1. CHAPTER 1 :MATERIAL STRUCTUREAND BINARY ALLOYSYSTEM

2. STRUCTURE OFMATERIALS AND EPT 3. ATOMParticle ChargeElectron Negative (-)Proton Positive (+)NeutronNeutral Atom is unit of matter; the smallest unit of achemical element. Each atom consists of a nucleus, which has apositive charge, and a set of electrons that move 4. ELEMENT Is a combination of 2 or more same atoms whichform a bond. Atoms in elements all have the same number ofprotons - i.e. the same atomic number. Example of element; Cl2 5. MIXTURE Combination of two or more different substanceswhich are mixed together but are not combinedchemically. Example of mixture; salt water, concrete.Putting Together And Breaking Apart 6. COMPOUND Is a pure chemical substance consisting of two ormore different chemical elements that can beseparated into simpler substances by chemicalreactions. Example of compound; Carbon Dioxide (CO2). 7. ATOMIC NUMBER Is the number of protons found in the nucleus of an atom and therefore identical to the charge number of the nucleus. 8. ATOMIC MASS Is the total number of protons and neutrons in the nucleus of an atom. Atomic Mass = No. of proton + No. ofneutron 9. ATOMIC ORBITS Electrons if filled to atomic orbits by using formula2n2 as below. The highest no. of electron on the outer shell/orbitsis 8.No. ofNo. of orbit (n) electronFirst orbit (n=1) 2Second orbit (n=2)8Third orbit (n=3)18Fourth orbit (n=4) 32 10. Example : Determine the electrons configuration and number of orbital for below elements. i) Oxygen (Atom no. = 8) ii) Magnesium (Atom no. = 12) iii)Chlorine (Atom no. = 19) iv) Arsenic (Atom no. = 33) Answer : i) Electrons configuration = 2:6 , No. of orbital = 2 ii) Electrons configuration = 2:8:2 , No. of orbital = 3 iii) Electrons configuration = 2:8:8:1 , No. of orbital = 4 iv) Electrons configuration = 2:8:18:5 , No. of orbital = 4 11. AtomsNumber Atoms Mass7 14Elements Symbol NNitrogenElementsName 2:5 Electronsconfiguration 12. ELEMENT PERIODICAL TABLE 13. CHARACTERISTICS OF EPT Have 18 lines in vertical and 7 lines in horizontal. Elements in the periodic table are arranged inperiods (rows) and groups (columns) base onatomic number.Group Period 14. Groups- Elements in same group having the sameelectron configuration in their outer shell. E.g ;element in group 1 has 1 electron in outer shell,element in group 2 has 2 electron in outer shell.- Elements in groups sharing similar chemicalproperties. Period- Elements in same period having the same no. oforbit.- Each of the seven periods is filled sequentiallyby atomic number When valance electron increase, metal propertiesof element decrease. 15. FUNCTION OF EPT To ease the classification of elements. Able to provide information especially forproperties of the elements due to elements arearrange in respective group. Easier to analyze and understand reactionbetween elements. 16. CRYSTALLIZE STRUCTURE The atoms arrange themselves into variousorderly configuration, called crystal. Crystal structure is a unique arrangement ofatoms or molecules in a crystalline liquid or solid. Patterns are located upon the points of a lattice,which is an array of points repeating periodicallyin three dimensions. The points can be thought of as forming identicaltiny boxes, called unit cells, that fill the space ofthe lattice 17. There are 4 types of crystal structure:Types of crystallizestructureBody HexagonalFace centeredSimple cube centeredClose packed cubic (FCC) cubic (BCC) (HCP) 18. SIMPLE CUBE Is a cube (all sides of the same length and all faceperpendicular to each other) with an atom at eachcorner of the unit cell. Contains only one atom per unit cell. 19. BODY CENTERED CUBIC (BCC) Is a cube (all sides of the same length and all faceperpendicular to each other) with an atom at eachcorner of the unit cell and an atom in the center ofthe unit cell. Contains two atoms per unit cell. 20. FACE CENTERED CUBIC (FCC) Is a cube (all sides of the same length and all faceperpendicular to each other) with an atom at eachcorner of the unit cell and an atom situated in themiddle of each face of the unit cell. Contains four atoms per unit cell. 21. HEXAGANOL CLOSEDPACKED (HCP) is a unit cell with an atomic packing arrangementin which 12 atoms surround a central identical atom. Contains six atoms per unit cell. 22. COVALENT BOND Bond occur between non-metals. Covalent chemical bonds involve the sharing of apair of valence electrons by two atoms. Example ; Cl2 !!! Remember : Covalent = sharing atoms 23. IONIC BONDING Bonds occur between metals and non-metals. The metal gives its outer electrons to the non-metal - electrons are transferred in this type ofbonding. The metal has lost electrons, and is now apositive ion or cation. The non-metal has gained electrons, and isnow a negative ion or anion. Both the metal and non-metal now have fullouter shells of electrons. 