sheet 1 of material science & engineering
questions on chapter 2 Atomic structures
and chapter 3 density computations
DR. Ahmed Ramadan 2016 - summer course
A crystalline solid possesses rigid and long-range order, with atoms occupying specific positions. An amorphous solid lacks a well-defined arrangement and long-range order. A unit cell is the basic repeating structural unit of a crystalline solid and defines the positions of atoms, molecules, or ions within the structure.
The document provides information on solidification processes and binary alloy systems. It discusses:
1) The three main steps in the solidification process: formation of stable nuclei, growth of nuclei into crystals, and formation of a grain structure.
2) The different types of solid solutions including substitutional and interstitial solid solutions. Substitutional solutions involve solute atoms replacing solvent atoms, while interstitial solutions involve solute atoms filling spaces between solvent atoms.
3) Phase diagrams and how they represent the relationship between temperature, composition, and phases in equilibrium for a binary alloy system. Key points include liquidus lines, triple points, and using phase diagrams to interpret cooling curves.
4) An
The document summarizes Week 2 of an MME 323 materials science course focusing on atomic structure and interatomic bonding. It outlines the lecture topics which include atomic number, mass, and configuration, quantum numbers, the periodic table, and primary bonding types like ionic, covalent, and metallic. The learning objectives are to define key atomic concepts and describe different bonding mechanisms. Ionic bonding occurs between metals and non-metals and involves electron transfer. Covalent bonding is between non-metals and the sharing of electrons. Metallic bonding is within metals and due to positively charged metal ions in a "sea" of delocalized electrons.
The document discusses key concepts in material technology including:
1. It defines the basic structure of atoms and different types of materials including elements, mixtures, and compounds.
2. It describes atomic structure including atomic number, atomic mass, and atomic orbits. The periodic table is introduced as a way to classify and understand elements and their properties.
3. Different types of crystal structures are defined including body centered cubic, face centered cubic, and hexagonal close packed. Bonding types such as covalent, metallic, and ionic are also introduced.
4. Terminology used in phase diagrams is defined including phases, equilibrium, composition, liquidus, and solidus. Binary alloy systems containing two components are also
This document contains 6 problems related to calculating properties of crystalline solids based on their crystal structure and lattice parameters:
1. Calculate the density of copper given its face-centered cubic (fcc) unit cell length and atomic mass.
2. Calculate the molecular mass of silver given its fcc unit cell length, density, and that it contains 4 atoms per unit cell.
3. Calculate the density of cesium chloride given its body-centered cubic (bcc) unit cell length and the atomic masses of cesium and chlorine.
4. Determine if iron crystals with a given unit cell length and density have a body-centered cubic or face-centered cubic structure based on its atomic mass.
The document discusses the crystal structures of crystalline solids. It describes three common crystal structures - face centered cubic (FCC), body centered cubic (BCC), and hexagonal close packed (HCP). FCC has a total of four atoms in the unit cell and is found in metals like copper and gold. BCC has an atomic packing factor of 0.68 and is exhibited by metals like iron and chromium. HCP has the same coordination number and packing factor as FCC and is found in metals such as magnesium and zinc. Crystallographic directions and planes are also introduced and ways to determine their indices are explained.
- The document discusses different crystal structures including simple cubic, body-centered cubic, face-centered cubic, and hexagonal closely packed.
- Key properties like number of atoms per unit cell, atomic radius, coordination number, and atomic packing factor are defined and calculated for each structure.
- There are seven basic crystal systems that materials can belong to depending on their lattice parameters and angles between axes. The most common systems are cubic, hexagonal, and tetragonal.
This document discusses crystal structures and their properties. It describes how atoms are arranged in crystalline solids through ordered unit cells that form a repeating lattice. The main crystal structures for metals are body-centered cubic, face-centered cubic, and hexagonal close-packed. It explains how to calculate properties like density from the unit cell parameters and atomic positions. Direction vectors are used to describe crystallographic directions.
A crystalline solid possesses rigid and long-range order, with atoms occupying specific positions. An amorphous solid lacks a well-defined arrangement and long-range order. A unit cell is the basic repeating structural unit of a crystalline solid and defines the positions of atoms, molecules, or ions within the structure.
The document provides information on solidification processes and binary alloy systems. It discusses:
1) The three main steps in the solidification process: formation of stable nuclei, growth of nuclei into crystals, and formation of a grain structure.
