Chemistry notes Chapter 12. Section 1 “Liquids”  Properties Definite volume Definite volume Takes the shape of its container Takes the shape of its container.

Slides:



Advertisements
Similar presentations
The Kinetic Theory of Matter
Advertisements

I. Kinetic Molecular Theory KMT
CHAPTER 10 STATES OF MATTER
States of Matter Newport High School Academic Chemistry Modified from a PowerPoint found at
Intermolecular Forces and
I. Intermolecular Forces (Ch. 6, p )
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.
Liquids and Solids.
States of Matter Liquids. States of Matter  Objectives  Describe the motion of particles in liquids and the properties of liquids according to the kinetic-molecular.
Why did you not smell the odor of the vapor immediately?
Intermolecular Forces, Liquids and Solids
Chapter 14: Liquids and Solids
Modern Chemistry Chapter 10 States of Matter
Chapter 12 – Liquids and Solids. Which one represents a liquid? Why?
States of Matter: Liquids and Solids Chapter 14. Chapter 112 Copyright © by Houghton Mifflin Company. All rights reserved. States of Matter Comparison.
Chapter 12 Liquids and Solids.
Intermolecular Forces and Liquids and Solids Chapter 11.
Liquids & Solids Chapter 12. Properties of Liquids O Have definite volume & take shape of container O Lower kinetic energy than gases O Particles move.
Liquids and Solids Chapter 12.
Properties of Liquids and Solids
Liquids and Solids.
Solids. Motion & Arrangement Vibrate about center of mass. – Cannot “translate” or move from place to place. – Cannot slide past each other or flow. Packed.
STATES OF MATTER Chemistry CP.
Intermolecular Forces. Kinetic Molecular Theory  Describes the behavior of subatomic particles Liquids, solids, and gases are composed of small particles.
States of Matter.
Liquids & Solids I. Intermolecular Forces. A. Definition of IMF  Attractive forces between molecules.  Much weaker than chemical bonds within molecules.
The Kinetic-Molecular Theory of Gases
Chapter 10. The kinetic-molecular theory is based on the idea that particles of matter are always in motion. used to explain the properties of solids,
Chapter 12 Liquids and Solids Definitions!!!!  Fluid- a substance that can flow and therefore take the shape of its container.  Liquids and Gases.
Chapter *. Kinetic Molecular Theory Particles of matter are in constant motion.
Chapter 13 States of Matter Read pgs Kinetic Molecular Theory The kinetic molecular theory describes the behavior of gases in terms of particles.
Chapter 10 States of Matter Kinetic Molecular Theory (KMT) “Particles of Matter are always in motion” States of Matter We will discuss the KMT in.
Chapter 10, Section 2  LIQUIDS. Liquids & Kinetic-Molecular Theory  1. Liquid particles are closer together than gas particles.
Kinetic Molecular Theory A theory that envisions molecules in motion Best describes properties and behaviors of gases Can be applied to all states of.
Properties of Liquids. Reminder: Kinetic-molecular Theory says the particles of matter are always in motion I.Properties of Liquids & the Kinetic-Molecular.
Liquids & Solids. Objectives 12-1 describe the motion of particles of a liquid and the properties of a liquid using KMT define and discuss vaporization.
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.
Preview Lesson Starter Objectives Properties of Liquids and the Kinetic-Molecular TheoryProperties of Liquids and the Kinetic-Molecular Theory Chapter.
States of Matter Kinetic Molecular Theory: the idea that particles of matter are always in motion; this applies to all states of matter Used to explain.
Chapter 13 – Liquids and Solids. Which one represents a liquid? Why?
1. Intro a. Least common state of matter in universe b. Can only exist within a relatively narrow range of temps 2. Properties a. Definite volume and.
Condensed States of Matter: Liquids and Solids Chapter 14
Lesson Starter Compare the plaster of Paris mixture before it hardens to the product after it hardens. Section 3 Solids Chapter 10.
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.
Kinetic molecular theory and liquids and solids
Chemistry Kinetic Molecular Theory States of Matter Chapter 15.
Chapter 10 States of Matter Pages The Kinetic-Molecular Theory of Matter …states that particles of matter are always in motion. An _____________.
Chemistry notes Chapter 12. Section 1 “Liquids”  Properties  Definite volume  Takes the shape of its container  Particles are in constant motion 
The behavior of gases in motion is described by the kinetic molecular theory. Kinetic molecular theory:  gases are small particles, separated by empty.
13.2 The Nature of Liquids. Describe the particles in a liquid.
CHAPTER 14: LIQUIDS AND SOLIDS.  Condensed State- substances in these states have much higher densities than they do in the gaseous state CONDENSED.
Liquids and Solids. Intermolecular Forces  Intermolecular Forces are the attraction between molecules  They vary in strength, but are generally weaker.
Liquids and solids.
Table of Contents The Kinetic-Molecular Theory of Matter
Liquids and Solids Changes of State.
Liquids and Solids H2O (g) H2O (s) H2O ().
Kinetic Molecular Theory
Chemistry: Chapter 13 States of Matter.
Modern Chemistry Chapter 10 States of Matter
Chapter 13 Liquids and solids.
The Kinetic-Molecular Theory of Gases
Properties of Liquids The attraction between liquid particles is caused by the intermolecular forces: London dispersion forces dipole-dipole forces hydrogen.
CHAPTER 12 LIQUIDS and SOLIDS
Gases, Liquids and Solids
Ch 10 States of Matter 10.1 Kinetic Theory
Properties of Solids and the Kinetic-Molecular Theory
Liquids and Solids Chapter 13.
Liquids and Solids Chapter 12.
States of Matter Solids.
Liquids and Solids Chapter 12.
Presentation transcript:

