1. States of Matter Chapter 12

2. 12.1 - Gases Kinetic molecular theory = describes how gases behave, has 3 major assumptions: Kinetic molecular theory = describes how gases behave, has 3 major assumptions: 1. Particle size = particles are small compared to volume of empty space, no forces between particles 2. Particle motion = particles are in constant motion, move in a straight line until they collide with other particles or container walls, elastic collisions (no loss of kinetic energy)

3. 12.1… 3. Particle energy = determined by mass and velocity of a particle (KE=1/2 mv 2 ) In a sample of a gas, all particles have same mass but different velocity (so KE of particles varies) In a sample of a gas, all particles have same mass but different velocity (so KE of particles varies) Temperature = measure of average KE of particles in a sample (so at a given temp., all particles have same average KE) Temperature = measure of average KE of particles in a sample (so at a given temp., all particles have same average KE)

4. 12.1 – Gas Behavior Low density = lots of space between gas particles Low density = lots of space between gas particles Compression and expansion = empty space in a gas container can easily be pushed into a smaller volume (ex. Squishing memory foam) Compression and expansion = empty space in a gas container can easily be pushed into a smaller volume (ex. Squishing memory foam) Diffusion and effusion = random motion of gas particles causes them to mix until they are evenly distributed Diffusion and effusion = random motion of gas particles causes them to mix until they are evenly distributed

5. 12.1 - Diffusion and Effusion Diffusion = movement of one material through another from area of high concentration to area of low concentration (ex. Spraying perfume) Diffusion = movement of one material through another from area of high concentration to area of low concentration (ex. Spraying perfume) Effusion = gas particles escape through a tiny opening (ex. Popping a balloon) Effusion = gas particles escape through a tiny opening (ex. Popping a balloon) At the same temp., heavier particles effuse/diffuse slower than lighter ones (Graham’s law of effusion: rate is inversely proportional to molar mass. At the same temp., heavier particles effuse/diffuse slower than lighter ones (Graham’s law of effusion: rate is inversely proportional to molar mass.

6. 12.1 – Gas Pressure Pressure = force exerted by gas particles colliding with the walls of the container Pressure = force exerted by gas particles colliding with the walls of the container Barometer = measures atmospheric pressure, height of mercury determined by gravity exerting downward force on mercury and upward force of air pressing down on surface of mercury (increase in air pressure = mercury rises, decrease in air pressure = mercury falls), air pressure depends on temp. and humidity Barometer = measures atmospheric pressure, height of mercury determined by gravity exerting downward force on mercury and upward force of air pressing down on surface of mercury (increase in air pressure = mercury rises, decrease in air pressure = mercury falls), air pressure depends on temp. and humidity

7. 12.1 – Units of Pressure Pascal (Pa) = SI unit of pressure Pascal (Pa) = SI unit of pressure Average air pressure at sea level = Average air pressure at sea level = 760 mm Hg 760 mm Hg 760 torr 760 torr 101.3 kilopascals (kPa) 101.3 kilopascals (kPa) 14.7 psi 14.7 psi One atmosphere (1 atm) One atmosphere (1 atm)

8. Pressure Demos! How to get an egg inside a milk bottle (vacuum inside the bottle) How to get an egg inside a milk bottle (vacuum inside the bottle) How to get an egg inside a milk bottle (vacuum inside the bottle) How to get an egg inside a milk bottle (vacuum inside the bottle) How to make a film canister explode (vacuum outside the canister) How to make a film canister explode (vacuum outside the canister) Extreme Shaving Cream Extreme Shaving Cream Monster Marshmallows Monster Marshmallows

9. 12.1 – Dalton’s Law of Partial Pressures Dalton’s Law of Partial Pressures = total pressure of a mixture of gases is equal to the sum of the pressures of all gases in the mixture Dalton’s Law of Partial Pressures = total pressure of a mixture of gases is equal to the sum of the pressures of all gases in the mixture Portion of the total pressure contributed by one gas is called its partial pressure Portion of the total pressure contributed by one gas is called its partial pressure Partial pressure of a gas depends on the number of moles of gas, size of the container, and temp. Partial pressure of a gas depends on the number of moles of gas, size of the container, and temp.

10. 12.2 – Forces of Attraction Intramolecular forces = attractive forces that hold particles together (bonds) Intramolecular forces = attractive forces that hold particles together (bonds) Intermolecular forces = attractive forces between particles Intermolecular forces = attractive forces between particles

11. 12.2 – Intermolecular Forces Dispersion forces = weak force between two non-polar molecules (those with evenly distributed electrons) Dispersion forces = weak force between two non-polar molecules (those with evenly distributed electrons) Electrons always moving, electron clouds of non-polar molecules repel each other Electrons always moving, electron clouds of non-polar molecules repel each other Electron density around the nucleus shifts so one side of the molecule is more negative than the other Electron density around the nucleus shifts so one side of the molecule is more negative than the other Leads to weak attraction between these temporary dipoles Leads to weak attraction between these temporary dipoles

