States of matter. Chapter 11. Kinetic Molecular Theory of Liquids and Solids. Kinetic Molecular Theory of Solids Intermolecular Forces
|
|
- Sheena Nelson
- 6 years ago
- Views:
Transcription
1 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 part of system in contact with other parts of system, separated by well-defined boundary e.g., ice in water, subliming dry ice, evaporating isopropanol Kinetic Molecular Theory of Liquids and Solids Liquids and solids = condensed states Liquids Molecules are close together w/ little empty space difficult to compress Molecules held together by attractive forces Liquid has definite volume Molecules can move past each other freely, flow into shape of container Kinetic Molecular Theory of Solids Solids Molecules are held rigidly in place vibrate about a fixed point Less compressible than liquids. Usually solid is denser than liquid important exception = water Definite shape and volume 11.2 Intermolecular Forces Attractive forces between molecules. As T of gas drops, intermolecular forces overcome thermal motion Condensation gas molecules slow until attraction pulls them together into liquid Intermolecular forces < intramolecular forces (bonds) Stronger intermolecular force d higher boiling and melting points
2 Types of Intermolecular Forces Ion - dipole Dipole - dipole * Dipole - induced dipole * Dispersion (London) forces * Hydrogen bond * van der Waals force Ion-dipole interactions Cations generally have stronger interactions because they are smaller, with more concentrated charge than anions. Dipole-Dipole Pairs of cation-anion attractions align polar molecules Ion-Induced Dipole & Dipole-Induced Dipole Non-polarized atom Polarized atoms Induced dipole = separation of + and - charges in atom or nonpolar molecule caused by proximity of ion or polar molecule Induced Dipoles Polarizability - ease with which e - distribution of atom can be distorted More e - s d greater polarizability Often anions, with more diffuse charge, are more polarizable than cations Molecules w/ dipoles can be polarized, causing them to become more polar Instantaneous dipole induced dipole attraction Instantaneous dipole any atom or non-polar molecule is briefly polar because of separation between e - and + nucleus Instantaneous dipole can induce dipole in adjacent molecule Attraction between instantaneous and induced dipole is very weak London or dispersion forces
3 Melting Points of Nonpolar CX 4 MELTING POINT COMPOUND ( O C) CH CF CCl CBr CI Larger molecule Why? d higher melting point Dispersion forces Occur in all substances (polar and non-polar) Allow non-polar molecules to condense Increase w/ polarizability, which increases with molar mass Polar molecules have dipole-dipole attractions as well as dispersion forces For polar molecules, larger dipole moment d stronger attraction. For any molecule, larger molar mass (more e - ) d greater intermolecular attraction For a large molecule, dispersion force can exceed dipole-dipole attraction Hydrogen Bond Special dipole-dipole interaction between H on N, O or F and a nearby N, O or F weak H-bonds with other elements such as S and P H-bonds are strong intermolecular attractions Large effects on intermolcular organization higher b.p. and m.p. alignment of protein molecules Approximate energies in kj/mol Compare to covalent single bonds, kj/mol weak up to 45 F H F - HO H OH Strong hydrogen bonds Weak or no hydrogen bonds Identify intermolecular forces H 2 O CH 2 Cl 2 KBr F - + H 2 O I 2 CH 3 OH PCl 3 C 6 H 6 SiH 4 Fe N(CH 3 ) 3 CS 2 BCl 3 Na + + NH 3
4 11.3 Properties of Liquids Surface Tension amount of energy required to increase surface area of liquid by a unit area Interior molecules are attracted in all directions Surface molecules are attracted selectively into liquid Anisotropic forces differ with direction Isotropic forces same in all directions Capillary action Cohesion intermolecular attraction between like molecules (pure liquid) Adhesion intermolecular attraction between unlike molecules (liquid and its container) Adhesion > cohesion H 2 O in glass Concave meniscus Cohesion > adhesion Hg in glass Convex meniscus Viscosity Measure of a fluid s resistance to flow High viscosity ( thick ) = slow flow Strong intermolecular forces d high viscosity glucose (typical sugar) is viscous because of