Chemistry notes Chapter 12

Section 1 “Liquids”  Properties Definite volume Definite volume Takes the shape of its container Takes the shape of its container Particles are in constant motion Particles are in constant motion Vibrational, rotational, translationalVibrational, rotational, translational Adjacent particles are held together with dipole-dipole forces; London dispersion forces and Hydrogen bonding (these forces work on gases too, but not as strongly as they work in liquids) Adjacent particles are held together with dipole-dipole forces; London dispersion forces and Hydrogen bonding (these forces work on gases too, but not as strongly as they work in liquids)

Intermolecular forces  Dipole-Dipole forces The force of attraction between two polar molecules The force of attraction between two polar molecules

London dispersion Forces  Intermolecular attraction from the constant motion of electrons and the creation of instantaneous dipoles

Hydrogen bonding  Hydrogen atom is bonded to a highly electronegative atom and attracted to another nearby highly electronegative atom in an adjacent molecule

Fluid  Any substance that can flow and therefore take the shape of its container.  Liquids and gases are considered fluids

Density  Most liquids are about 10% less dense than they are as a solid  Water is one of the few substances that becomes less dense as a solid

Pressure  Liquids under pressure only condense to about 4% smaller than original volume. This is very similar in solids. Gases under pressure condense many times more.

Diffusion  Much slower in liquids than in gases Increased temperature increases diffusion rate Increased temperature increases diffusion rate

Surface tension  A force that tends to pull adjacent parts of a liquid’s surface together, thereby decreasing surface area to the smallest possible size the smallest possible size  This is why liquid droplets form a spherical shape form a spherical shape

Capillary action  The attraction of the surface of a liquid to the surface of a solid This causes the meniscus in a This causes the meniscus in a graduated cylinder and how roots transport liquids UP the plant graduated cylinder and how roots transport liquids UP the plant

Phase Changes  Vaporization: the process of a liquid or a solid changing to a gas  Evaporation: a form of vaporization where the particles escape from the surface of a non- boiling liquid  Freezing: the physical change of a liquid to a solid by removing heat (also called solidification)  We will look at this a lot more with phase diagrams What other changes are there? What other changes are there?

SECTION 2 “Solids”  Properties of a solid Intermolecular forces are stronger in solids than in liquids Intermolecular forces are stronger in solids than in liquids Molecules are more closely packed together Molecules are more closely packed together Molecular motion is restricted to vibrational movement around a specific point Molecular motion is restricted to vibrational movement around a specific point What does that do to Diffusion?What does that do to Diffusion? How does that affect a solids lack of a fluid nature?How does that affect a solids lack of a fluid nature?

Crystalline solid  Most solids are crystalline  Consists of crystals: orderly, repeating geometric pattern Crystal structure: total 3 dimensional arrangement of particles Crystal structure: total 3 dimensional arrangement of particles Lattice: the coordinate system that represents the arrangement of particles Lattice: the coordinate system that represents the arrangement of particles Unit cell: the smallest portion of a crystal lattice that shows the 3 dimensional pattern Unit cell: the smallest portion of a crystal lattice that shows the 3 dimensional pattern

4 types of crystals  Ionic crystals: usually a mix of group 1 or 2 with group 16 or 17: usually hard and brittle, high melting point and good insulators usually a mix of group 1 or 2 with group 16 or 17: usually hard and brittle, high melting point and good insulators  Covalent network crystals: Usually a single element covalently bonded with itself in a large network of atoms: examples include quartz, diamonds and oxides of transition metals: they are also hard and brittle with high melting points and are usually nonconductors or semiconductors Usually a single element covalently bonded with itself in a large network of atoms: examples include quartz, diamonds and oxides of transition metals: they are also hard and brittle with high melting points and are usually nonconductors or semiconductors

4 types of crystals (continued)  Metallic crystals Metal atoms surrounded by a sea of pooled electrons: they are highly conductive: melting points vary greatly Metal atoms surrounded by a sea of pooled electrons: they are highly conductive: melting points vary greatly  Covalent molecular crystals ( low melting point, relatively soft, good insulators Polar: water and ammonia held together by all types of intermolecular forces Polar: water and ammonia held together by all types of intermolecular forces Nonpolar: hydrogen, methane, benzene are all held together by weak london dispersion Nonpolar: hydrogen, methane, benzene are all held together by weak london dispersion

