Chapter 2: INTERMOLECULAR BONDING (4rd session)
|
|
- Charlotte Elliott
- 6 years ago
- Views:
Transcription
1 Chapter 2: INTERMOLECULAR BONDING (4rd session) ISSUES TO ADDRESS... Secondary bonding The structure of crystalline solids 1
2 REVIEW OF PREVIOUS SESSION Bonding forces & energies Interatomic vs. intermolecular bonds Interatomic bonds 1) ionic bonding 2) covalent bonding 3) metallic bonding 2
3 INTERATOMIC & INTERMOLECULAR BONDS There different types of primary or chemical bond are found in solids: Ionic bonding Covalent bonding Metallic bonding Secondary or van der Waals bonding (physical forces) Fluctuating induced dipole bonds Polar molecule-induced dipole bonds Permanent dipole bonds 3
4 SECONDARY BONDING Whereas primary bonds involve atom-to-atom attractive forces, secondary bonds involve attraction forces between molecules -No transfer or sharing of electrons -Bonds are weaker than primary bonds Arises from interaction between atomic or molecular dipoles Fig 2.12 Schematic illustration of can der Waals bonding between two dipoles 4
5 POLAR MOLECULE Polar molecules have an asymmetrical electrical structure due to the difference in negative and positive charge found throughout the molecule (unequal distribution of charges) Fig 2.14 Schematic representation of a polar hydrogen chloride molecule. 5
6 PERMANENT DIPOLE BONDS Arises from interaction btw adjacent dipoles-molecule (polar molecules) -general case: secondary bonding Adapted from Fig. 2.15, Callister & Rethwisch 8e. -ex: liquid HCl H Cl secondary bonding H Cl -ex: polymer secondary bonding Hydrogen bonding is a special case of polar molecule bonding 6
7 HYDROGEN BONDING -ex: polymer secondary bonding Hydrogen bond is a special case of polar molecule bonding Nylon 6,6 structure 7
8 HYDROGEN BONDING Source: 8
9 FLUCTUATING INDUCED DIPOLES Small electric dipoles were created because of the constant vibrational motion of atoms Fig 2.13 (a) an electrically symmetric atom and (b) an induced atomic dipole. ex: liquid H 2 H 2 H 2 asymmetric electron clouds secondary bonding H H H secondary bonding H Adapted from Fig Polar molecule-induced dipole bonds 9
10 Type Ionic Summary: BONDING Bond Energy Comments Large! Nondirectional (ceramics) Covalent Metallic Variable large-diamond small-bismuth Variable large-tungsten small-mercury Directional (semiconductors, ceramics polymer chains) Nondirectional (metals) Secondary smallest Directional inter-chain (polymer) inter-molecular 10
11 Summary: Primary Bonds Ceramics (Ionic & covalent bonding): Metals (Metallic bonding): Large bond energy large T m large E small a Variable bond energy moderate T m moderate E moderate a Polymers (Covalent & Secondary): Directional Properties Secondary bonding dominates small T m small E large a 11
12 Chapter 3: THE STRUCTURE OF CRYSTALLINE SOLIDS Crystalline materials... atoms pack in repeating or periodic 3D arrays over large atomic distances typical of: -metals -many ceramics -some polymers Noncrystalline materials... atoms have no periodic packing disordered & random atomic distribution occurs for: -complex structures -rapid cooling "Amorphous" = Noncrystalline crystalline SiO2 Adapted from Fig. 3.23(a), Callister & Rethwisch 8e. Si Oxygen noncrystalline SiO2 Adapted from Fig. 3.23(b), Callister & Rethwisch 8e. 12
13 UNIT CELLS The smallest repeat entities subdivided from the crystal structure (lattice) Unit cell is the basic structural unit or building block of the crystal structure which contains the complete lattice pattern of a crystal Unit sells build up the macroscopic 3-D structure of the lattice (crystal structure) Adapted from Fig. 3.2(c), Callister & Rethwisch 8e. 13
14 UNIT CELLS (con t) Atoms are modeled as identical hard-spheres. Corners of a unit cell coincides with the center of the hard-sphere atoms. In a metal, each atom has the same number of nearestneighbor or touching atoms = coordination number 14
15 METALLIC CRYSTAL STRUCTURES (con t) How can we stack metal atoms to minimize empty space? 2-dimensions vs. Now stack these 2-D layers to make 3-D structures How much can be filled? Pack as tightly as possible 15
16 SIMPLE CUBIC STRUCTURE (SC) Rare due to low packing density (only Po has this structure) Close-packed directions are cube edges. Coordination # = 6 (# nearest neighbors) (Courtesy P.M. Anderson) (Source: 16
