Stone Age (40,000 to 100,000 yrs ago): Stone tools, clay pots, skin
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1 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 Identify and distinguish between the types of atomic bonding 1-2 CHAPTER OUTLINE Chapter Outline Historical Overview What is Materials Science & Engineering Classification of Materials Atomic Structure Atomic Bonding Stone Age (40,000 to 100,000 yrs ago): Stone tools, clay pots, skin Copper Age (5,000 to 10,000 yrs ago): Copper ornaments, earthenware, metal smelting Bronze Age (3,000 to 5,000 yrs ago): Bronze (Cu/Sn), glass, iron smelting Iron Age ( yrs ago): Carburized Iron, improved forging, porcelain Steel and concrete ( yrs ago) Advanced Materials (beginning early 1900s): polymers, ceramics, composites, semiconductors MATERIALS MATERIALS
2 Chapter Outline Chapter Outline Performance Performance/ Cost Materials Engineering Designing the structure to achieve specific properties of materials. Structure Processing Structure Processing Materials Science Investigating the relationship between structure and properties of materials. Processing Structure Performance are the way materials responds to external forces or the environment Mechanical Electrical and magnetic Optical Chemical To obtain the desired properties the material must have the appropriate structure Processing can produce the appropriate structure Classification of Materials Metals Ceramics Polymers: Thermoplastics and Thermosets Composition, bonding, crystal structure, and microstructure define materials properties Semiconductors Composite Materials
3 Classification of Materials Engineering Materials 2003 Brooks/Cole Publishing / Thomson Learning Functional Classification of Materials Aerospace Biomedical Electronic Materials Energy Technology and Environmental Technology Magnetic Materials Photonic or Optical Materials Smart Materials Structural Materials 2003 Brooks/Cole Publishing / Thomson Learning Atomic Structure Atomic Structure Atomic structure is made of: Protons: positive (+) charge Neutrons: no charge (neutral) Electrons: negative (-) charge The nucleus contains the mass of an atom: Protons + Neutrons Layers of electrons that orbit around the nucleus are called orbitals or energy-level shells
4 Periodic Table of Elements Atomic Number (# of protons) Atomic weight = # protons + average # neutrons Electronegativity Electronegativity is defined as the measure of how willing atoms are to accept electrons Subshells with one electron: low electronegativity Subshells with one missing electron: high electronegativity Periodic Table of Elements Ions Low electronegativity High electronegativity When an atom loses or gains an electron to or from another atom, it is called an ion Types of Ions: CATIONS a loss of electrons: positive (+) charge ANIONS a gain of electrons: negative (-) charge Atomic Bonding Ionic Bonding Atomic bonding is the formation of compounds by combining two or more elements In an atomic bonding electrons are gained, lost or shared There are 4 main types of bonding: Ionic bonding occurs between + and ions Requires electron transfer between atoms forming attracting ions Ionic bonding Covalent bonding Metallic bonding Van der waals Primary Bonding Secondary Bonding Example: sodium chloride (NaCl) Other compounds having ionic bonding: MgO, CsCl
5 Ionic Bonding Characteristics of Ionic Bonding Ionic compounds are usually hard, rigid and brittle: the results of ions being held in specific positions Covalent Bonding In covalent bonding the electrons are shared between atoms Covalent bonds are more stable and stronger than ionic bonds e.g; Diamond (Carbon) Metallic Bonding Metallic Bonding Metallic bonding: Valence electrons are detached from atoms, and spread in an electron sea that glues the ions together Characteristics of metallic bonding Metallic bonds occur between metals Good conductors of electricity and heat (due to the mobility of electrons) Malleability (can be shaped) and Ductility (can be drawn into wires) Brightness and strong light reflection Examples: copper (Cu), gold (Au), silver (Ag) Metallic Bonding Secondary Bonding Atomic bonding without electron transfer or sharing Arises from interaction between dipoles Fluctuating dipoles asymmetric electron clouds secondary bonding ex: liquid H2 H2 H2 H H H H secondary bonding
6 Secondary Bonding Secondary Bonding Permanent dipoles-molecule induced -ex: Polymer (PVC) -general case: + - secondary bonding + - -ex: liquid H 2 O Summary: Atomic Bonding Examples of bonding in materials Metals : metallic bonding Moderate T m and E Ceramics : ionic/covalent high T m and high E Polymers : covalent and secondary Small T m and small E Semiconductors: covalent and covalent/ionic T m : melting temperature, E: stiffness
Atomic Structure. Atomic weight = m protons + m neutrons Atomic number (Z) = # of protons Isotope corresponds to # of neutrons
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Primary bonding: e- are transferred or shared Strong ( KJ/mol or 1-10 ev/atom) Secondary Bonding: no e -
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