intermolecular hydrogen bonding O HC O H C H H C OH OH C H O H C H CH2 O H Newtonian Fluids viscosity is independent of shear rate Non-Newtonian Fluids (examples) Thixotropic viscosity decreases with time under constant shear (gel-flow paint) Dilatant viscocity increases with shear rate (Silly Putty) Viscosity Liquid Viscosity (N s/m 2 ) Water (H 2 O) 1.01 x 10-3 Ethanol (C 2 H 5 OH) 1.20 x 10-3 Glycerol (HOCH 2 CHOHCH 2 OH) 1.49 Blood 4 x 10-3 More hydrogen bonds d more viscous liquid Viscosity Liquid Viscosity (N s/m 2 ) Water (H 2 O) 1.01 x 10-3 Ethanol (C 2 H 5 OH) 1.20 x 10-3 Glycerol (HOCH 2 CHOHCH 2 OH) 1.49 Blood 4 x 10-3 Water Large specific heat bodies of water moderate climate by absorbing and releasing heat Liquid is denser than solid (ice floats) H 2 O can form 2 H-bonds per molecule, leading to a very open solid structure. More hydrogen bonds d more viscous liquid
5 Large open cavities in solid ice are filled in liquid water, increasing density Ice 11.4 Crystal Structure Crystalline solid has rigid, longrange order Amorphous solid lacks welldefined arrangement and long range order Unit cell basic repeating structural unit of a crystalline solid Lattice point atom, molecule, or fixed arrangement of atoms Coordination number (CN) number of atoms (ions) surrounding an atom (ion) in a crystal lattice CN of an atom is a simple cubic lattice is 6 1/8 of each corner atom is inside the unit cell
6 How many atoms are in a body-centered cubic unit cell? Corner atom is shared by 8 cells. Edge atom is shared by 4 cells Face-centered atom is shared by two cells. 8 corner atoms: 8 x 1/8 = 1 1 central atom: 1 x 1 = 1 d 1+1 = 2 atoms in body-centered cubic cell (a) Most efficient arrangement of spheres (b) 2nd layer (c) Hexagonal closest packing ABABA... (d) Cubic closest packing ABCABC... Closest packing (a) Hexagonal close packing ABABA... (b) Cubic close packing ABCABC... Cubic close packing is identical to facecentered cubic packing Hexagonal vs. cubic close packing A B A A B C A X-Ray Diffraction X-Ray diffraction by a crystal Scattering of X-rays by the atoms of a crystalline solid Atoms in a crystal absorb then re-emit X-radiation When scattered X-rays from adjacent layers of atoms are in phase, constructive interference occurs at certain point in space
7 X-rays of wavelength nm are used to analyze a metallic crystal. 1st-order diffraction (n = 1) occurs at What is the layer spacing? What is the 2ndorder angle (n = 2)? nλ = 2d sinθ When additional distance traveled by an X-ray (BC + CD = 2d sinθ) equals integral number of wavelengths (nλ), waves are in phase nλ = 2d sinθ (n = 1, 2, 3...) 11.6 Types of Crystals Ionic Crystals array of anions and cations high-melting brittle NaCl, Li 2 O, CaF 2, MgO Ionic bonds become stronger but more covalent as charges increase Covalent crystals 3-D network of covalent bonds high-melting, often hard diamond, graphite and quartz (SiO 2 ) 154 pm Diamond: sp 3 carbon 142 pm Graphite: sp 2 carbon Types of Crystals Molecular crystals lattice points occupied by molecules, held together by van der Waals forces and/or H-bonding low -melting (<100 o C) Metallic crystals metal atoms at lattice points dense, conductive, shiny etc. metal ions in sea of electrons Amorphous solids Lack a regular, three-dimensional arrangement of atoms Glass (optically transparent) fusion product of (inorganic) materials cooled to non-crystalline rigid state Common glass is mainly SiO 2 (quartz), w/ B 2 O 3 (Pyrex) or CaO, Na 2 O (lime glass) Transition metal oxides color glass
8 11.8 Phase Changes Transformation between phases Energy (usually heat) is added or removed Liquid-vapor equilibrium Liquid-solid equilibrium Solid-vapor equilibrium Liquid - Vapor Equilibrium Evaporation (vaporization) process in which a liquid is transformed into a gas Occurs when molecules have enough energy to escape from the liquid s surface Higher T d more KE d faster evaporation Low T d fewer energetic molecules High T d more energetic molecules (Equilibrium) Vapor Pressure Pressure exerted by evaporated gas molecules above a liquid When rate of evaporation = rate of condensation, dynamic equilibrium is reached P at this point = (equilibrium) vapor pressure Vacuum Hg Heat of Vaporization, H vap E required to vaporize 1 mole of a liquid X(l) d X(g) H vap Stronger intermolecular forces d larger H vap Table 11.6 Everyday experience evaporating water or alcohol makes you feel cold heat required to vaporize liquid comes from your skin Quantitative relationship between vapor pressure (P) and temperature (T) Clausius-Clapeyron Equation ln P = - H vap + C RT at a single T; C is a constant plot log P vs. 1/T to find H vap P 1 ln = Hvap P 2 R T 2 T 1 Form to compare two temperatures
