Lecture 3512/2/05. Quiz 1. For any given substance, how do you get its boiling point from its vapor pressure curve? 2. How much energy does it take to.

Slides:



Advertisements
Similar presentations
State Changes Heat of Fusion Heat energy required to convert a solid at its melting point to a liquid Value for water: 333 J/g Heat of Vaporization Heat.
Advertisements

Solid phase (s): Strong attractive forces hold particles in fixed location. Regular definite geometric shape; crystalline Liquid phase (l): Particles have.
The Kinetic Theory of Matter
Phase Changes.
Pure Substances Thermodynamics Professor Lee Carkner Lecture 5.
Change of state. Change of state and energy consumption.
All gases consist of small particles
States of Matter—Gases, Liquids and Solids. The Kinetic Molecular Theory The theory of moving molecules -Use to explain the properties of solids, liquids,
I. Intermolecular Forces (Ch. 6, p )
Intermolecular Forces and Liquids and Solids Chapter 11.
Lecture 3211/21/05 2 seminars left. London Dispersion Forces: Induced dipole / Induced dipole Non-polar / non-polar interaction 0.05 – 40 KJ/mol.
Figure 16.44: Behavior of a liquid in a closed container.
Figure 16.44: Behavior of a liquid in a closed container.
Chapter 10 States of Matter. Section 1: The Kinetic-Molecular Theory of Matter.
Chapter 10 States of Matter
How many joules are needed to change 120.g of
Heating and Cooling Curve Definitions: Specific Heat: Amount of energy required to raise the temperature of 1 gram of a substance by 1⁰ Celsius Enthalpy.
Practice Energy Calculation Quiz. How much energy does it take to convert 722 grams of ice at  211  C to steam at 675  C? (Be sure to draw and label.
Mark S. Cracolice Edward I. Peters Mark S. Cracolice The University of Montana Chapter 15 Gases, Liquids, and Solids.
Phase Changes. solidliquidgas melting freezing vaporizing condensing sublimination endothermic exothermic.
Calculating Heat. Specific Heat Amount of heat energy needed to raise the temp of 1 ml of a substance 1°C For water the specific heat is 4.19 J/g °C,
Intermolecular Forces. Kinetic Molecular Theory  Describes the behavior of subatomic particles Liquids, solids, and gases are composed of small particles.
Heat: Phase Change. 'change of phase' 'change of state'. The term 'change of phase' means the same thing as the term 'change of state'. o These changes.
Chapters 13 & 17 Phases and Heat. Phases of Matter Chapter 13.
John E. McMurry Robert C. Fay Lecture Notes Alan D. Earhart Southeast Community College Lincoln, NE General Chemistry: Atoms First Chapter 10 Liquids,
Liquids & Solids I. Intermolecular Forces. A. Definition of IMF  Attractive forces between molecules.  Much weaker than chemical bonds within molecules.
The Nature of Solids & Changes of State Miss K. Marshall.
PHYSICAL BEHAVIOR OF MATTER
2 pt 3 pt 4 pt 5pt 1 pt 2 pt 3 pt 4 pt 5 pt 1 pt 2pt 3 pt 4pt 5 pt 1pt 2pt 3 pt 4 pt 5 pt 1 pt 2 pt 3 pt 4pt 5 pt 1pt States of Matter Solids Liquids Gases.
States of Matter Water. States of Matter  Objectives  Describe the structure of a water molecule  Discuss the physical properties of water. Explain.
Molar Enthalpy of Vaporization
States of Matter Solids, Liquids & gases State of matter Definite Mass? Definite Shape? Definite volume? Particle Energy Particle Spacing Examples Solid.
States of Matter 3 States of Matter: 1)solid- a substance with a definite shape and a definite volume. The particles of a solid vibrate, but do not move.
Chapter 13 States of Matter Liquids and Solids Changes of State.
PHYSICAL PROPERTIES OF MATTER Phases of Matter.
Properties of Solids and the Kinetic- Molecular Theory The particles of a solid are more closely packed than those of a liquid or a gas. All interparticle.
