Chapter 10: Liquids, Solids, and Phase Changes

Size: px
Start display at page:

Download "Chapter 10: Liquids, Solids, and Phase Changes"

Transcription

1 Chapter 10: Liquids, Solids, and Phase Changes In-chapter exercises: , 10.11; End-of-chapter Problems: 10.26, 10.31, 10.32, 10.33, 10.34, 10.35, 10.36, 10.39, 10.40, 10.42, 10.44, 10.45, 10.66, 10.82, 10.84, Kinetic Molecular Theory of Liquids and Solids phase (=physical state): solid, liquid, or gas Solids have the lowest kinetic energy (KE) i.e. do not move very much Highest attraction between particles particles are stuck in specific sites = very confined Liquids have slightly higher KE i.e. particles moving more than in solid Particles are still attracted and maintain contact with one another but can move past one another particles are less confined Gases have greatest KE i.e. particles move quickly and randomly Attractive forces almost (if not) completely overcome, so particles can fly freely within container particles are far away from each other = unrestricted 10.2 INTERMOLECULAR FORCES intermolecular forces: Attractive forces between 2 molecules e.g. between 2 water molecules Ion-Dipole Forces Attraction between an ion and the oppositely charged end of a polar molecule e.g. between Na + and the negative end of a H 2 O molecule (O in H 2 O) or between Cl and the positive end of a H 2 O molecule (H atoms in H 2 O) CHM 150 Chapter 10 McMurry-Fay Notes page 1 of 14

2 Dispersion (London or Induced-Dipole) Forces Attraction between temporary or induced dipoles in adjacent molecules Electrons constantly shift and can sometimes concentrate in one region instantaneous dipole that goes away once electrons shift again Chocolate-chip cookie dough analogy Most common type and weakest of intermolecular forces, found between all types of molecules Only type of intermolecular force between nonpolar molecules In general, larger molecules w/ more electrons are more polarizable polarizable = tendency to experience electron shifts that result in charges the larger the molecule, the stronger the dispersion forces Dispersion (Induced-dipole) Forces Electrons shift in one molecule and concentrate on one side temporary dipole (light area = +ve; dark area = ve) The temporary dipole causes electrons to shift in adjacent molecules another temporary dipole When electrons shift again, the temporary dipoles go away. Dipole-Dipole Forces: Attraction between polar molecules generally stronger than dispersion forces because attraction is due to permanent dipoles rather than temporary dipoles Note: Van der Waals forces refer to intermolecular forces due to either London dispersion forces or dipole-dipole forces. Hydrogen Bonds: CHM 150 Chapter 10 McMurry-Fay Notes page 2 of 14

3 Exist between molecules with following bonds: H F, H O, H N Special type of dipole-dipole force caused by small radii and large electronegativity differences between H and O, N, and F atoms strongest type of intermolecular force Responsible for the relatively high melting and boiling points for water, bending and twisting in proteins, DNA, and other important biological molecules Note: Hydrogen bonds are the strongest type of intermolecular force but ionic and covalent bonds are stronger than hydrogen bonds. How to determine type of intermolecular forces involved: yes hydrogen bonding Is the molecule polar or nonpolar polar nonpolar Are there H F, H O, or H N bonds dispersion (London) forces no dipole-dipole forces Example: For each of the following, identify the type of bond holding atoms together in the molecules and the type of intermolecular forces between the molecules. A B A: B: CHM 150 Chapter 10 McMurry-Fay Notes page 3 of 14

4 A B A: B: Ex. 2: Consider the following six choices: A. ionic bond D. dispersion (induced-dipole) forces B. polar covalent bond E. dipole-dipole forces C. nonpolar covalent bond F. hydrogen bond Identify the type of bond or intermolecular force described for each below: a. The C C bond in C 2 H 6. b. The bonds in NaCl. c. The bonds holding HBr molecules together. d. The bonds holding atoms together in a water molecule. e. The bonds holding two NH 3 molecules together. f. The bonds holding atoms together in a HF molecule. g. The bonds broken when KBr dissolves in water. h. The bonds formed when KBr dissolves in water. Ex. 3 Circle the molecule in each pair which experiences the stronger intermolecular forces: a. N 2 or NO b. H 2 S or H 2 O c. Cl 2 or Br 2 CHM 150 Chapter 10 McMurry-Fay Notes page 4 of 14

5 10.3 SOME PROPERTIES OF LIQUIDS 10.5 EVAPORATION, VAPOR PRESSURE, AND BOILING POINT evaporation: for a liquid to vaporize, the surface molecules must break the intermolecular forces with other molecules in the liquid at the boiling point, molecules have enough energy to break the intermolecular forces with other molecules and become gas Boiling Point: temperature where vapor pressure of liquid is equal to external pressure (usually atmospheric pressure) stronger intermolecular forces more energy is required to break intermolecular bonds between molecules in the liquid higher boiling point normal boiling point is the boiling point at a pressure of 1 atm e.g. water boils at 100 C at 1 atm, but it boils at ~95 C in Denver where the atmospheric pressure is ~0.85 atm Vapor Pressure: partial pressure exerted by gas molecules above the liquid varies for different liquids, varies for different temperatures more gas molecules higher vapor pressure The weaker the intermolecular forces more molecules can go from liquid to vapor higher vapor pressure In the examples below, liquid A has weaker intermolecular forces than B A B Viscosity: resistance of a liquid to flow for example, honey has high viscosity; water has low viscosity stronger intermolecular forces = stronger attraction higher viscosity CHM 150 Chapter 10 McMurry-Fay Notes page 5 of 14

