Ionic solids - PowerPoint PPT Presentation
Chapter 3: Structures of Metals & Ceramics
Chapter 3: Structures of Metals & Ceramics Structures The properties of some materials are directly related to their crystal structures. Significant property differences exist between crystalline and noncrystalline materials having the same composition. Energy and Packing Energy
By Ava
II. Crystal Structure
II. Crystal Structure. Lattice, Basis, and the Unit Cell Common Crystal Structures Miller Indices for Crystal Directions and Planes The Reciprocal Lattice.
By issac
Chapter 9 Chemical Bonding
Chapter 9 Chemical Bonding. 1 type of Potential Energy : Gravitational P.E. Ball On Top of a Hill. m. P.E. = mgh. h. Section 9.1: Why does bonding occur in the first place?. Bonding lowers the potential energy between positive and negative particles (p341). What is potential energy?.
By Mercy
Chapter 8 Review “Covalent Bonding”
Chapter 8 Review “Covalent Bonding”. Pre-AP Chemistry Charles Page High School Stephen L. Cotton. Chapter 8 Review. What is the correct electron configuration arrangement of the four valence electrons of the carbon atom in a methane molecule (CH 4 ): a) 2s 2 2p 2 , or b) 2s 1 2p 3 ?
By alva
Entropy
What’s wrong with these events?. Entropy. Introduction. We’ve all spent enough time in this universe to know that things don’t work this way… but how do we explain it?. ©1965, James Frankfort & The Curtis Publishing Co. Entropy. Here are some things we observe:
By diep
Organic Chemistry
Organic Chemistry. William H. Brown Christopher S. Foote Brent L. Iverson. Covalent Bonding & Shapes of Molecules. Chapter 1. Organic Chemistry. The study of the compounds of carbon Over 10 million compounds have been identified about 1000 new ones are identified each day!
By Samuel
Computational Physics (Lecture 6)
Computational Physics (Lecture 6) . PHY4370. Matrix Operations. Matrix operations involved in many numerical and analytical scientific problems. Schemes developed for the matrix problems can be applied to the related problems encountered in ordinary and partial differential equations.
By lisbet
Liquids and Solids
Liquids and Solids. AP Chem Unit 10. Sections. Intermolecular Forces Liquid state Solid Structures Metal Structures Carbon and Silicon Networks. Sections. Molecular Solids Ionic Solids Vapor pressure and State Change Phase Diagrams. States of Matter.
By mari
CHEM 938: Density Functional Theory
CHEM 938: Density Functional Theory. condensed-phase systems. February 9, 2010. Examples of Condensed-Phase Systems. many interesting processes occur in the condensed phase. Crystalline :. ordered network of atoms. examples are metals, ionic solids, covalent solids and molecular crystals.
By caden
Particles in Solution
Particles in Solution. The Nature of Solvents. What dissolves what or why does a substance dissolve in one solvent but not another? Solvents with non-polar molecules dissolve solutes with non-polar molecules Solvents with polar molecules dissolve solutes with polar molecules
By abril
Ch. 20: Entropy and Free Energy
Ch. 20: Entropy and Free Energy. Thermodynamics: the science of energy transfer Objective: To learn how chemists predict when reactions will be product-favored vs. when they will be reactant-favored Spontaneous Processes and Entropy
By samson
Bonding
Bonding. Types of Bonds Electronegativity Polarity & Dipole Moment Ions Ionic Compounds Lattice Energy Covalent Bonds Bond Energy Lewis Structures Resonance Formal Charge VESPR. Who bonds? Who doesn’t?. Atoms shift valence electrons to complete the outer energy level.
By shel
Solutions Unit
Solutions Unit. Final Exam Study Notes. What is a solution?. Solution Terminology: Solute, solvent, saturated, unsaturated, supersaturated, aqueous, homogeneous, heterogeneous, soluble, insoluble, miscible (alcohol and water), immiscible (water and oil), dilute, concentrated
By quang
Names and Formulas of
Names and Formulas of. Ionic Compounds. Chemical Bonds . The bond is the force that holds two or more atoms together to form a molecule of a compound- two types Ionic and covalent Atom is to element as H He Fe Na Molecule is to compound H 2 O. Na + , Cl−, Ca ++ , S = H2SO4.
By rodney
Ionic and Metallic Bonding
Ionic and Metallic Bonding. Chapter 7. Valence Electrons. The ________________in an atom Their arrangement determines the bonding prosperities and activities of an atom S-Block– they are the same as the group number Na= 1 valence electron
By darrin
Reactions in Solution
AP Chemistry. Reactions in Solution. solution : a homogeneous mixture of two or more substances. -- The ______ is present in greatest quantity. . solvent. -- Any other substance present is called a ______. . solute. aqueous solutions : solutions in which water is the
By nate
Nature of Solids
Nature of Solids. Crystalline Solids. Solid in which the representative particles exist in a highly ordered, repeating pattern. Most solids are crystalline solids Has a sharp melting point where it becomes a free flowing liquid Ex. (Salt, Sugar, Snow)
By isla
2: Intermolecular forces
Date. 2: Intermolecular forces. BIG picture. What skills will you be developing this lesson? ICT Numeracy Literacy Team work Self management Creative thinking Independent enquiry Participation Reflection How is this lesson relevant to every day life? (WRL/CIT). Connector.
By najwa
Covalent Bonding
Covalent Bonding. …electrons are shared. How does H 2 form?. The nuclei repel. But they are attracted to electrons. They share the electrons. +. +. Covalent bonds. Nonmetals hold onto their valence electrons. They can’t give away electrons to bond. Still want noble gas configuration.
By arnie
Square packing: Not most space efficient
Square packing: Not most space efficient. Hexagonal packing: Most space efficient. Unit Cells: the simplest repeating motif. Can be different shapes and sizes. The Rhomb Is the Unit cell Shape Of Hexagonal lattices. Packing: layers build up 3D solid.
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