2) The different types of solid solutions including substitutional and interstitial solid solutions. Substitutional solutions involve solute atoms replacing solvent atoms, while interstitial solutions involve solute atoms filling spaces between solvent atoms.
3) Phase diagrams and how they represent the relationship between temperature, composition, and phases in equilibrium for a binary alloy system. Key points include liquidus lines, triple points, and using phase diagrams to interpret cooling curves.
4) An
The document summarizes Week 2 of an MME 323 materials science course focusing on atomic structure and interatomic bonding. It outlines the lecture topics which include atomic number, mass, and configuration, quantum numbers, the periodic table, and primary bonding types like ionic, covalent, and metallic. The learning objectives are to define key atomic concepts and describe different bonding mechanisms. Ionic bonding occurs between metals and non-metals and involves electron transfer. Covalent bonding is between non-metals and the sharing of electrons. Metallic bonding is within metals and due to positively charged metal ions in a "sea" of delocalized electrons.
The document discusses key concepts in material technology including:
1. It defines the basic structure of atoms and different types of materials including elements, mixtures, and compounds.
2. It describes atomic structure including atomic number, atomic mass, and atomic orbits. The periodic table is introduced as a way to classify and understand elements and their properties.
3. Different types of crystal structures are defined including body centered cubic, face centered cubic, and hexagonal close packed. Bonding types such as covalent, metallic, and ionic are also introduced.
4. Terminology used in phase diagrams is defined including phases, equilibrium, composition, liquidus, and solidus. Binary alloy systems containing two components are also
This document contains 6 problems related to calculating properties of crystalline solids based on their crystal structure and lattice parameters:
1. Calculate the density of copper given its face-centered cubic (fcc) unit cell length and atomic mass.
2. Calculate the molecular mass of silver given its fcc unit cell length, density, and that it contains 4 atoms per unit cell.
3. Calculate the density of cesium chloride given its body-centered cubic (bcc) unit cell length and the atomic masses of cesium and chlorine.
4. Determine if iron crystals with a given unit cell length and density have a body-centered cubic or face-centered cubic structure based on its atomic mass.
The document discusses the crystal structures of crystalline solids. It describes three common crystal structures - face centered cubic (FCC), body centered cubic (BCC), and hexagonal close packed (HCP). FCC has a total of four atoms in the unit cell and is found in metals like copper and gold. BCC has an atomic packing factor of 0.68 and is exhibited by metals like iron and chromium. HCP has the same coordination number and packing factor as FCC and is found in metals such as magnesium and zinc. Crystallographic directions and planes are also introduced and ways to determine their indices are explained.
- The document discusses different crystal structures including simple cubic, body-centered cubic, face-centered cubic, and hexagonal closely packed.
- Key properties like number of atoms per unit cell, atomic radius, coordination number, and atomic packing factor are defined and calculated for each structure.
- There are seven basic crystal systems that materials can belong to depending on their lattice parameters and angles between axes. The most common systems are cubic, hexagonal, and tetragonal.
This document discusses crystal structures and their properties. It describes how atoms are arranged in crystalline solids through ordered unit cells that form a repeating lattice. The main crystal structures for metals are body-centered cubic, face-centered cubic, and hexagonal close-packed. It explains how to calculate properties like density from the unit cell parameters and atomic positions. Direction vectors are used to describe crystallographic directions.
Crystal structures are periodic arrangements of atoms that exhibit long-range order that can be measured. Metals, ceramics, and some polymers form crystal structures with closely packed, high bond energy structures, while amorphous materials like glass lack long-range order. There are 7 crystal systems that are built by varying lattice parameters like edge lengths and angles. Common metallic crystal structures important for engineering include body-centered cubic (BCC), face-centered cubic (FCC), and hexagonal close-packed (HCP). Crystal structure determines properties and whether materials behave anisotropically or isotropically.
Chapter 1: Material Structure and Binary Alloy Systemsyar 2604
This is an introduction to material structure and periodic table system. This topic also describes microstructure of the metals and alloys solidification.
Ch 27.2 crystalline materials & detects in crystalline materialsNandan Choudhary
Crystalline materials have atoms arranged in a specific, repeating pattern called a crystal structure. There are several common crystal structures including face-centered cubic, body-centered cubic, and hexagonal close packed.
A crystal structure is built from a repeating three-dimensional pattern called a unit cell, which contains one or more atoms. The unit cell is characterized by the types and positions of atoms within it, the cell dimensions and angles, and the number of atoms per cell. Common unit cells include simple cubic, body-centered cubic, and face-centered cubic.
