The Solid State. Phase diagrams Crystals and symmetry Unit cells and packing Types of solid
|
|
- Alison Newton
- 5 years ago
- Views:
Transcription
1 The Solid State Phase diagrams Crystals and symmetry Unit cells and packing Types of solid
2 Learning objectives Apply phase diagrams to prediction of phase behaviour Describe distinguishing features of the four solid types Describe principles of X-ray diffraction Apply symmetry operations to simple patterns Distinguish packing sequences among the four common types of crystal lattice Use unit cell to determine crystal composition
3 Phase diagrams Phase diagrams summarize the states of a substance as function of pressure and temperature They reveal: The areas where one phase is stable The lines where two phases are in equilibrium The points where three phases are in equilibrium Summed up in Phase Rule: C + 2 = P + F
4 Phase diagram for water Ice at 1 atm pressure converts to liquid at 0ºC and to gas at 100ºC Below 6 x 10-3 atm ice converts directly to gas (sublimation) At triple point three phases are in equilibrium single T and P Beyond critical point is region of supercritical fluid: Cannot be condensed no matter what the pressure (critical temperature) Cannot be vaporized no matter what the temperature (critical pressure)
5 Sublimation and the phase diagram
6 Phase diagrams explain well known phenomena The slope of the solidliquid phase boundary for water is negative, while for CO 2 it is positive A sample of ice under pressure melts A sample of liquid CO 2 under pressure solidifies At 1 atm pressure: Ice melts on heating Solid CO 2 sublimes (dry ice)
7 Chemistry and Metamucil: Regularity is everything At equilibrium atom tends to occupy position of lowest energy (highest stability) One position more stable than any others If true for one atom then true for all Regular crystal lattice results Not all solids are crystalline Amorphous solids have no regular structure - atoms occupy many sites Tend to be metastable - revert to crystalline form
8 Four solids of the apocalypse Ionic Ionic bonds Brittle, hard, high m.p. NaCl, K 2 O Molecular Van der Waals Soft, low m.p. CO 2, I 2 Covalent lattice Covalent bonds Hard, v. high m.p. Diamond, SiO 2 Metallic Metallic bonds Variable hardness and m.p. W, Cu, Hg conductors
9 Probing crystal structures Light is scattered by objects that are larger than the wavelength Crystal lattices are too small for visible light X-rays have wavelengths on the order of the interatomic distance in crystals X-rays suffer diffraction by crystals like visible light diffracted by blinds X-ray diffraction is the most powerful structural tool developed
10 Diffraction and interference Diffraction arises by interference of electromagnetic radiation Constructive interference waves are in phase increase in intensity Destructive interference waves are out of phase loss of intensity X-ray beams diffract from a crystal to give a pattern of spots where constructive interference has occurred on a sea of destructive interference
11 The crystal lattice and Bragg scattering X-rays are scattered by the electrons in the atoms The array of atoms in the crystal is like a diffraction grating for X-rays as a set of slits is for visible light Diffraction only occurs under conditions of constructive interference The Bragg equation gives the conditions
12 The Bragg condition: it s incurable Waves reflected from adjacent layers must be in phase For constructive interference, the path length difference must then be a whole number of wavelengths n 2d sin
13 X-ray diffraction and data A crystal or powder is swept through range of angles of θ and positions of reflections are tabulated Analysis of d spacings gives information about type of crystal lattice Deeper analysis of reflection intensities gives complete description of structure collection
14 Symmetry and crystal structure Symmetry underlies chemistry Arrangements of atoms in crystals Determination of spectra Mixtures of orbitals in bonds Symmetry operators relate the positions of the atoms in the unit cell
15 Common symmetry elements Translation Rotation Reflection After application of a symmetry operation to a set of atoms related by symmetry, the system appears unchanged
16 Symmetry operations Translation Reflection Rotation