Amorphous solid  “Without Shape”  Glass and plastics are amorphous  Particles are arranged in a random order  Some are said to “flow”: you can see old panes of glass that are thicker at the bottom

Melting Point  Physical change of solid to liquid at a certain temperature Kinetic energy of particles overcome the forces that are holding them together Kinetic energy of particles overcome the forces that are holding them together Crystalline solids have definite melting points whereas amorphous solids have no definite melting point and can become supercooled liquids Crystalline solids have definite melting points whereas amorphous solids have no definite melting point and can become supercooled liquids

Density  Higher density than liquids and gases  Less compressible than liquids and are usually considered “incompressible” If you compress a cork, it’s the air pockets inside the cork that is being compressed, not the wood If you compress a cork, it’s the air pockets inside the cork that is being compressed, not the wood

Diffusion  Diffusion occurs in solids, but only millions of times slower than in liquids Zinc and copper plates that are compressed together for a long period of time Zinc and copper plates that are compressed together for a long period of time Rock / sediment that is compressed for hundreds or thousands of years Rock / sediment that is compressed for hundreds or thousands of years

Section 3 “Changes of State”  Equilibrium: a dynamic condition in which two opposing changes occur at equal rate in a closed system  Condensation: the process by which a gas changes to a liquid  Liquid + heat energy ↔ vapor

Le Chatelier’s principle  When a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress Stress is usually a change in concentration, pressure or temperature Stress is usually a change in concentration, pressure or temperature

How Temperature affects Equilibrium  Increase in temperature favors the forward reaction (endothermic)  Decrease in temperature favors the backwards (reverse) equation (exothermic)  Liquid + heat energy ↔ vapor

How concentration affects equilibrium  Decrease in vapor concentration (increase in volume) less condensation occurs – equilibrium shifts to the right  Liquid + heat energy ↔ vapor See table 12-3 on page 375

How Vapor pressure affects equilibrium  Equilibrium vapor pressure: the pressure exerted by a vapor in equilibrium with its corresponding liquid at a give temperature EVP increases with increasing temperature EVP increases with increasing temperature

Volatile liquids  Liquids that evaporate easily  Ethanol is a good example of a volatile liquid. The intermolecular forces are very weak.

Boiling  Occurs when the EVP of the liquid equals the atmospheric pressure Liquid turns to vapor within the liquid as well as on the surface Liquid turns to vapor within the liquid as well as on the surface Boiling point: temperature at which EVP = atm. Pressure and boiling occurs for given substance Boiling point: temperature at which EVP = atm. Pressure and boiling occurs for given substance Energy used to separate intermolecular forces of liquids is stored in the vapor as potential energy Energy used to separate intermolecular forces of liquids is stored in the vapor as potential energy

Molar Heat of Vaporization  The amount of heat energy needed to vaporize one mole of liquid at its boiling point (  Hv) The greater the M.H. of V. the stronger the intermolecular forces of the liquid The greater the M.H. of V. the stronger the intermolecular forces of the liquid Water has a very high MHV Water has a very high MHV Makes it affective as a cooling agent (it absorbs heat away from the surface as it evaporates)Makes it affective as a cooling agent (it absorbs heat away from the surface as it evaporates)

Freezing and Melting  Occur at the same temperature but in reverse directions  Freezing point = The temperature at which the solid and liquid are in equilibrium at standard pressure  Solid + heat energy ↔ liquid

Molar Heat of Fusion  The amount of heat energy needed to melt one mole of solid at its melting point (  Hf)

Sublimation and Deposition  Solid + heat energy ↔ vapor  Low temp and pressure does not allow liquids to exist  Sublimation = change from solid to gas  Deposition = change from gas to solid  Both dry ice and iodine sublime at normal temperatures

Phase Diagram  Triple point: indicate the temperature and pressure condition at which the solid, liquid and vapor of the substance can coexist at equilibrium  Critical point: critical temp and press  Critical temperature: above this temperature, liquid cannot exist  Critical pressure: lowest pressure liquid can exist at the critical temperature

Phase diagrams

Liquid water is more dense than ice Water Ice Water Ice Water molecules are most dense at 3.98°C

The only math in this section  Molar heat of fusion is kJ/mole  At standard pressure, molar heat of vaporization is kJ/mol 1. a) How much heat energy is absorbed when 47.0g of ice melts at STP? b) How much is absorbed when this same mass of liquid water boils? a) 15.7 kJ b) 106 kJ

The only math in this section  Molar heat of fusion is kJ/mole  At standard pressure, molar heat of vaporization is kJ/mol 2. What quantity of heat energy is released when 506 g of liquid water freezes? 169 kJ

The only math in this section  Molar heat of fusion is kJ/mole  At standard pressure, molar heat of vaporization is kJ/mol 3. What mass of steam is required to release 4.97 x 10 5 kJ of heat energy on condensation? 2.19 x 10 5 g