17 ATOMIC PACKING FACTOR (APF) APF = Volume of atoms in unit cell* Volume of unit cell APF for a simple cubic structure = 0.52 a *assume hard spheres close-packed directions contains 8 x 1/8 = 1 atom/unit cell Adapted from Fig. 3.24, Callister & Rethwisch 8e. R=0.5a atoms unit cell APF = 1 volume 4 3 p (0.5a) 3 atom a 3 volume unit cell 17
18 FACE CENTERED CUBIC (FCC) Atoms touch each other along face diagonals. --Note: All atoms are identical; the face-centered atoms are shaded differently only for ease of viewing. ex: Al, Cu, Au, Pb, Ni, Pt, Ag Coordination # = 12 (Courtesy P.M. Anderson) Adapted from Fig. 3.1, Callister & Rethwisch 8e. 4 atoms/unit cell: 6 face x 1/2 + 8 corners x 1/8 (Source: 18
19 ATOMIC PACKING FACTOR: FCC APF for a face-centered cubic structure = 0.74 maximum achievable APF 2 a a Adapted from Fig. 3.1(a), Callister & Rethwisch 8e. atoms unit cell APF = Close-packed directions: length = 4R = 2 a Unit cell contains: 6 x 1/2 + 8 x 1/8 = 4 atoms/unit cell p ( 2 a/4 ) 3 a 3 volume atom volume unit cell 19
20 BODY CENTERED CUBIC (BCC) Atoms touch each other along cube diagonals (closed-pack. --Note: All atoms are identical; the center atom is shaded differently only for ease of viewing. ex: Cr, W, Fe (a), Tantalum, Molybdenum Coordination # = 8 (Courtesy P.M. Anderson) Adapted from Fig. 3.2, Callister & Rethwisch 8e. 2 atoms/unit cell: 1 center + 8 corners x 1/8 (Source: 20
21 ATOMIC PACKING FACTOR: BCC APF for a body-centered cubic structure = a a 2 a Adapted from Fig. 3.2(a), Callister & Rethwisch 8e. atoms unit cell APF = R 2 a 4 3 p ( 3 a/4 ) 3 a 3 Close-packed directions: length = 4R = 3 a volume unit cell volume atom 21
22 THEORETICAL DENSITY, r Density = r = r = Mass of Atoms in Unit Cell Total Volume of Unit Cell n A V C N A where n = number of atoms/unit cell A = atomic weight V C = Volume of unit cell = a 3 for cubic N A = Avogadro s number = x atoms/mol 22
23 Theoretical Density, r Ex: Cr (BCC) A = g/mol R = nm n = 2 atoms/unit cell Adapted from Fig. 3.2(a), Callister & Rethwisch 8e. volume unit cell atoms unit cell r = R a a x a = 4R/ 3 = nm g mol r theoretical r actual atoms mol = 7.18 g/cm 3 = 7.19 g/cm 3 23
24 Densities of Material Classes In general r metals > r ceramics > r polymers Why? Metals have... close-packing (metallic bonding) often large atomic masses Ceramics have... less dense packing often lighter elements Polymers have... low packing density (often amorphous) lighter elements (C,H,O) Composites have... intermediate values r (g/cm 3 ) Metals/ Alloys Platinum Gold, W Tantalum Silver, Mo Cu,Ni Steels Tin, Zinc Titanium Aluminum Magnesium Graphite/ Ceramics/ Semicond Polymers Data from Table B.1, Callister & Rethwisch, 8e. Composites/ fibers B ased on data in Table B1, Callister *GFRE, CFRE, & AFRE are Glass, Carbon, & Aramid Fiber-Reinforced Epoxy composites (values based on 60% volume fraction of aligned fibers in an epoxy matrix). Zirconia Al oxide Diamond Si nitride Glass - soda Concrete Silicon G raphite PTFE Silicone PVC PET PC H DPE, PS PP, LDPE Glass fibers GFRE* Carbon fibers CFRE * A ramid fibers AFRE * Wood 24
25 SUMMARY Atoms may assemble into crystalline or amorphous structures. Common metallic crystal structures are SC, FCC, BCC, and HCP. We can predict the density of a material, provided we know the atomic weight, atomic radius, and crystal geometry (e.g., FCC, BCC, HCP). 25
26 Summary: CHARACTERISTICS OF METALS Crystalline structures in the solid state, almost without exception BCC, FCC, or HCP unit cells Atoms held together by metallic bonding Properties: high strength and hardness, high electrical and thermal conductivity FCC metals are generally ductile
27 Summary: CHARACTERISTICS OF CERAMICS Most ceramics have crystalline structures, while glass (SiO 2 ) is amorphous Molecules characterized by ionic or covalent bonding, or both Properties: high hardness and stiffness, electrically insulating, refractory, and chemically inert
28 Summary: CHARACTERISTICS OF POLYMERS Many repeating mers in molecule held together by covalent bonding Polymers usually carbon plus one or more other elements: H, N, O, and Cl Amorphous (glassy) structure or mixture of amorphous and crystalline Properties: low density, high electrical resistivity, low thermal conductivity, strength and stiffness vary widely