6 Surface Tension: attraction between surface molecules in a liquid stronger intermolecular forces = stronger attraction surface molecules are held together more strongly higher surface tension Ex. 1: Water molecules experience hydrogen bonding and hexane molecules experience induced-dipole (or dispersion) forces. Which of the following statements are true/false? a. Water's intermolecular forces are weaker than hexane's. T F b. Hexane s vapor pressure is higher than water s. T F c. Hexane s boiling point is lower than water s. T F d. Water s surface tension is higher than hexane s. T F e. Water s viscosity is lower than hexane s. T F Ex. 2: Explain each the following in terms of intermolecular forces: a. Why O 2 's boiling point is -183 C while NO's boiling point is -151 C. b. Why N 2 's boiling point is -196 C while Br 2 's boiling point is 59 C. c. Why H 2 S s boiling point is 61 C and H 2 O s boiling point is 100 C. CHM 150 Chapter 10 McMurry-Fay Notes page 6 of 14

7 10.6 KINDS OF SOLIDS Crystalline Solids: Have an ordered arrangement extending over a long range different types of crystalline solids: molecular solids, covalent network solids, ionic and metallic solids. Molecular Solids: consist of molecules held together by intermolecular forces The Structure and Properties of Ice Ice is an example of a molecular solid. The hydrogen bonds between water molecules are responsible for many unusual properties of ice and water. The density of ice (d=0.917 g/cm 3 ) is less than the density of liquid water (d=1.00 g/cm 3 ). With all other substances, the solid is more dense than its liquid. The density of ice (d=0.917 g/cm 3 ) is less than the density of liquid water (d=1.000 g/cm 3 ) whereas for all other substances, the solid is more dense than its liquid. Because of the hydrogen bonds, the arrangement of water molecules in ice crystal has "holes" or empty space. When ice melts, the water molecules fill in the holes, so liquid water is more dense than ice. Note the hexagonal holes in the molecular-level image above. Snowflakes have hexagonal symmetry because of the hexagonal holes in the molecular-level arrangement of water molecules in ice! CHM 150 Chapter 10 McMurry-Fay Notes page 7 of 14

8 Ionic Crystals: lattice of metal & nonmetal ions e.g. NaCl, MgO, CaBr 2 3D network of ions held together by electrostatic attraction high melting points, hard and brittle conduct electricity when melted or dissolved in solution STRUCTURE OF SOME COVALENT NETWORK SOLIDS Covalent Network Solids are covalently bonded atoms that form a large network of indefinite size. (a) Graphite is made up of covalently bonded carbon atoms that form layers of sp 2 hybridized carbon atoms. (b) Diamond is made up of covalently bonded carbon atoms that form such a network of sp 3 hybridized carbon atoms in 3D tetrahedral structure. Diamond is so hard because so many covalent bonds must be broken to break up the diamond crystal. CHM 150 Chapter 10 McMurry-Fay Notes page 8 of 14

9 Fullerenes are a class of covalently bonded carbon atoms, similar to graphite. (a) C 60 has a shape similar to a soccer ball and is often called a Buckyball. (b) Nanotubes consist of sheets of graphite rolled into tubes. up to ten times as strong as steel Amorphous Solids: solids lacking 3D arrangement of atoms Silica (SiO 2 ) makes up sand and quartz glass: optically transparent solid of inorganic materials cooled to a rigid but non-crystalline arrangement of Si-O bonded atoms called quartz glass CHM 150 Chapter 10 McMurry-Fay Notes page 9 of 14

10 10.7 Probing the Structure of Solids: X-Ray Crystallography X-ray diffraction: scattering of X-rays by units of a solid crystal we can construct electron density contour map, where maximum densities are near center of each atom can be used to determine the positions of nuclei bond lengths and bond angles in crystals Metallic Crystals: positive metal ions surrounded by a sea of electrons electrons are delocalized i.e. free to move around the entire metal electrons move freely throughout the metal resulting in good heat and electrical conductivity electrons act as a glue holding nuclei together, so shape of metal can be easily manipulated metals are malleable and ductile some metals will react with water but are never soluble in water or other solvents 10.4 Phase Changes: change from one physical state to another sublimation SOLID fusion freezing LIQUID vaporization condensation GAS deposition The Equilibrium Nature of Phase Changes dynamic equilibrium: rate of forward process is exactly equal to the rate of reverse process CHM 150 Chapter 10 McMurry-Fay Notes page 10 of 14

11 Liquid-Solid Equilibrium freezing: liquid solid melting (or fusion): solid liquid melting point: temperature at which solid and liquid phases coexist in equilibrium normal melting point is melting point at 1 atm Consider solid-liquid equilibrium of water and ice (at 0 C and 1 atm): ice water When ice cubes are placed into a glass of water, the ice cubes begin to melt, but some water between the ice cubes freezes, causing ice cubes to fuse molar heat of fusion ( H fus ): energy required to melt one mole of solid supercooling: a substance remains liquid even below its freezing point results when a liquid is cooled so rapidly that molecules don't have time to arrange themselves properly unstable condition; stirring or adding "seed" crystal causes solidification For example, supercooling can happen in your refrigerator. A bottle of carbonated soda can be supercooled, so when you pick it up, you give it enough energy to freezes instantly ice crystals form Liquid-Gas Equilibrium: liquid vapor evaporation (or vaporization): liquid vapor condensation: vapor liquid the process of a gas liquefying can result from two ways: 1. cooling sample of gas lower KE, and molecules start to aggregate to form small drops of liquid, eventually causing condensation 2. applying pressure to gas minimize space between molecules, so molecules are attracted to each other to form droplets, eventually causing condensation CHM 150 Chapter 10 McMurry-Fay Notes page 11 of 14

12 Solid-Gas Equilibrium: Consider the dynamic equilibrium: solid vapor For example, dry ice, CO 2 (s), sublimes at room temperature, completely skipping a liquid phase. sublimation: solid gas (with no liquid phase) deposition: gas solid (with no liquid phase) molar heat of sublimation ( H sub ): energy required to sublime one mole of solid Heat of Phase Transition heating-cooling curve: Shows the phase changes that occur when heat is added or removed from a sample Temperature ( C) Heat Added Draw a heating curve indicating the following: 1. Regions for solid only, liquid only, gas only, solid-liquid, liquid-gas 2. The relationship between melting point and phases present 3. The relationship between boiling point and phases present 4. Where the curve is flat, where the slope is positive CHM 150 Chapter 10 McMurry-Fay Notes page 12 of 14