17 Packing of spheres and simple structures Atoms and simple molecules can be treated like spheres The crystal lattice can be derived from packing together spheres There are limited possibilities
18 Cubic packing In simple cubic the atoms stack directly on top of each other: a a a a Not close packed (very uncommon) Body-centered cubic: denser packing achieved by putting a layer in the depression of the first: a b a b a b Not close packed (quite common)
19 Close packing Oranges do it Atoms do it
20 Adding layers: choices Two arrangements achieve a higher density Hexagonal closepacked- abab Face-centered cubic abcabc Both very common for metals
21 Close packing in metals
22 Summary of packing arrangements Structure Packing sequence Coordination number Packing density/% Simple cubic a-a-a-a Body centered cubic (BCC) Hexagonal CP (HCP) Face centered cubic (FCC) a b a b 8 68 a-b-a-b a-b-c-a-b-c 12 74
23 Building patterns with unit cells A floor is made from a mosaic of tiles A wall is made from stacking of bricks A crystal is made from Unit cell stacking unit cells In each case the basic unit contains all information required to describe structure completely with no gaps, deficiencies or redundancies
24 Unit cell accountancy Consider a cube Component of cube Number in cell Center Face Edge Corner
25 Sharing in unit cells Place an atom on each of the unit cell locations: center, face, edge, corner How many unit cells share the atom? What fraction of atom is in the unit cell Component Center Shared between 0 Fraction of atom in cell 1 Face Edge Corner
26 Unit cell contents and composition Count atoms as follows: Ratio of atoms in unit cell must equal composition One atom on: Number of components in unit cell Fraction in cell Number of atoms in cell Center 1 1 Face Edge Corner
27 Primitive and body-centered Primitive: 8 atoms on the corners each contribute 1/8 th to the contents overall cell contents = 1 BCC: 8 atoms on the corners contribute 1 1 atom in center contributes 1 Overall contents = 2; composition AB cells
28 Face-centered cube Two views of the FCC lattice Also viewed along 3- fold axis which is perpendicular to the close-packed layers Contents: 8 at corners = 1 6 on faces = 3 Total contents = 4
29 Calculations with unit cells Calculating unit-cell size from atom size In FCC cell, the atoms touch along the diagonal Length of diagonal = 4r Length of edge = d 8r
30 Estimate density If we know the unit cell size we can calculate the unit cell volume If we know the unit cell contents we know the total mass of the cell Density = mass/volume
31 Simple ionic compounds In general, anions are larger than cations Lattices can be described by close packing of anions with cations occupy regular holes in the anion lattice
32 Sodium chloride unit cell Chloride ions (purple) form FCC lattice Sodium ions (green) occupy octahedral holes Composition check: Cl: 8 on corners = 1 6 on faces = 3 Total = 4 Na: 12 on edges = 3 1 in center = 1 Total = 4
33 Covalent networks Ionic lattices are characterized by high coordination numbers and non-directional bondin Covalent lattices have low coordination numbers and highly directional bonding The bonds are formed from hybridized atomic orbitals to use the valence bond model
34 Diamonds are forever The diamond lattice is a very common covalent lattice It is a three dimensional tetrahedral net Bonds are made from sp 3 hybrid orbitals Very strong covalent bonds make the lattice extremely stable
35 Compounds also have diamond In GaAs, the Ga and As atoms alternate in the diamond lattice GaAs is an important semiconductor and laser material Many other similar materials lattice
36 Diamond and graphite Infinite covalent lattices in different dimensions Graphite 2D Diamond 3D Graphite is more stable than diamond, but can be transformed into diamond by application of high pressure Buckyballs Nanotubes
37 Metallic bonding: adrift on an Why do metals conduct electricity? Too few electrons for covalent bonds Low ionization energies Lattice consists of positive ions held together by delocalized valence electrons electron sea
Diamond. There are four types of solid: -Hard Structure - Tetrahedral atomic arrangement. What hybrid state do you think the carbon has?
