Semiconductors. Types of Solids. Figure 10.30: Energy-level diagrams for (a) an n-type semiconductor and (b) a ptype semiconductor.
|
|
- Collin Patterson
- 6 years ago
- Views:
Transcription
1 Figure 102: Partial representation of the molecular orbital energies in (a) diamond and (b) a typical metal Figure 1024: The p orbitals (a) perpendicular to the plane of the carbon ring system in graphite can combine to form (b) an extensive π-bonding network Figure 1025: Graphite consists of layers of carbon atoms Figure 1026: (top) The structure of quartz (empirical formula SiO2) Quartz contains chains of SiO4 tetrahedra (bottom) that share oxygen atoms Figure 1027: Examples of silicate anions, all of which are based on SiO44- tetrahedra Figure 1028: Twodimensional representations of (a) a quartz crystal and (b) a quartz glass 1
2 Figure 100: Energy-level diagrams for (a) an n-type semiconductor and (b) a ptype semiconductor Semiconductors substance in which some electrons can cross the band gap onductivity is enhanced by doping with group a or group 5a elements Figure 1029: (a) silicon crystal doped with arsenic, which has one more valence electron than silicon (b) silicon crystal doped with boron, which has one less electron than silicon Figure 101: The p-n junction involves the contact of a p-type and an n-type semiconductor Types of Solids molecular solid is a solid that consists of molecules held together by intermolecular forces Many solids are of this type Examples include solid sulfur, solid water (ice), and solid carbon dioxide (dry ice) 2
3 Figure 104: (a) Sulfur crystals (yellow) contain S8 molecules (b) White phosphorus (containing P4 molecules) is so reactive with the oxygen in air that it must be stored under water Figure 105: The holes that exist among closest packed uniform spheres (a) The trigonal hole formed by three spheres in a given plane (b) The tetrahedral hole formed when a sphere occupies a dimple formed by three spheres in an adjacent layer (c) The octahedral hole formed by six spheres in two adjacent layers Figure 106: (a) The location (X) of a tetrahedral hole in the face-centered cubic unit cell (b) One of the tetrahedral holes (c) The unit cell for ZnS where the S2- ions (yellow) are closest packed with the Zn2+ ions (red) in alternating tetrahedral holes Types of Solids n ionic solid is a solid that consists of cations and anions held together by electrical attraction of opposite charges (ionic bond) Examples include cesium chloride, sodium chloride, and zinc sulfide (but ZnS has considerable covalent character) Figure 107: (a) The locations (gray X) of the octahedral holes in the face-centered cubic unit cell (b) Representation of the unit cell for solid Nal
4 Figure 109: The rates of condensation and evaporation over time for a liquid sealed in a closed container Vapor Pressure is the of the vapor present at equilibrium is determined principally by the size of the intermolecular forces in the liquid increases significantly with Volatile liquids have high vapor s Figure 108: ehavior of a liquid in a closed container Figure 1040: (a) The vapor of a liquid can be measured easily using a simple barometer of the type shown here (b) The three liquids, water, ethanol (2H5OH), and diethyl ether [(2H5)2O], have quite different vapor s Figure 1041: iagram showing the reason vapor depends on 4
5 If we know the vapor, P 1, of a pure substance at, T 1, and want to determine the vapor, P 2, of the substance at a new, T 2, we can use the lausius-lapeyron equation Since for a pure substance: ln P 1 = - )H vap /RT 1 (1), and ln P 2 = - )H vap /RT 2, (2) we can subtract equation (1) from (2) to get: ln P 2 -lnp 1 = - )H vap /RT 2 -(-)H vap /RT 1 ) nd, collecting terms ln (P 2 /P 1 ) = ()H vap /R)(1/T 1-1/T 2 ) lausius-lapeyron Equation We noted earlier that vapor was a function of It has been demonstrated that the logarithm of the vapor of a liquid varies linearly with absolute, at equilibrium onsequently, the vapor of a liquid at two different s is described by: P H ln = P R 2 1 vap ( 1 T 1 1 T 2 ) Problem to onsider arbon disulfide, S 2, has a normal boiling point of 46 o (vapor = 760 mmhg) and a heat of vaporization of 268 kj/mol What is the vapor of carbon disulfide at 5 o? Substituting into the lausius-lapeyron equation, we obtain: P J/mol ln = ( 1 1 ) (760 mm Hg) 81 J/(mol K) 19 K 08 K = (225 K) ( K ) = 061 Figure 1042: (a) The vapor of water, ethanol, and diethyl ether as a function of (b) Plots of In(P vap ) versus 1/T (Kelvin ) for water, ethanol, and diethyl ether Problem to onsider arbon disulfide, S 2, has a normal boiling point of 46 o (vapor = 760 mmhg) and a heat of vaporization of 268 kj/mol What is the vapor of carbon disulfide at 5 o? Taking the antiln we obtain: P 2 = antiln(-061) (760 mm Hg) P 2 = antiln(-061) 760 mm Hg P 2 = 50 mm Hg
