Presentation on theme: "States of Matter: Gases, Liquids, and Solids"— Presentation transcript:
1 States of Matter: Gases, Liquids, and Solids Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.Chapter 6States of Matter:Gases, Liquids, and SolidsDenniston Topping Caret4th Edition
2 6.1 The Gaseous State Ideal Gas Concept Ideal gas - a model of the way that particles of a gas behave at the microscopic level.We can measure the following of a gas:temperature,volume,pressure andquantity (mass)We can systematically change one of the properties and see the effect on each of the others.
3 6.1 The Gaseous State Measurement of Gases The most important gas laws involve the relationship betweennumber of moles (n) of gasvolume (V)temperature (T)pressure (P)Pressure - force per unit area.Gas pressure is a result of force exerted by the collision of particles with the walls of the container.6.1 The Gaseous State
4 6.1 The Gaseous State Barometer - measures atmospheric pressure. Invented by Evangelista TorricelliA commonly used unit of pressure is the atmosphere (atm).1 atm is equal to:760 mmHg760 torr76 cmHg6.1 The Gaseous State
5 6.1 The Gaseous State Boyle’s Law 1 Boyle’s Law - volume of a gas is inversely proportional to pressure if the temperature and number of moles is held constant.6.1 The Gaseous StatePV = k1orPiVi = PfVf
7 Examples using Boyle's Law 21. A 5.0 L sample of a gas at 25oC and 3.0 atm is compressed at constant temperature to a volume of 1.0 L. What is the new pressure?2. A 3.5 L sample of a gas at 1.0 atm is expanded at constant temperature until the pressure is 0.10 atm. What is the volume of the gas?6.1 The Gaseous State
8 6.1 The Gaseous State 1 Charles’ Law Charles’ Law - volume of a gas varies directly with the absolute temperature (K) if pressure and number of moles of gas are constant.6.1 The Gaseous Stateor
10 Examples Using Charles' Law 21. A 2.5 L sample of gas at 25oC is heated to 50oC at constant pressure. Will the volume double?2. What would be the volume in question 1?3. What temperature would be required to double the volume in question 1?6.1 The Gaseous State
11 6.1 The Gaseous State Combined Gas Law 1 This law is used when a sample of gas undergoes change involving volume, pressure, and temperature simultaneously.6.1 The Gaseous State
12 Example Using the Combined Law2Calculate the temperature when a 0.50 L sample of gas at 1.0 atm and 25oC is compressed to 0.05 L of gas at 5.0 atm.6.1 The Gaseous State
13 6.1 The Gaseous State Avogadro’s Law 1 Avogadro’s Law - equal volumes of an ideal gas contain the same number of moles if measured under the same conditions of temperature and pressure.6.1 The Gaseous Stateor
14 Example Using Avogaro's Law 2Assuming no change in temperature and pressure, how many moles of gas would be needed to double the volume occupied by 0.50 moles of gas?6.1 The Gaseous State
15 6.1 The Gaseous State Molar Volume of a Gas Molar Volume - the volume occupied by 1 mol of any gas.STP - Standard Temperature and PressureT = 273 K (or 0oC)P = 1 atmAt STP the molar volume of a gas is 22.4 LWe will learn to calculate the volume later.6.1 The Gaseous State
16 6.1 The Gaseous State Gas Densities We know: density = mass/volume Let’s calculate the density of H2.What is the mass of 1 mol of H2?2.0 gWhat is the volume of 1 mol of H2?22.4 LDensity = 2.0 g/22.4 L = g/L6.1 The Gaseous State
17 6.1 The Gaseous State 1 The Ideal Gas Law Combining Boyle’s Law, Charles’ Law and Avogadro’s Law gives the Ideal Gas Law.6.1 The Gaseous StatePV=nRTR (ideal gas constant) = L.Atm/mol.K
18 Let’s calculate the molar volume at STP using the ideal gas law: PV = nRTWhat would be the pressure?1 atmWhat would be the temperature?273 KWhat would be the number of moles?1 mol26.1 The Gaseous State22.4 L
19 6.1 The Gaseous State Examples using The Ideal Gas Law 1. What is the volume of gas occupied by 5.0 g CH4 at 25oC and 1 atm?2. What is the mass of N2 required to occupy 3.0 L at 100oC and 700 mmHg?6.1 The Gaseous State
20 6.1 The Gaseous State 1 Dalton’s Law of Partial Pressures Dalton’s Law - a mixture of gases exerts a pressure that is the sum of the pressures that each gas would exert if it were present alone under the same conditions.6.1 The Gaseous StatePt=p1+p2+p3+...For example, the total pressure of our atmosphere is equal to the sum of the pressures of N2 and O2.
