1. STATES OF MATTER
Four States
Solid
Liquid
Gas
Plasma

2. STATES OF MATTER Based upon particle arrangement
Based upon energy of particles
Based upon distance between particles

3. Kinetic Theory of Matter
Matter is made up of particles which are in continual random motion.

4. KINETIC THEORY
Kinetic Theory states that the tiny particles in all forms of matter are in constant motion.
Kinetic refers to motion
Helps you understand the behavior of solid, liquid, and gas atoms/molecules as well as the physical properties
Provides a model behavior based off three principals

5. KINETIC THEORY 3 Principles of Kinetic Theory
All matter is made of tiny particles
These particles are in constant motion
When particles collide with each other or the container, the collisions are perfectly elastic (no energy is lost)

6. STATES OF MATTER
4 States of Matter
Solid
Liquid
Gas
Plasma

7. STATES OF MATTER SOLIDS
Particles of solids are tightly packed, vibrating about a fixed position.
Solids have a definite shape and a definite volume.
Heat

8. SOLIDS Particles are tightly packed and close together
Particles do move but not very much
Definite shape and definite volume (because particles are packed closely and do not move)
Most solids are crystals
Crystals are made of unit cells (repeating patterns)
The shape of a crystal reflects the arrangement of the particles within the solid

9. SOLIDS
Unit cells put together make a crystal lattice (skeleton for the crystal)
Unit cell  crystal lattice  solid

10. SOLIDS Amorphous Solid: A solid with no defined shape (not a crystal)
A solid that lacks an ordered internal structure
Examples: Clay, PlayDoh, Rubber, Glass, Plastic, Asphalt

11. SOLIDS
Allotropes:
Solids (elements or compounds) that appear in more than one form
2 or more different molecular forms of the same element in the same physical state (have different properties)
Example: Carbon
Powder = Graphite
Pencil “lead” = graphite
Hard solid = diamond

12. SOLIDS

13. SOLIDS Allotropes of Carbon: diamond b) graphite c) lonsdaleite
d) buckminsterfullerene (buckyball)
e) C540
f) C70
g) amorphous carbon
h) single-walled (buckytube)

14. STATES OF MATTER LIQUID
Particles of liquids are tightly packed, but are far enough apart to slide over one another.
Liquids have an indefinite shape and a definite volume.
Heat

15. LIQUIDS Particles are spread apart
Particles move slowly through a container
No definite shape but do have a definite volume
Flow from one container to another
Viscosity – resistance of a liquid to flowing
Honey – high viscosity
Water – low viscosity

16. STATES OF MATTER GAS
Particles of gases are very far apart and move freely.
Gases have an indefinite shape and an indefinite volume.
Heat

17. GASES Particles are very far apart Particles move very fast
No definite shape and No definite volume

18. Description of Phase Change
PHASE CHANGES
Description of Phase Change
Term for Phase Change
Heat Movement During
Phase Change
Solid to liquid
Melting
Heat goes into the solid as it melts.
Liquid to solid
Freezing
Heat leaves the liquid as it freezes.
A Phase is another way of saying a State (of Matter)

19. Description of Phase Change
PHASE CHANGES
Description of Phase Change
Term for Phase Change
Heat Movement During
Phase Change
Liquid to gas
Vaporization, which includes boiling and evaporation
Heat goes into the liquid as it vaporizes.
Gas to liquid
Condensation
Heat leaves the gas as it condenses.
Solid to gas
Sublimation
Heat goes into the solid as it sublimates.

20. Will everything just be a gas?
But what happens if you raise the temperature to super-high levels… between 1000°C and 1,000,000,000°C ?
Will everything just be a gas?

21. STATES OF MATTER PLASMA
A plasma is an ionized gas.
A plasma is a very good conductor of electricity and is affected by magnetic fields.
Plasmas, like gases have an indefinite shape and an indefinite volume.
Plasma is the
common state
of matter
Ions = charged particles

22. STATES OF MATTER LIQUID PLASMA SOLID GAS
Tightly packed, in a regular pattern
Vibrate, but do not move from place to place
Close together with no regular arrangement.
Vibrate, move about, and slide past each other
Well separated with no regular arrangement.
Vibrate and move freely at high speeds
Has no definite volume or shape and is composed of electrical charged particles

23. PLASMA Particles are extremely far apart Particles move extremely fast
Only exists above 3000 degrees Celsius
Basically, plasma is a hot gas
When particles collide, they break apart into protons, neutrons, and electrons
Occurs naturally on the sun and stars

24. Some places where plasmas are found…
Flames

25. Lightning

26. Aurora (Northern Lights)

27. The Sun is an example of a star in its plasma state

30. A graph showing the heating curve for a substance.

31. A phase diagram showing the relationships of the states for a substance at different temperatures and pressures.

32. Any characteristic of a material that can be observed or measured without changing the identity of the material is a physical property.
In a physical change, the physical properties of a substance change, but the identity of the substance does not change.
A chemical property is any characteristic that gives a substance the ability to undergo a change that results in a new substance.
A chemical change is a change in the identity of a substance due to the chemical properties of that substance.