6 Figure 1044: The heating curve (not drawn to scale) for a given quantity of water where energy is added at a constant rate Heat of Phase Transition To melt a pure substance at its melting point requires an extra boost of energy to overcome lattice energies The heat needed to melt 1 mol of a pure substance is called the heat of fusion and denoted Hfus For ice, the heat of fusion is 601 kj/mol H 2O(s ) H 2O(l ); H fus = 601 kj Freezing Point The at which a pure liquid changes to a crystalline solid, or freezes, is called the freezing point The melting point is identical to the freezing point and is defined as the at which a solid becomes a liquid Unlike boiling points, melting points are affected significantly by only large changes Melting Point Figure 1046: Solid and liquid phases in equilibrium with the vapor Molecules break loose from lattice points and solid changes to liquid (Temperature is constant as melting occurs) vapor of solid = vapor of liquid 6
7 Figure 1047: Water in a closed system with a of 1 atm exerted on the piston No bubbles can form within the liquid as long as the vapor is less than 1 atm oiling Point The at which the vapor of a liquid equals the exerted on the liquid is called the boiling point s the of a liquid increases, the vapor increases until it reaches atmospheric t this point, stable bubbles of vapor form within the liquid This is called boiling The normal boiling point is the boiling point at 1 atm Figure 1048: The supercooling of water The extent of supercooling is given by S oiling chip releasing air bubbles acts as a nucleating agent for the bubbles that form when water boils oiling Point onstant when added energy is used to vaporize the liquid vapor of liquid = of surrounding atmosphere Problem 77, p 504
8 Problem to onsider The heat of vaporization of ammonia is 24 kj/mol How much heat is required to vaporize 100 kg of ammonia? First, we must determine the number of moles of ammonia in 100 kg (1000 g) 1mol NH g NH = 170 g NH 588 mol NH Phase iagrams elow is a typical phase diagram It consists of three curves that divide the diagram into regions labeled solid, liquid, and solid liquid Problem to onsider The heat of vaporization of ammonia is 24 kj/mol How much heat is required to vaporize 100 kg of ammonia? Then we can determine the heat required for vaporization 588 mol NH 24 kj/mol = Problem 8, p 504 kj Phase iagrams urve, dividing the solid region from the liquid region, represents the conditions under which the solid and liquid are in equilibrium solid liquid Phase iagram Represents phases as a function of and critical : above which the vapor can not be liquefied critical : required to liquefy T the critical critical point: critical and (for water, T c = 74 and 218 atm) Phase iagrams Usually, the melting point is only slightly affected by For this reason, the melting point curve,, is nearly vertical solid liquid
9 Phase iagrams If a liquid is more dense than its solid, the curve leans slightly to the left, causing the melting point to decrease with Phase iagrams urve, which divides the solid region from the eous region, represents the vapor s of the solid at various s solid liquid solid liquid Phase iagrams If a liquid is less dense than its solid, the curve leans slightly to the right, causing the melting point to increase with Phase iagrams The vapor at the critical is called the critical Note that curve ends at the critical point, P crit solid liquid solid liquid (see Figure 111) T crit Phase iagrams Figure 111: Observing the critical phenomenon urve, which divides the liquid region from the eous region, represents the boiling points of the liquid for various s solid liquid
10 Figure 1049: The phase diagram for water Figure 1052: The phase diagram for carbon dioxide Figure 1050: iagrams of various heating experiments on samples of water in a closed system Figure 1051: The phase diagram for water t point X on the phase diagram, water is a solid 10
Chapter 10. Liquids and Solids
Chapter 10. Liquids and Solids Three States of Matter H 2 O Volume constant constant no Shape constant no no Why in three different states? 1 Intermolecular Force dipole-dipole attraction V dip-dip : 1.
More informationChapter 16. Liquids and Solids. Chapter 16 Slide 1 of 87
Chapter 16 Liquids and Solids Chapter 16 Slide 1 of 87 Chapter Preview Intramolecular forces determine such molecular properties as molecular geometries and dipole moments. Intermolecular forces determine
More informationChapter 12: Intermolecular Forces and Liquids and Solids
1. Which one of the following substances is expected to have the highest boiling point? A) Br 2 B) Cl 2 C) F 2 D) I 2 3. Which one of the following substances is expected to have the highest boiling point?
More informationChapter 12 Metals. crystalline, in which particles are in highly ordered arrangement. (Have MP.)
