1. Section 2: Changes in Matter
Chapter 3: Matter and Energy
Section 2: Changes in Matter

2. Learning Objectives
Distinguish between physical and chemical properties.
Distinguish between physical and chemical changes.
Apply the law of conservation of mass.

3. Properties of Matter
Physical property: a property that a substance displays without changing its composition.
Chemical property: a property that a substance displays only through changing its composition.

4. Physical Properties
state of matter
melting point
mass
color

5. Chemical Properties flammability reacts with an acid
reacts with oxygen

6. Properties of Matter Gasoline:
Physical property: its characteristic odor
gasoline does not change its composition when it exhibits its odor
Chemical property: its flammability
gasoline does change its composition when it burns

7. Properties of Matter
The atomic or molecular composition of a substance does not change when the substance displays its physical properties.

8. Properties of Matter
A chemical or physical property can also be described as either intensive or extensive.
Intensive Properties: Properties that do not depend on the amount of substance present
Examples: color, melting point, density, luster

9. Properties of Matter
Extensive Properties: Properties that do depend on the amount of substance present.
Examples: mass, volume, amount of energy within a substance

10. Changes in Matter Physical property: the boiling point of water
How is the water changing once it boils?
When water boils, it turns into a gas, but the water molecules are the same in both the liquid water and the gaseous steam.

11. Changes in Matter
Physical change: matter changes its appearance but not its composition
When ice melts, it looks different but its molecular composition is the same. Solid ice and liquid water are both composed of water molecules, so melting is a physical change.

12. Changes in Matter Chemical change: matter does change its composition
For example, copper turns green upon continued exposure to air because it reacts with gases in air to form new compounds. This is a chemical change.

13. Changes in Matter
State changes: transformations from one state of matter to another, such as from solid to liquid
These are always physical changes

15. Changes in Matter Condensation Freezing Melting Evaporating
Gas to liquid
Freezing
Liquid to solid
Melting
Solid to liquid
Evaporating
Liquid to gas
Sublimation
Solid to gas
Deposition
Gas to solid

16. Physical Changes
cutting
boiling
breaking
tearing

17. Chemical Changes Four good indications of a chemical change...
color change
gas released (often with an odor)
energy change (light, heat, …)
precipitate formed

18. Changes in Matter
A chemical property: The susceptibility of iron to rusting.
Is rusting a physical or chemical change?
When iron rusts, it turns from iron to iron oxide.

19. Practice Classify each property as physical or chemical.
the tendency of copper to turn green when exposed to air
the tendency of automobile paint to dull over time
the tendency of gasoline to evaporate quickly when spilled
the low mass (for a given volume) of aluminum relative to other metals

20. Changes in Matter
Matter undergoes a chemical change when it undergoes a chemical reaction.
In a chemical reaction, the substances present before the chemical change are called reactants. The substances present after the change are called products.

21. Changes in Matter
The difference between chemical and physical changes is seen at the molecular and atomic level.

22. Changes in Matter
In physical changes, the atoms that compose the matter do not change their fundamental associations, even though the matter may change its appearance.
A physical change results in a different form of the same substance.

23. Changes in Matter
In chemical changes, atoms do change their fundamental associations, resulting in matter with a new identity.
A chemical change results in a completely new substance.

24. Practice Classify each change as physical or chemical.
the rusting of iron
the evaporation of fingernail-polish remover (acetone) from the skin
the burning of coal
the fading of a carpet upon repeated exposure to sunlight

25. Practice In this figure liquid water is vaporizing into steam.
Which diagram best represents the molecules in the steam?

26. Separation of Mixtures
Compounds are pure substances
Compounds can only be separated by chemical reactions.
Mixtures can never consist of only a single substance
Mixtures can be separated by physical changes

27. Separation Techniques
Filtration
Separates liquid from a solid
The mixture is poured over a mesh-like filter paper and the liquid is allows to pass through, leaving behind the solid

28. Separation Techniques
Density
Liquids of different densities will separate into layers.
The lowest density liquid will rest on top.

29. Separation Techniques
Centrifuge
A centrifuge is a machine that separates solids from liquids by spinning very quickly.
This causes solids to fall to the bottom of the test tube, separating them from the liquids in the mixture.

30. Separation Techniques
Decant
Separates solid from liquid by pouring the liquid off the top and leaving the solid behind
It can be difficult to ensure that all of the liquid is removed by this technique

31. Separation Techniques
Magnetism
Can be used to remove magnetic solids from a mixture
Magnetic elements include iron, nickel, and cobalt

32. Separation Techniques
Distillation
To separate a mixture of liquids, the liquid can be heated to force components, which have different boiling points, into the gas phase. The gas is then condensed back into liquid form and collected. 
Can be used to separate several different substances

34. Separation Techniques
Chromatography
Techniques which use a stationary phase (e.g. paper) and a mobile phase (e.g. some sort of solvent like water or alcohol) to physically separate substances.

35. Separation Techniques
A sample of the mixture is placed on the paper (stationary phase). The solvent will then dissolve the components of the mixture.
The components of the mixture will move with the solvent (mobile phase) up the paper.
Based on the properties of each component (e.g., polarity) the components will travel at different speeds with the solvent.
Many complex variations, but basic principles stay the same

37. Law of Conservation of Mass
Law of Conservation of Mass: matter is neither created nor destroyed in a chemical reaction.
In a nuclear reaction, significant changes in mass can occur.
During physical and chemical changes, the total amount of matter remains constant.

38. Law of Conservation of Mass
Suppose that we burn 58 g of butane in a lighter. It will react with 208 g of oxygen to form 176 g of carbon dioxide and 90 g of water.

39. Practice
A chemist forms 16.6 g of potassium iodide by combining 3.9 g of potassium with 12.7 g of iodine. Show that these results are consistent with the law of conservation of mass.

40. Practice
Suppose 12 g of natural gas combines with 48 g of oxygen in a flame. The chemical change produces 33 g of carbon dioxide. How many grams of water form?

41. Classify each property as physical or chemical.
(a) the explosiveness of hydrogen gas
(b) the bronze color of copper
(c) the shiny appearance of silver
(d) the ability of dry ice to sublime (change from solid directly to vapor)

42. Classify each change as physical or chemical.
(a) copper metal forming a blue solution when it is dropped into colorless nitric acid
(b) a train flattening a penny placed on a railroad track
(c) ice melting into liquid water
(d) a match igniting a firework

43. Consider a drop of water that is put into a flask, sealed with a cap, and heated until the droplet vaporizes. Is the mass of the container and water different after heating?