Bonding in Solids Bonding in Solids There are four types of solid: 1. Molecular (formed from molecules) - usually soft with low melting points and poor conductivity. 2. Covalent network - very hard with
More informationThere are four types of solid:
Bonding in Solids There are four types of solid: 1. Molecular (formed from molecules) - usually soft with low melting points and poor conductivity. 2. Covalent network - very hard with very high melting
More informationMetallic & Ionic Solids. Crystal Lattices. Properties of Solids. Network Solids. Types of Solids. Chapter 13 Solids. Chapter 13
1 Metallic & Ionic Solids Chapter 13 The Chemistry of Solids Jeffrey Mack California State University, Sacramento Crystal Lattices Properties of Solids Regular 3-D arrangements of equivalent LATTICE POINTS
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 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 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 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 informationSolids. properties & structure
Solids properties & structure Determining Crystal Structure crystalline solids have a very regular geometric arrangement of their particles the arrangement of the particles and distances between them is
More informationChapter 12 Solids and Modern Materials
Sec$on 10.3 An Introduc+on to Structures and Types of Solids Chapter 12 Solids and Modern Materials Sec$on 10.3 An Introduc+on to Structures and Types of Solids Solids Amorphous Solids: Disorder in the
More informationStructure of Crystalline Solids
Structure of Crystalline Solids Solids- Effect of IMF s on Phase Kinetic energy overcome by intermolecular forces C 60 molecule llotropes of Carbon Network-Covalent solid Molecular solid Does not flow
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 informationMetallic and Ionic Structures and Bonding
Metallic and Ionic Structures and Bonding Ionic compounds are formed between elements having an electronegativity difference of about 2.0 or greater. Simple ionic compounds are characterized by high melting
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 informationChapter 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 informationProperties of Liquids and Solids. Vaporization of Liquids. Vaporization of Liquids. Aims:
Properties of Liquids and Solids Petrucci, Harwood and Herring: Chapter 13 Aims: To use the ideas of intermolecular forces to: Explain the properties of liquids using intermolecular forces Understand the
More informationProperties of Liquids and Solids. Vaporization of Liquids
Properties of Liquids and Solids Petrucci, Harwood and Herring: Chapter 13 Aims: To use the ideas of intermolecular forces to: Explain the properties of liquids using intermolecular forces Understand the
More informationFor this activity, all of the file labels will begin with a Roman numeral IV.
I V. S O L I D S Name Section For this activity, all of the file labels will begin with a Roman numeral IV. A. In Jmol, open the SCS file in IV.A.1. Click the Bounding Box and Axes function keys. Use the
More informationNotes on Solids and Liquids
THE LIQUID STATE Notes on Solids and Liquids Why do liquids tend to bead up when on a solid surface? The effect of uneven pull on surface molecules draws them into the body of the liquid causing droplet
More informationStates 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 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 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 informationChem 728 Introduction to Solid Surfaces
Chem 728 Introduction to Solid Surfaces Solids: hard; fracture; not compressible; molecules close to each other Liquids: molecules mobile, but quite close to each other Gases: molecules very mobile; compressible
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 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 informationCrystalline Solids. Amorphous Solids
Crystal Structure Crystalline Solids Possess rigid and long-range order; atoms, molecules, or ions occupy specific positions the tendency is to maximize attractive forces Amorphous Solids lack long-range
More informationCHEM Principles of Chemistry II Chapter 10 - Liquids and Solids
CHEM 1212 - Principles of Chemistry II Chapter 10 - Liquids and Solids 10.1 Intermolecular Forces recall intramolecular (within the molecule) bonding whereby atoms can form stable units called molecules
More informationWhat happens when substances freeze into solids? Less thermal energy available Less motion of the molecules More ordered spatial properties
Chapter #16 Liquids and Solids 16.1) Intermolecular Forces 16.2) The Liquid State 16.3) An Introduction to Structures and Types of Solids 16.4) Structure and Bonding of Metals 16.5) Carbon and Silicon:
