1. Chapter 1
Matter and Change

2. What is Matter? Matter is anything that takes up space and has mass.
Mass is the amount of matter in an object.
Mass is resistance to change in motion along a smooth and level surface.
Examples

3. Types of Matter Pure Substance- a particular kind of matter - pure
Mixture- more than one kind of matter, not chemically combined

5. What are Pure Substances?
Substances which have a single composition throughout. These can be elements or compounds
The simplest forms of matter are the elements. There are nearly 120 different elements currently known on the earth.
The smallest particles of an element are atoms.
Atoms of an element are unique. For example lead atoms are completely different from gold atoms.

6. Substances Elements- simplest kind of matter
Cannot be broken down into simpler
All one kind of atom.
Compounds are substances that can be broken down by chemical methods
When they are broken down, the pieces have completely different properties than the compound. Salt
Made of molecules- two or more atoms stuck together

7. A molecule is the smallest particle of a compound that acts as a unit
A molecule is the smallest particle of a compound that acts as a unit. Water molecule. Molecules are made of a fixed ratio of atoms.

8. What is a chemical formula?
A chemical formula tells the kind and number of atoms in a molecule.
The formula uses the symbols of the element to identify the elements present and subscripts (lowered numbers beside the symbol) to indicate how many atoms are present.

9. Compound or Mixture Compound Mixture One kind of piece- Molecules
More than one kind -
Molecule or atoms
chemical change
Required to make
physical change
Can still separate parts
New substance
With different properties
Than the original parts
Variable composition
Parts Keep their
properties

10. Which is it?
Compound
Mixture
Element

11. Properties Words that describe matter (adjectives)
Physical Properties- a property that can be observed and measured without changing the substance.
Chemical Properties- a property that can only be observed by changing the type of substance.
Both physical and chemical properties can be used to help identify a substance

12. Physical Properties
Color
Melting
Boiling

13. Chemical Properties
Flammability
Radioactivity
Reactivity

14. Properties Words that describe matter (adjectives)
Extensive Properties- only depends on the amount of matter
Intensive Properties- only depends on the type of matter, not the amount
Both intensive and extensive properties can be used to help identify a substance

15. Extensive Properties
Volume
Mass

16. Intensive Properties
Density
Luster
Color

18. Physical Changes
A change that changes appearances, without changing the composition.
Examples?
Chemical changes - a change where a new form of matter is formed.
Also called chemical reaction.
Not phase changes
Ice is still water.

19. Chemical Reactions Another name for chemical change
When one or more substances are changed into new substances.
Reactants- stuff you start with
Products- What you make
NEW PROPERTIES
Because each substance has its own properties

20. Indications of a chemical reaction
Energy absorbed or released
Color change
Odor change
Precipitate- solid that separates from solution
Not easily reversed
Only clues not certainty

21. Chemical symbols There are 116 elements
Each has a 1 or two letter symbol
First letter always capitalized second never
Some from Latin or other languages

22. Chemical symbols Used to write chemical formulas
Subscripts tell us how many of each atom
H2O
C3H8
HBrO3

23. Conservation of Mass
Mass can not be created or destroyed in ordinary (not nuclear) changes.
All the mass can be accounted for.
Mass at the start = mass at end

24. The Law of Conservation of Mass
Matter cannot be created nor destroyed.

25. Mixtures Made up of two substances. Variable composition.
Heterogeneous- mixture is not the same from place to place.
Chocolate chip cookie, gravel, soil.
Homogeneous- same composition throughout.
Kool-aid, air.
Every part keeps its properties.

27. What are homogeneous mixtures?
Solutions are homogeneous mixtures. Solution particles are very small and compose molecules, atoms, or ions.
Colloids are homogeneous mixtures. Colloid particles are larger than solution particles but do not settle as suspension do.
Examples of colloids are fog, mayonnaise, jello, whipped cream.
What is the Tyndall Effect and Brownian motion?

28. What are heterogeneous mixtures?
Heterogeneous mixtures (suspensions) are made of larger particles than that of homogeneous mixtures. These particles remain suspended temporarily and will eventually settle or separate.
Examples are chocolate milk, orange juice, muddy water.

29. What are liquid mixtures?
Liquids which evenly mix are said to be miscible. Gasoline, antifreeze and water.
Liquids which do not mix are said to be immiscible. Oil and water; oil and vinegar.
Can gases mix with liquids?
How do fish breathe?
What are carbonated soft drinks?

30. Phases
A part of a sample with uniform composition, therefore uniform properties
Homogeneous- 1 phase
Heterogeneous – more than 1

31. Separating mixtures Only a physical change- no new matter
Filtration- separate solids from liquids with a barrier
Distillation- separate because of different boiling points
Heat mixture
Catch vapor in cooled area
Chromatography- different substances are attracted to paper or gel, so move at different speeds

32. Chromatography

33. How can physical changes be used to separate mixtures?
Impurities mixed with water can be separated by distillation.
What is distillation?
Distillation is a process of separating parts of a mixture by differences in boiling points.

34. Solutions Homogeneous mixture Mixed molecule by molecule
Can occur between any state of matter.
Solid in liquid- Kool-aid
Liquid in liquid- antifreeze
Gas in gas- air
Solid in solid - brass
Liquid in gas- water vapor

35. Solutions
Like all mixtures, they keep the properties of the components.
Can be separated by physical means
Not easily separated- can be separated without creating anything new.

36. States of matter
Solid- matter that can not flow and has definite volume.
Liquid- definite volume but takes the shape of its container (flows).
Gas- a substance without definite volume or shape and can fl

37. States of Matter Definite Volume? Definite Shape? Temp. increase
Com-pressible?
Small Expans.
Solid
YES
YES NO
Small Expans.
Liquid NO NO
YES
Large Expans.
Gas NO NO
YES

38. States of Matter
Moderate Kinetic Energy - molecules move around more than in solids
Low Kinetic Energy - molecules barely move
High Kinetic Energy – molecules in rapid, constant motion

39. Condense
Freeze
Melt
Evaporate
Solid
Liquid
Gas

40. States of Matter There are more Plasma More at very low temp
high temperature low pressure
electrons separate from nucleus
Most common in the universe
More at very low temp
Bose- Einstein condensate
Quantum superfluids

41. Another Way to Change States
Pressure
For some substances it will turn solids to liquids
For others it will turn liquids to solids
Silly putty
Will turn gas to liquid-
Compressor in refrigerator and AC

42. Energy The ability to do work.
Work - cause a change or move an object.
Many types- all can be changed into the other.

43. Types of energy Potential- stored energy
Kinetic Energy- energy something has because its moving
Heat- the energy that moves because of a temperature difference.
Chemical energy- energy released or absorbed in a chemical change.
Electrical energy - energy of moving charges

44. Types of Energy
Radiant Energy- energy that can travel through empty space (light, UV, infrared, radio)
Nuclear Energy – Energy from changing the nucleus of atoms
All types of energy can be converted into others.
If you trace the source far enough back, you will end up at nuclear energy.

45. Conservation of Energy
Energy can be neither created or destroyed in ordinary changes (not nuclear), it can only change form.
Its not just a good idea, its the law.

46. What about nuclear? E = mc2 energy = mass x (speed of light)2
speed of light = 3 x 108
A little mass can make a lot of energy
Law of Conservation of Mass - Energy the total of the mass and energy remains the same in any change