9 Boiling Point T at which vapor pressure of a liquid = applied pressure Stronger intermolecular forces d higher boiling point Normal boiling point defined at 1 atm Critical Points Critical Temperature (T c ) T above which gas cannot be liquefied at any pressure Critical Pressure (P c ) minimum P needed to liquefy a gas at T c Supercritical fluids (phase above T c ) are industrially important supercritical CO 2 is used to decaffeinate coffee, extract oils from grain, dry-clean clothing, etc. Liquid-Solid Equililbrium Freezing phase change from liquid to solid Melting or Fusion phase change from solid to liquid Melting point (freezing point) T at which the solid and liquid phases coexist in equilibrium Normal m.p. (f.p.) defined at 1 atm (Molar) Heat of Fusion, H fus E required to melt one mole of a solid Table 11.8 H fus < H vap molecules are closely packed in the liquid and solid states, but widely separated in the gas state Compare slopes: s (solid > liquid > gas) How much heat is required to convert 425 g of ice at -15 C to steam at 125 C? (specific heats: ice = 2.03 J/g C, water = 4.18 J/g C, steam = 1.99 J/g C; H fus = 6.01 kj/mol; H vap = kj/mol) Σ heats of 126 o C segments q 5 = msdt = total heat 100 o C q 4 = ndh vap Compare lengths: H fus < H vap 0 o C -10 o C q 1 = msdt q 2 = ndh fus q 3 = msdt
10 Solid-Vapor Equilibrium Sublimation conversion of solid directly to vapor Deposition vapor to solid (Molar) heat of sublimation, H sub = E required to sublime one mole of solid H sub = H fus + H vap Evaporations (up) are endothermic Condensations (down) are exothermic 11.9 Phase Diagrams H 2 O CO 2 Triple point condition in which all 3 phases are in equilibrium Slope of curve (line) between phases d P dependence of transition mp ice decreases at higher P mp CO 2 increases at higher P
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 informationChapter 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 informationIntermolecular 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 informationIntermolecular 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 informationCHAPTER 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 informationIntermolecular 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 informationCHAPTER 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 informationIntermolecular 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 informationIntermolecular 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 information2. 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- 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 informationChapter 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 informationGeneral 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 informationThe 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 informationLondon 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 information2. 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 informationChapter 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 informationCh. 11: Liquids and Intermolecular Forces
Ch. 11: Liquids and Intermolecular Forces Learning goals and key skills: Identify the intermolecular attractive interactions (dispersion, dipole-dipole, hydrogen bonding, ion-dipole) that exist between
More informationLiquids, 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 informationก ก ก Intermolecular Forces: Liquids, Solids, and Phase Changes
ก ก ก Intermolecular Forces: Liquids, Solids, and Phase Changes ก ก ก ก Mc-Graw Hill 1 Intermolecular Forces: Liquids, Solids, and Phase Changes 12.1 An Overview of Physical States and Phase Changes 12.2
More informationLiquids, 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 informationThe 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 informationcompared 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 informationChapter 11 SOLIDS, LIQUIDS AND GASES Pearson Education, Inc.