12. 12.2 – Dispersion Forces

13. 12.2 – Intermolecular Forces… Dipole-Dipole forces = forces between oppositely charged regions of polar molecules (permanent dipoles) Dipole-Dipole forces = forces between oppositely charged regions of polar molecules (permanent dipoles) Ex. HCl Ex. HCl Partially positive H in one molecule of HCl lines up with partially negative Cl in another molecule Partially positive H in one molecule of HCl lines up with partially negative Cl in another molecule

14. 12.2 – Intermolecular Forces… Hydrogen bonds = a type of dipole-dipole attraction between molecules that contain hydrogen and a highly electronegative atom with at least one lone pair Hydrogen bonds = a type of dipole-dipole attraction between molecules that contain hydrogen and a highly electronegative atom with at least one lone pair Explains why water is a liquid at room temperature and not a gas  life on Earth! Explains why water is a liquid at room temperature and not a gas  life on Earth! Hydrogen atom has large partial positive charge and is attracted to oxygen’s large partial negative charge on another molecule Hydrogen atom has large partial positive charge and is attracted to oxygen’s large partial negative charge on another molecule

15. 12.2 – Hydrogen Bonds Hydrogen BondsHydrogen Bonds

16. 12.3 – Liquids and Solids

17. 12.3 – Liquids and Solids… Liquids are much denser than gases due to intermolecular forces that hold particles together Liquids are much denser than gases due to intermolecular forces that hold particles together Liquids cannot be compressed as much as gases because particles are already closely packed together Liquids cannot be compressed as much as gases because particles are already closely packed together Molecules in a liquid Molecules in a liquid Molecules in a liquid Molecules in a liquid

18. 12.3 – Liquids and Solids… Fluidity = ability to flow, both gases and liquids are considered fluids because they can diffuse through one another Fluidity = ability to flow, both gases and liquids are considered fluids because they can diffuse through one another Liquids are less fluid than gases due to intermolecular forces that slow down their movement Liquids are less fluid than gases due to intermolecular forces that slow down their movement Ex. Water pipe leak vs. natural gas leak Ex. Water pipe leak vs. natural gas leak

19. 12.3 – Liquids and Solids… Viscosity = resistance of a liquid to flow Viscosity = resistance of a liquid to flow Stronger intermolecular forces  higher viscosity Stronger intermolecular forces  higher viscosity Bigger molecules  higher viscosity Bigger molecules  higher viscosity Lower temperature  higher viscosity Lower temperature  higher viscosity Ex. Motor oil = need less viscous oil in winter to make sure it keeps flowing at low temperatures, need more viscous oil in summer to make sure it stays thick enough to lubricate the engine at very high temperatures Ex. Motor oil = need less viscous oil in winter to make sure it keeps flowing at low temperatures, need more viscous oil in summer to make sure it stays thick enough to lubricate the engine at very high temperatures

20. 12.3 – Liquids and Solids Surface tension = energy required to increase surface area of a liquid by a given amount Surface tension = energy required to increase surface area of a liquid by a given amount Stronger attractions between particles  higher surface tension Stronger attractions between particles  higher surface tension Water has a very high surface tension due to hydrogen bonding, allows small insects to walk on water, why we need water AND soap to clean dishes/clothes Water has a very high surface tension due to hydrogen bonding, allows small insects to walk on water, why we need water AND soap to clean dishes/clothes Surface tension of water Surface tension of water Surface tension of water Surface tension of water Magic milk Magic milk Magic milk Magic milk

21. 12.3 – Liquids and Solids… Capillary action = occurs when adhesion to walls of container is greater than cohesion in the liquid Capillary action = occurs when adhesion to walls of container is greater than cohesion in the liquid Adhesion = force of attraction between molecules that are different Adhesion = force of attraction between molecules that are different Cohesion = force of attraction between identical molecules Cohesion = force of attraction between identical molecules Ex. Meniscus in graduated cylinder, absorbance of paper towels and diapers Ex. Meniscus in graduated cylinder, absorbance of paper towels and diapers

22. 12.3 – Liquids and Solids… Solids = not considered to be fluids, very ordered, more dense than liquids because particles are more closely packed together Solids = not considered to be fluids, very ordered, more dense than liquids because particles are more closely packed together Exception = water, solid ice is less dense than liquid water due to three dimensional structure of water molecules (ice cubes and glaciers float, keeps aquatic life alive in the winter) Exception = water, solid ice is less dense than liquid water due to three dimensional structure of water molecules (ice cubes and glaciers float, keeps aquatic life alive in the winter) Why ice floats... Why ice floats... Why ice floats... Why ice floats...