Chapter 12 Metals 12.1 Classification of Solids Covalent Ionic Molecular Metallic Solids Solids Solids Solids Molecular consist of molecules held next to each other by IMF s. Relatively low to moderate
More information6. In this temperature time graph for the heating of H 2O at a constant rate, the segment DE represents the
1. Which of the following contains particles with the least freedom of motion? A) CO 2( ) B) HCl(aq) C) F 2(g) D) MgBr 2(s) E) C 6H 12O 6(aq) 2. During boiling, the temperature of a pure liquid substance
More informationThe Liquid State. The Liquid State. The Liquid State. The Liquid State. The Liquid State. Chemistry: The Molecular Science Moore, Stanitski and Jurs
Chemistry: The Molecular Science Moore, Stanitski and Jurs Chapter 11: Liquids, Solids and Materials A liquid forms when a gas condenses. This occurs at low T (and/or high P). Average intermolecular attraction
More informationFigure 16.31: Two-dimensional representations of (a) a quartz crystal and (b) a quartz glass.
Figure 16.31: Two-dimensional representations of (a) a quartz crystal and (b) a quartz glass. Figure 16.28: The p orbitals (a) perpendicular to the plane of th carbon ring system in graphite can combine
More informationChapter 11. States of Matter Liquids and Solids. Enthalpy of Phase Change
Chapter 11 solids: rigid ordered arrangement or particles fixed volume and shape not compressible particles very close together States of Matter Liquids and Solids liquids: fluid (flow) fixed volume but
More informationSolid State-1 1) Ionic solids are characterised by 1) Good conductivity in solid state 2) High vapour pressure 3) Low melting point 4) Solubility in polar solvents 2) Three metals X, Y and Z are crystallised
More informationSolids SECTION Critical Thinking
SECTION 10.3 Solids A gas has neither a definite volume nor a definite shape. A liquid has a definite volume, but not a definite shape. A solid, the third state, has a definite volume and a definite shape.
More informationCHAPTER THE SOLID STATE
133 CHAPTER THE SOLID STATE 1. The ability of a substances to assume two or more crystalline structures is called [1990] Isomerism Polymorphism Isomorphism Amorphism 2. Most crystals show good cleavage
More informationClass XII Chapter 1 The Solid State Chemistry
Class 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
More informationPhysical pharmacy. dr basam al zayady
Physical pharmacy Lec 5 dr basam al zayady Liquefaction of Gases: When a gas is cooled, it loses some of its kinetic energy in the form of heat, and the velocity of the molecules decreases. If pressure
More informationChapter 8: Molecules and Materials
Chapter 8: Molecules and Materials Condensed Phases - Solids Bonding in Solids Metals Insulators Semiconductors Intermolecular Forces Condensed Phases - Liquids Carbon There are three forms of the element
More information(a) 7.27 m (b) m (c) 5.38 m (d) 5380 m (e) m
1. The density of liquid cesium at 30 C is 1.87 g/ml. Because of its wide liquid range (28 to 678 C), cesium could be used as a barometer fluid at high temperatures. What height of cesium will be supported
More informationChapter 1. Crystal Structure
Chapter 1. Crystal Structure Crystalline solids: The atoms, molecules or ions pack together in an ordered arrangement Amorphous solids: No ordered structure to the particles of the solid. No well defined
More informationQ1. Which of the following diatomic species is paramagnetic?
Q1. Which of the following diatomic species is paramagnetic? A) O 2 B) N 2 C) F 2 D) CO E) NO + Q2. Which of the following statements about the CO 3 2 ion is false? A) One C O bond is shorter than the
More informationChemistry 145 Exam number 4 name 11/19/98 # Faraday s constant is 96,500 c/mole of electrons.
Chemistry 145 Exam number 4 name 11/19/98 # Faraday s constant is 96,500 c/mole of electrons. A.(16) An electrochemical cell is prepared with a strip of manganese metal dipping in to a 1.0 M MnSO 4 solution
More information(3) The compound boron nitride (BN) has a high melting point (2967 ºC), high density, and is very hard. What is the best classification of this solid?
Solids and Liquids Name: Period: (1) Identify the type of solid formed by each compound. (a) Ag (b) CO 2 (c) SiO 2 (d) wax (e) MgCl 2 (f) Fe (g) graphite (h) SO 2 (i) CaCO 3 (j) I 2 (k) rubber (l) SiC
More informationA. Description of the solid state according to the kinetic-molecular theory (KMT):
A. Description of the solid state according to the kinetic-molecular theory (KMT): Have a definite shape and volume and a slow average kinetic energy Particles of a SOLID appear to vibrate around fixed
More informationCHEM 200/202. Professor Gregory P. Holland Office: GMCS-213C. All s are to be sent to:
CHEM 200/202 Professor Gregory P. Holland Office: GMCS-213C All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 12:00 pm to 2:00 pm or by appointment.
More informationUnit-1 THE SOLID STATE QUESTIONS VSA QUESTIONS (1 - MARK QUESTIONS)
Unit-1 THE SOLID STATE QUESTIONS VSA QUESTIONS (1 - MARK QUESTIONS) 1. What are anistropic substances. 2. Why are amorphous solids isotropic in nature?. Why glass is regarded as an amorphous solid? 4.