13 10.11 Phase Diagrams summarize the conditions at which a substance exists as solid, liquid, or gas allow us to determine melting and boiling points at different external pressures Water s phase diagram is shown in Fig graph divided into three regions corresponding to each phase lines separating two regions indicate conditions when both phases exist triple point: point at which all three curves meet when all three phases exist in equilibrium with one another for water, at C and about atm Phase Diagram for Water (Fig ) Phase Diagram for CO 2 (Fig ) CHM 150 Chapter 10 McMurry-Fay Notes page 13 of 14

14 Phase Diagram for Water versus that for CO 2 : Note that line separating solid and liquid phases has positive slope for CO 2 but negative slope for H 2 O for CO 2, the solid is more dense than the liquid, so increasing pressure converts the liquid to a solid for H 2 O, the solid is less dense than the liquid, so increasing pressure converts the solid to a liquid Critical Temperature and Pressure: critical temperature (T c ): above which its gas form cannot be made to liquefy, no matter how great the applied pressure highest temperature at which a substance can exist as a liquid intermolecular attraction is a finite quantity for given substance below T c, molecules are moving slowly enough to maintain contact above Tc, molecular motion so energetic that molecules will always break away from attraction critical pressure (P c ): minimum pressure that must be applied to liquefy sample at the critical temperature Given a Phase Diagram, be able to do the following: Determine what phase(s) is/are present at a given temperature and pressure Indicate the melting point or boiling point at a given pressure e.g. the normal melting or boiling point Describe what phase change occurs when temperature is changed at a constant pressure Describe what phase change occurs when pressure is changed at a constant temperature. CHM 150 Chapter 10 McMurry-Fay Notes page 14 of 14

London Dispersion Forces (LDFs) Intermolecular Forces Attractions BETWEEN molecules. London Dispersion Forces (LDFs) London Dispersion Forces (LDFs)

London Dispersion Forces (LDFs) Intermolecular Forces Attractions BETWEEN molecules. London Dispersion Forces (LDFs) London Dispersion Forces (LDFs) LIQUIDS / SOLIDS / IMFs Intermolecular Forces (IMFs) Attractions BETWEEN molecules NOT within molecules NOT true bonds weaker attractions Represented by dashed lines Physical properties (melting points,

More information

Chapter 11. Intermolecular Forces and Liquids & Solids

Chapter 11. Intermolecular Forces and Liquids & Solids Chapter 11 Intermolecular Forces and Liquids & Solids The Kinetic Molecular Theory of Liquids & Solids Gases vs. Liquids & Solids difference is distance between molecules Liquids Molecules close together;

More information

- intermolecular forces forces that exist between molecules

- intermolecular forces forces that exist between molecules Chapter 11: Intermolecular Forces, Liquids, and Solids - intermolecular forces forces that exist between molecules 11.1 A Molecular Comparison of Liquids and Solids - gases - average kinetic energy of

More information

The Liquid and Solid States

The Liquid and Solid States : The Liquid and Solid States 10-1 10.1 Changes of State How do solids, liquids and gases differ? Figure 10.4 10-2 1 10.1 Changes of State : transitions between physical states Vaporization/Condensation

More information

compared to gases. They are incompressible. Their density doesn t change with temperature. These similarities are due

compared to gases. They are incompressible. Their density doesn t change with temperature. These similarities are due Liquids and solids They are similar compared to gases. They are incompressible. Their density doesn t change with temperature. These similarities are due to the molecules being close together in solids

More information

Chemistry 101 Chapter 14 Liquids & Solids

Chemistry 101 Chapter 14 Liquids & Solids Chemistry 101 Chapter 14 Liquids & Solids States of matter: the physical state of matter depends on a balance between the kinetic energy of particles, which tends to keep them apart, and the attractive

More information

Intermolecular Forces and Liquids and Solids. Chapter 11. Copyright The McGraw Hill Companies, Inc. Permission required for

Intermolecular Forces and Liquids and Solids. Chapter 11. Copyright The McGraw Hill Companies, Inc. Permission required for Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw Hill Companies, Inc. Permission required for 1 A phase is a homogeneous part of the system in contact with other parts of the

More information

The Liquid and Solid States

The Liquid and Solid States : The Liquid and Solid States 10-1 10.1 Changes of State How do solids, liquids and gases differ? Figure 10.4 10-2 10.1 Changes of State : transitions between physical states Vaporization/Condensation

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A phase is a homogeneous part of the system in contact

More information

They are similar to each other

They are similar to each other They are similar to each other Different than gases. They are incompressible. Their density doesn t change much with temperature. These similarities are due to the molecules staying close together in solids

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids PowerPoint Lecture Presentation by J. David Robertson University of Missouri Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction

More information

They are similar to each other. Intermolecular forces

They are similar to each other. Intermolecular forces s and solids They are similar to each other Different than gases. They are incompressible. Their density doesn t change much with temperature. These similarities are due to the molecules staying close

More information

Chapter 12. Insert picture from First page of chapter. Intermolecular Forces and the Physical Properties of Liquids and Solids

Chapter 12. Insert picture from First page of chapter. Intermolecular Forces and the Physical Properties of Liquids and Solids Chapter 12 Insert picture from First page of chapter Intermolecular Forces and the Physical Properties of Liquids and Solids Copyright McGraw-Hill 2009 1 12.1 Intermolecular Forces Intermolecular forces

More information

Intermolecular Forces and Liquids and Solids

Intermolecular Forces and Liquids and Solids Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 A phase is a homogeneous part of the system in contact

More information

Liquids & Solids. Mr. Hollister Holliday Legacy High School Regular & Honors Chemistry