Chapter 11 SOLIDS, LIQUIDS AND GASES States of Matter Because in the solid and liquid states particles are closer together, we refer to them as. The States of Matter The state of matter a substance is
More informationChapter 10: Liquids, Solids, and Phase Changes
Chapter 10: Liquids, Solids, and Phase Changes In-chapter exercises: 10.1 10.6, 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,
More informationChapter 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 informationIntermolecular 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 informationChapters 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 informationStates 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 informationChapter 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 informationChapter 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 informationIntermolecular 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 informationChapter 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 informationThey 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 informationSome 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 informationChapter 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 informationChapter 10. Liquids and Solids
Chapter 10 Liquids and Solids Section 10.1 Intermolecular Forces Section 10.1 Intermolecular Forces Section 10.1 Intermolecular Forces Section 10.1 Intermolecular Forces Metallic bonds Covalent bonds Ionic
More informationChem 112 Dr. Kevin Moore
Chem 112 Dr. Kevin Moore Gas Liquid Solid Polar Covalent Bond Partial Separation of Charge Electronegativity: H 2.1 Cl 3.0 H Cl δ + δ - Dipole Moment measure of the net polarity in a molecule Q Q magnitude
More informationThey 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 informationQuestion 2 Identify the phase transition that occurs when CO 2 solid turns to CO 2 gas as it is heated.
For answers, send email to: admin@tutor-homework.com. Include file name: Chemistry_Worksheet_0039 Price: $4 (c) 2012 www.tutor-homework.com: Tutoring, homework help, help with online classes. Chapter 11
More informationChapter 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 information2) Of the following substances, only has London dispersion forces as its only intermolecular force.
11.1 Multiple Choice and Bimodal Questions 1) Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point? A) CH 3CH 2 CH3 B) CH 3OCH3
More informationChapter 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 informationChapter 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 informationChap. 12 INTERMOLECULAR FORCES
Chap. 12 INTERMOLECULAR FORCES Know how energy determines physical properties and how phase changes occur as a result of heat flow. Distinguish between bonding (intermolecular) and nonbonding (intermolecular)
More information9/2/10 TYPES OF INTERMOLECULAR INTERACTIONS
Tro Chpt. 11 Liquids, solids and intermolecular forces Solids, liquids and gases - A Molecular Comparison Intermolecular forces Intermolecular forces in action: surface tension, viscosity and capillary
More informationChapter 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 informationCh 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 informationChapter 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 informationCHEMISTRY The Molecular Nature of Matter and Change
CHEMISTRY The Molecular Nature of Matter and Change Third Edition Chapter 12 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 11 INTERMOLECULAR FORCES
More informationSome Properties of Solids, Liquids, and Gases
AP Chemistry: Intermolecular Forces, Liquids, and Solids Sec 1. A Molecular Comparison of Liquids and Solids Physical properties of liquids and solids are due to intermolecular forces. These are forces
More informationChemistry: 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 informationChapter 12 INTERMOLECULAR FORCES. Covalent Radius and van der Waals Radius. Intraand. Intermolecular Forces. ½ the distance of non-bonded
Chapter 2 INTERMOLECULAR FORCES Intraand Intermolecular Forces Covalent Radius and van der Waals Radius ½ the distance of bonded ½ the distance of non-bonded Dipole Dipole Interactions Covalent and van
More informationINTERMOLECULAR 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 informationCHEMISTRY 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 informationLiquids & 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 informationChapter 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 informationChapter 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 informationChapter 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 informationngac (ttn793) H11: Solids and Liquids mccord (51600) 1
ngac (ttn793) H11: Solids and Liquids mccord (51600) 1 This print-out should have 25 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. 001
More informationLiquids & Solids: Section 12.3
Liquids & Solids: Section 12.3 MAIN IDEA: The particles in and have a range of motion and are not easily. Why is it more difficult to pour syrup that is stored in the refrigerator than in the cabinet?