29 ANNOUNCEMENTS Answer: Why water expands upon freezing? Core problems to be solved: 2.23, 3.2, 3.3, 3.7, 3,8, and 3.9. Next lecture: Single crystals & polycrystals Crystal Systems 29
ENGR 151: Materials of Engineering MIDTERM 1 REVIEW MATERIAL
ENGR 151: Materials of Engineering MIDTERM 1 REVIEW MATERIAL MIDTERM 1 General properties of materials Bonding (primary, secondary and sub-types) Properties of different kinds of bonds Types of materials
More informationMetal Structure. Chromium, Iron, Molybdenum, Tungsten Face-centered cubic (FCC)
Metal Structure Atoms held together by metallic bonding Crystalline structures in the solid state, almost without exception BCC, FCC, or HCP unit cells Bodycentered cubic (BCC) Chromium, Iron, Molybdenum,
More informationAtomic Structure. Atomic weight = m protons + m neutrons Atomic number (Z) = # of protons Isotope corresponds to # of neutrons
Atomic Structure Neutrons: neutral Protons: positive charge (1.6x10 19 C, 1.67x10 27 kg) Electrons: negative charge (1.6x10 19 C, 9.11x10 31 kg) Atomic weight = m protons + m neutrons Atomic number (Z)
More informationMaterials for Civil and Construction Engineers CHAPTER 2. Nature of Materials
Materials for Civil and Construction Engineers CHAPTER 2 Nature of Materials Bonds 1. Primary Bond: forms when atoms interchange or share electrons in order to fill the outer (valence) shells like noble
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 informationPhysics of Materials: Bonding and Material Properties On The basis of Geometry and Bonding (Intermolecular forces) Dr.
: Bonding and Material Properties On The basis of Geometry and Bonding (Intermolecular forces) Dr. Anurag Srivastava Atal Bihari Vajpayee Indian Institute of Information Technology and Manegement, Gwalior
More informationStructure-Property Correlation [2] Atomic bonding and material properties
MME 297: Lecture 05 Structure-Property Correlation [2] Atomic bonding and material properties Dr. A. K. M. Bazlur Rashid Professor, Department of MME BUET, Dhaka Topics to discuss today... Review of atomic
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 informationCHAPTER 2: BONDING AND PROPERTIES
CHAPTER 2: BONDING AND PROPERTIES ISSUES TO ADDRESS... What promotes bonding? What types of bonds are there? What properties are inferred from bonding? Chapter 2-1 Atomic Structure (Freshman Chem.) atom
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 2. Atomic Structure
Chapter 2 Atomic Structure 2 6 (a) Aluminum foil used for storing food weighs about 0. g per square cm. How many atoms of aluminum are contained in one 6.25 cm 2 size of foil? (b) Using the densities and
More informationPhysics of Materials: Classification of Solids On The basis of Geometry and Bonding (Intermolecular forces)
Physics of Materials: Classification of Solids On The basis of Geometry and Bonding (Intermolecular forces) Dr. Anurag Srivastava Atal Bihari Vajpayee Indian Institute of Information Technology and Manegement,
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 informationClassification of Solids, Fermi Level and Conductivity in Metals Dr. Anurag Srivastava
Classification of Solids, Fermi Level and Conductivity in Metals Dr. Anurag Srivastava Web address: http://tiiciiitm.com/profanurag Email: profanurag@gmail.com Visit me: Room-110, Block-E, IIITM Campus
More informationChap 10 Part 3a.notebook December 12, 2017
Metallic Bonding and Semiconductors Chapter 10 Sect 4 Metallic Bonding positive metal ions surrounded by a "sea of electrons" Bonding is strong and nondirectional Iron, Silver, alloys, Brass, Bronze Forces
More informationChapter 2: Atomic structure and interatomic bonding
Chapter 2: Atomic structure and interatomic bonding Fundamental concepts Electrons in atoms Periodic table Bonding forces and energies Chapter 2 - Chapter 2: Atomic structure and interatomic bonding Fundamental
More informationChapter 2 Atoms, chemical bonding, material structure, and physical properties Homework Solutions
Chapter 2 Atoms, chemical bonding, material structure, and physical properties Homework Solutions Concept questions 1. The Pauli exclusion principle says that no two electrons that occupy the same space
