1. Solid, Liquid, and Gas Day 2

2. Curriculum Big Idea: Changes in matter are accompanied by changes in energy. Big Idea: Changes in matter are accompanied by changes in energy. Competency: Demonstrate how changes in matter are accompanied by changes in energy. Competency: Demonstrate how changes in matter are accompanied by changes in energy. PA Standard 3.2.C.A3: Describe the three normal states of matter in terms of energy, particle motion, and phase transitions.

3. Today’s Agenda Opener: Trade flipbooks with the person sitting next to you. Discuss in small groups and as a class. Opener: Trade flipbooks with the person sitting next to you. Discuss in small groups and as a class. Review the heating curve of water, and sketch a cooling curve of water Review the heating curve of water, and sketch a cooling curve of water Notes on solids, liquids, and gases Notes on solids, liquids, and gases Investigate: Discover the affect of temperature on the volume of a gas (Day 2 – Volume Changes) in packet Investigate: Discover the affect of temperature on the volume of a gas (Day 2 – Volume Changes) in packet Observe the sublimation of iodine crystals to a purple gas! Observe the sublimation of iodine crystals to a purple gas! Checking Up on page 19 Checking Up on page 19 Closure Question: What is sublimation? Closure Question: What is sublimation? Take Home Assignment: Chemistry to Go on pages 20-21

4. Today’s Chemistry Vocabulary temperature: the measure of the average kinetic energy of all the particles of the material. temperature: the measure of the average kinetic energy of all the particles of the material. kinetic energy: a form of energy related to the motion of a particle. kinetic energy: a form of energy related to the motion of a particle. normal melting point: the characteristic temperature, at 1 atm, at which a material changes from a solid state to its liquid state. normal melting point: the characteristic temperature, at 1 atm, at which a material changes from a solid state to its liquid state. potential energy: stored energy of the material as a result of its position in an electric, magnetic, or gravitational field. potential energy: stored energy of the material as a result of its position in an electric, magnetic, or gravitational field. normal boiling point: the temperature at which the vapor pressure of the pure liquid equals 1 atm. normal boiling point: the temperature at which the vapor pressure of the pure liquid equals 1 atm.

5. Today’s Chemistry Vocabulary Vaporization: the change of state from a liquid to a gas Vaporization: the change of state from a liquid to a gas Sublimation: the change of state of a solid material to a gas without going through the liquid state Sublimation: the change of state of a solid material to a gas without going through the liquid state

6. solid liquid gas solid liquid gas

7. The Nature of Solids Solids have an orderly arrangement of particles in fixed locations. Solids have an orderly arrangement of particles in fixed locations. The particles of a solid vibrate in place. The particles of a solid vibrate in place. Most solid substances are crystalline. Most solid substances are crystalline. Crystal – has particles that are arranged in an orderly, repeating, three- dimensional pattern called a crystal lattice Crystal – has particles that are arranged in an orderly, repeating, three- dimensional pattern called a crystal lattice

9. Non-Crystalline Solids Amorphous solid – lacks an ordered internal structure and its atoms are arranged randomly Amorphous solid – lacks an ordered internal structure and its atoms are arranged randomly Examples: Rubber, plastic, glass, asphalt Examples: Rubber, plastic, glass, asphalt

10. The Nature of Liquids Intermolecular attractions keep the particles in a liquid close together Intermolecular attractions keep the particles in a liquid close together Liquids are much more dense than gasses. Liquids are much more dense than gasses.

11. Evaporation Vaporization – the conversion of a liquid to a gas Vaporization – the conversion of a liquid to a gas Evaporation – Vaporization of a liquid that is not boiling. Only those molecules with a certain minimum kinetic energy can escape from the surface of the liquid. Evaporation – Vaporization of a liquid that is not boiling. Only those molecules with a certain minimum kinetic energy can escape from the surface of the liquid.

12. Boiling Point the temperature at which the vapor pressure is equal to the atmospheric pressure the temperature at which the vapor pressure is equal to the atmospheric pressure When a liquid is heated to a temperature at which particles throughout the liquid have enough kinetic energy to vaporize, the liquid begins to boil. When a liquid is heated to a temperature at which particles throughout the liquid have enough kinetic energy to vaporize, the liquid begins to boil.

13. Boiling Point and Pressure Changes As the Vapor pressure increases, the boiling point increases. As the Vapor pressure increases, the boiling point increases. normal boiling point – the boiling point of a liquid at a pressure of 101.3 kPa (1atm). normal boiling point – the boiling point of a liquid at a pressure of 101.3 kPa (1atm). Example: the normal boiling point of water is 100 ºC

14. The Nature of Gases Kinetic energy – energy of motion Kinetic energy – energy of motion Kinetic theory – all matter consists of tiny particles that are in constant motion. Kinetic theory – all matter consists of tiny particles that are in constant motion. Gas particles – small (insignificant volume) Gas particles – small (insignificant volume) Collisions between gas particles are perfectly elastic (the total kinetic energy remains constant). Collisions between gas particles are perfectly elastic (the total kinetic energy remains constant).

15. The Nature of Gases They collide with one another and with the walls of their container. They collide with one another and with the walls of their container. They travel in straight line paths between collisions. They travel in straight line paths between collisions. They fill all the available space in their container. They fill all the available space in their container.

16. The Nature of Gasses Gas pressure – results from the force exerted by a gas per unit surface area of an object Gas pressure – results from the force exerted by a gas per unit surface area of an object This force is due to the simultaneous collisions of billions of rapidly moving particles in a gas with an object. This force is due to the simultaneous collisions of billions of rapidly moving particles in a gas with an object.

17. Temperature Is proportional to the average kinetic energy of the particles of a material. Is proportional to the average kinetic energy of the particles of a material. Kinetic Energy – energy of motion Kinetic Energy – energy of motion As the temperature of a material increases, the particles move faster and the average kinetic energy of the material increases. As the temperature of a material increases, the particles move faster and the average kinetic energy of the material increases.

18. Absolute Zero The temperature at which the motion of particles theoretically ceases The temperature at which the motion of particles theoretically ceases 0 Kelvin or -273 ºCelsius 0 Kelvin or -273 ºCelsius Absolute zero has never been produced in the laboratory. Absolute zero has never been produced in the laboratory.