Liquids & Solids. Mr. Hollister Holliday Legacy High School Regular & Honors Chemistry Liquids & Solids Mr. Hollister Holliday Legacy High School Regular & Honors Chemistry 1 Liquids 2 Properties of the States of Matter: Liquids High densities compared to gases. Fluid. The material exhibits

More information

Chapters 11 and 12: Intermolecular Forces of Liquids and Solids

Chapters 11 and 12: Intermolecular Forces of Liquids and Solids 1 Chapters 11 and 12: Intermolecular Forces of Liquids and Solids 11.1 A Molecular Comparison of Liquids and Solids The state of matter (Gas, liquid or solid) at a particular temperature and pressure depends

More information

CHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS. Chemistry 1411 Joanna Sabey

CHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS. Chemistry 1411 Joanna Sabey CHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS Chemistry 1411 Joanna Sabey Forces Phase: homogeneous part of the system in contact with other parts of the system but separated from them by a

More information

Chapter 10. Dipole Moments. Intermolecular Forces (IMF) Polar Bonds and Polar Molecules. Polar or Nonpolar Molecules?

Chapter 10. Dipole Moments. Intermolecular Forces (IMF) Polar Bonds and Polar Molecules. Polar or Nonpolar Molecules? Polar Bonds and Polar Molecules Chapter 10 Liquids, Solids, and Phase Changes Draw Lewis Structures for CCl 4 and CH 3 Cl. What s the same? What s different? 1 Polar Covalent Bonds and Dipole Moments Bonds

More information

Intermolecular forces Liquids and Solids

Intermolecular forces Liquids and Solids Intermolecular forces Liquids and Solids Chapter objectives Understand the three intermolecular forces in pure liquid in relation to molecular structure/polarity Understand the physical properties of liquids

More information

Chapter 10: Liquids and Solids

Chapter 10: Liquids and Solids Chapter 10: Liquids and Solids Chapter 10: Liquids and Solids *Liquids and solids show many similarities and are strikingly different from their gaseous state. 10.1 Intermolecular Forces Intermolecular

More information

Intermolecular Forces and Liquids and Solids Chapter 11

Intermolecular Forces and Liquids and Solids Chapter 11 Intermolecular Forces and Liquids and Solids Chapter 11 A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well defined boundary. Phases

More information

Liquids, Solids and Phase Changes

Liquids, Solids and Phase Changes Chapter 10 Liquids, Solids and Phase Changes Chapter 10 1 KMT of Liquids and Solids Gas molecules have little or no interactions. Molecules in the Liquid or solid state have significant interactions. Liquids

More information

INTERMOLECULAR FORCES: LIQUIDS, SOLIDS & PHASE CHANGES (Silberberg, Chapter 12)

INTERMOLECULAR FORCES: LIQUIDS, SOLIDS & PHASE CHANGES (Silberberg, Chapter 12) INTERMOLECULAR FORCES: LIQUIDS, SOLIDS & PASE CANGES (Silberberg, Chapter 12) Intermolecular interactions Ideal gas molecules act independently PV=nRT Real gas molecules attract/repulse one another 2 n

More information

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces. John D. Bookstaver St. Charles Community College Cottleville, MO

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces. John D. Bookstaver St. Charles Community College Cottleville, MO Lecture Presentation Chapter 11 Liquids and Intermolecular Forces John D. Bookstaver St. Charles Community College Cottleville, MO Properties of Gases, Liquids, and Solids State Volume Shape of State Density

More information

Chapter 10: States of Matter. Concept Base: Chapter 1: Properties of Matter Chapter 2: Density Chapter 6: Covalent and Ionic Bonding

Chapter 10: States of Matter. Concept Base: Chapter 1: Properties of Matter Chapter 2: Density Chapter 6: Covalent and Ionic Bonding Chapter 10: States of Matter Concept Base: Chapter 1: Properties of Matter Chapter 2: Density Chapter 6: Covalent and Ionic Bonding Pressure standard pressure the pressure exerted at sea level in dry air

More information

2. As gas P increases and/or T is lowered, intermolecular forces become significant, and deviations from ideal gas laws occur (van der Waal equation).

2. As gas P increases and/or T is lowered, intermolecular forces become significant, and deviations from ideal gas laws occur (van der Waal equation). A. Introduction. (Section 11.1) CHAPTER 11: STATES OF MATTER, LIQUIDS AND SOLIDS 1. Gases are easily treated mathematically because molecules behave independently. 2. As gas P increases and/or T is lowered,

More information

CHAPTER ELEVEN KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS

CHAPTER ELEVEN KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS CHAPTER ELEVEN AND LIQUIDS AND SOLIDS KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS Differences between condensed states and gases? KINETIC MOLECULAR THEORY OF LIQUIDS AND SOLIDS Phase Homogeneous part

More information

Chapter 11. Liquids and Intermolecular Forces

Chapter 11. Liquids and Intermolecular Forces Chapter 11 Liquids and Intermolecular Forces States of Matter The three states of matter are 1) Solid Definite shape Definite volume 2) Liquid Indefinite shape Definite volume 3) Gas Indefinite shape Indefinite

More information

CHAPTER 13. States of Matter. Kinetic = motion. Polar vs. Nonpolar. Gases. Hon Chem 13.notebook

CHAPTER 13. States of Matter. Kinetic = motion. Polar vs. Nonpolar. Gases. Hon Chem 13.notebook CHAPTER 13 States of Matter States that the tiny particles in all forms of matter are in constant motion. Kinetic = motion A gas is composed of particles, usually molecules or atoms, with negligible volume

More information

Chapter 11. Intermolecular Forces, Liquids, and Solids

Chapter 11. Intermolecular Forces, Liquids, and Solids Chapter 11. Intermolecular Forces, Liquids, and Solids A Molecular Comparison of Gases, Liquids, and Solids Physical properties of substances are understood in terms of kinetic-molecular theory: Gases

More information

Chapter 11. Kinetic Molecular Theory. Attractive Forces

Chapter 11. Kinetic Molecular Theory. Attractive Forces Chapter 11 KMT for Solids and Liquids Intermolecular Forces Viscosity & Surface Tension Phase Changes Vapor Pressure Phase Diagrams Solid Structure Kinetic Molecular Theory Liquids and solids will experience

More information

Chapter 11. Liquids and Intermolecular Forces

Chapter 11. Liquids and Intermolecular Forces Chapter 11. Liquids and Intermolecular Forces 11.1 A Molecular Comparison of Gases, Liquids, and Solids Gases are highly compressible and assume the shape and volume of their container. Gas molecules are

More information

Chapter 10. Lesson Starter. Why did you not smell the odor of the vapor immediately? Explain this event in terms of the motion of molecules.