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 informationProblem Set # 1 Solutions CHAPTERS 2 & 3 ATOMIC STRUCTURE AND INTERATOMIC BONDING and THE STRUCTURE OF CRYSTALLINE SOLIDS
Problem Set # Solutions CHAPTERS & ATOMIC STRUCTURE AND INTERATOMIC BONDING and THE STRUCTURE OF CRYSTALLINE SOLIDS Assigned:.7(a),.9,.,.6,.8,.7(a),.7,.9,. (graded problems indicated in bold).7 (a) The
More informationEGN 3365 Review on Bonding & Crystal Structures by Zhe Cheng
EGN 3365 Review on Bonding & Crystal Structures 2017 by Zhe Cheng Expectations on Chapter 1 Chapter 1 Understand materials can be classified in different ways by composition, property, application, or
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 informationWeek 11/Th: Lecture Units 28 & 29
Week 11/Th: Lecture Units 28 & 29 Unit 27: Real Gases Unit 28: Intermolecular forces -- types of forces between molecules -- examples Unit 29: Crystal Structure -- lattice types -- unit cells -- simple
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 informationDiamond. 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 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 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 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 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 informationRemember the purpose of this reading assignment is to prepare you for class. Reading for familiarity not mastery is expected.
Remember the purpose of this reading assignment is to prepare you for class. Reading for familiarity not mastery is expected. After completing this reading assignment and reviewing the intro video you
More informationME 254 MATERIALS ENGINEERING 1 st Semester 1430/ st Med-Term Exam (1.5 hrs)
ME 254 MATERIALS ENGINEERING 1 st Semester 1430/1431 1 st Med-Term Exam (1.5 hrs) قسم الهندسة الميكانيكية Question 1 a) Classify the materials based on their properties and performance, give some examples.
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 informationThe Science and Engineering of Materials, 4 th ed Donald R. Askeland Pradeep P. Phulé. Chapter 2 Atomic Structure
The Science and Engineering of Materials, 4 th ed Donald R. Askeland Pradeep P. Phulé Chapter 2 Atomic Structure Objectives of Chapter 2 The goal of this chapter is to describe the underlying physical
More informationAtomic Structure & Interatomic Bonding
Atomic Structure & Interatomic Bonding Chapter Outline Review of Atomic Structure Atomic Bonding Atomic Structure Atoms are the smallest structural units of all solids, liquids & gases. Atom: The smallest
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 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 3 THE STRUCTURE OF CRYSTALLINE SOLIDS PROBLEM SOLUTIONS
CHAPTER THE STRUCTURE OF CRYSTALLINE SOLIDS PROBLEM SOLUTIONS Fundamental Concepts.1 What is the difference between atomic structure and crystal structure? Atomic structure relates to the number of protons
More informationAtomic Bonding & Material Properties
Lecture 1 cont.. Atomic Bonding & Material Properties Bonding Forces and Energies Consider two isolated atoms separated by inter-atomic dist r r At large r, atoms do not interact. As r gets smaller, an
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 informationChapter 12: Structures & Properties of Ceramics
Chapter 12: Structures & Properties of Ceramics ISSUES TO ADDRESS... Bonding and structure of ceramic materials as compared with metals Chapter 12-1 Atomic Bonding in Ceramics Bonding: -- Can be ionic
More informationCHAPTER 2: BONDING AND PROPERTIES
CHAPTER 2: BONDING AND PROPERTIES ISSUES TO ADDRESS... What promotes bonding? What types of bonds are there? What properties are inferred from bonding? Chapter 2 1 Fundamental concepts Proton and electron,
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 informationAtomic Bonding and Materials Properties
MME131: Lecture 5 Atomic Bonding and Materials Properties A. K. M. B. Rashid Professor, Department of MME BUET, Dhaka Today s Topics What promote bonding? Classification and characteristics of atomic bond
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 2. Atomic Packing
Chapter 2. Atomic Packing Contents 2-1. Packing of directional bonding atoms 2-2. Packing of indirectional bonding in same size atoms 2-3. Packing of indirectional bonding in different size atoms 2-4.