Miller indices are used to describe directions and planes in a crystal structure. They are represented by sets of integers that indicate the intercepts of a plane or
Chapter 1 material structure and binary alloy systemsakura rena
This document discusses the structure of materials and binary alloy systems. It begins by defining key terms like atom, element, mixture, compound, atomic number, atomic mass, and atomic orbits. It then explains the periodic table, including its characteristics, groups, periods, and function. The document also covers crystal structures, bonding types, solidification of metals and alloys, solid solutions, and equilibrium phase diagrams.
Solid-state chemistry, also sometimes referred as materials chemistry, is the study of the synthesis, structure, and properties of solid phase materials, particularly, but not necessarily exclusively of, non-molecular solids. It therefore has a strong overlap with solid-state physics, mineralogy, crystallography, ceramics, metallurgy, thermodynamics, materials science and electronics with a focus on the synthesis of novel materials and their characterisation. Solids can be classified as crystalline or amorphous on basis of the nature of order present in the arrangement of their constituent particles,
1. The document calculates the packing efficiency of different crystal structures - simple cubic (SC), body centered cubic (BCC), and face centered cubic (FCC).
2. For SC structure, the packing efficiency is 52.36% as only one atom occupies the corner of each unit cell.
3. For BCC structure, the packing efficiency is 68% as atoms occupy the corners and the center of each unit cell.
4. For FCC structure, the packing efficiency is 74% as atoms occupy the corners and face centers of each unit cell.
Chapter1 material structure and binary alloy system Wan Zulfadli
This document provides information about Material Technology 1 course offered by PN. Norhazlina Bte Amon. The course covers topics like material structure, binary alloy systems, ferrous materials, metal working processes, corrosion and non-ferrous metals over 18 weeks. Students will be assessed through quizzes, theory tests and other tasks like end of chapter exercises and presentations.
This document discusses the crystalline structure of metals. It begins by introducing the concepts of space lattices, unit cells, and crystalline lattices which describe the ordered arrangement of atoms in solid crystalline materials. It then discusses different crystal systems including body centered cubic (BCC), face centered cubic (FCC), and hexagonal close packed (HCP) which are the principal crystal structures that most elemental metals form. Tables are provided listing properties of various metals that crystallize in BCC and FCC structures.
The document discusses different types of crystal defects including point defects, stoichiometric defects, and non-stoichiometric defects. Stoichiometric defects include Schottky and Frenkel defects which involve cation-anion pairs missing or cation dislocations. Non-stoichiometric defects result from deviations from the ideal ratio of cations to anions and include metal excess or deficiency defects involving anion or cation vacancies. Common examples of different defect types in various crystals are provided.
Materials science and engineering involves the study of atomic structure and bonding in materials. There are three primary types of atomic bonding - ionic, covalent, and metallic. Crystalline solids can have face-centered cubic (FCC), body-centered cubic (BCC), or hexagonal close-packed (HCP) crystal structures which influence material properties. Crystalline materials can assemble into either crystalline or amorphous structures, and material properties depend on crystal orientation in single crystals but are isotropic in polycrystalline materials with randomly oriented grains.
This document discusses different types of crystalline solids. It defines a crystalline solid as having a well-ordered structure with definite arrangements of particles. Crystalline solids are made up of repeating units called unit cells, which together form a crystal lattice. The document describes the different packing arrangements of particles in unit cells and classifies crystalline solids into four main types - ionic, covalent, metallic and molecular crystals - based on the type of bonding forces between particles. Each type of crystalline solid is characterized by distinct properties like melting point, conductivity, hardness and thermal stability.
This document discusses the atomic arrangement and properties of crystalline solids such as metals. It begins by describing the long-range order in crystalline solids compared to the short-range order in amorphous solids. It then discusses various crystal structures including cubic, hexagonal, and body-centered cubic. It provides examples of calculating properties like atomic packing factor and theoretical density based on crystal structure. Finally, it discusses using X-ray diffraction to determine crystal structure by measuring spacing between crystal planes.
Solids can be either crystalline or amorphous. Crystalline solids have a definite shape and sharp melting point, while amorphous solids lack a definite shape and melting point. There are two main types of crystalline solids: ionic crystals composed of ions and molecular crystals composed of molecules. Ionic crystals form lattice structures with ions arranged in repeating patterns. The characteristics and structures of different types of ionic crystals depend on factors like the ions' sizes and their ratio.