More information1. Nickel has a face-centered-cubic unit cell. The density of nickel is 6.84 g/cm 3. Calculate the atomic radius of nickel.
ADDITIONAL PRACTICE ON UNIT CELLS 1. Nickel has a face-centered-cubic unit cell. The density of nickel is 6.84 g/cm 3. Calculate the atomic radius of nickel. 2. Tungsten metal exists in a body-centered-cubic
More informationAP Chemistry A. Allan Chapter 18 - The Representative Elements: Groups 1A through 4A
AP Chemistry A. Allan Chapter 18 - The Representative Elements: Groups 1A through 4A 18.1 A Survey of the Representative Elements A. Basic Trends 1. Metals tend to lose electrons and form cations 2. Nonmetals
More information6) Place the following substances in order of increasing vapor pressure at a given temperature.
CHM2045 F12 Exam #3 2012.12.07 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Choose the substance with the lowest viscosity. A) Cl 3 CCHCl 2
More informationInorganic Chemistry with Doc M. Fall Semester, 2012 Day 13. Ionic Thrills Part 3.
Inorganic Chemistry with Doc M. Fall Semester, 2012 Day 13. Ionic Thrills Part 3. Name(s): Element: Topics: 1. Octahedral and tetrahedral holes and the hcp lattice 2. Occupying the octahedral and tetrahedral
More informationLecture 3: Description crystal structures / Defects
Lecture 3: Description crystal structures / Defects Coordination Close packed structures Cubic close packing Hexagonal close packing Metallic structures Ionic structures with interstitial sites Important
More information19. H, S, C, and G Diagrams Module
HSC 8 - HSC Diagrams November 5, 4 43-ORC-J (8 9. H, S, C, and G Diagrams Module The diagram module presents the basic thermochemical data for the given species in graphical format. Eight different diagram
More informationGeneral Characteristics of Solid State
General Characteristics of Solid State (i) They have definite mass, volume and shape. (ii) Intermolecular distances are short. (iii) Intermolecular forces are strong. (iv) Their constituent particles (atoms,
More informationChapter 3: Atomic and Ionic Arrangements. Chapter 3: Atomic and Ionic Arrangements Cengage Learning Engineering. All Rights Reserved.
Chapter 3: Atomic and Ionic Arrangements 3-1 Learning Objectives 1. 2. 3. 4. 5. 6. 7. 8. Short-range order versus long-range order Amorphous materials Lattice, basis, unit cells, and crystal structures
More informationSolid State Device Fundamentals
Solid State Device Fundamentals ENS 345 Lecture Course by Alexander M. Zaitsev alexander.zaitsev@csi.cuny.edu Tel: 718 982 2812 Office 4N101b 1 Interatomic bonding Bonding Forces and Energies Equilibrium
More informationSolids. The difference between crystalline and non-crystalline materials is in the extent of ordering
Chapter 3 The Structure t of Crystalline Solids The difference between crystalline and non-crystalline materials is in the extent of ordering Both materials have the same composition but one is ordered
More information19. H, S, C, and G Diagrams Module
HSC - HSC Diagrams 15012-ORC-J 1 (8) 19. H, S, C, and G Diagrams Module The diagram module presents the basic thermochemical data for the given species in graphical format. Eight different diagram types
More informationCHAPTER. The Structure of Crystalline Solids
CHAPTER 4 The Structure of Crystalline Solids 1 Chapter 4: The Structure of Crystalline Solids ISSUES TO ADDRESS... What are common crystal structures for metals and ceramics? What features of a metal
More informationOrder in materials. Making Solid Stuff. Primary Bonds Summary. How do they arrange themselves? Results from atomic bonding. What are they?
Making Solid Stuff Primary Bonds Summary What are they? Results from atomic bonding So the atoms bond together! Order in materials No long range order to atoms Gases little or no interaction between components
More informationInorganic Chemistry with Doc M. Day 10. Ionic Thrills, Part 1.