21 6.1 The Gaseous State 3 Kinetic Molecular Theory of Gases Provides an explanation of the behavior of gases that we have studied in this chapter. Summary follows:1. Gases are made up of small atoms or molecules that are in constant and random motion.2. The distance of separation is very large compared to the size of the atoms or molecules.the gas is mostly empty space.6.1 The Gaseous State
22 6.1 The Gaseous State 3. All gas particles behave independently. No attractive or repulsive forces exist between them.4. Gas particles collide with each other and with the walls of the container without losing energy.The energy is transferred from one atom or molecule to another.5. The average kinetic energy of the atoms or molecules is proportional to absolute temperature.K.E. = 1/2mv2 so as temperature goes up, the speed of the particles goes up.6.1 The Gaseous State
23 4How does the Kinetic Molecular Theory of Gases explain the following statements?Gases are easily compressible.Gases will expand to fill any available volume.Gases have low density.6.1 The Gaseous State
24 Remember: pressure is a force per unit area resulting from collision of gas particles with the walls of the container.If pressure remains constant why does volume increase with temperature?6.1 The Gaseous State
25 Gases behave most ideally at low pressure and high temperatures. Ideal Gases Vs. Real Gases6.1 The Gaseous StateIn reality there is no such thing as an ideal gas. Instead this is a useful model to explain gas behavior.Non-polar gases behave more ideally than polar gases because attractive forces are present in polar gases.
26 6.2 The Liquid State 5 Liquids are practically incompressible. Enables brake fluid to work in your carViscosity - a measure of a liquids resistance to flow.Flow occurs because the molecules can easily slide past each other.Glycerol - example of a very viscous liquid.Viscosity decreases with increased temperature.
27 Surface tension - a measure of the attractive forces exerted among molecules at the surface of a liquid.Surface molecules are surrounded and attracted by fewer liquid molecules than those below.Net attractive forces on surface molecules pull them downward.Results in “beading”Surfactant - substance added which decreases the surface tensionexample: soap6.2 The Liquid State
28 6.2 The Liquid State Vapor Pressure of a Liquid 6 What happens when you put water in a sealed container?Both liquid water and water vapor will exist in the container.How does this happen below the boiling point?Kinetic Theory - Liquid molecules are in continuous motion, with their average kinetic energy directly proportional to the Kelvin temperature.6.2 The Liquid State
29 The green line represents the minimum energy required to break the intermolecular attractions. Even at the cold temp, some molecules can be converted.6.2 The Liquid Stateenergy + H2O(l) H2O(g)
30 Once there are molecules in the vapor phase, they can be converted back to the liquid phase H2O(g) H2O(l) + energy6.2 The Liquid Stateevaporation - the process of conversion of liquid to gas, at a temperature too low to boilcondensation - conversion of the gas to the liquid state.
31 6.2 The Liquid StateWhen the rate of evaporation equals the rate of condensation, the system is at equilibrium.Vapor pressure of a liquid - the pressure exerted by the vapor at equilibriumH2O(g) H2O(l)
32 Boiling point - the temperature at which the vapor pressure of the liquid becomes equal to the atmospheric pressure.Normal boiling point - temperature at which the vapor pressure of the liquid is equal to 1 atm.What happens when you go to a mountain where the atmospheric pressure is lower than 1 atm?The boiling point lowers.6.2 The Liquid State
33 Boiling point is dependant on the intermolecular forces Polar molecules have higher b.p. than nonpolar molecules.6.2 The Liquid State
34 6.2 The Liquid State Van der Waals Forces 7 Van der Waals Forces are types of intermolecular forces.Consists of:Dipole-dipole interactions (section 4.5)London forces6.2 The Liquid State
35 6.2 The Liquid State London forces: Electrons are in constant motion. exist between all molecules,is the only attractive force between nonpolar atoms or molecules,and dipole-dipole attractions occur between polar molecules.Electrons are in constant motion.Electrons can be, in an instant, arranged in such a way that they have a dipole. (Instantaneous dipole)The temporary dipole interacts with other temporary dipoles to cause attraction.6.2 The Liquid State
36 6.2 The Liquid State Hydrogen Bonding 8 Hydrogen bonding: not considered a Van der Waals Forceis a special type of dipole-dipole attractionis a very strong intermolecular attraction causing higher than expected b.p. and m.p.Requirement for hydrogen bonding:molecules have hydrogen directly bonded to O, N, or F6.2 The Liquid State
37 Examples of hydrogen bonding: H2ONH3HF6.2 The Liquid State
38 6.3 The Solid State9Particles highly organized and well defined fashionFixed shape and volumeProperties of Solids:incompressiblem.p. depends on strength of attractive force between particlesCrystalline solid - regular repeating structureAmorphous solid - no organized structure.
39 6.3 The Solid State Types of Crystalline Solids 1. Ionic Solids held together by electrostatic forceshigh m.p. and b.p.hard and brittleif dissolves in water, electrolytesNaCl2. Covalent SolidHeld together entirely by covalent bondsextremely hardDiamond6.3 The Solid State
40 6.3 The Solid State 3. Molecular solids 4. Metallic solids molecules are held together with intermolecular forcesoften softlow m.p.often volatileice4. Metallic solidsmetal atoms held together with metal bondsmetal bondsoverlap of orbitals of metal atomsoverlap causes regions of high electron density where electrons are extremely mobile - conducts electricity6.3 The Solid State
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