23. 12.3 – Liquids and Solids… Crystalline solids = atoms, ions, or molecules arranged in an orderly, geometric, 3-D structure Crystalline solids = atoms, ions, or molecules arranged in an orderly, geometric, 3-D structure Individual pieces are called crystals Individual pieces are called crystals Unit cell = smallest part of a crystal retaining the crystal shape Unit cell = smallest part of a crystal retaining the crystal shape Molecules in solids Molecules in solids Molecules in solids Molecules in solids

24. 12.3 – Liquids and Solids 4 types of crystalline solids: 4 types of crystalline solids: Molecular solids = soft, poor conductors of heat and electricity, low to moderate melting points Molecular solids = soft, poor conductors of heat and electricity, low to moderate melting points Allotropes = 2 different solid forms of the same element (ex. Carbon as graphite or diamond), very hard, poor conductors, high melting points Allotropes = 2 different solid forms of the same element (ex. Carbon as graphite or diamond), very hard, poor conductors, high melting points Ionic solids = hard, brittle, poor conductors, high melting points Ionic solids = hard, brittle, poor conductors, high melting points Metallic solids = soft to hard, excellent conductors, low to high melting points Metallic solids = soft to hard, excellent conductors, low to high melting points

25. 12.3 – Liquids and Solids… Amorphous solids = do not contain crystals, no repeating pattern, form when a molten material cools too quickly Amorphous solids = do not contain crystals, no repeating pattern, form when a molten material cools too quickly Ex. Glass, rubber, plastics Ex. Glass, rubber, plastics

26. 12.4 – Phase Changes Intro to phase changes Intro to phase changes Intro to phase changes Intro to phase changes

27. 12.4 – Phase Changes Why do substances melt? Why do substances melt? As molecules are heated, they gain enough KE to overcome attractive forces that hold them together as a solid As molecules are heated, they gain enough KE to overcome attractive forces that hold them together as a solid Melting point = temperature at which forces holding crystal lattice together are broken and solid becomes liquid Melting point = temperature at which forces holding crystal lattice together are broken and solid becomes liquid REQUIRES energy REQUIRES energy

28. 12.4 – Phase Changes Why do substances freeze? Why do substances freeze? As heat is removed, molecules lose KE and slow down As heat is removed, molecules lose KE and slow down Freezing point = temperature at which a liquid is converted into a crystalline solid Freezing point = temperature at which a liquid is converted into a crystalline solid RELEASES energy RELEASES energy

29. 12.4 – Phase Changes Why do liquids become gases? Why do liquids become gases? When energy is added to a liquid, the temperature increases and molecules gain KE and escape the liquid When energy is added to a liquid, the temperature increases and molecules gain KE and escape the liquid Vaporization = process by which a liquid changes to a gas or vapor Vaporization = process by which a liquid changes to a gas or vapor Evaporation = vaporization that occurs on the surface of a liquid that is not boiling Evaporation = vaporization that occurs on the surface of a liquid that is not boiling REQUIRES energy REQUIRES energy

30. 12.4 – Phase Changes… Vapor pressure = pressure exerted by a vapor over a liquid Vapor pressure = pressure exerted by a vapor over a liquid Boiling point = temperature at which vapor pressure of a liquid is equal to atmospheric pressure, molecules throughout the liquid have enough energy to vaporize and bubbles of vapor rise to the surface Boiling point = temperature at which vapor pressure of a liquid is equal to atmospheric pressure, molecules throughout the liquid have enough energy to vaporize and bubbles of vapor rise to the surface Water boiling in a vacuum Demo! Water boiling in a vacuum Demo!

31. 12.4 – Phase Changes… Why do gases become liquids? Why do gases become liquids? When a vapor molecule loses energy, it slows down and is more likely to collide with another molecule and bond, releasing energy and becoming a liquid When a vapor molecule loses energy, it slows down and is more likely to collide with another molecule and bond, releasing energy and becoming a liquid Condensation = Process by which a gas or vapor becomes a liquid Condensation = Process by which a gas or vapor becomes a liquid RELEASES energy RELEASES energy Evaporation and Condensation Evaporation and Condensation Evaporation and Condensation Evaporation and Condensation

32. 12.4 – Phase Changes… What happens when we sweat? What happens when we sweat? Water molecules in sweat gain energy from heat coming off the body Water molecules in sweat gain energy from heat coming off the body Some molecules gain enough energy to evaporate, taking energy with them Some molecules gain enough energy to evaporate, taking energy with them Molecules left behind have less energy and therefore, a lower temperature Molecules left behind have less energy and therefore, a lower temperature

33. 12.4 – Phase Changes… Sublimation = solid changes directly to a gas without passing through the liquid phase Sublimation = solid changes directly to a gas without passing through the liquid phase Ex. Dry ice Ex. Dry ice REQUIRES energy REQUIRES energy Deposition = gas or vapor changes directly to a solid without passing through the liquid phase Deposition = gas or vapor changes directly to a solid without passing through the liquid phase

34. 12.4 – Phase Changes Phase diagram = Pressure vs. Temperature, shows relationship between pressure/temperature/phase of a substance Phase diagram = Pressure vs. Temperature, shows relationship between pressure/temperature/phase of a substance Triple point = point on the diagram that shows the temp. and pressure at which all three phases can exist in equilibrium with eachother Triple point = point on the diagram that shows the temp. and pressure at which all three phases can exist in equilibrium with eachother Critical point = point on the diagram that shows the temp. and pressure at which water can no longer exist as a liquid Critical point = point on the diagram that shows the temp. and pressure at which water can no longer exist as a liquid

35. 12.4 - Phase Diagram