Exploring Matter: Atoms, Molecules, and Properties

1. The Nature of Matter Bill Nye Atoms and Molecules

2. Matter • Matter: anything that has mass and takes up space

3. Matter • Element: cannot be broken down into smaller parts and contains only one type of atom • 96 are found in nature • 20 are man made • Gold, oxygen, helium, iron

4. Matter • Compound: contains 2 or more different atoms • Water (H₂O) carbon dioxide (CO₂)

5. Mixtures • Mixture: a blend of 2 or more substances that can be separated • Homo: same • Hetero: different

6. Matter • Homogeneousmixtures or solutions: a mixture that is even in composition • Cannot be separated easily • Soda, vinegar, Salt water, sugar water

7. Mixtures • Heterogeneousmixture: a mixture that is not even in composition • Can be separated easily • Granite, concrete, pizza, soup, salad

9. Matter • Colloid: a mixture with large particles that don’t settle to the bottom • Paint, fog, smoke, milk, jello, liquid soap

10. Matter • Suspension: a heterogeneous mixture that has visible particles in it • Lake or pond water

11. Distillation • Distillation: separating parts of a mixture by boiling off the liquid • solar still

13. Learning Check • How is a compound similar to a homogeneous mixture? • Give an example of a heterogeneous mixture. • Give an example of a homogeneous mixture. • Give an example of a suspension. • If a product says “shake well before using”, what type of substance is it? • Describe the difference between a colloid and a suspension.

14. Properties of Matter • PhysicalProperty: a characteristic that you can observe without changing the substance • Color • Shape • Mass • Volume • Malleability • Boiling or melting point • Density • Weight • Texture

15. Properties of Matter • PhysicalChange: a change in the shape, size or state of matter but the matter itself does not change • cutting, melting, boiling, freezing, erosion of rocks by wind

16. Properties of Matter • ChemicalProperties: a characteristic of a substance that indicates whether or not it can undergo a chemical change • Flammable, react with light or water

17. Properties of Matter • ChemicalChange: changing one substance into one or more new substances • Examples: burning paper, rusting of iron • Bill Nye Chemical Changes

18. Chemical Change Signs • Production of odor • Change in color • Formation of bubbles (gas) • Temperature change • Formation of a new substance

19. Conservation of Mass • Law of the conservation of mass: mass cannot be created or destroyed • The mass of the reactants = the mass of the products

22. Kinetic Energy of Matter • KineticTheory: the explanation of how particles in matter behave • All matter is composed of atoms • The atoms are in constant, random motion • The atoms are colliding with each other and their container

23. Thermal Energy of Matter • ThermalEnergy: because all matter is moving, all matter has thermal energy • Kineticenergy: the temperature of a substance is equal to the substance’s kinetic energy

24. States of Matter • states of matter • Solid: a rigid substance with a definite shape • Molecules are tightly packed together

25. States of Matter • Liquid: has a definite volume but takes the shape of its container • Molecules glide over one another

26. Liquid State • Meltingpoint: the temperature at which a solid begins to liquefy • Heatoffusion: the amount of energy needed to change the phase of a substance

27. States of Matter • Gas: takes the shape and volume of its container • Molecules are in constant motion and rarely touch each other • States of Matter Bill Nye

28. Boiling Point • BoilingPoint: the temperature at which the particles in an object start to vaporize • Heatofvaporization: the amount of energy needed for a liquid to become a gas

29. Plasma • Plasma: matter that is made up of positive and negative charges • Example: stars, the sun, lightning, neon lights, auroras

30. Expansion of matter • ThermalExpansion: the increase in size of a substance when the temperature is increased • Cold: molecules are tightly packed together • Hot: molecules are far apart from each other

31. Density • Density: how tightly packed molecules are in a substance • Equation: d = m/V

32. Density • Corn syrup • Water • Dish soap • Vegetable oil • Vinegar • Die • Maple syrup • Bead • Rock • Plastic dinosaur

33. Oil • Water • Vinegar • Maple syrup • Dish soap • Corn syrup

34. Properties of Fluids • Buoyancy: the ability of a fluid (liquid or gas) to exert an upward force • Floating: buoyant force = weight of the object • Sinking: the objects weight is greater than the buoyant force

35. Archimedes’ Principle • Archimedes’ Principle: the buoyant force on an object is equal to the weight of the fluid that is displaced by the object

36. Bernoulli’s Principle • Bernoulli’sPrinciple: as the velocity of a fluid increases, the pressure it exerts decreases

37. Viscosity • Viscosity: a fluids resistance to flow freely • Lowviscosity: flows easily • Highviscosity: does not flow easily

38. Viscosity • Corn syrup • Water • Dish soap • Vegetable oil • Rubbing alcohol • Milk • Honey • Coke

39. Critical thinking questions • What might happen to a fluid’s viscosity if we increase the temperature of a fluid? • How is the density of a fluid related to the viscosity of a fluid?

40. Behavior of Gases • Pressure of a gas = the number of collisions the gas has with the container it is in • Pascal: the unit of measure for gas pressure Pa, kPa • Air pressure at sea level: 101.3 Pascals • 101,300 Newtons per square meter

43. Pascal’s Principle • Pascal’sPrinciple: the force exerted on an area equals the force over the area • Equation: P = F/A • Measured in Newtons • Example: a hydraulic lift is used to raise up a machine that is pushing down on a 2.8 m² piston with a force of 3700 N. What force needs to be exerted on a 0.072 m² piston to lift the machine? • A₁ = • F₁ = • A₂ = • F₂ =

44. Using Pascal’s Principle • A heavy crate applied a force of 1500 N on a 25 m² piston. What force needs to be exerted on the 0.80 m² piston to lift the crate? • A₁ = • F₁ = • A₂ = • F₂ =

45. Boyle’s Law • Boyle’sLaw: if the volume of the container a gas is in decreases, the pressure of the gas increases

46. Boyle’s Law • Equation: P₁V₁ = P₂V₂ • Example: a balloon has a volume of 10 L at a pressure of 101 kPa. What will the new volume be when the pressure drops to 43 kPa? • P₁ = • V₁ = • P₂ = • V₂ =

47. Using Boyle’s Law • A volume of helium occupies 11 L at 98 kPa. What is the new volume if the pressure drops to 86.2 kPa? • P₁ = • V₁ = • P₂ = • V₂ =

48. Pressure-Temperature Relationships • Charles’s Law: the volume of a gas increases when the temperature increases • Equation: V₁T₁ = V₂T₂ • What would be the resulting volume of a 2 L balloon at 25⁰ C that is placed in a container of ice water that is 3⁰ C ?

49. Using Charles’s Law • If a 5 L balloon at 25⁰ C was heated to 30⁰ C, what new volume would the balloon have? • V₁ = • T₁ = • T₂ = • V₂