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 informationLecture 6 - Bonding in Crystals
Lecture 6 onding in Crystals inding in Crystals (Kittel Ch. 3) inding of atoms to form crystals A crystal is a repeated array of atoms Why do they form? What are characteristic bonding mechanisms? How
More informationCHEM1902/ N-2 November 2014
CHEM1902/4 2014-N-2 November 2014 The cubic form of boron nitride (borazon) is the second-hardest material after diamond and it crystallizes with the structure shown below. The large spheres represent
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. 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
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 informationPractice Problems Set II
P1. For the HCP crystal structure, (a) show that the ideal c/a ratio is 1.633; (b) show that the atomic packing factor for HCP is 0.74. (a) A sketch of one-third of an HCP unit cell is shown below. Consider
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 informationStone Age (40,000 to 100,000 yrs ago): Stone tools, clay pots, skin
UTM UNIVERSITI TEKNOLOGI MALAYSIA COURSE LEARNING OBJECTIVES Introduce the field of Materials Science and Engineering 1. INTRODUCTION & ATOMIC STRUCTURE Provide introduction to the classification of materials
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 informationChapter 2: Atomic Structure
Chapter 2: Atomic Structure 2-1 What is meant by the term composition of a material? The chemical make-up of the material. 2-2 What is meant by the term structure of a material? The spatial arrangement
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 informationIntroduction to Engineering Materials ENGR2000 Chapter 14: Polymer Structures. Dr. Coates
Introduction to Engineering Materials ENGR2000 Chapter 14: Polymer Structures Dr. Coates 14.1 Introduction Naturally occurring polymers Wood, rubber, cotton, wool, leather, silk Synthetic polymers Plastics,
More informationVERY SHORT ANSWER TYPE QUESTIONS (1 Mark)
UNIT I 10 Chemistry-XII THE SOLID STATE VERY SHORT ANSWER TYPE QUESTIONS (1 Mark) Q. 1. What do you mean by paramagnetic substance? Ans. Weakly attracted by magnetic eld and these substances are made of
More informationATOMIC BONDING Atomic Bonding
ATOMIC BONDING Atomic Bonding Primary Bonds Secondary Bonds Ionic Covalent Metallic van der Waals 1. IONIC BONDING q 11 Na & 17 Cl These two ions are attracted to eachother by the electrostatic force developed
More informationChapter 2: Atomic structure and interatomic bonding. Chapter 2: Atomic structure and interatomic bonding
Chapter 2: Atomic structure and interatomic bonding Fundamental concepts Electrons in atoms Periodic table Bonding forces and energies Chapter 2: Atomic structure and interatomic bonding Fundamental concepts
More informationDensity. Physical Properties of Materials. Which Ones? THEORETICAL DENSITY, ρ. What would make a material dense? Concept Question. Physical Properties
Physical Properties of Materials Let s get physical!! density Physical Properties electrical thermal expansion shock Density Which Ones? melting point What is density? = THEORETICAL DENSITY, ρ Concept
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 information1. Demonstrate that the minimum cation-to-anion radius ratio for a coordination number of 8 is
1. Demonstrate that the minimum cation-to-anion radius ratio for a coordination number of 8 is 0.732. This problem asks us to show that the minimum cation-to-anion radius ratio for a coordination number
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 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 informationPrimary bonding: e- are transferred or shared Strong ( KJ/mol or 1-10 ev/atom) Secondary Bonding: no e -
Types of Bondings Primary bonding: e- are transferred or shared Strong (100-1000 KJ/mol or 1-10 ev/atom) Ionic: Strong Coulomb interaction among negative atoms (have an extra electron each) and positive
More informationRam Seshadri MRL 2031, x6129, These notes complement chapter 6 of Anderson, Leaver, Leevers and Rawlings
Crystals, packings etc. Ram Seshadri MRL 2031, x6129, seshadri@mrl.ucsb.edu These notes complement chapter 6 of Anderson, Leaver, Leevers and Rawlings The unit cell and its propagation Materials usually
More informationIMFA 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 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 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 informationChem 112 Exam 1 Version A Spring /16/ :00am/Odago, M. O.