Chapter 10. Lesson Starter. Why did you not smell the odor of the vapor immediately? Explain this event in terms of the motion of molecules. Preview Lesson Starter Objectives The Kinetic-Molecular Theory of Gases The Kinetic-Molecular Theory and the Nature of Gases Deviations of Real Gases from Ideal Behavior Section 1 The Kinetic-Molecular

More information

Chapter 10 Liquids and Solids. Problems: 14, 15, 18, 21-23, 29, 31-35, 37, 39, 41, 43, 46, 81-83, 87, 88, 90-93, 99, , 113

Chapter 10 Liquids and Solids. Problems: 14, 15, 18, 21-23, 29, 31-35, 37, 39, 41, 43, 46, 81-83, 87, 88, 90-93, 99, , 113 Chapter 10 Liquids and Solids Problems: 14, 15, 18, 21-23, 29, 31-35, 37, 39, 41, 43, 46, 81-83, 87, 88, 90-93, 99, 104-106, 113 Recall: Intermolecular vs. Intramolecular Forces Intramolecular: bonds between

More information

Chapter 10. The Liquid and Solid States. Introduction. Chapter 10 Topics. Liquid-Gas Phase Changes. Physical State of a Substance

Chapter 10. The Liquid and Solid States. Introduction. Chapter 10 Topics. Liquid-Gas Phase Changes. Physical State of a Substance Introduction Chapter 10 The Liquid and Solid States How do the properties of liquid and solid substances differ? How can we predict properties based on molecular- level structure? Glasses Wires Reshaping

More information

Liquids and Solids. H fus (Heat of fusion) H vap (Heat of vaporization) H sub (Heat of sublimation)

Liquids and Solids. H fus (Heat of fusion) H vap (Heat of vaporization) H sub (Heat of sublimation) Liquids and Solids Phase Transitions All elements and compounds undergo some sort of phase transition as their temperature is increase from 0 K. The points at which these phase transitions occur depend

More information

States of Matter. Solids Liquids Gases

States of Matter. Solids Liquids Gases States of Matter Solids Liquids Gases 1 Solid vs. Liquid vs. Gas Depends on only two things: What? Attractions Kinetic between particles vs Energy of particles 2 Intermolecular Forces (Molecular Attractions)

More information

States of Matter. Solids Liquids Gases

States of Matter. Solids Liquids Gases States of Matter Solids Liquids Gases 1 Solid vs. Liquid vs. Gas Depends on only two things: What? Attractions Kinetic between particles vs Energy of particles 2 Intermolecular Forces (Molecular Attractions)

More information

States of matter. Chapter 11. Kinetic Molecular Theory of Liquids and Solids. Kinetic Molecular Theory of Solids Intermolecular Forces

States of matter. Chapter 11. Kinetic Molecular Theory of Liquids and Solids. Kinetic Molecular Theory of Solids Intermolecular Forces States of matter Chapter 11 Intermolecular Forces Liquids and Solids By changing the T and P, any matter can exist as solid, liquid or gas. Forces of attraction determine physical state Phase homogeneous

More information

Ch. 9 Liquids and Solids

Ch. 9 Liquids and Solids Intermolecular Forces I. A note about gases, liquids and gases. A. Gases: very disordered, particles move fast and are far apart. B. Liquid: disordered, particles are close together but can still move.

More information

Upon successful completion of this unit, the students should be able to:

Upon successful completion of this unit, the students should be able to: Unit 9. Liquids and Solids - ANSWERS Upon successful completion of this unit, the students should be able to: 9.1 List the various intermolecular attractions in liquids and solids (dipole-dipole, London

More information

States of Matter; Liquids and Solids. Condensation - change of a gas to either the solid or liquid state

States of Matter; Liquids and Solids. Condensation - change of a gas to either the solid or liquid state States of Matter; Liquids and Solids Phase transitions - a change in substance from one state to another Melting - change from a solid to a liquid state Freezing - change of a liquid to the solid state

More information

PROPERTIES OF SOLIDS SCH4U1

PROPERTIES OF SOLIDS SCH4U1 PROPERTIES OF SOLIDS SCH4U1 Intra vs. Intermolecular Bonds The properties of a substance are influenced by the force of attraction within and between the molecules. Intra vs. Intermolecular Bonds Intramolecular

More information

CHEM. Ch. 12 Notes ~ STATES OF MATTER

CHEM. Ch. 12 Notes ~ STATES OF MATTER CHEM. Ch. 12 Notes ~ STATES OF MATTER NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 12.1 topics States of Matter: SOLID, LIQUID, GAS, PLASMA I. Kinetic Theory

More information

Intermolecular Forces and States of Matter AP Chemistry Lecture Outline

Intermolecular Forces and States of Matter AP Chemistry Lecture Outline Intermolecular Forces and States of Matter AP Chemistry Lecture Outline Name: Chemical properties are related only to chemical composition; physical properties are related to chemical composition AND the

More information

Intermolecular Forces, Liquids, & Solids

Intermolecular Forces, Liquids, & Solids , Liquids, & Solids Mr. Matthew Totaro Legacy High School AP Chemistry States of Matter The fundamental difference between states of matter is the distance between particles. States of Matter Because in