Solid phase (s): Strong attractive forces hold particles in fixed location. Regular definite geometric shape; crystalline Liquid phase (l): Particles have.
November 26 DO NOW: FILL IN THE BLANKS Ideal gases particles have no ________ and they have no ________ to each other. Ideal gases particles have no ________.
Thermochemistry Enthalpy: change in heat. Energy and Change of State You do not have to write this When energy is added to a solid substance, its temperature.
Liquids and Solids 1. To learn about dipole-dipole, hydrogen bonding and London dispersion forces 2. To understand the effect of intermolecular forces.
Condensed States of Matter: Liquids and Solids Chapter 14
Energy Conservation and Transfer Chm States of Matter Solid KMT –particles packed tightly together –high attraction –Lowest energy of all states.
Copyright©2004 by Houghton Mifflin Company. All rights reserved. 1 Introductory Chemistry: A Foundation FIFTH EDITION by Steven S. Zumdahl University of.
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.
I. States of Matter –Kinetic Molecular Theory –States of Matter.
DE CHEMISTRY: King William High School.  Pure substances (elements & compounds) have definite composition  Mixture is two or more different substances.
Phase Changes Heating Curve: Heat of Fusion From solid to liquid or liquid to solid Heat of Vaporization From gas to liquid or liquid to gas Always larger.
Calculating Heat During Change of Phase Heat Added (J)
In covalent solids, atoms are held together in an extensive three- dimensional network entirely by covalent bonds. Types of solids 12.4.
A Closer Look at Physical Properties Thermochemistry: States of Matter Thermochemistry:
Solids and Phase Changes. How is Kinetic Theory Applied to Solids? As liquid cools, particles move more slowly. Finally particles take fixed positions.
Intermolecular forces (van der Waals forces) London dispersion- instantaneous dipole moment -increases with mass -found between all molecules Dipole-dipole-
Table of Contents The Kinetic-Molecular Theory of Matter
Kinetic Molecular Theory
Properties of Liquids The attraction between liquid particles is caused by the intermolecular forces: London dispersion forces dipole-dipole forces hydrogen.
Solids.
II. Physical Properties (p )
Solids Section 10.3.
II. Physical Properties (p )
States of Matter Solids Liquids Gases.
Solids Chapter 10 Section 3.
Properties of Solids and the Kinetic-Molecular Theory
Liquids and Solids Chapter 13.
States of Matter Solids.
Changes of State units: J/g Heat of Vaporization
“Changing” Your mind Not Phased At All Give me an “E” “Word” to
Station 1 IM Forces- What happens to vapor pressure if the forces of a liquid decrease? What happens to vapor pressure if the forces of a liquid increase?
Chapter 10 Two Types of Solids
Solid phase (s): Strong attractive forces hold particles in fixed location. Regular definite geometric shape; crystalline Liquid phase.
II. Physical Properties (p )
Presentation transcript:

Lecture 3512/2/05

Quiz 1. For any given substance, how do you get its boiling point from its vapor pressure curve? 2. How much energy does it take to completely convert 10 g of ice at -10 °C to water at 0 °C? ΔH fusion = 333 J/gΔH vaporization = 2250 J/g C ice = 2.06 J/g-KC water = J/g-K

Types of Solids Ionic Metallic Molecular Network Amorphous

Solids crystalline solids solids with long-range ordering homogenous solid formed by a repeating, three- dimensional pattern, having fixed distances between constituent parts amorphous solids lacking definite form solids with no long-range ordering

Fig , p.511

Fig , p.512

Fig , p.513

Size, Volume, and Density

Feedback: Privacy Policy Feedback
Do Not Sell My Personal Information
About project: SlidePlayer Terms of Service

© 2024 SlidePlayer.com Inc. All rights reserved.