33. Pure Substances
Pure substances contain only one sort of particle. Many substances that in everyday language we call pure are really mixtures.
A pure substance can only be an element or a compound.
For example, a bottle of pure mineral water has, according to the label, the following contents :
Calcium
Magnesium
Sodium
Potassium
Bicarbonate
Chloride
Sulphate
Fluoride!
If it was really pure water, in the scientific meaning of the word, it would contain only water particles, H20.

34. Elements, Molecules and Compounds
Some elements, such as the noble gases, exist as individual atoms.
Often, elements consist of two or more atoms joined together. We call these molecules.
If more than one type of atom is in a molecule, we call it a compound.

35. By asking these questions scientists can classify matter into:
Mixtures – two or more substances that are not chemically combined with each other and can be separated by physical means. The substances in a mixture retain their individual properties.
Solutions – a special kind of mixture where one substance dissolves in another.
Elements – simplest form of pure substance. They cannot be broken into anything else by physical or chemical means.
Compounds – pure substances that are the unions of two or more elements. They can be broken into simpler substances by chemical means.

37. Is it uniform throughout?
If the answer is no, the matter is a heterogeneous mixture.
Considered the “least mixed.”
Does not appear to be the same throughout.
Particles are large enough to be seen and to be separated from the mixture.

38. Examples of heterogeneous mixtures
Sand and pebbles
Oil and water
Powdered iron and powdered sulfur

39. Granite is a heterogeneous mixture.

40. Heterogeneous mixture Homogeneous mixture
Matter
Can it be separated by physical means
yes no
Mixture
Pure substance
Is it uniform throughout
Can it be decomposed into other substances by chemical processes
yes no no
yes
Heterogeneous mixture
Homogeneous mixture
Element
Compound
Dissolved down to atomic or molecular level no
yes
Colloid
Solution
contains
Solute
Solvent

41. Is it uniform throughout?
If the answer is yes, the matter is a homogeneous mixture (looks the same throughout).
A mixture that appears to be the same throughout.
It is “well mixed.”
The particles that make up the mixture are very small and not easily recognizable.

42. Colloids Particles are mixed together but not dissolved.
The particles are relatively large and are kept permanently suspended.
However, the particles are larger than individual atoms or molecules.

43. Colloids A colloid will not separate upon standing.
The particles are constantly colliding, and this allows a colloid to scatter light – thus colloids often seem cloudy.

44. Solutions
If the particles in a homogeneous mixture are at an atomic or molecular level (breaks down to individual atoms or molecules) – it is a solution.
A solution is a type of homogeneous mixture formed when one substance dissolves in another.
It is the best mixed of all mixtures.
A solution always has a substance that is dissolved and a substance that does the dissolving.
The substance that is dissolved is the solute and the substance that does the dissolving is the solvent.

45. Ocean water is a solution

46. The universal solvent: Water

47. Water as a solvent Many liquid solutions contain water as the solvent.
Ocean water is basically a water solution that contains many salts.
Body fluids are also water solutions.

48. Metals dissolved in metals are called alloys.
Types of solutions
Solute
Solvent
Example
Gas
Air (oxygen in nitrogen)
Liquid
Soda water (carbon dioxide in water)
Solid
Ocean water (salt in water)
Solid
Gold jewelry (copper in gold)
Metals dissolved in metals are called alloys.

49. Air is a solution of oxygen and other gases dissolved in nitrogen

50. Alloys Stainless steel is a mixture of iron and chromium.
Brass is an alloy of copper
and zinc.

52. Can it be separated by physical means?
If the answer is no, the matter is a pure substance.
An element
Or a compound

53. Elements Elements are the simplest pure substance.
An element can not be changed into a simpler substance by heating or any chemical process.
The smallest particle of an element that has the properties of that element is called an atom.
An atom is the basic building block of matter.
There are more than one hundred known elements in the universe listed on the periodic table of elements.
These elements combine in such a way to create millions of compounds.