More information

Chapter 14. Liquids and Solids

Chapter 14. Liquids and Solids Chapter 14 Liquids and Solids Section 14.1 Water and Its Phase Changes Reviewing What We Know Gases Low density Highly compressible Fill container Solids High density Slightly compressible Rigid (keeps

More information

Chapter 11. Freedom of Motion. Comparisons of the States of Matter. Liquids, Solids, and Intermolecular Forces

Chapter 11. Freedom of Motion. Comparisons of the States of Matter. Liquids, Solids, and Intermolecular Forces Liquids, Solids, and Intermolecular Forces Chapter 11 Comparisons of the States of Matter The solid and liquid states have a much higher density than the gas state The solid and liquid states have similar

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids. Intermolecular Forces

Chapter 11 Intermolecular Forces, Liquids, and Solids. Intermolecular Forces Chapter 11, Liquids, and Solids States of Matter The fundamental difference between states of matter is the distance between particles. States of Matter Because in the solid and liquid states particles

More information

Chapter 12 Intermolecular Forces and Liquids

Chapter 12 Intermolecular Forces and Liquids Chapter 12 Intermolecular Forces and Liquids Jeffrey Mack California State University, Sacramento Why? Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature

More information

Chapter 11. Intermolecular Forces, Liquids, and Solids

Chapter 11. Intermolecular Forces, Liquids, and Solids 11.2 Intermolecular Forces Intermolecular forces are much weaker than ionic or covalent bonds (e.g., 16 kj/mol versus 431 kj/mol for HCl). Melting or boiling = broken intermolecular forces Intermolecular

More information

Name: Class: Date: SHORT ANSWER Answer the following questions in the space provided.

Name: Class: Date: SHORT ANSWER Answer the following questions in the space provided. CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. a. The gas

More information

CHEMISTRY Matter and Change. Chapter 12: States of Matter

CHEMISTRY Matter and Change. Chapter 12: States of Matter CHEMISTRY Matter and Change Chapter 12: States of Matter CHAPTER 12 States of Matter Section 12.1 Section 12.2 Section 12.3 Section 12.4 Gases Forces of Attraction Liquids and Solids Phase Changes Click

More information

CHAPTER 11: Intermolecular Forces, Liquids, and Solids. Are there any IDEAL GASES? The van der Waals equation corrects for deviations from ideality

CHAPTER 11: Intermolecular Forces, Liquids, and Solids. Are there any IDEAL GASES? The van der Waals equation corrects for deviations from ideality CHAPTER 11: Intermolecular Forces, Liquids, and Solids Are there any IDEAL GASES? The van der Waals equation corrects for deviations from ideality Does the KMT break down? Kinetic Molecular Theory 1. Gas

More information

Solid to liquid. Liquid to gas. Gas to solid. Liquid to solid. Gas to liquid. +energy. -energy

Solid to liquid. Liquid to gas. Gas to solid. Liquid to solid. Gas to liquid. +energy. -energy 33 PHASE CHANGES - To understand solids and liquids at the molecular level, it will help to examine PHASE CHANGES in a little more detail. A quick review of the phase changes... Phase change Description

More information

Chapter 10. Liquids and Solids

Chapter 10. Liquids and Solids Chapter 10 Liquids and Solids Chapter 10 Table of Contents 10.1 Intermolecular Forces 10.2 The Liquid State 10.3 An Introduction to Structures and Types of Solids 10.4 Structure and Bonding in Metals 10.5

More information

CHAPTER 9: LIQUIDS AND SOLIDS

CHAPTER 9: LIQUIDS AND SOLIDS CHAPTER 9: LIQUIDS AND SOLIDS Section 9.1 Liquid/Vapor Equilibrium Vaporization process in which a liquid vapor open container - evaporation continues until all liquid evaporates closed container 1) Liquid

More information

Chapter 11. Liquids, Solids, and Intermolecular Forces. Water, No Gravity. Lecture Presentation

Chapter 11. Liquids, Solids, and Intermolecular Forces. Water, No Gravity. Lecture Presentation Lecture Presentation Chapter 11 Liquids, Solids, and Intermolecular Forces Water, No Gravity In the space station there are no spills. Rather, the water molecules stick together to form a floating, oscillating

More information

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces Pearson Education, Inc.

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces Pearson Education, Inc. Lecture Presentation Chapter 11 Liquids and States of Matter The fundamental difference between states of matter is the strength of the intermolecular forces of attraction. Stronger forces bring molecules

More information

Intermolecular forces (IMFs) CONDENSED STATES OF MATTER

Intermolecular forces (IMFs) CONDENSED STATES OF MATTER Intermolecular forces (IMFs) CONDENSED STATES OF MATTER States of Matter: - composed of particles packed closely together with little space between them. Solids maintain a. - any substance that flows.

More information

Ch 10 -Ch 10 Notes Assign: -HW 1, HW 2, HW 3 Blk 1 Ch 10 Lab

Ch 10 -Ch 10 Notes Assign: -HW 1, HW 2, HW 3 Blk 1 Ch 10 Lab Advanced Placement Chemistry Chapters 10 11 Syllabus As you work through each chapter, you should be able to: Chapter 10 Solids and Liquids 1. Differentiate between the various types of intermolecular

More information

Chemistry: The Central Science

Chemistry: The Central Science Chemistry: The Central Science Fourteenth Edition Chapter 11 Liquids and Intermolecular Forces Intermolecular Forces The attractions between molecules are not nearly as strong as the intramolecular attractions

More information

Intermolecular Forces. Chapter 16 Liquids and Solids. Intermolecular Forces. Intermolecular Forces. Intermolecular Forces. Intermolecular Forces

Intermolecular Forces. Chapter 16 Liquids and Solids. Intermolecular Forces. Intermolecular Forces. Intermolecular Forces. Intermolecular Forces Big Idea: Systems that form macromolecules (ionic, metallic, and covalent network) have the strongest interactions between formula units. Systems that cannot form macro molecules still contain intermolecular

More information

Ch. 11 States of matter

Ch. 11 States of matter Ch. 11 States of matter States of Matter Solid Definite volume Definite shape Liquid Definite volume Indefinite shape (conforms to container) Gas Indefinite volume (fills any container) Indefinite shape

More information

Calderglen High School CfE Higher Chemistry. Chemical Changes & Structure Structure and Bonding. Page 1 of 21

Calderglen High School CfE Higher Chemistry. Chemical Changes & Structure Structure and Bonding. Page 1 of 21 Calderglen High School CfE Higher Chemistry Chemical Changes & Structure Structure and Bonding Page 1 of 21 No. Learning Outcome Understanding? 1 2 The bonding types of the first twenty elements; metallic

More information

- As for the liquids, the properties of different solids often differ considerably. Compare a sample of candle wax to a sample of quartz.