Chem 112 Exam 1 Version A Spring 2011 02/16/2011 10:00am/Odago, M. O. 1. The pressure of a certain gas is measured to be 25.1 mmhg. What is this pressure expressed in units of pascals? (1 atm=1.0125 x10
More informationModule-2. Atomic Structures, Interatomic Bonding and Structure of Crystalline Solids
Module-2 Atomic Structures, Interatomic Bonding and Structure of Crystalline Solids Contents 1) Atomic Structure and Atomic bonding in solids 2) Crystal structures, Crystalline and Noncrystalline materials
More informationmaterials and their properties
materials and their properties macroscopic properties phase state strength / stiffness electrical conductivity chemical properties color / transparence spectroscopical properties surface properties density
More informationThe Solid State. Phase diagrams Crystals and symmetry Unit cells and packing Types of solid
The Solid State Phase diagrams Crystals and symmetry Unit cells and packing Types of solid Learning objectives Apply phase diagrams to prediction of phase behaviour Describe distinguishing features of
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 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 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 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 informationChapter 12: Structures & Properties of Ceramics
Chapter 12: Structures & Properties of Ceramics ISSUES TO ADDRESS... How do the crystal structures of ceramic materials differ from those for metals? How do point defects in ceramics differ from those
More information***Occurs when atoms of elements combine together to form compounds.*****
CHEMICAL BONDING ***Occurs when atoms of elements combine together to form compounds.***** Formation of compounds Involves valence electrons. PE is lower in bonded atoms. Attractive force that develops
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 informationOutlines. Types of bonds: - Ionic - Covalent - Metallic - Secondary bonding. Examples: - relation between bond energy and properties.
Outlines Types of bonds: - Ionic - Covalent - Metallic - Secondary bonding Examples: - relation between bond energy and properties Summary IONIC BONDING Electrostatic attraction between oppositely charged
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 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 informationIntroduction to Crystal Structure and Bonding. Prof.P. Ravindran, Department of Physics, Central University of Tamil Nadu, India
Introduction to Crystal Structure and Bonding 1 Prof.P. Ravindran, Department of Physics, Central University of Tamil Nadu, India http://folk.uio.no/ravi/semi2013 Fundamental Properties of matter 2 Matter:
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 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 informationChapter 2: Atomic Structure. Atomic structure, short- and long-range atomic arrangements, nanostructure, microstructure, and macrostructure.
Science and Engineering of Materials 7th Edition Askeland SOLUTIONS MANUAL Full clear download (no formatting errors) at: https://testbankreal.com/download/science-engineering-materials-7thedition-askeland-solutions-manual/
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 informationThe particles in a solid hold relatively fixed positions.
Section 3 Solids Key Terms crystalline solid melting crystal structure crystal melting point unit cell amorphous solid supercooled liquid The common expression solid as a rock suggests something that is
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 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 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 informationClass XII Chapter 1 The Solid State Chemistry
Question 1.1: Define the term 'amorphous'. Give a few examples of amorphous solids. Amorphous solids are the solids whose constituent particles are of irregular shapes and have short range order. These
More informationLecture Outline: Atomic Structure
Lecture Outline: Atomic Structure Electronic Structure of the Atom Periodic Table Types of Atomic Bonding, primary/secondary bonds Coordination and next neighbors Binding Energy, Interatomic Spacing, &
More informationMATERIAL SCIENCE TEST
MATERIAL SCIENCE TEST Answer the following questions about quartz. 1) The predominant type of bonding or attraction that holds quartz in a solid state is... a. Metallic bonding b. Covalent network bonding
More informationName AP CHEM / / Chapter 10 Outline Liquids and Solids
Name AP CHEM / / Chapter 10 Outline Liquids and Solids Intermolecular Forces The solid and liquid states are referred to as the condensed states of matter. Intramolecular forces exist within a molecule
More informationActivity 5&6: Metals and Hexagonal Close-Packing
Chemistry 150 Name(s): Activity 5&6: Metals and Hexagonal Close-Packing Metals are chemicals characterized by high thermal and electrical conductivity, malleability and ductility. Atoms are the smallest
More informationAtomic structure & interatomic bonding. Chapter two
Atomic structure & interatomic bonding Chapter two 1 Atomic Structure Mass Charge Proton 1.67 х 10-27 kg + 1.60 х 10-19 C Neutron 1.67 х 10-27 kg Neutral Electron 9.11 х 10-31 kg - 1.60 х 10-19 C Electron
More information