This document provides an overview of solid state chemistry and properties of solid surfaces. It discusses the following key points:
- Solids have definite shapes and volumes due to strong forces holding their atoms, molecules, or ions in fixed positions. This gives solids their rigidity and mechanical strength.
- There are two main types of solids - crystalline solids which have a regular repeating structure and amorphous solids which lack long-range order.
- Techniques for characterizing solid surfaces include low-energy electron diffraction (LEED) and X-ray photoelectron spectroscopy (XPS) which can provide information about surface structure and composition.
- LEED specifically works by bombarding a crystalline surface
This document discusses atomic packing factors and unit cell structures for body centered cubic (BCC) and face centered cubic (FCC) crystal lattices. It provides the following key details:
- The packing factor is the fraction of space occupied by atoms, assuming hard spheres, and is calculated as the number of atoms in the unit cell multiplied by the volume of each atom, divided by the volume of the unit cell.
- A BCC unit cell has an atom at its center and eight atoms at the corners, for a total of two atoms. Its packing factor is 0.68 or 68%.
- An FCC unit cell has an atom at the center of each face and eight corner atoms, for a
The document discusses the crystal structures of materials. It begins by explaining that the properties of some materials are directly related to their crystal structures. For example, magnesium and beryllium have different properties than gold and silver due to differences in their crystal structures. It then lists the key learning objectives which include describing different crystal structures, computing densities, and distinguishing between single crystals and polycrystalline materials. The document goes on to explain common metallic crystal structures like body centered cubic and face centered cubic, as well as non-metallic structures like rock salt and cesium chloride. It also discusses factors that determine crystal structure such as the relative sizes of ions to maximize interactions and maintain charge neutrality.
The document discusses the structure of materials at the atomic level. It explains that the internal structure of materials, including the arrangement of atoms and bonds between atoms, determines properties and behaviors. There are four main types of atomic structure: crystalline solids with repeating patterns have defined properties, while amorphous solids lack order; molecules are formed by chemical bonds between different atoms; compounds contain two or more elements; and mixtures combine substances without chemical bonds. The structures of metals are explained by metallic bonds in which valence electrons are delocalized among the whole structure.
This document provides an overview of solid state physics. It discusses the main types of solids as crystalline and amorphous. Crystalline solids have a long-range ordered structure while amorphous solids lack long-range order. It also describes different crystal structures like unit cells, Bragg's equation for determining crystal structure from X-ray diffraction, and the four main types of crystals: molecular, covalent, metallic and ionic.
There are four basic atomic arrangements that determine the properties of metals: simple cubic, body-centered cubic, face-centered cubic, and hexagonal close-packed. The atomic packing factor, which represents the fraction of unit cell volume occupied by atoms, increases in the order of simple cubic, body-centered cubic, and face-centered cubic structures. Face-centered cubic has the highest atomic packing factor of 0.74 and is therefore the most dense arrangement. Different metallic crystal structures can explain variations in density and other material properties between metals.
The document contains a chemistry unit on the solid state with questions ranging from one to three marks. It includes questions about crystal lattices, crystal defects, stoichiometric and non-stoichiometric defects, crystal structures, and properties of solids such as ionic bonding and conductivity. Numerical problems calculate properties like density from information about the unit cell structure and composition.
1) The document describes the structure of materials at different length scales from atomic to macroscopic levels. It discusses how atomic structure influences properties and technological applications of materials.
2) Key concepts covered include the structure of the atom, electronic configuration, periodic table, different types of atomic bonding, and how bonding influences properties like conductivity and strength.
3) Examples calculate the number of atoms in materials and compare properties like electronegativity between elements. Diagrams illustrate different types of bonding and how structure determines properties.
This document provides examples of materials science calculations involving properties of unit cells for various metals. It includes calculating the atomic radius of aluminum given its lattice parameter, calculating the lattice parameter of tantalum given its atomic radius and temperature, and calculating the percent change in volume of iron's unit cell when it changes structure from body-centered cubic to face-centered cubic with a change in temperature and atomic radii. It also provides examples of calculating the volume of zinc's hexagonal unit cell given structural parameters, computing the density of copper given its atomic radius and weight, and determining the dimension of chromium's unit cell given its atomic weight, density, and number of atoms per cell.
Crystal structures are periodic arrangements of atoms that exhibit long-range order that can be measured. Metals, ceramics, and some polymers form crystal structures with closely packed, high bond energy structures, while amorphous materials like glass lack long-range order. There are 7 crystal systems that are built by varying lattice parameters like edge lengths and angles. Common metallic crystal structures important for engineering include body-centered cubic (BCC), face-centered cubic (FCC), and hexagonal close-packed (HCP). Crystal structure determines properties and whether materials behave anisotropically or isotropically.