Inorganic Chemistry with Doc M. Day 10. Ionic Thrills, Part 1. Topics: 1. Properties of ionic substances 7. Octahedral and tetrahedral holes 2. Cubic lattices and the periodic table 8. The cesium chloride
More informationSOLID STATE
SOLID STATE Short Answer Questions: 1. Derive Bragg s equation? Ans. Bragg s equation: W.H. Bragg has proposed an equation to explain the relation between inter planar distance (d) and wave length ( λ
More informationCHEM J-2 June 2014
CHEM1102 2014-J-2 June 2014 The diagram below shows the structure of an alloy of copper and gold with a gold atom at each of the corners and a copper atom in the centre of each of the faces. 2 What is
More informationPart 1. References: Gray: Chapter 6 OGN: Chapter 19 and (24.1)
Part 1 References: Gray: Chapter 6 OGN: Chapter 19 and (24.1) Aspects of Chemical Bonds Bonding in Chem 1a Atomic Structure Explain Atomic Line Spectra, Galaxies, etc. Shapes of Orbitals in Atoms for Bonding
More informationECE440 Nanoelectronics. Lecture 08 Review of Solid State Physics
ECE440 Nanoelectronics Lecture 08 Review of Solid State Physics A Brief review of Solid State Physics Crystal lattice, reciprocal lattice, symmetry Crystal directions and planes Energy bands, bandgap Direct
More informationNPTEL COURSE ADVANCED CERAMICS FOR STRATEGIC APPLICATIONS QUESTIONS AND ANSWERS
NPTEL COURSE ADVANCED CERAMICS FOR STRATEGIC APPLICATIONS QUESTIONS AND ANSWERS Q1: What do you understand by Ceramics? Ans: Ceramics are a group of chemical compounds, either simple (consisting of only
More informationCHAPTER 4: Oxidation. Chapter 4 1. Oxidation of silicon is an important process in VLSI. The typical roles of SiO 2 are:
Chapter 4 1 CHAPTER 4: Oxidation Oxidation of silicon is an important process in VLSI. The typical roles of SiO 2 are: 1. mask against implant or diffusion of dopant into silicon 2. surface passivation
More informationChapter Eight. Molecules and Materials. Chapter Eight Slide 1 of 99
Chapter Eight Molecules and Materials Chapter Eight Slide 1 of 99 Chapter Preview Intramolecular forces determine such molecular properties as molecular geometries and dipole moments. Intermolecular forces
More informationEngineering 45 The Structure and Properties of Materials Midterm Examination October 26, 1987
Engineering 45 The Structure and Properties of Materials Midterm Examination October 26, 1987 Problem 1: (a) The compound CsCl is an ordered arrangement of Cs and Cl over the sites of a BCC lattice. Draw
More informationE45 Midterm 01 Fall 2007! By the 0.2% offset method (shown on plot), YS = 500 MPa
1.!Mechanical Properties (20 points) Refer to the following stress-strain plot derived from a standard uniaxial tensile test of a high performance titanium alloy to answer the following questions. Show
More informationSOLID-STATE STRUCTURE.. FUNDAMENTALS
SOLID-STATE STRUCTURE.. FUNDAMENTALS Metallic Elements & Sphere Packing, Unit Celis, Coordination Number, Ionic Structures Stoichiometry PRELAB ASSIGNMENT Properties of Shapes & Patterns following question
More information(06) WMP/Jun10/CHEM5
Period 3 Elements 6 2 Sodium, aluminium and silicon are solid elements with a silver colour. These elements react with oxygen to form oxides with high melting points. Aluminium is a reactive metal, but
More informationCRYSTAL STRUCTURE TERMS
CRYSTAL STRUCTURE TERMS crystalline material - a material in which atoms, ions, or molecules are situated in a periodic 3-dimensional array over large atomic distances (all metals, many ceramic materials,
More informationLab IV: Electrical Properties
Lab IV: Electrical Properties Study Questions 1. How would the electrical conductivity of the following vary with temperature: (a) ionic solids; (b) semiconductors; (c) metals? Briefly explain your answer.
More informationThese metal centres interact through metallic bonding
The structures of simple solids The majority of inorganic compounds exist as solids and comprise ordered arrays of atoms, ions, or molecules. Some of the simplest solids are the metals, the structures
More information3.3 Minerals. Describe the characteristics that define minerals.