- As for the liquids, the properties of different solids often differ considerably. Compare a sample of candle wax to a sample of quartz. 32 SOLIDS * Molecules are usually packed closer together in the solid phase than in the gas or liquid phases. * Molecules are not free to move around each other as in the liquid phase. Molecular/atomic

More information

Chemistry B11 Chapter 6 Gases, Liquids, and Solids

Chemistry B11 Chapter 6 Gases, Liquids, and Solids Chapter 6 Gases, Liquids, and Solids States of matter: the physical state of matter depends on a balance between the kinetic energy of particles, which tends to keep them apart, and the attractive forces

More information

Chapter 11: Intermolecular Forces. Lecture Outline

Chapter 11: Intermolecular Forces. Lecture Outline Intermolecular Forces, Liquids, and Solids 1 Chapter 11: Intermolecular Forces Lecture Outline 11.1 A Molecular Comparison of Gases, Liquids and Solids Physical properties of substances are understood

More information

Professor K. Intermolecular forces

Professor K. Intermolecular forces Professor K Intermolecular forces We've studied chemical bonds which are INTRAmolecular forces... We now explore the forces between molecules, or INTERmolecular forces which you might rightly assume to

More information

Scientists learned that elements in same group on PT react in a similar way. Why?

Scientists learned that elements in same group on PT react in a similar way. Why? Unit 5: Bonding Scientists learned that elements in same group on PT react in a similar way Why? They all have the same number of valence electrons.which are electrons in the highest occupied energy level

More information

Polar Molecules. Textbook pg Molecules in which the charge is not distributed symmetrically among the atoms making up the molecule

Polar Molecules. Textbook pg Molecules in which the charge is not distributed symmetrically among the atoms making up the molecule Textbook pg. 251-283 Polar Molecules Molecules in which the charge is not distributed symmetrically among the atoms making up the molecule Electronegativity and Polar Molecules Pauling realized that electron

More information

Liquids & Solids. For the condensed states the ave KE is less than the attraction between molecules so they are held together.

Liquids & Solids. For the condensed states the ave KE is less than the attraction between molecules so they are held together. Liquids & Solids Intermolecular Forces Matter exists in 3 states. The state of matter is influenced by the physical properties of a substance. For liquids & solids, the condensed states, many of the physical

More information

Chapter 13 States of Matter Forces of Attraction 13.3 Liquids and Solids 13.4 Phase Changes

Chapter 13 States of Matter Forces of Attraction 13.3 Liquids and Solids 13.4 Phase Changes Chapter 13 States of Matter 13.2 Forces of Attraction 13.3 Liquids and Solids 13.4 Phase Changes I. Forces of Attraction (13.2) Intramolecular forces? (forces within) Covalent Bonds, Ionic Bonds, and metallic

More information

IMFA s. intermolecular forces of attraction Chez Chem, LLC All rights reserved.

IMFA s. intermolecular forces of attraction Chez Chem, LLC All rights reserved. IMFA s intermolecular forces of attraction 2014 Chez Chem, LLC All rights reserved. **London Dispersion Forces Also know as Van der Waals forces A momentary non symmetrical electron distribution that can

More information

2. As gas P increases and/or T is lowered, intermolecular forces become significant, and deviations from ideal gas laws occur (van der Waal equation).

2. As gas P increases and/or T is lowered, intermolecular forces become significant, and deviations from ideal gas laws occur (van der Waal equation). A. Introduction. (Section 11.1) CHAPTER 11: STATES OF MATTER, LIQUIDS AND SOLIDS 1. Gases are easily treated mathematically because molecules behave independently. 2. As gas P increases and/or T is lowered,

More information

Chapter 16: Phenomena. Chapter 16 Liquids and Solids. intermolecular forces? Intermolecular Forces. Intermolecular Forces. Intermolecular Forces

Chapter 16: Phenomena. Chapter 16 Liquids and Solids. intermolecular forces? Intermolecular Forces. Intermolecular Forces. Intermolecular Forces Chapter 16: Phenomena Phenomena: The tables below show melting points and boiling points of substances. What patterns do you notice from the data? Melting Boiling Substance Point Point CaO 2886 K 4123

More information

Name Date Class THE NATURE OF GASES

Name Date Class THE NATURE OF GASES 13.1 THE NATURE OF GASES Section Review Objectives Describe the assumptions of the kinetic theory as it applies to gases Interpret gas pressure in terms of kinetic theory Define the relationship between

More information

Intermolecular Forces I

Intermolecular Forces I I How does the arrangement of atoms differ in the 3 phases of matter (solid, liquid, gas)? Why doesn t ice just evaporate into a gas? Why does liquid water exist at all? There must be some force between

More information

Chapter 11. Intermolecular Forces, Liquids, and Solids

Chapter 11. Intermolecular Forces, Liquids, and Solids 11.2 Intermolecular Forces Intermolecular forces are much weaker than ionic or covalent bonds (e.g., 16 kj/mol versus 431 kj/mol for HCl). Melting or boiling = broken intermolecular forces Intermolecular

More information

Ch 9 Liquids & Solids (IMF) Masterson & Hurley

Ch 9 Liquids & Solids (IMF) Masterson & Hurley Ch 9 Liquids & Solids (IMF) Masterson & Hurley Intra- and Intermolecular AP Questions: 2005 Q. 7, 2005 (Form B) Q. 8, 2006 Q. 6, 2007 Q. 2 (d) and (c), Periodic Trends AP Questions: 2001 Q. 8, 2002 Q.