Chapter 1: Material Structure and Binary Alloy Systemsyar 2604
This is an introduction to material structure and periodic table system. This topic also describes microstructure of the metals and alloys solidification.
Ch 27.2 crystalline materials & detects in crystalline materialsNandan Choudhary
Crystalline materials have atoms arranged in a specific, repeating pattern called a crystal structure. There are several common crystal structures including face-centered cubic, body-centered cubic, and hexagonal close packed.
A crystal structure is built from a repeating three-dimensional pattern called a unit cell, which contains one or more atoms. The unit cell is characterized by the types and positions of atoms within it, the cell dimensions and angles, and the number of atoms per cell. Common unit cells include simple cubic, body-centered cubic, and face-centered cubic.
Miller indices are used to describe directions and planes in a crystal structure. They are represented by sets of integers that indicate the intercepts of a plane or
Chapter 1 material structure and binary alloy systemsakura rena
This document discusses the structure of materials and binary alloy systems. It begins by defining key terms like atom, element, mixture, compound, atomic number, atomic mass, and atomic orbits. It then explains the periodic table, including its characteristics, groups, periods, and function. The document also covers crystal structures, bonding types, solidification of metals and alloys, solid solutions, and equilibrium phase diagrams.
Solid-state chemistry, also sometimes referred as materials chemistry, is the study of the synthesis, structure, and properties of solid phase materials, particularly, but not necessarily exclusively of, non-molecular solids. It therefore has a strong overlap with solid-state physics, mineralogy, crystallography, ceramics, metallurgy, thermodynamics, materials science and electronics with a focus on the synthesis of novel materials and their characterisation. Solids can be classified as crystalline or amorphous on basis of the nature of order present in the arrangement of their constituent particles,
1. The document calculates the packing efficiency of different crystal structures - simple cubic (SC), body centered cubic (BCC), and face centered cubic (FCC).
2. For SC structure, the packing efficiency is 52.36% as only one atom occupies the corner of each unit cell.
3. For BCC structure, the packing efficiency is 68% as atoms occupy the corners and the center of each unit cell.
4. For FCC structure, the packing efficiency is 74% as atoms occupy the corners and face centers of each unit cell.
Chapter1 material structure and binary alloy system Wan Zulfadli
This document provides information about Material Technology 1 course offered by PN. Norhazlina Bte Amon. The course covers topics like material structure, binary alloy systems, ferrous materials, metal working processes, corrosion and non-ferrous metals over 18 weeks. Students will be assessed through quizzes, theory tests and other tasks like end of chapter exercises and presentations.
This document discusses the crystalline structure of metals. It begins by introducing the concepts of space lattices, unit cells, and crystalline lattices which describe the ordered arrangement of atoms in solid crystalline materials. It then discusses different crystal systems including body centered cubic (BCC), face centered cubic (FCC), and hexagonal close packed (HCP) which are the principal crystal structures that most elemental metals form. Tables are provided listing properties of various metals that crystallize in BCC and FCC structures.
The document discusses different types of crystal defects including point defects, stoichiometric defects, and non-stoichiometric defects. Stoichiometric defects include Schottky and Frenkel defects which involve cation-anion pairs missing or cation dislocations. Non-stoichiometric defects result from deviations from the ideal ratio of cations to anions and include metal excess or deficiency defects involving anion or cation vacancies. Common examples of different defect types in various crystals are provided.
Materials science and engineering involves the study of atomic structure and bonding in materials. There are three primary types of atomic bonding - ionic, covalent, and metallic. Crystalline solids can have face-centered cubic (FCC), body-centered cubic (BCC), or hexagonal close-packed (HCP) crystal structures which influence material properties. Crystalline materials can assemble into either crystalline or amorphous structures, and material properties depend on crystal orientation in single crystals but are isotropic in polycrystalline materials with randomly oriented grains.
This document discusses different types of crystalline solids. It defines a crystalline solid as having a well-ordered structure with definite arrangements of particles. Crystalline solids are made up of repeating units called unit cells, which together form a crystal lattice. The document describes the different packing arrangements of particles in unit cells and classifies crystalline solids into four main types - ionic, covalent, metallic and molecular crystals - based on the type of bonding forces between particles. Each type of crystalline solid is characterized by distinct properties like melting point, conductivity, hardness and thermal stability.