3.3 Minerals Describe the characteristics that define minerals. Are you a mineral? There used to be a TV commercial that said "you are what you eat." If that s true - and to some extent it is - then you
More informationChem 241. Lecture 19. UMass Amherst Biochemistry... Teaching Initiative
Chem 241 Lecture 19 UMass Amherst Biochemistry... Teaching Initiative Announcement March 26 Second Exam Recap Water Redox Comp/Disproportionation Latimer Diagram Frost Diagram Pourbaix Diagram... 2 Ellingham
More informationChapter 12: Structures & Properties of Ceramics
Chapter 12: Structures & Properties of Ceramics ISSUES TO ADDRESS... Review of structures for ceramics How are impurities accommodated in the ceramic lattice? In what ways are ceramic phase diagrams similar
More informationEXPERIMENT 3: Identification of a Substance by Physical Properties
EXPERIMENT 3: Identification of a Substance by Physical Properties Materials: Hot plate Digital balance Capillary tubes (3) Thermometer Beakers (250 ml) Watch glass Graduated Cylinder (10 ml) Mel-Temp
More informationFrom sand to silicon wafer
From sand to silicon wafer 25% of Earth surface is silicon Metallurgical grade silicon (MGS) Electronic grade silicon (EGS) Polycrystalline silicon (polysilicon) Single crystal Czochralski drawing Single
More informationTopic: Bargg Equation
1. Calculate the interplanar distance that has a second order reflection of 22.9 C for X-rays of wavelength of 0.348 nm. a) 0.384 nm b) 0.447 nm c) 0.894 nm d) 1.79 nm e) 0.302 nm 2. The interplanar distance
More informationPhase Diagrams Revised: 1/27/16 PHASE DIAGRAMS. Adapted from Bill Ponder, Collin College & MIT OpenCourseWare INTRODUCTION
PHASE DIAGRAMS Adapted from Bill Ponder, Collin College & MIT OpenCourseWare INTRODUCTION A phase diagram is a graphical representation of the physical states of a substance as they relate to temperature
More informationChemical reactions and electrolysis
Chemical reactions and electrolysis Higher Revision Questions Name: Class: Date: Time: 95 minutes Marks: 95 marks Comments: Page of 29 (a) Magnesium metal is shaped to make magnesium ribbon. Explain why
More informationUnit 1 The Solid State
Points to Remember Amorphous and Crystalline Solids Unit 1 The Solid State Amorphous- short range order, Irregular shape eg-glass Crystalline Solids- long range order, regular shape eg : NaCl Molecular
More informationMSE 352 Engineering Ceramics II
Kwame Nkrumah University of Science & Technology, Kumasi, Ghana MSE 352 Engineering Ceramics II 3 Credit Hours Ing. Anthony Andrews (PhD) Department of Materials Engineering Faculty of Mechanical and Chemical
More informationNeighbour s envy, Owner s pride, Silicon Valley s delight, a girl s best friend, Miner s blackjack! Is that you?
Introduction Neighbour s envy, Owner s pride, Silicon Valley s delight, a girl s best friend, Miner s blackjack! Is that you? Learning Objectives On completion of this topic you will be able to: 1. Identify
More informationWork hard. Be nice. Name: Period: Date: UNIT 10: Energy Lesson 5: Calculating Heat using q = mcδt!
Name: Period: Date: UNIT 10: Energy Lesson 5: Calculating Heat using q = mcδt! By the end of today, you will have an answer to: How can we calculate the amount of heat it takes to change the temperature?
More informationPhase Changes & Heating Curves
Add Important Phase Changes & Heating Curves Page: 579 Phase Changes & Heating Curves NGSS Standards: HS-PS3-1 MA Curriculum Frameworks 2006): 3.3 Knowledge/Understanding Goals: phases and phase changes
More informationHalbleiter Prof. Yong Lei Prof. Thomas Hannappel
Halbleiter Prof. Yong Lei Prof. Thomas Hannappel yong.lei@tu-ilmenau.de thomas.hannappel@tu-ilmenau.de http://www.tu-ilmenau.de/nanostruk/ Solid State Structure of Semiconductor Semiconductor manufacturing
More informationFree Electron Model What kind of interactions hold metal atoms together? How does this explain high electrical and thermal conductivity?
Electrical Good conductors of heat & electricity Create semiconductors Oxides are basic ionic solids Aqueous cations (positive charge, Lewis acids) Reactivity increases downwards in family Mechanical Lustrous
More informationDouble Award Science: Chemistry
New Specification Centre Number Candidate Number General Certificate of Secondary Education 2014 2015 Double Award Science: Chemistry Unit C1 Higher Tier ML [GSD22] WEDNESDAY 25 FEBRUARY 2015, MORNING
More informationSeawater TA Initials: for finished Activity. 1 & 2 Or lose 10% of credit!
Name: Section/ TA: Seawater TA Initials: for finished Activity. 1 & 2 Or lose 10% of credit! Seawater is an unusual substance. It is pure water mixed with various salts, trace elements, and gases. The
More informationMultiple choices (3 points each): 1. Shown on the right is A. an ethylene mer B. an ethylene monomer C. a vinyl monomer D.
Materials Science and Engineering Department MSE 200, Exam #4 ID number First letter of your last name: Name: No notes, books, or information stored in calculator memories may be used. Cheating will be
More informationMetallic crystal structures The atomic bonding is metallic and thus non-directional in nature
Chapter 3 The structure of crystalline solids Hw: 4, 6, 10, 14, 18, 21, 26, 31, 35, 39, 42, 43, 46, 48, 49, 51, 56, 61 Due Wensday 14/10/2009 Quiz1 on Wensday 14/10/2009 Why study the structure of crystalline
More information(a) Would you expect the element P to be a donor or an acceptor defect in Si?