More informationWhat 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 informationLecture 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 informationChapter 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 informationChapter 10 Review Packet
Chapter 10 Review Packet Name 1. If water and carbon dioxide molecules did interact, what major intermolecular force will exist between these molecules? a) Hydrogen bonding b) London dispersion c) Dipole-dipole
More informationCHAPTER 10. States of Matter
CHAPTER 10 States of Matter Kinetic Molecular Theory Kinetikos - Moving Based on the idea that particles of matter are always in motion The motion has consequences Explains the behavior of Gases, Liquids,
More informationCHAPTER 10. Kinetic Molecular Theory. Five Assumptions of the KMT. Atmospheric Pressure
Kinetic Molecular Theory CHAPTER 10 States of Matter Kinetikos - Moving Based on the idea that particles of matter are always in motion The motion has consequences Explains the behavior of Gases, Liquids,
More informationChapter 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 informationUnit Five: Intermolecular Forces MC Question Practice April 14, 2017
Unit Five: Intermolecular Forces Name MC Question Practice April 14, 2017 1. Which of the following should have the highest surface tension at a given temperature? 2. The triple point of compound X occurs
More informationIntermolecular 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 informationCh 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 informationChapter 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 informationKinetic Theory (Kinetikos - Moving ) Based on the idea that particles of matter are always in motion
Chapter 10 Kinetic Theory (Kinetikos - Moving ) Based on the idea that particles of matter are always in motion The motion has consequences Behavior of Gases Physical Properties of Gases Ideal Gas an imaginary
More informationChapter 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 informationForces, Liquids, and Solids
11 Intermolecular Forces, Liquids, and Solids Visualizing Concepts 11.1 The diagram best describes a liquid. In the diagram, the particles are close together, mostly touching but there is no regular arrangement
More informationLecture 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 informationChapter 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- 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 informationAP* Chapter 10. Liquids and Solids. Friday, November 22, 13
AP* Chapter 10 Liquids and Solids AP Learning Objectives LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses
More informationGases and States of Matter: Unit 8
Gases and States of Matter: Unit 8 States of Matter There are three states (also called phases) of matter. The picture represents the same chemical substance, just in different states. There are three
More informationChemistry 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 informationChapter 11/12: Liquids, Solids and Phase Changes Homework: Read Chapter 11 and 12 Keep up with assignments
P a g e 1 Unit 3: Chapter 11/12: Liquids, Solids and Phase Changes Homework: Read Chapter 11 and 12 Keep up with assignments Liquids and solids are quite different from gases due to their attractive forces
More information= = 10.1 mol. Molar Enthalpies of Vaporization (at Boiling Point) Molar Enthalpy of Vaporization (kj/mol)
Ch 11 (Sections 11.1 11.5) Liquid Phase Volume and Density - Liquid and solid are condensed phases and their volumes are not simple to calculate. - This is different from gases, which have volumes that
More informationSOLIDS 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 informationMr. Bracken. Intermolecular Forces Notes #1
Mr. Bracken AP Chemistry Name Period Intermolecular Forces Notes #1 States of Matter: A gas expands to fill its container, has neither a fixed volume nor shape, and is easily compressible. A liquid has
More informationChapter 11 part 2. Properties of Liquids Viscosity Surface Tension Capillary Action. Phase Changes (energy of phase changes)
Chapter 11 part 2 Properties of Liquids Viscosity Surface Tension Capillary Action Phase Changes (energy of phase changes) Dynamic Equilibrium Vapor pressure Phase diagram 1 Structure Affects Function
More informationSOLIDS 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 informationIntermolecular 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 informationIntermolecular Forces: Liquids, and Solids. Chapter 11
Intermolecular Forces: Liquids, and Solids Chapter 11 1 Review Practice Excited Na atoms may emit radiation having a wavelength of 589 nm. a) What is the wavelength in meters? b) What is the frequency
More informationGeneral Chemistry I. Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University. Module 3: The Three States of Matter
General Chemistry I Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University Module 3: The Three States of Matter Gas state (Equation of state: ideal gas and real gas). Liquid state
More informationNestor S. Valera Ateneo de Manila. Chapter 12 - Intermolecular Forces
Nestor S. Valera Ateneo de Manila Chapter 12 - Intermolecular Forces 1 A phase is a region that differs in structure and/or composition from another region. 2 Phases Solid phase - ice Liquid phase - water
More informationLiquids & 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 informationCRYSTAL STRUCTURE, PHASE CHANGES, AND PHASE DIAGRAMS
CRYSTAL STRUCTURE, PHASE CHANGES, AND PHASE DIAGRAMS CRYSTAL STRUCTURE CRYSTALLINE AND AMORPHOUS SOLIDS Crystalline solids have an ordered arrangement. The long range order comes about from an underlying
More informationCh. 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 informationChapter 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 informationIntermolecular Forces
Intermolecular Forces Molecular Compounds The simplest molecule is H 2 : Increased electron density draws nuclei together The pair of shared electrons constitutes a covalent bond. Intermolecular Forces
More informationChapter 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 informationChapter 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 informationChapter 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 informationIntermolecular Forces, Liquids and Solids Chap. 10
Page III-10-1 / Chapter Ten Lecture Notes Intermolecular Forces, and Solids Chap. 10 States of Matter The fundamental difference between states of matter is the distance between particles. Chemistry 222
More information