1. Matter
Chapter 2

2. Definition Matter is anything that has mass and takes up space.
Mass is a measure of the amount of matter.
Volume is a measure of the amount of space.

3. Types of Matter
An element is a substance that cannot be separated or broken down into simpler substances by chemical means.
An atom is the smallest unit of an element that maintains the properties of that element.

4. Combinations of Matter
A compound is a substance made up of atoms of two or more different elements joined by chemical bonds.
A molecule is the smallest unit of a substance that keeps all of the physical and chemical properties of that substance.

5. Chemical Formulas
Chemical formula shows how many atoms of each element are in a unit of a substance.
Chemical symbols represent the element.
Subscripts indicate how many atoms of each element are in one molecule of the compound.

6. Mixtures
Pure substances is matter that has a fixed composition and definite properties.
A mixture is a combination of two or more substances that are not chemically combined.

7. Types of Mixtures
Heterogeneous mixture aren’t mixed uniformly and are not evenly distributed.
Homogeneous mixture are evenly distributed and the mixture is the same throughout.

8. Physical Properties
Physical Properties are characteristics of a substance that does not involve a chemical change, such as density, color or hardness.
Examples are melting point, boiling point, strength, hardness, conductivity, magnetism, heat.

9. Chemical Properties
Chemical properties are characteristics of matter that describes a substance's ability to participate in chemical reactions.
Examples are reactivity with oxygen, acid, water, or other substances; flammability.

10. Physical Changes
Physical changes are changes of matter from one form to another without a change in chemical properties.
Examples are cutting, dissolving, mixing, melting, evaporating, subliming.

11. Chemical Changes
Chemical changes are changes that occur when a substance changes composition by forming one or more new substances.
Examples are burning, rusting, and ripening of fruit.

12. Triple Point of Carbon Dioxide
Under certain conditions, you can see dry ice as a solid, liquid and gas all at the same time.
Dry ice under pressure will exhibit all three states of matter.
Under normal conditions, dry ice will sublime from a solid to a gas.

13. Kinetic Theory
All matter is made of atoms and molecules that act like tiny particles.
These tiny particles are always in motion. The higher the temperature of the substance, the faster the particles move.
At the same temperature, more massive particles move slower than less massive particles.

14. States of Matter
Chapter 3

15. What variable needs to be changed in order to see carbon dioxide in a liquid state?
Energy.
Pressure.
Temperature.
Both pressure and temperature. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

16. Different States of Matter
Solids
Definite volume.
Definite shape.
Low energy, molecules close together.
Liquids
No definite shape.
More energy, molecules farther apart.

17. Different States of Matter
Gases
No definite volume.
No definite shape.
Lots of energy, molecules are very far apart.
Plasma
Particles have been broken apart.

18. Which of the following states of matter has the highest energy?
Gas.
Liquid.
Solid.
Plasma 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

19. Energy in States of Matter
Energy is the ability to change or move matter.
Thermal energy is the total kinetic energy of the particles that make up an object.

20. Change in States of Matter
Evaporation is the change of a substance from a liquid to a gas.
Boiling point is the evaporation of a liquid at a certain temperature.
Sublimation is the process by which a solid turns directly into a gas.

21. Changes is States of Matter
Condensation is the changes of state from a gas to a liquid.
Melting is the process of a solid changing into a liquid.
Freezing is the reverse of melting.

22. What is it called when a solid goes directly to a gas without a liquid state?
Evaporation.
Melting.
Freezing.
Sublimation. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

23. Conservation of Mass & Energy
The law of conservation of mass states that mass cannot be created or destroyed.
The law of conservation of energy states that energy cannot be created or destroyed.

24. Fluids Buoyant force is the upward force that fluids exert on matter.
All fluids exert pressure, which is the amount of force exerted on a given area.

25. Air is a fluid. True False 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 1718 19 20 21 22 23 24 25 26 27 28 29 30

26. Archimedes’ Principle
Archimedes Principle states that the buoyant force on an object in a fluid is an upward force equal to the weight of the fluid that the object displaces.

27. How do you calculate density?
Divide volume by mass.
Divide mass by volume.
Multiply mass by volume.
Multiply volume by mass. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

28. Fluid & Pressure Pressure is the amount of force applied over an area.
Pressure=force/area

29. Pascal’s Principle
Pascal’s principle states that a change in pressure at any point in an enclosed fluid will be transmitted equally to all part of the fluid.

30. Fluids in motion Viscosity is a liquid’s resistance to flow.
Bernoulli’s principle states that as the speed of a moving fluid increases, the pressure of the moving fluid decreases.

31. Properties of Gases
Gases have no definite shape or volume, and they expand to completely fill their container.
Gas particles move rapidly in all directions.
Gases are fluids.

32. Properties of Gases
Gas molecules are in constant motion, and they frequently collide with one another and with the walls of their container.
Gases have a very low density because their particles are so far apart. Because of this property, gases are used to inflate tires and balloons.

33. Properties of Gases Gases are compressible.
Gases spread out easily and mix with one another. Unlike solids and liquids, gases are mostly empty space.

34. Gas Laws
Gas laws explain the relationship between volume, temperature and pressure of gases.
Different Laws:
Boyle’s Law
Charles’ Law
Gay-Lussac’s Law

35. Boyle’s Law
Boyle’s Law states that for a fixed amount of gas at a constant temperature, the volume of a gas increases as its pressure decreases.
P1V1=P2V2

36. Charles’ Law
Charles Law states that for a fixed amount of gas at a constant pressure, the volume of the gas increases as its temperature increases.
K=V/T

37. Gay-Lussac’s Law
Gay-Lussac’s Law states that the pressure of a gas increases as the temperature increases if the volume of the gas does not change.

38. Boyle’s Law Charles’ Law Gay-Lussac’s Law Help me!
Which of the gas laws states that volume changes as temperature changes if the pressure is constant?
Boyle’s Law
Charles’ Law
Gay-Lussac’s Law
Help me! 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30

39. Homework
Chapter 3 Review.
Pages
Questions 1-22.