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 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 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 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 informationIntroduction to Solid State Physics or the study of physical properties of matter in a solid phase
Introduction to Solid State Physics or the study of physical properties of matter in a solid phase Prof. Germar Hoffmann 1. Crystal Structures 2. Reciprocal Lattice 3. Crystal Binding and Elastic Constants
More informationChapter 3. The structure of crystalline solids 3.1. Crystal structures
Chapter 3. The structure of crystalline solids 3.1. Crystal structures 3.1.1. Fundamental concepts 3.1.2. Unit cells 3.1.3. Metallic crystal structures 3.1.4. Ceramic crystal structures 3.1.5. Silicate
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 informationLiquids 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 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 informationIntermolecular Forces, Liquids, Solids. IM Forces and Physical Properties
Intermolecular Forces, Liquids, Solids Interactions Between Molecules: What does it take to separate two (or more) molecules from one another? or What holds molecules close to one another? Structure/Property
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 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 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 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 informationChapter 12. Solids and Modern Materials
Lecture Presentation Chapter 12 Solids and Modern Materials Graphene Thinnest, strongest known material; only one atom thick Conducts heat and electricity Transparent and completely impermeable to all
More informationS.No. Crystalline Solids Amorphous solids 1 Regular internal arrangement of irregular internal arrangement of particles
Classification of solids: Crystalline and Amorphous solids: S.No. Crystalline Solids Amorphous solids 1 Regular internal arrangement of irregular internal arrangement of particles particles 2 Sharp melting
More information1.4 Crystal structure
1.4 Crystal structure (a) crystalline vs. (b) amorphous configurations short and long range order only short range order Abbildungen: S. Hunklinger, Festkörperphysik, Oldenbourg Verlag represenatives of
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 informationAtomic Arrangement. Primer Materials For Science Teaching Spring
Atomic Arrangement Primer Materials For Science Teaching Spring 2016 31.3.2015 Levels of atomic arrangements No order In gases, for example the atoms have no order, they are randomly distributed filling
More informationSolids. Adapted from a presentation by Dr. Schroeder, Wayne State University
Solids Adapted from a presentation by Dr. Schroeder, Wayne State University Properties of Solids Definite shape, definite volume Particles are CLOSE together, so Attractive forces (bonds or IMF s) are
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 information4. Interpenetrating simple cubic
2 1. The correct structure t of CsClCl crystal is 1. Simple cubic 2. Body centered cubic 3. Face centered cubic 4. Interpenetrating simple cubic If corner as well as the particle at the center are same
More informationChapter 9. Liquids and Solids
Chapter 9 Liquids and Solids Chapter 9 Table of Contents (9.1) (9.2) (9.3) (9.4) (9.5) (9.6) (9.7) (9.8) (9.9) (9.10) Intermolecular forces The liquid state An introduction to structures and types of solids
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 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 informationSOLID STATE MODULE - 3. Objectives. Solid State. States of matter. Notes
Solid State MODULE - 3 8 SOLID STATE Y ou are aware that the matter exists in three different states viz., solid, liquid and gas. In these, the constituent particles (atoms, molecules or ions) are held
More informationSOLID STATE CHEMISTRY
SOLID STATE CHEMISTRY Crystal Structure Solids are divided into 2 categories: I. Crystalline possesses rigid and long-range order; its atoms, molecules or ions occupy specific positions, e.g. ice II. Amorphous
More informationAtomic Arrangement. Primer in Materials Spring
Atomic Arrangement Primer in Materials Spring 2017 30.4.2017 1 Levels of atomic arrangements No order In gases, for example the atoms have no order, they are randomly distributed filling the volume to
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 informationPhysical Chemistry I. Crystal Structure
Physical Chemistry I Crystal Structure Crystal Structure Introduction Crystal Lattice Bravis Lattices Crytal Planes, Miller indices Distances between planes Diffraction patters Bragg s law X-ray radiation
More informationWhy is water so awesome?
