Chapter 1 States of Matter PDF

Chapter 1: States of Matter Chapter 1: States of Matter Chapter 1: State of Matter 1.1 Everything is made of particles 1.2 Solids, liquid, and gases 1.3 The particles in solids, liquids, and gases 1.4 Heating and cooling curves 1.5 A closer look at gas 1.1 Everything is...

Chapter 1: States of Matter Chapter 1: States of Matter Chapter 1: State of Matter 1.1 Everything is made of particles 1.2 Solids, liquid, and gases 1.3 The particles in solids, liquids, and gases 1.4 Heating and cooling curves 1.5 A closer look at gas 1.1 Everything is made of particle (P. 2) 1.1 Everything is made of particle 1.1 Everything is made of particle Three are three types of particles that you will meet: atoms ions molecule 1.1 Everything is made of particle Atoms The smallest particles that we cannot break down further in chemical reactions 1.1 Everything is made of particle Molecules A particle consisting of two or more atoms joining together 1.1 Everything is made of particle Ions (charged particles) 1.1 Everything is made of particle Evidence of Particles Cooking smells We are sensing particles! Why can you smell them even when you are studying in your room? 1.1 Everything is made of particle Diffusion 1.1 Everything is made of particle  Diffusion is a mixing process that particles mix and spread by colliding with other particles and bouncing off in all direction.  Due to the random movement of particles, particles flow from a region where they are at a high concentration to a region where they are at a low concentration until all the particles are evenly mixed.  It takes places in liquids and gases.  1.1 Everything is made of particle Why can you smell them even when you are studying in your room? The ‘smells’ from cooking are due to the particles because they mix and spread by colliding with the particles in air from a region of high concentration (e.g.: kitchen) to a region of low concentration (e.g. bedroom). You can smell them when they reach your nose. 1.2 Solid, liquids, and gases 1.2 Solids, liquids, and gases Properties Solid Liquid Gas Fixed Shape ✔ ❌ ❌ Fixed Volume ✔ ✔ ❌ Other Cannot be take the shape spread out to compressed of the container fill its container 1.2 Solids, liquids, and gases Three States of Water 1.2 Solids, liquids, and gases 2 1 Melting: the process that occurs when a solid turns into liquid. 2 Melting Point: The 1 temperature at which a substance melts. Each substance has a specific melting point. Water has a 1.2 Solids, liquids, and gases 2 3 Evaporation: The process that occurs at the 3 surface of a liquid as it turns into a gas. Evaporation can 1 occur at temperatures lower than the boiling point of a liquid. 1.2 Solids, liquids, and gases 2 5 4 Boiling: The process that occurs 3 when a liquid turns into gas. 5 Boiling Point: 1 4 The temperature at which a substance boils. Each substance has a specific boiling point. Water has a boiling point of  1.2 Solids, liquids, and gases ★ Common Misconception about Boiling and Evaporating ★ ❌Only boiling involves changing liquid to gas.  Wrong  Boiling and evaporating are both changes of state that involve a liquid changing to a gas.  Evaporation can occur at temperatures lower than the boiling point of a liquid. (Imagine that you put a cup of water in your room, the volume of water will slowly reduce.) 1.2 Solids, liquids, and gases 2 5 6 Condensation: The process that occurs 3 when a gas turns into a liquid. 1 4 6 1.2 Solids, liquids, and gases 2 5 7 Freezing: The process that occurs 8 3 when a liquid turns into a solid. 8 Freezing Point: 1 4 The process that occurs 7 6 when a gas turns into a liquid. 1.2 Solids, liquids, and gases Exception 1.2 Solids, liquids, and gases Other physical change – sublimation and deposition Unlike regular ice, dry To create a layer of fog ice (carbon dioxide) on stage does not melt into a liquid as it warms up  1.2 Solids, liquids, and gases Other physical change – sublimation and deposition Sublimati on Depositi on Sublimation: The process that occurs when a solid turns into a gas without turning into a liquid Deposition: The process that occurs when a gas turns into a solid without turning into a liquid. Other example: Dry ice, Iodine, and Ammonium Chloride  1.2 Solids, liquids, and gases  Summary (Diagram) 1.3 The particles in solids, liquids, and gases 1.3 The particles in solids, liquids, and gases Kinetic Particle Theory 1.3 The particles in solids, liquids, and gases  Ice (Solid). The particles are closely ___________ packed and arranged in a regular ________________. Attraction force between the particles arestrong pattern/lattice ________. They vibrate ________ to and fro but not moving apart. When you apply pressure, the particle cannot move closer, so the volumedoes not change __________________. 1.3 The particles in solids, liquids, and gases  Water (Liquid). The particles are closely ___________ packed and arranged irregularly ________________. Attraction force between the particles are weaker ________ than solid. They move about and slide past other ___________________________each When you apply pressure, the particle cannot move closer, so the volumedoes not change __________________. 1.3 The particles in solids, liquids, and gases  Water Vapor (Gas). The particles are _____________ far apart and arranged irregularly ____________. There is almost no attractionbetween particles. ______________ They move freelycollide with each other, and bounce off in _____________, all direction. The particles can move a lot closer, so the gas __________________ can be pushed into a smaller volume. 1.3 The particles in solids, liquids, and gases Kinetic Particle Theory Changing States 1.3 The particles in solids, liquids, and gases Kinetic Particle Theory: Melting  Using kinetic particle theory to explain melting: 1. When the solid is hotter, the particles takes in more heat energy and transform to kinetic energy. The particles vibrate more, weakening the force that hold the solid. 2. Thus, the spaces between the particles become larger, and the solid expands. 