54. Elements All elements are made of atoms.
Atoms of the same element are alike.
Atoms of different elements are different.

55. Elements
In 1813, a system of representing elements with symbols was introduced.
Each symbol consists of one or two letters.
Two letters are needed for a chemical symbol when the first letter of that element’s name has already been used.

56. Common Elements Aluminum Al Bromine Br Calcium Ca Carbon C Gold Au
Helium He
Hydrogen H
Nitrogen N

57. Compounds Compounds are also pure substances.
But compounds are made from more than one element.
Water is a compound.
Water can be broken down into simpler substances – hydrogen and oxygen.

59. For example, hydrogen can react with oxygen :
Chemical Reactions
Chemical reactions, or chemical changes, happen when the atoms in one or more chemicals split up and join together in new ways.
For example, hydrogen can react with oxygen :
hydrogen + oxygen →
water

60. hydrogen + oxygen → water Chemical Reactions
Before the reaction the oxygen atoms go round in pairs, and the hydrogen atoms go round in pairs. When they react we get two new molecules, of the compound water.
Each of these molecules has three atoms, two hydrogen atoms joined to one oxygen atom.
We can write this as H2O.
hydrogen + oxygen →
water

61. thermal decomposition
Types of Reaction
There are several different groups that we can put reactions into. These include :
combustion
displacement
neutralization
oxidation
precipitation
thermal decomposition
The reaction of sugar with concentrated sulphuric acid.

62. This is the Law of Conservation of Matter
Types of Reaction
When a reaction takes place, things happen. There may be a gas given off, a colour change or a solid material appearing. There could also be changes we can’t see, such as a temperature change.
One important thing to remember about chemical reactions is that the mass of the reactants (the chemicals we start with) is always the same as the mass of the products (the chemicals we end with).
This is the Law of Conservation of Matter

63. Most fuels burn in air to form water and carbon dioxide :
Combustion
This is the name we give to reactions when things burn in air. Combustion is a special sort of oxidation reaction. It happens quickly and a flame is produced which heats the surroundings.
As we have already seen, hydrogen will react with oxygen – it burns to form water.
Most fuels burn in air to form water and carbon dioxide :
methane + oxygen
carbon dioxide + water

64. For example iron will go rusty :
Oxidation
In oxidation reactions, oxygen combines with a substance to make an oxide.
For example iron will go rusty :
iron + oxygen
iron oxide
Adding pure oxygen makes reactions go faster than they would in air. Here is a picture of a biscuit burning!

65. For example, copper carbonate will decompose when heated :
Thermal Decomposition
In this type of reaction, a substance breaks down into simpler parts when it is heated.
For example, copper carbonate will decompose when heated :
heat
copper carbonate
copper oxide + carbon dioxide
If we measure the mass of copper carbonate before the reaction, and then the mass of copper oxide left after the reaction, the mass of the copper oxide will be lower.
The mass has not disappeared. The missing mass is that of the carbon dioxide gas which has escaped into the air.

66. In a displacement reaction, one metal ‘kicks out’ a less reactive one.
For example, when iron filings are added to copper sulphate solution, copper metal starts to appear.
iron + copper sulphate
copper + iron sulphate

67. Displacement
The iron wants to be with the sulphate more than the copper does. We say that iron is more reactive than copper.
When the iron atoms are mixed with the copper sulphate atoms, the iron atoms ‘kick out’ the copper atoms and join on to the sulphate ions (particles).
We see the red / brown copper metal start to appear in place of the grey iron, and the solution changes colour from blue to green, as copper sulphate is blue but iron sulphate is green.
iron + copper sulphate
copper + iron sulphate

68. Displacement
If an insoluble product is formed in a reaction, it suddenly appears. We say it precipitates, and the solid is called the precipitate.
This reaction happens if we blow into lime water (calcium oxide solution). The carbon dioxide from our breath joins up with the calcium oxide to form calcium carbonate, which is a white, insoluble material.

69. neutralization
Neutralization (or acid/base) occurs when an acid combines with a base to produce a salt and water
HCl (aq) + NaOH (aq) → NaCl + H2O

70. Precipitation
If an insoluble product (a solid in the liquid solution) is formed in a reaction, it suddenly appears. We say it precipitates, and the solid is called the precipitate.
This reaction happens if we blow into lime water (calcium oxide solution). The carbon dioxide from our breath joins up with the calcium oxide to form calcium carbonate, which is a white, insoluble material.
calcium oxide + carbon dioxide
calcium carbonate