Why is water so awesome? (Near) universal solvent The high polarity (and, therefore, hydrogen bonding power) of water means it can dissolve so many compounds ionic compounds, polar, nonionic compounds
More informationIonic Bonding. Example: Atomic Radius: Na (r = 0.192nm) Cl (r = 0.099nm) Ionic Radius : Na (r = 0.095nm) Cl (r = 0.181nm)
Ionic Bonding Ion: an atom or molecule that gains or loses electrons (acquires an electrical charge). Atoms form cations (+charge), when they lose electrons, or anions (- charge), when they gain electrons.
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 informationStates of Matter SM VIII (post) Crystallography. Experimental Basis. Experimental Basis Crystal Systems Closed Packing Ionic Structures
States of Matter SM VIII (post) Crystallography Experimental Basis Crystal Systems Closed Packing Ionic Structures Ref 12: 8 22-1 Experimental Basis is X-ray diffraction; see HT Fig. 21.1, Pet. Fig. 12.43
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 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 informationUnit wise Marks Distribution of 10+2 Syllabus
Unit wise Marks Distribution of 10+2 Syllabus S.No Unit Name Marks 1 I Solid State 4 2 II Solutions 5 3 III Electro Chemistry 5 4 IV Chemical Kinetics 5 5 V Surface Chemistry 4 6 VI General Principles
More informationEverything starts with atomic structure and bonding
Everything starts with atomic structure and bonding not all energy values can be possessed by electrons; e- have discrete energy values we call energy levels or states. The energy values are quantized
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 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 informationPROPERTIES 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 informationCRYSTAL STRUCTURES WITH CUBIC UNIT CELLS
CRYSTAL STRUCTURES WITH CUBIC UNIT CELLS Crystalline solids are a three dimensional collection of individual atoms, ions, or whole molecules organized in repeating patterns. These atoms, ions, or molecules
More informationChapter 10. Liquids and Solids. Copyright 2017 Cengage Learning. All Rights Reserved.
Chapter 10 Liquids and Solids Chapter 10 Table of Contents (10.1) (10.2) (10.3) (10.4) (10.5) Intermolecular forces The liquid state An introduction to structures and types of solids Structure and bonding
More informationLiquids and Solids Chapter 10
Liquids and Solids Chapter 10 Nov 15 9:56 AM Types of Solids Crystalline solids: Solids with highly regular arrangement of their components Amorphous solids: Solids with considerable disorder in their
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 information1051-3rd Chem Exam_ (A)
1051-3rd Chem Exam_1060111(A) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The molecular-orbital model for Ge shows it to be A) a conductor,
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 information1051-3rd Chem Exam_ (B)
1051-3rd Chem Exam_1060111(B) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) In liquids, the attractive intermolecular forces are. A) strong enough
More information1051-3rd Chem Exam_ (C)
1051-3rd Chem Exam_1060111(C) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The hybridizations of iodine in IF3 and IF5 are and, respectively.
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 informationSolid Type of solid Type of particle Al(s) aluminium MgCl2 Magnesium chloride S8(s) sulfur
QUESTION (2017:1) (iii) Sodium chloride, NaCl, is another compound that is excreted from the body in sweat. Use your knowledge of structure and bonding to explain the dissolving process of sodium chloride,
More information1 8 =1 8 8 =1 6 =3. Unit cell Atoms at corner Atoms at faces Atoms at centre. Total no. of atoms per unit cell. bcc. fcc
Q. No. Amorphous substances show () Short and long range order (2) Short range order (3) Long range order (4) Have no sharp M.P. Option and 3 are correct Option 2 2 and 3 are correct Option 3 3 and 4 are
More informationCovalent bonding does not involve electrostatic attraction between oppositely charged particles.