3. When the temperature reaches its melting point, the particles vibrate so much that they break free from their positions. 4. The solid turns liquid. 1.3 The particles in solids, liquids, and gases Kinetic Particle Theory: Boiling  Using kinetic particle theory to explain boiling: 1. When the liquid is heated, the particles get more heat energy and change to kinetic energy. Thus, they vibrate faster. The move faster, collide more often, and bounce further apart. 2. The spaces between the particles become larger so the liquid expands. 3. When the temperature reaches its boiling point, the particles get enough kinetic energy to overcome the forces between them. 4. The liquid becomes gas. 1.3 The particles in solids, liquids, and gases Reversing the changes As a gas cools, its particles lose energy and move less quickly. When they collide, they do not have enough energy to bounce away. So they stay close, and form a liquid. 1.3 The particles in solids, liquids, and gases Reversing the changes (Heat energy is absorbed from the surroundings) (Heat energy is released to the surrounding) When a gas is cooled down, particles lose energy and move less vigorously. When they collide, they do not have energy to bounce away. The distance between particles  Checkpoint Class Practice 2 1. Determine the physical state of the following substances in room temperature Substance Melting Boiling State at Point (°C) Point (°C) 20°C Oxygen -219 -183 Gas Mercury -39 357 Liquid Ethanol -15 78 Liquid Water 0 100 Liquid Sodium 98 890 Solid Table salt (sodium 801 1465 Solid Solid chloride) Solid Iron 1540 2900 Oxygen 2. Which substance has the lowest melting point? Diamond 3550 4832 Diamond 3. Which substance has the highest melting point? 1.4 Heating and cooling curves 1.4 Heating and cooling curves  A heating curve shows the changes of state occurring when the temperature of ice is gradually increased. liquid-gas solid-liquid Flat line: Changing State Steep Line: Changing Temperature (no change in temperature) (no change in state) 1.4 Heating and cooling curves  A cooling curve shows how the temperature of a substance changes as you cool it down liquid-gas liquid-solid Flat line: Changing State Steep Line: Changing Temperature (no change in temperature) (no change in state) 1.4 Heating and cooling curves  Impurity  Changes of state will occur over a range of temperature, not sharply  They lines corresponding to melting and boiling will be tilted, not flat.  1.4 Heating and cooling curves  Drawing Heating curve for water 1. Title Heating curve for water 2. Label x and y axis 100 Temperature (°C) 3. Plot data point Melting Point of Water: 0°C Boiling Point of Water : 100 °C 0 4. Connect them Time (minutes)  Checkpoint 1.4 Heating and cooling curves 4 Question 1 17°C 115°C liquid  Checkpoint 1.4 Heating and cooling curves 4 Question 2 Draw a cooling curve of water Cooling curve for water Temperature (°C) Time (minutes) 1.5 A closer look at gases  1.5 A closer look at gases  Gas pressure  Gas particles exert a force on the wall during the collision.  The accumulation of all these forces distributed over the area of the walls of the container causes something we call pressure.  When you blow up a balloon, you fill it with air particles.  Collide with the side of the balloon  Pressure  1.5 A closer look at gases  Gas pressure  Increase / decrease the temperature of gas  The same is true for all gases, at constant pressure,  When you heat a gas, its volume increases  When you cool a gas, its volume decreases.  1.5 A closer look at gases  Gas pressure  Increase / decrease the pressure of gas  The same is true for all gases, at constant temperature,  An increase in pressure means a decrease in volume, for a gas.  A decrease in pressure means an increase in volume, for a gas. 1.5 A closer look at gases The Rate of diffusion of gases Ammonia gas diffuses   Hydrogen chloride gas diffuses 1.5 A closer look at gases  Which one travel faster?  Thelower the mass of its particles, the faster a gas will diffuse.  Thelower its relative molecular mass, the faster a gas will diffuse.  1.5 A closer look at gases The Rate of diffusion of gases Ammonia gas diffuses to the right Hydrogen chloride gas diffuses to the right The lower its relative molecular mass, the faster a gas will diffuse. Answer: D Key Terms Terms Definitions Melting The process that occurs when a solid turns into liquid. Melting point The temperature at which a substance melts. Each substance has a specific melting point. Boiling The process that occurs when a liquid turns into gas. Boiling point The temperature at which a substance boils. Each substance has a specific boiling point. Evaporation The process that occurs at the surface of a liquid as it turns into a gas. Evaporation can occur at temperatures lower than the boiling point of a liquid. Freezing The process that occurs when a liquid turns into a solid. Freezing point The temperature at which a substance freezes. This has the same value as the melting point. Condensation The process that occurs when a gas turns into a liquid. Sublimation The process that occurs when a solid turns into a gas without turning into a liquid. Deposition The process that occurs when a gas turns into a solid without turning into a liquid. Diffusion The mixing and spreading process that occurs when particles move from a region of high concentration to low concentration. Make sure you are able to:  State the distinguishing properties of solids, liquids and gases  Describe the structures of solids, liquids and gases in terms of particle separation, arrangement and motion  Describe changes of state in terms of melting, boiling, evaporating, freezing and condensing  Describe the effects of temperature and pressure on the volume of a gas  Explain changes of state in terms of kinetic particle theory, including the interpretation of heating and cooling curves  Explain, in terms of kinetic particle theory, the effects of temperature and pressure on the volume of a gas  Describe and explain diffusion in terms of kinetic particle theory  Describe and explain the effect of relative molecular mass on the rate of diffusion of gases