MSE 200A Survey of Materials Science Fall, 2008 Problem Set No. 2 Problem 1: At high temperature Fe has the fcc structure (called austenite or γ-iron). Would you expect to find C atoms in the octahedral
More informationSECTION A. NATURAL SCIENCES TRIPOS Part IA. Friday 4 June to 4.30 MATERIALS AND MINERAL SCIENCES
NATURAL SCIENCES TRIPOS Part IA Friday 4 June 1999 1.30 to 4.30 MATERIALS AND MINERAL SCIENCES Answer five questions; two from each of sections A and B and one from section C. Begin each answer at the
More information7.3 Bonding in Metals > Chapter 7 Ionic and Metallic Bonding. 7.3 Bonding in Metals. 7.1 Ions 7.2 Ionic Bonds and Ionic Compounds
Chapter 7 Ionic and Metallic Bonding 7.1 Ions 7.2 Ionic Bonds and Ionic Compounds 7.3 Bonding in Metals 1 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. CHEMISTRY & YOU What
More informationMetals and Semi-Conductors
Metals and Semi-Conductors Unit Cells for Cubic Close- Packed Spheres Hexagonal Close- Packed Spheres Inorganic Chemistry Chapter 1: Table 3.2 What are the characteristics of the metals that might be correlated
More informationCHAPTER 5 IMPERFECTIONS IN SOLIDS PROBLEM SOLUTIONS
CHAPTER 5 IMPERFECTIONS IN SOLIDS PROBLEM SOLUTIONS Vacancies and Self-Interstitials 5.1 Calculate the fraction of atom sites that are vacant for copper at its melting temperature of 1084 C (1357 K). Assume
More informationImperfections: Good or Bad? Structural imperfections (defects) Compositional imperfections (impurities)
Imperfections: Good or Bad? Structural imperfections (defects) Compositional imperfections (impurities) 1 Structural Imperfections A perfect crystal has the lowest internal energy E Above absolute zero
More informationChapter 6. Multiphase Systems. Dr. M. A. A. Shoukat Choudhury Website:
Chapter 6 Multiphase Systems Dr. M. A. A. Shoukat Choudhury Email: shoukat@buet.ac.bd Website: http://teacher.buet.ac.bd/shoukat/ Multiphase Systems Why Study? - Phase change operations such as freezing,
More informationCrystal Defects. Perfect crystal - every atom of the same type in the correct equilibrium position (does not exist at T > 0 K)
Crystal Defects Perfect crystal - every atom of the same type in the correct equilibrium position (does not exist at T > 0 K) Real crystal - all crystals have some imperfections - defects, most atoms are
More informationCalcium Chloride A Guide to Physical Properties
Calcium Chloride A Guide to Physical Properties Table of Contents About This Guide... 1 Physical Properties of Calcium Chloride Physical Properties of Calcium Chloride and Hydrates... 2 Solubility.....................................................................................2
More informationStacking Oranges. Packing atoms together Long Range Order. What controls the nearest number of atoms? Hard Sphere Model. Hard Sphere Model.
{ Stacking atoms together Crystal Structure Stacking Oranges Packing atoms together Long Range Order Crystalline materials... atoms pack in periodic, 3D arrays typical of: -metals -many ceramics -some
More informationWarm-up: 2/6/15 2/9/2015 LATENT HEAT AND PHASE CHANGES INTERNAL ENERGY
If thermal energy is added to the water at a rate of 84 W, how much time would it take to bring the vat of water from room temperature (21.0 C) to boiling (100.0 C)? Warm-up: 2/6/15 { George Washington
More informationProcessing of Semiconducting Materials Prof. Pallab Banerjee Department of Material Science Indian Institute of Technology, Kharagpur
Processing of Semiconducting Materials Prof. Pallab Banerjee Department of Material Science Indian Institute of Technology, Kharagpur Lecture - 35 Oxidation I (Refer Slide Time: 00:24) Today s topic of
More informationNANDI NORTH DISTRICT JOINT MOCK EVALUATION TEST 2013
NAME:. SIGNATURE: INDEX NO:. DATE :.. 233/1 CHEMISTRY PAPER 1 THEORY JULY / AUGUST 2013 TIME: 2 HOURS NANDI NORTH DISTRICT JOINT MOCK EVALUATION TEST 2013 Kenya Certificate of Secondary Education (K.C.S.E.)
More informationThe Science and Engineering of Materials, 4 th ed Donald R. Askeland Pradeep P. Phulé. Chapter 3 Atomic and Ionic Arrangements
The Science and Engineering of Materials, 4 th ed Donald R. Askeland Pradeep P. Phulé Chapter 3 Atomic and Ionic Arrangements 1 Objectives of Chapter 3 To learn classification of materials based on atomic/ionic
More informationALE 20. Crystalline Solids, Unit Cells, Liquids and the Uniqueness of Water
Name Chem 162, Section: Group Number: ALE 20. Crystalline Solids, Unit Cells, Liquids and the Uniqueness of Water (Reference: pp. 463 473 of Sec. 12.6 Silberberg 5 th edition) How are the particles within
More informationFree Electron Model What kind of interactions hold metal atoms together? How does this explain high electrical and thermal conductivity?