SCH3U7 - Topic 4: Bonding Review SL Which of these bonding types would not be classified as strong? Metallic Covalent Ionic Dipole dipole The bond dissociation energy of NaCl is 411 kj mol -1, while that
More informationChemical Bonding Ionic Bonding. Unit 1 Chapter 2
Chemical Bonding Ionic Bonding Unit 1 Chapter 2 Valence Electrons The electrons responsible for the chemical properties of atoms are those in the outer energy level. Valence electrons - The s and p electrons
More informationModule 6 : PHYSICS OF SEMICONDUCTOR DEVICES Lecture 32 : Bonding in Solids
Module 6 : PHYSICS OF SEMICONDUCTOR DEVICES Lecture 32 : Bonding in Solids Objectives In this course you will learn the following Bonding in solids. Ionic and covalent bond. Structure of Silicon Concept
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 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 informationHW# 5 CHEM 281 Louisiana Tech University, POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3. Structures of Ionic Solids. Why?
HW# 5 CHEM 281 Louisiana Tech University, POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3. Structures of Ionic Solids. Why? Many ionic structures may be described as close-packed
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 informationCritical Temperature - the temperature above which the liquid state of a substance no longer exists regardless of the pressure.
Critical Temperature - the temperature above which the liquid state of a substance no longer exists regardless of the pressure. Critical Pressure - the vapor pressure at the critical temperature. Properties
More informationINTERMOLECULAR FORCES AND CONDENSED STATES
INTERMOLECULAR FORCES AND CONDENSED STATES I. Intermolecular Forces A. Types of Intermolecular Forces. 1. Van der Waals forces = attractive forces that exist between neutral molecules. a. Are much weaker
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 informationIonic Bonding. Chem
Whereas the term covalent implies sharing of electrons between atoms, the term ionic indicates that electrons are taken from one atom by another. The nature of ionic bonding is very different than that
More informationAtoms & Their Interactions
Lecture 2 Atoms & Their Interactions Si: the heart of electronic materials Intel, 300mm Si wafer, 200 μm thick and 48-core CPU ( cloud computing on a chip ) Twin Creeks Technologies, San Jose, Si wafer,
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 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 informationSolid State. Subtopics
01 Solid State Chapter 01: Solid State Subtopics 1.0 Introduction 1.1 Classification of solids 1.2 Classification of crystalline solids 1.3 Unit cell, two and three dimensional lattices and number of atoms
More informationCrystallographic structure Physical vs Chemical bonding in solids
Crystallographic structure Physical vs Chemical bonding in solids Inert gas and molecular crystals: Van der Waals forces (physics) Water and organic chemistry H bonds (physics) Quartz crystal SiO 2 : covalent
More informationUnit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules
Unit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules 1. Ionic bonds 2. Covalent bonds (also co-ordinate covalent bonds) 3. Metallic bonds 4. Van der Waals forces
More informationBonding and Packing: building crystalline solids
Bonding and Packing: building crystalline solids The major forces of BONDING Gravitational forces: F = G m m 1 2 F = attractive forces between 2 bodies G = universal graviational constant (6.6767 * 10
More informationExperiment 7: Understanding Crystal Structures
Experiment 7: Understanding Crystal Structures To do well in this laboratory experiment you need to be familiar with the concepts of lattice, crystal structure, unit cell, coordination number, the different
More informationBonding and Dynamics. Outline Bonding and Dynamics Water Interactions Self Ionization of Water Homework
Liquid Water Structure In liquid water, most of the water molecules have the same local environment as in ice but the long range structure of ice disappears due to motion of the molecules. Bonds between
More information554 Chapter 10 Liquids and Solids
554 Chapter 10 Liquids and Solids above 7376 kpa, CO 2 is a supercritical fluid, with properties of both gas and liquid. Like a gas, it penetrates deep into the coffee beans; like a liquid, it effectively
More information