This document discusses the atomic arrangement and properties of crystalline solids such as metals. It begins by describing the long-range order in crystalline solids compared to the short-range order in amorphous solids. It then discusses various crystal structures including cubic, hexagonal, and body-centered cubic. It provides examples of calculating properties like atomic packing factor and theoretical density based on crystal structure. Finally, it discusses using X-ray diffraction to determine crystal structure by measuring spacing between crystal planes.
Solids can be either crystalline or amorphous. Crystalline solids have a definite shape and sharp melting point, while amorphous solids lack a definite shape and melting point. There are two main types of crystalline solids: ionic crystals composed of ions and molecular crystals composed of molecules. Ionic crystals form lattice structures with ions arranged in repeating patterns. The characteristics and structures of different types of ionic crystals depend on factors like the ions' sizes and their ratio.
This document provides an overview of solid state chemistry and properties of solid surfaces. It discusses the following key points:
- Solids have definite shapes and volumes due to strong forces holding their atoms, molecules, or ions in fixed positions. This gives solids their rigidity and mechanical strength.
- There are two main types of solids - crystalline solids which have a regular repeating structure and amorphous solids which lack long-range order.
- Techniques for characterizing solid surfaces include low-energy electron diffraction (LEED) and X-ray photoelectron spectroscopy (XPS) which can provide information about surface structure and composition.
- LEED specifically works by bombarding a crystalline surface
This document discusses atomic packing factors and unit cell structures for body centered cubic (BCC) and face centered cubic (FCC) crystal lattices. It provides the following key details:
- The packing factor is the fraction of space occupied by atoms, assuming hard spheres, and is calculated as the number of atoms in the unit cell multiplied by the volume of each atom, divided by the volume of the unit cell.
- A BCC unit cell has an atom at its center and eight atoms at the corners, for a total of two atoms. Its packing factor is 0.68 or 68%.
- An FCC unit cell has an atom at the center of each face and eight corner atoms, for a
The document discusses the crystal structures of materials. It begins by explaining that the properties of some materials are directly related to their crystal structures. For example, magnesium and beryllium have different properties than gold and silver due to differences in their crystal structures. It then lists the key learning objectives which include describing different crystal structures, computing densities, and distinguishing between single crystals and polycrystalline materials. The document goes on to explain common metallic crystal structures like body centered cubic and face centered cubic, as well as non-metallic structures like rock salt and cesium chloride. It also discusses factors that determine crystal structure such as the relative sizes of ions to maximize interactions and maintain charge neutrality.
The document discusses the structure of materials at the atomic level. It explains that the internal structure of materials, including the arrangement of atoms and bonds between atoms, determines properties and behaviors. There are four main types of atomic structure: crystalline solids with repeating patterns have defined properties, while amorphous solids lack order; molecules are formed by chemical bonds between different atoms; compounds contain two or more elements; and mixtures combine substances without chemical bonds. The structures of metals are explained by metallic bonds in which valence electrons are delocalized among the whole structure.
This document provides an overview of solid state physics. It discusses the main types of solids as crystalline and amorphous. Crystalline solids have a long-range ordered structure while amorphous solids lack long-range order. It also describes different crystal structures like unit cells, Bragg's equation for determining crystal structure from X-ray diffraction, and the four main types of crystals: molecular, covalent, metallic and ionic.
There are four basic atomic arrangements that determine the properties of metals: simple cubic, body-centered cubic, face-centered cubic, and hexagonal close-packed. The atomic packing factor, which represents the fraction of unit cell volume occupied by atoms, increases in the order of simple cubic, body-centered cubic, and face-centered cubic structures. Face-centered cubic has the highest atomic packing factor of 0.74 and is therefore the most dense arrangement. Different metallic crystal structures can explain variations in density and other material properties between metals.
The document contains a chemistry unit on the solid state with questions ranging from one to three marks. It includes questions about crystal lattices, crystal defects, stoichiometric and non-stoichiometric defects, crystal structures, and properties of solids such as ionic bonding and conductivity. Numerical problems calculate properties like density from information about the unit cell structure and composition.
1) The document describes the structure of materials at different length scales from atomic to macroscopic levels. It discusses how atomic structure influences properties and technological applications of materials.
2) Key concepts covered include the structure of the atom, electronic configuration, periodic table, different types of atomic bonding, and how bonding influences properties like conductivity and strength.