Electrical Good conductors of heat & electricity Create semiconductors Oxides are basic ionic solids Aqueous cations (positive charge, Lewis acids) Reactivity increases downwards in family Free Electron
More informationDURATION: 1 hour 30 minutes
1 Our country, our future 545/1 S4 CHEMISTRY Exam 14 PAPER 1 DURATION: 1 hour 30 minutes Instructions - This paper consists of 50 compulsory objective questions - Answer the questions by writing the correct
More informationMcCord CH302 Exam 1 Spring 2017
112 version last name first name signature McCord CH302 Exam 1 Spring 2017 50375 / 50380 Reminder: Be sure and correctly bubble in your name, uteid, and version number on your bubblesheet. The Periodic
More informationOxygen Formula: O 2 Bonding: covalent Appearance: colourless gas. Oxygen is one of the two main gases in our atmosphere, the other being nitrogen.
Composition of the air Air is a mixture of gases. The approximate amount if each gas in dry air is shown in the pie chart (right), but you should be aware that air also contains a variable amount of water
More informationEFFECT OF CRYSTALORIENTATIONIN OXIDATION PROCESS OF VLSI FABRICATION
International Journal of Research in Engineering, Technology and Science, Volume VII, Special Issue, Feb 2017 www.ijrets.com, editor@ijrets.com, ISSN 2454-1915 EFFECT OF CRYSTALORIENTATIONIN OXIDATION
More informationICSE-Science 2 (Chemistry) 1996
ICSE-Science 2 (Chemistry) 1996 Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 15 minutes. This time is to be spent in reading
More informationChapter 16 Corrosion and Degradation of Materials
Chapter 16 Corrosion and Degradation of Materials Concept Check 16.1 Question: Would you expect iron to corrode in water of high purity? Why or why not? Answer: Iron would not corrode in water of high
More informationSECTION I (40 Marks) Attempt all questions from this Section
General Instructions 1. SECTION I (40 Marks) Attempt all questions from this Section Question 1 (a) Chlorine is subject of the following questions: [5] i. What is the atomicity of chlorine? ii. Name the
More informationChapter 13 THE GROUP 13 ELEMENTS. Exercises
Chapter 13 THE GROUP 13 ELEMENTS Exercises 13.2 (a) BBr 3 (l) + 3 H 2 O(l) H 3 BO 3 (aq) + 3 HBr(aq) (b) 2 Al(s) + 6 H + (aq) 2 Al 3+ (aq) + 3 H 2 (g) (c) 2 TlOH(aq) + CO 2 (g) Tl 2 CO 3 (s) + H 2 O(l)
More informationThermal decomposition. Metal carbonates
Decomposition reactions Copy correctly Up to 3% of a workbook Copying or scanning from ESA workbooks is subject to the New Zealand Copyright Act which limits copying to 3% of this workbook. Many compounds
More informationCHEMISTRY. SCIENCE Paper 2. (Two hours) You will not be allowed to write during the first 15 minutes.
CHEMISTRY SCIENCE Paper 2 (Two hours) Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 15 minutes. This time is to be spent in reading
More informationMR. D HR UV AS HE R I.C.S.E. BOA RD PAP ER ICSE-2005
MR D HR UV AS HE R ICSE BOA RD PAP ER 200 5 1 ICSE-2005 Section A (40 Marks) (Attempt all questions from this section) Question 1 (a) Write balanced equation s for the following reactions: - [5] (i) Potassium
More informationFINAL EXAM KEY. Professor Buhro. ID Number:
FINAL EXAM Chemistry 465 KEY 10 May 011 Professor Buhro KEY Signature KEY Print Name Clearly ID Number: Information. This is a closed-book exam; no books, notes, other students, other student exams, or
More informationThe forces between iodine molecules are stronger 1. (b) anything in range +30 to It contains ions which can move 1. (f) hydrogen iodine 1 [6]
M.(a) The forces between iodine molecules are stronger (b) anything in range +30 to +20 (c) Brown (d) 2 I + Cl 2 I 2 + 2 Cl (e) It contains ions which can move (f) hydrogen iodine [6] Page 2 M2.(a) giant
More informationLecture C4b Microscopic to Macroscopic, Part 4: X-Ray Diffraction and Crystal Packing
Lecture C4b Microscopic to Macroscopic, Part 4: X-Ray Diffraction and Crystal Packing X-ray Diffraction Max von Laue won the 1914 Nobel Prize for his discovery of the diffraction of x-rays by crystals.
More informationSEAWATER 101. Seawater s Amazing Physical and Chemical Properties. Introductory Oceanography Ray Rector - Instructor
SEAWATER 101 Seawater s Amazing Physical and Chemical Properties Introductory Oceanography Ray Rector - Instructor The Nature of Water Topics To Be Covered Elements of Water Chemical Bonding The Water
More information