24. Example ; NaCl!!! Remember : Ionic = gain/loose atoms 25. METALLIC BONDING The bonding in metal elements is called metallicbonding. In metals, the metal atoms lose their outerelectrons to form metal cations. The electronsfrom all the metal atoms form a "sea" of electronsthat can flow around these metal cations. Theseelectrons are "not fixed in one place" or "free tomove". 26. Metal cations and the electrons are oppositely charged. They will be attracted to each other, and also to other metal cations. These electrostatic forces are called metallic bonds, and these are what hold the particles together in metals. 27. SOLIDIFICATION OFMETAL AND ALLOYS 28. SOLIDIFICATION PHASES First StageSecondThird StageFourth Stage StageNucleus formation Dendrite grow Dendrite growth & Solidification endsarms meet to form the with the formation ofgrain boundarygrain 29. METAL VS ALLOYMetalAlloy Metal is made up of Alloy is a mixture of two only one element.or more metals, ormetal and non-metal. Has a relatively high Has a low melting melting point. point. 30. SOLID SOLUTION Terms in solid solution> Solute : is the element that is added to thesolvent. Eg. Sugar.> Solvent : a liquid substance capable ofdissolving other substances. Eg. Water. Solid solution : when solute is added to thesolvent, the crystal structure of the solventremains unchanged and the mixture remains in asingle homogeneous phase. 2 types of solid solution :i) Substitution solid solutionii) interstitial solid solution 31. COMPARISON ON TYPES OF SOLID SOLUTIONSubstitutionInterstitial Formation : If the Formation : The solute atoms of the solvent atom does not displace (host atom) area solvent atom (host replaced in the crystalatom), but rather it lattice by atoms of theenters one of the holes solute metal.or interstices betweenthe solvent atoms. 32. Atomic size : Solute Atomic size : Soluteand solvent atomic atoms must have aradii have the smaller atomic radiidifference in atomic less than oneradii less than aboutangstrom compare to15 percent.solvent atom. Others : Have 2 typesof substitution solidsolution. Disorderedand Ordered. 33. Ordered substitutionalThe solute atoms move into definite positions in thelattice. 34. Disordered substitutionalThe solute atoms do not occupy any specificposition but are distributed at random in the latticestructure of the solvent. 35. SOLIDIFICATION PROCESS 36. Solid Liquid Liquid Solid When certain metal is Kinetic energy for heated constantly, it willatoms increase. start to melt. Atoms arrangement If the heatingchange from disordered continued, metal will position to certain melt entirely.geometry position. The constant melting Solid materials temperature is meltingformed either in point.amorphous or At the melting point crystalline structure. the solid and liquid phase exist in!!! Amorphous : Atoms do not have a long-range crystalline structure. equilibriumHave no grain boundaries and atoms are randomly packed. 37. EQUILIBRIUM PHASE DIAGRAM 38. Point 100% Cu & 0% Ni - solidification temperature 1084 C Point 80% Cu & 20% Ni - solidification starts at 1190 C. - Complete at 1135 C. Point 80% Ni & 20% Cu - solidification starts at 1410 C. - Complete at 1380 C. Point 100% Ni & 0% Cu - solidification temperature 1445 C 39. TERMINOLOGIES IN PHASE DIAGRAM Phase : is a physical distinct and homogenous portion in amaterial. Equilibrium phase : are graphical representations of whatphases are present under equilibrium conditions at varioustemperature, pressure and composition. Composition : Are percentage of certain materials addedpurposely or not, to another material. With this it can causechanges in phases, the properties and the shape of themicrostructures. Liquidus : The minimum temperature at which allcomponents of a mixture (such as an alloy) can be in a