3) Examples calculate the number of atoms in materials and compare properties like electronegativity between elements. Diagrams illustrate different types of bonding and how structure determines properties.
This document provides examples of materials science calculations involving properties of unit cells for various metals. It includes calculating the atomic radius of aluminum given its lattice parameter, calculating the lattice parameter of tantalum given its atomic radius and temperature, and calculating the percent change in volume of iron's unit cell when it changes structure from body-centered cubic to face-centered cubic with a change in temperature and atomic radii. It also provides examples of calculating the volume of zinc's hexagonal unit cell given structural parameters, computing the density of copper given its atomic radius and weight, and determining the dimension of chromium's unit cell given its atomic weight, density, and number of atoms per cell.
The document summarizes research on cobalt-carbon nanocomposites prepared by RF sputtering and RF plasma-enhanced chemical vapor deposition. Three cobalt-carbon nanocomposite films were prepared under different deposition pressures. Atomic force microscopy showed the average particle size and surface roughness decreased with increasing pressure. X-ray diffraction identified cobalt nanoparticles in the FCC phase and cobalt oxide. Optical absorbance measurements showed the surface plasmon resonance band shifted to higher wavelengths with decreasing pressure, indicating larger particle sizes. The composition of the films was confirmed with EDX to contain cobalt, oxygen, and carbon from the matrix. In conclusion, lower deposition pressures favored the formation of larger cobalt nanoparticles while higher pressures increased cobalt oxide formation.
This document discusses different crystal structures and materials. It begins by describing three common crystal structures - face-centered cubic (FCC), body-centered cubic (BCC), and hexagonal close-packed (HCP) - and provides examples of metals that adopt each structure. It then discusses ceramic crystal structures and how the size and charge of ions influence the structure. Key ceramic structures described include rock salt, cesium chloride, and zinc blende. The document also examines properties of carbon including different allotropes like diamond, graphite, fullerenes, and carbon nanotubes.
This document is the first unit of a course on the structure, arrangements, and movements of atoms taught by Dr. Edgar García Hernández. The unit introduces materials science and engineering concepts. It discusses atomic structure, crystalline arrangements of metals and ceramics, imperfections in crystals like point defects and dislocations, and atomic movements in solids under mechanical treatments. The unit provides information on crystal structures, unit cells, coordination numbers, and calculating material properties based on structure.
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Module 7 - Ceramics, Structures and properties of ceramicsMissRozu
This document discusses ceramics, including their structures, properties, classifications, and applications. Ceramics are inorganic materials made by shaping and hardening compounds with heat. They are hard, corrosion-resistant, and brittle. Ceramics form ionic or covalent bonds and various crystal structures that give them useful properties but also brittleness. Major ceramic classes include glasses, clay products, refractories, advanced ceramics, and more. Each has distinct compositions and applications like containers, bricks, furnace linings.
1 Packing of spheres: Unit cell and description of crystal structure, close
packing of spheres, holes in closed-packed structures.
2 Structure of Metals: Polytypism, structures that are not closed packed, polymorphism of metals, atomic radii of metals, alloys.
3 Ionic solids: Characteristic structures of ionic solids, the rationalization of structures, the energetics of ionic bonding, consequences of lattice enthalpy.
This document describes a study on the structural and magnetic characterization of Co2+ substituted nanostructured copper-zinc spinel ferrites. Nano particles of Cu0.61-xCoxZn0.39Fe2O4 were synthesized using a sol-gel auto combustion method. Various characterization techniques were used to analyze the effect of Co2+ substitution on properties like particle size, lattice constant, density, cation distribution, and magnetic properties. It was found that lattice parameter and particle size increased with Co2+ content while density decreased. Cation distribution analysis showed a preference of Co2+ and Cu2+ for octahedral sites and Zn2+ for tetrahedral sites. Magnetic properties like saturation magnetization and coerc
This document summarizes the synthesis and characterization of two novel phosphonate-based cobalt cages. The first cage (Co15) has an inorganic core shaped like a distorted cubic structure composed of pentagonal faces. The second cage (Co12) has an inorganic core resembling a butterfly shape composed of hexagonal and triangular faces forming a tetrahedral geometry. Magnetic characterization shows both cages exhibit intramolecular antiferromagnetic interactions and zero field splitting at low temperatures.
Synthesis and Characterisation of Copper Oxide nanoparticlesIOSR Journals
Cupric oxide (CuO) nanoparticles were prepared by the chemical route by calcinations at a higher temperature from 300oC to 400 oC. For the comparison transmission electron microscopy (TEM) and x-ray diffraction (XRD) measurements were made through JCPDS. There is good agreement between data produced by spectroscopy and the microscopic measurements.