More information

Ionic Compounds and Ionic Bonding

Ionic Compounds and Ionic Bonding Ionic Compounds and Ionic Bonding Definitions Review: Crystal Lattice - 3D continuous repeating pattern of positive and negative ions in an ionic solid Formula Unit- smallest possible neutral unit of an

More information

NOTES: 8.4 Polar Bonds and Molecules

NOTES: 8.4 Polar Bonds and Molecules NOTES: 8.4 Polar Bonds and Molecules ELECTRONEGATIVITY: We ve learned how valence electrons are shared to form covalent bonds between elements. So far, we have considered the electrons to be shared equally.

More information

Chapter 10: Liquids and Solids

Chapter 10: Liquids and Solids Chapter 10: Liquids and Solids STATES OF MATTER: At any temperature above absolute zero, the atoms, molecules, or ions that make up a substance are moving. In the kinetic theory of gases, this motion is

More information

Kirkcaldy High School CfE Higher Chemistry. Chemical Changes & Structure Structure and Bonding

Kirkcaldy High School CfE Higher Chemistry. Chemical Changes & Structure Structure and Bonding Kirkcaldy High School CfE Higher Chemistry Chemical Changes & Structure Structure and Bonding Page 1 of 26 No. Learning Outcome Understanding? The bonding types of the first twenty elements; metallic (Li,

More information

RW Session ID = MSTCHEM1 Intermolecular Forces

RW Session ID = MSTCHEM1 Intermolecular Forces RW Session ID = MSTCHEM1 Intermolecular Forces Sections 9.4, 11.3-11.4 Intermolecular Forces Attractive forces between molecules due to charges, partial charges, and temporary charges Higher charge, stronger

More information

General Chemistry 202 CHM202 General Information. General Chemistry 202 CHM202 Policies. General Chemistry 202 CHM202 Laboratory Guidelines

General Chemistry 202 CHM202 General Information. General Chemistry 202 CHM202 Policies. General Chemistry 202 CHM202 Laboratory Guidelines General Chemistry 202 CHM202 General Information Instructor Meeting times and places Text and recommended materials Website Email Grading Schedule 1 General Chemistry 202 CHM202 Policies Equipment Instruction

More information

Ch 11: Intermolecular Forces, Liquids, and Solids

Ch 11: Intermolecular Forces, Liquids, and Solids AP Chemistry: Intermolecular Forces, Liquids, and Solids Lecture Outline 11.1 A Molecular Comparison of Liquids and Solids Physical properties of liquids and solids are due to intermolecular forces. These

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 11, Liquids, and Solids States of Matter The fundamental difference between states of

More information

What determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction

What determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction Liquids and Solids What determines the phase of a substance? Temperature Pressure Interparticle Forces of Attraction Types of Interparticle Forces Ionic Bonding Occurs between cations and anions Metallic

More information

Some Properties of Solids, Liquids, and Gases

Some Properties of Solids, Liquids, and Gases AP Chemistry: Intermolecular Forces, Liquids, and Solids Lecture Outline 11.1 A Molecular Comparison of Liquids and Solids Physical properties of liquids and solids are due to intermolecular forces. These

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The F-B-F bond angle in the BF3 molecule is. A) 109.5e B) 120e C) 180e D) 90e E) 60e

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 11, Liquids, and Solids John D. Bookstaver St. Charles Community College Cottleville,

More information

SOLIDS AND LIQUIDS - Here's a brief review of the atomic picture or gases, liquids, and solids GASES

SOLIDS AND LIQUIDS - Here's a brief review of the atomic picture or gases, liquids, and solids GASES 30 SOLIDS AND LIQUIDS - Here's a brief review of the atomic picture or gases, liquids, and solids GASES * Gas molecules are small compared to the space between them. * Gas molecules move in straight lines

More information

Q. What happens when you boil (melt) a compound?

Q. What happens when you boil (melt) a compound? Intermolecular Forces (MHR Text p. 202 206) Molecular compounds are: 1) made up of molecules 2) are made up of two or more nonmetallic atoms 3) held together by covalent bonds (sharing e ) Q. But what

More information

CHAPTER 6 Intermolecular Forces Attractions between Particles

CHAPTER 6 Intermolecular Forces Attractions between Particles CHAPTER 6 Intermolecular Forces Attractions between Particles Scientists are interested in how matter behaves under unusual circumstances. For example, before the space station could be built, fundamental

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Chapter 11 Intermolecular Forces, Liquids, and Solids Dissolution of an ionic compound States of Matter The fundamental difference between states of matter is the distance between particles. States of

More information

States of Matter. We can explain the properties that we observe in the various states of matter with these postulates.

States of Matter. We can explain the properties that we observe in the various states of matter with these postulates. States of Matter Kinetic Molecular Theory When discussing the properties of matter, it is not enough just to classify them. We must also create a model that helps to explain the properties that we see.

More information

Properties of Liquids and Solids

Properties of Liquids and Solids Properties of Liquids and Solids World of Chemistry Chapter 14 14.1 Intermolecular Forces Most substances made of small molecules are gases at normal temperature and pressure. ex: oxygen gas, O 2 ; nitrogen

More information

Liquids, Solids, and Phase Changes

Liquids, Solids, and Phase Changes C h a p t e r 10 Liquids, Solids, and Phase Changes KMT of Liquids and Solids 01 Gases have little or no interactions. Liquids and solids have significant interactions. Liquids and solids have well-defined

More information

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 11 Intermolecular Forces, Liquids, and Solids John D. Bookstaver St. Charles Community

More information