Physical Properties of Matter - Part 1 Student PDF

Physical Properties of Matter States of Matter The entire universe and all the changes that occur in it can be described by two concepts: matter and energy Chemistry CHEMISTRY – the study of the structure and properties of matter MATTER – anything that has mass and takes up space Th...

Physical Properties of Matter States of Matter The entire universe and all the changes that occur in it can be described by two concepts: matter and energy Chemistry CHEMISTRY – the study of the structure and properties of matter MATTER – anything that has mass and takes up space Three States of Matter There are three physical states of matter. Certain characteristics of each state can distinguish between these states. State of Matter: Solid ▪ Have a definite shape and volume. ▪ Shape doesn’t depend on the container. ▪ Particles are tightly packed together, often in an ordered arrangement. ▪ Will expand slightly when heated. ▪ Usually Incompressible. ▪ Varying density ex.) iron 7.87g/cm3, gold 19.3 g/cm3, calcium 1.54 g/cm3. State of Matter: Liquid ▪ Particles of a liquid are in close contact, but arrangement is not rigid or orderly. ▪ Flow freely, liquids take the shape of the container (some liquids pour easier than others). ▪ Volume remains constant, even if shape changes. ▪ Usually incompressible. ▪ Will expand slightly when heated. ▪ Can diffuse easily from areas of high concentrations to low concentrations. ▪ Varying densities ex.) mercury 13.53 g/mL, water 1 g/mL. State of Matter: Gas ▪ Flows freely, will take the shape of the container. ▪ Will expand to fill any volume. ▪ Particles in a gas are much farther apart than solids and liquids. ▪ Easily compressed. ▪ Can diffuse easily from areas of high concentrations to low concentrations. ▪ Varying densities ex.) hydrogen 0.089 g/cm3, oxygen 1.43 g/cm3, chlorine 3.21 g/cm3.  SOLID LIQUID GAS Shape definite shape takes the shape of its container takes the shape of its container Volume takes the volume definite volume definite volume of its container Density usually much less usually less dense usually very dense dense than solids than solids and liquids Compressibility not easily not easily easily compressed compressed compressed Diffusion does not easily easily diffuses diffuses very easily diffuse State of Matter: Plasma ▪ A gaseous mixture of positive ions and electrons. ▪ Formed at high temperatures greater than 100 million Celsius when electrons are stripped from neutral atoms. ▪ Very unstable. ▪ The most common form of matter in the universe, comprising 99% of the visible universe, but are the least common on Earth. ▪ DO NOT occur naturally on Earth except in the form of lightning bolts. ▪ Examples include aurora borealis, lightening, fluorescent lights, and stars. ▪ Neon sign - glass tubes filled with gas, electricity is turned on and charges the gas, creating plasma inside the tube and the colour depends on type of gas. State of Matter: Summary State of Matter: Summary Lab 1: The Behaviour of Gases (Inquiry Activity) The Nature of Gas ▪ ENERGY – ability to do work □ work: movement of a force (push or pull) through a distance □ two types: kinetic and potential energy Potential Energy Kinetic Energy energy of motion ○ formula: KE = 1/2mv2 ○ m = mass of the particle ○ V = velocity of the particle energy of an object can be increased by increasing the velocity of the object Kinetic Molecular Theory Kinetic Molecular Theory 1. Gases are made up of extremely small particles called molecules. (volume is negligible in comparison with the volume of the container) Kinetic Molecular Theory 2. Molecules of a gas are in rapid, random, straight line motion. They collide with each other and with the walls of the container Kinetic Molecular Theory 3. All collisions are perfectly elastic; that is, there are no energy losses due to friction Kinetic Molecular Theory 4. There are no attractive forces between the molecules. Kinetic Molecular Theory 5. Molecules of different gases have equal average kinetic energies at the same temperature. If the temperature increases, the average kinetic energy of the molecules increases Energy: Kinetic Energy and Temperature ▪Kinetic Energy: energy due to motion of an object ▪Potential Energy: stored portion of energy ▪Average kinetic energy: used when talking about the kinetic energy of a substance. ▪Temperature: a measure of the average kinetic energy of the particles of a substance.  Energy: Absolute Zero ▪If kinetic energy and temperature are related, there is a temperature at which all particles of a substance will stop moving, called absolute zero. (-273°C or 0 Kelvin) ▪Kelvin Temperature: directly proportional to the average kinetic energy of the particles in a substance. K = °C + 273 Energy: Kinetic Energy Distribution Curve Markers for Boltzman Energy: Kinetic Energy Distribution Curve Energy: Kinetic Energy Distribution Curve 100 K = -173 C 300 K = 26 C 600 K = 327 C 1000 K = 727 C  How Does the Kinetic Molecular theory explain the properties of gases? 1. Volume of a gas is mostly empty space □ therefore it should be easy to force the molecules into a smaller space □ COMPRESSIBILITY  How Does the Kinetic Molecular theory explain the properties of gases? 3. Since there are no 2. Since the distance between molecules is intermolecular forces, large, it is always possible the gases will act to add more gas molecules independently in their collisions with the walls of the container 4. If molecules lost energy during non elastic collisions they would gradually slow down and come to rest at the bottom of the container (never been observed for any gas) KINETIC MOLECULAR THEORY  ASSIGNMENT LAB 1 BEHAVIOUR OF GAS WRITE UP  ASSIGNMENT 1. Read p. 413 – 417 – explain in a poster the following : ▪ scuba diving, basketballs, air bags, aerosol cans, pistons 2. Text p. 417 #1 – 6  LIQUIDS ▪ According to the Kinetic Theory, gas and liquid particles have kinetic energy □ this allows the particles to flow past each other (fluids – substances that can flow) ▪ allows them to take the shape of their container  LIQUIDS ▪ Liquids and solids are more dense than gases because intermolecular attractions reduce the amount of space between the particles in a liquid ▪ Since there is less space between the particles, liquids are harder to compress ▪ Expand less when heated than gases do (because of stronger forces of attraction)  ASSIGNMENT ▪ LAB 2: THE BEHAVIOUR OF LIQUIDS AND GASES ▪ Kinetic Theory states of matter ▪ animation states of matter The Nature of Solids  Solid Glass Crystal (Amorphous) Solids: Overview ▪There are two categories of solid: □ Crystal Glassy Crystalline □ Glass ▪Crystals are ordered ▪Glasses are disordered Crash Course Solids: Glassy or Amorphous Solids ▪ Few glasses ▪ Lack of order makes them poor conductors of heat and electricity ▪ No fracture planes ▪ Created by rapid cooling ▪ Examples include: glass, rubber, obsidian, plastic, and asphalt Crash Course Solids: Crystalline Solids ▪ Arranged into an orderly, repeating 3 dimensional pattern: a lattice. ▪ Ordered structure makes them great conductors of heat and electricity ▪ Lots of fracture planes (diamond armour is terrible) ▪ Created by slow cooling ▪ Examples include: salt, sugar, quartz, iron, and many more Crash Course Solids: Allotropes ▪ What are these made of? Solids: Allotropes ▪ What are these made of? Solids: Allotropes ▪ 2 or more molecular forms of the same element ▪ Allotropes of an element have different properties because of their arrangement of the atoms. ▪ Only a few elements have allotropes: □ Carbon □ Phosphorous □ Sulfur □ Oxygen □ Boron □ Antimony. Carbon Allotropes – Versatile Carbon