The document provides an overview of materials science and engineering, including definitions, topics covered, and examples. It discusses the relationship between structure and properties of materials from the atomic to macroscale. Key points include that materials properties depend on their structure, processing can change structure, and examples are given of how electrical, thermal, and magnetic properties vary with changes in composition or deformation.
1. A 2D coordination polymer was synthesized using cobalt trimers and the flexible ligand cis,cis-cyclohexane-1,3,5-tricarboxylate.
2. Single crystal X-ray diffraction shows the complex forms a 2D framework with channels and contains trinuclear cobalt secondary building units linked by the ligand.
3. Magnetic characterization reveals spin-canting ferromagnetic behavior at low temperatures based on AC susceptibility measurements. Gas adsorption experiments also show selectivity for CO2 over N2.
Crystalline structures can be classified as crystalline, polycrystalline, or amorphous. Crystalline structures have repeating arrangements of atoms or molecules. There are seven crystal systems and fourteen Bravais lattices that describe how points in the unit cell are arranged in three-dimensional space. Common metal structures include body centered cubic, face centered cubic, and hexagonal close packed. Ceramic and semiconductor structures often involve ionic bonding between metals and nonmetals. Polymeric structures can be crystalline but typically have disordered regions as well.
- Atoms can assemble into crystalline or amorphous structures. Common metallic crystal structures are FCC, BCC, and HCP which can be used to predict a material's density based on its atomic properties and structure.
- Materials exist as single crystals or polycrystals. Single crystals are anisotropic while polycrystals are typically isotropic if their grains are randomly oriented.
- X-ray diffraction is used to determine crystal structures and interplanar spacings by exploiting the diffraction of x-rays by crystalline materials.
- Atoms can assemble into crystalline or amorphous structures. Common metallic crystal structures are FCC, BCC, and HCP which can be used to predict a material's density based on its atomic properties and structure.
- Materials exist as single crystals or polycrystals. Single crystals are anisotropic while polycrystals are typically isotropic if grains are randomly oriented.
- X-ray diffraction is used to determine crystal structures and interplanar spacings by exploiting the diffraction of X-rays by crystalline materials.
The document discusses ceramic crystal structures and bonding. It covers rules for ionic structures based on charge neutrality and coordinating oppositely charged ions. Common crystal structures like NaCl and CsCl are presented based on filling space in a lattice. Predicting structures is based on ionic radii ratios and coordination numbers. Network structures of silicon oxides and glasses are also covered, along with defects in ceramics and glasses.
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materila science & engineering - sheet 1
1. Dr. Ahmed Ramadan Materials Technology Ex.2: Crystal Structure
1. What is the difference between atomic structure and crystal structure?
2. If the atomic radius of aluminum is 0.143 nm, calculate the volume of its unit cell in
cubic meters.
3. Show for the body-centered cubic crystal structure that the unit cell edge length and
the atomic radius (R) are related through a = 4R/√3
4. Show that the atomic packing factor for BCC is 0.68.
Density Computations
5. Iron has a BCC crystal structure, an atomic radius of 0.124 nm, and an atomic weight
of 55.85 g/mol. Compute and compare its theoretical density with the experimental
value found inside the table 1.
6. Calculate the radius of an iridium atom, given that Ir has an FCC crystal structure, a
density of 22.4 g/cm3 and an atomic weight of 192.2g/mol.
7. Calculate the radius of a vanadium atom, given that V has a BCC crystal structure,
a density of 5.96 g/cm3, and an atomic weight of 50.9 g/mol.
8. Using atomic weight, crystal structure, and atomic radius data tabulated inside the
table 1, compute the theoretical densities of lead, chromium, copper, and then
compare these values with the measured densities listed in this same table.
9. Rhodium has an atomic radius of 0.1345 nm and a density of 12.41 g/cm3.
Determine whether it has an FCC or BCC crystal structure.
10.The atomic weight, density, and atomic radius for three hypothetical alloys are
listed in the following table. For each, determine whether its crystal structure is FCC,
BCC, or simple cubic and then justify your determination. A simple cubic unit cell is
shown in next table.
Alloy Atomic Weight g/mol))
Density
(g/cm3
)
Atomic Radius
( nm)
A
77.4 8.22 0.125
B
107.6 13.42 0.133
C
127.3 9.23 0.142