. ___________ ___________ ___________ ___________ Phases

3. Particles relatively close together • Retains __________________ • Relatively _____ densities • Hard to ____________ • Does not flow easily • Types • Crystalline- regular order/ pattern to particles • Amorphous- no regular pattern to particles Solid

4. Particles more spaced apart • Retains ________________________________ • Intermediate densities • Hard to compress • Flows easily (____________) • Can ________- liquid molecules spread out through another liquid • Can display ______________- attraction of molecules at surface to each other • Can display _______________- attraction of liquid to solid surface causing it to flow Liquid

6. Particles spaced very far apart • Does ____ retain volume or shape • Very low densities • Compressible • Flows easily (fluidity) • Can diffuse and go through _________ • _________ collisions (no loss of energy during collision) • Ideal vs Real Gases • Ideal- no attraction between particles • Real- gases where particles are attracted to each other Gas

7. Occurs at very high _______________________ Also a fluid Mix of neutral atoms, free electrons, and ions Plasma

8. Density • ___________________ property • Mass per unit volume of substance (_____________) • Units • Solids and Liquids • _________________________ • Gases • __________________ • Density controls placement of fluids and solids • Less dense objects or fluids move to the top • More dense objects or fluids move to the bottom

9. D = m/V • Mass • Measured on a _______ • Volume • Solid • Regular Shape- can be __________ from other measurements • Irregular Shape- can be found by ________________________ • Liquid and Gas • Can be measured with instruments such as _________________________ Density (cont)

10. Amount of _____________ transferred from one substance to another Represented by ____ with units in ___________ When heat transfers, it affects the _______________ of the substances Heat

11. Measure of the ________________ in a sample • High temperatures mean the particles are moving __________ • Theoretically if the particles weren’t moving at all, the temperature would be 0 Kelvin (________________) • Remember K = °C + 273.15 Temperature

12. Heat will “flow” from the substance with a __________ temperature to the substance with a _______ temperature As the faster particles collide with slower particles, the faster ones will slow down and the slower ones will speed up Heat Flow

13. When heat transfers, it affects the temperatures of the substances involved in the transfer • How much will the temperature change? • Dependent on • ______________________________ • ______________________________ • _______________________________ Heat and Temperature Change

14. The more heat transferred, the greater the temperature change • If heat is ____________ by the sample • q is ________________ • Final temperature will be higher than the initial temperature • If heat is __________ by the sample • q is _____________ • Final temperature will be lower than the initial temperature Amount of Heat Transferred

15. A heat transfer will cause a bigger temperature change to a smaller mass than it will to a larger mass. Mass of Sample

16. Different substances absorb/release heat in different ways. • _________________(c) – is the amount of heat needed to change 1 gram of a particular substance by 1 °C. • Each type of substance has a different value Composition of the Sample

17. ___________________ • q is __________ • m is _________ • c is ____________________ • T is ___________________________ • Tf-Ti (final temperature – initial temperature) • Units need to match • For instance, if the specific heat value is given in J/g°C, heat should be in J, mass in grams, and temperature in °C Specific Heat Equation

18. Instrument used to measure heat transfer Process allows water and another substance to undergo a heat transfer until both are at the same temperature (thermal equilibrium) This means the heat gained (or lost) by the water equals the heat lost (or gained) by the substance Calorimeters

19. Solid absorbs heat and temperature increases (molecules moving faster) • Reaches a point that movement weakens IMF’s enough to allow flow (melting point) • Heat is still absorbed but temperature does not increase • Liquid absorbs heat and temperature increases (molecules moving faster) • Reaches a point that movement weakens IMF’s enough that they essentially no longer exist (boiling point) • Heat is still absorbed but temperature does not increase • Gas absorbs heat and temperature increases (molecules moving faster) Absorbing Heat

20. Plateaus at melting point • Heat still added • Used to weaken IMF’s • Called Heat of fusion Heating Curve • Another longer plateau will occur between liquid and gas • Called heat of vaporization

21. Heat is released from the gas and temperature decreases (molecules moving slower) • Reaches a point that molecules are close enough for IMF’s to be reestablished (condensation point) • Heat is still released but temperature does not decrease • Heat is released from the liquid and temperature decreases (molecules moving slower) • Reaches a point that molecules are close enough for IMF’s to strengthen (freezing point) • Heat is still released but temperature does not decrease • Heat is removed from the solid Releasing Heat

22. Heating/Cooling Curve

23. Solid  Liquid • Solid  Liquid = ____________ • Liquid  Solid = ____________ • Occurs at melting/ freezing point • Liquid  Gas • Liquid  Gas = _______________________________ • Gas  Liquid = _____________________ • Occurs at boiling/condensation point • Solid  Gas • Solid  Gas = __________________ • Gas  Solid = ___________________ Phase Changes

24. ___________________ • Occurs at temperatures below boiling point • Some molecules have enough energy to escape surface of liquid • ___________________ • Occurs at boiling point • Change to gaseous phase occurs throughout liquid Evaporation or Vaporization

25. Freezing point and Melting point • Same thing (occur at same temperature) • Named depending on the direction compound is going • Condensation point and Boiling point • Same thing (occur at same temperature) • Named depending on the direction compound is going • Each substance has its own points and heats (fusion and vaporization) Phase Change (cont)

26. Same substance • Pressure (mostly sways boiling point) • ________ points are points at standard pressure (1atm) • Lower pressures allow particles to spread out more (IMF’s can be overcome at lower temps) • Higher pressures compress molecules (Higher temp needed to overcome IMF’s) • Between different compounds • Strength of forces holding particles together • Metallic Bonds • Ionic Bonds • Covalent Bonds • IMF’s Influencing Points

27. Vapor pressure- Partial pressure of gas particles of substance over the liquid of that substance • Vapor pressure increases with temperature • More particles have energy to escape surface • Point at which vapor pressure of substance is equal to atmospheric pressure Boiling Point

28. Chart for each substance showing the temperature for phase changes according to pressure Crossing a line indicates a ________________ Phase Diagram

30. At any pressure, a horizontal line can be drawn. • Temperatures of phase changes are found where lines are crossed • The “normal” points are found by drawing a horizontal line at 1atm of pressure Phase Diagrams (cont)

32. ______________ • Pressure and Temperature where all three phases can be found • ________________ • Critical Temperature- highest temperature that the liquid phase of a substance can be found • Critical Pressure- pressure at critical point • Beyond this point the liquid and gas phase in indistinguishable (super critical fluid) Phase Diagrams (cont)