 Dominated by... ◦ Closely packed particles ◦ Relatively fixed position ◦ Highest intramolecular attractions  Are... ◦ Definite shape and volume ◦ Definite.

Slides:



Advertisements
Similar presentations
Solids differ: Hardness Melting point Flexibility Conductivity Solids form crystal lattice structures: Repeating pattern of molecules Determined by x-ray.
Advertisements

THE NATURE OF SOLIDS SECTION 10.3 After reading Section 10.3, you should know: properties of solids the difference between single-cubic, body- centered.
LIQUIDS AND SOLIDS. LIQUIDS: Why are they the least common state of matter? 1. Liquids and K.M.T.  Are particles in constant motion? Spacing? Kinetic.
Structure, Bonding & Properties of Solids
Solids & Liquids. CA Standards Students know the atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular.
Ch. 13 States of Matter Need Need I to I to Know Fuzzy Learn Know Fuzzy Learn 1. Describe the assumptions of the kinetic theory as it applies to solid,
(Section 2.1). Bonding – Electrostatic forces of attraction between pairs of atoms or ions. Compounds – Two or more elements that combine to form new.
Solids. Motion & Arrangement Vibrate about center of mass. – Cannot “translate” or move from place to place. – Cannot slide past each other or flow. Packed.
Liquids and Solids Solids.
SolidsSolids Adapted from a presentation by Dr. Schroeder, Wayne State University.
Chapter 2, Section 1 States of Matter Wednesday, September 30, 2009 Pages Wednesday, September 30, 2009 Pages
The Nature of Solids. A Model for Solids The particles in solids are not free to move about. They tend to vibrate about fixed points. In most solids,
The Nature of Solids Chapter 10. Solids: Gases = very free to move Liquids = relatively free to move Solids = not very free to move.
Nature of Solids. Crystalline Solids Solid in which the representative particles exist in a highly ordered, repeating pattern. Most solids are crystalline.
Metallic Bonds and Intramolecular Forces. Metallic Bond Bond that exists between metal atoms Alloy – two or more different metal atoms bonded together.
Properties of Liquids. Reminder: Kinetic-molecular Theory says the particles of matter are always in motion I.Properties of Liquids & the Kinetic-Molecular.
How can you describe the motion of particles in a solid? How can you describe the motion of particles in a liquid? How can you describe the motion of particles.
Solids AMORPHOUS- THOSE WITH MUCH DISORDER IN THEIR STRUCTURE. CRYSTALLINE- HAVE A REGULAR ARRANGEMENT OF COMPONENTS IN THEIR STRUCTURE.
Chap 12 Liquids and Solids. Properties of Liquids and the Kinetic-Molecular Theory Liquid- is a form of matter that has a definite volume and takes the.
Lesson Starter Compare the plaster of Paris mixture before it hardens to the product after it hardens. Section 3 Solids Chapter 10.
Types of Substances Unit 6 – Part II. Types of Substances Ionic Solid –3-D repeating pattern of + and – ions Crystal lattice Held together by ionic attractions.
Liquids and Solids. Introduction Chemical bonds hold atoms together in a molecule. Intermolecular forces hold molecules together, making them solids,
Chemistry Chapter 13 Notes #4 Liquids and Solids.
States of Matter Solids. States of Matter  Objectives  Describe the motion of particles in solids and the properties of solids according to the kinetic-molecular.
Free e - move rapidly in response to electric fields, thus metals are excellent conductors of electricity.
Solids Chemistry Mrs. Coyle. Solids Atoms vibrate about fixed positions.
S OLIDS 10.3 S OLIDS How do the particles in a solid behave? Shape and Volume Definite Definite Melting Point Melting – the physical change of a solid.
Properties of Solids  Definite shape and volume  Particles are close together so attractive forces (bonds and IMFs!) are strong  Highly ordered  Rigid,
Chapter Three: Solids, Liquids and Gases Section 1: States of Matter
An ionic lattice: a giant regular repeating pattern of alternating positive and negative ions in 3D. The packing structure of the ions depends on the relative.
Solids, Liquids, & Gases Chapter 3.
Physical Properties Liquids & Solids. Liquids vs. Solids LIQUIDS Stronger than in gases Y high N slower than in gases SOLIDS Very strong N high N extremely.
Chapter 10 Kinetic Molecular Theory 10.2 & 10.3 Liquids and Solids.
Three States of Matter Part I. Matter All matter is made up of tiny particles, called atoms, which cannot be seen even using normal (visible light) microscopes.
Properties of Solids.
10.3: Solids By: Grace, Rosa, Zoie and Jaylen. Properties of Solids in Kinetic- Molecular Theory The particles of a solid are closely packed, therefore.
Kintetic Molecular Theory
Atoms and molecules form solids by building repeating patterns.
Table of Contents The Kinetic-Molecular Theory of Matter
11.7 Solids There are two groups of solids: Crystalline solids
Kintetic Molecular Theory
John D. Bookstaver St. Charles Community College Cottleville, MO
Bonding and Structure in Solids
11.4 NOTES Solids.
Bonding and Structure in Solids
II. Physical Properties (p )
Solids Section 10.3.
II. Physical Properties (p )
Solids and Phase Changes
Solids, Liquids, and Gases
Solids, Liquids, and Gases
Structure and Properties of Solids
Solids Chapter 10 Section 3.
States of Matter d. Students know the states of matter (solid, liquid, gas) depend on molecular motion. e. Students know that in solids the atoms are closely.
Solids, Liquids, and Gases
Matter Any thing that has mass and takes up space.
Chemical Bonds.
Properties of Solids and the Kinetic-Molecular Theory
Liquids and Solids Chapter 12.
States of Matter Solids.
Structure and Properties of Solids
Solids and Phase Changes
Chapter 13.3 The Nature of Solids.
II. Physical Properties (p )
Solids.
CLASSIFICATION OF SOLIDS
States of Matter Chapter 3 Section 1.
Solids.
The Solid-State Structure of Metals and Ionic Compounds
Presentation transcript:

 Dominated by... ◦ Closely packed particles ◦ Relatively fixed position ◦ Highest intramolecular attractions  Are... ◦ Definite shape and volume ◦ Definite melting point ◦ High density ◦ Incompressible ◦ Low rate of diffusion

Can be crystallineCan be amorphous Insulin crystalsObsidian

Have a regular repeating pattern of particles

 Ionic crystals ◦ Made of ions – hard and brittle ◦ Ex. NaCl  Metallic crystals ◦ Made of metals with free moving electrons  Covalent crystals ◦ Made of molecules ◦ Ex. Quartz (SiO 2 ), water, sugar  Atomic Crystals ◦ Made of atoms of one element ◦ Ex. Diamond or graphite

 No regular pattern in the particles, without a particular shape  Ex. Glass, plastics, wax, cotton candy