1. Matter Unit Vocabulary

2. Matter
Kinetic Theory
Solid
Liquid
Gas
Plasma
Phase change
Freezing
Melting
Deposition
Sublimation
Condenstation
Vaporization
Physical properties
Ducility
Malleability
Melting point
Boiling point
Freezing point
Solubility
Reaction to light
Electrical conductivity
Chemical properties
Flammability
Oxidation
decomposition
Physical change
Chemical change
Demoritus
John Dalton
JJ Thomson
Ernest Rutherford
Niels Bohr
Atomos
Bohr Model
Cloud Model
Valence Electrons
Energy Levels
Shells
Properties of Water
Universal solvent
Adhesion
Cohesion
High specific heat
Capillary action
Surface tension
Polarity
States of matter
Heat of vaporization pH

3. Matter Anything that has mass and occupies space
The materials or “stuff” that all objects and substances in the universe are made of
4 States of Matter = Solid, liquid, gas, and plasma

4. Matter
Because all matter takes up space (has volume) and contains a certain amount of material (has mass), all matter can be detected and measured

5. Examples of Matter
Rocks, water, trees, bicycles, lighting, animals, stars, smoke, are all easily seen and observed
Dust mites that live in your furniture and rugs you may need a microscope to view
Air maybe invisible but we can feel it when the wind blows and see it bend the branches of trees (oxygen, nitrogen, hydrogen, CO2)

6. What is not matter?
Light
Sound
Gravity
Friction

7. Matter Atoms are the building blocks of matter
The elements in our periodic table make up all matter

8. Kinetic Theory
All matter consists of tiny particles that are in constant motion.

9. Kinetic Theory
1. All matter is composed of small particles (atoms, molecules, or ions). There is an attractive force between them.
2. They are in constant, random motion. The particles may collide with one another or the sides of their container.
3. As the temperature increases the speed of the particles increases. As the temperature decreases the speed of the particles decreases.

10. SOLIDS
State of matter that has a definite shape and a definite volume.
Particles of solids are tightly packed, vibrating about a fixed position.
Particles are strongly attracted to each other

11. LIQUID
A state of matter that has a definite volume but takes the shape of its container
Liquids do not have a definite shape
Particles of liquids are tightly packed, but are far enough apart to slide over one another, allowing it to flow

12. GAS
A state of matter that has no definite shape and no definite volume; expands to fill the shape of its container
Particles of gases are very far apart and move freely.
Attractive forces are very weak
• Contain mostly empty space – because the particles are so far apart
• Particles spread throughout a given volume until distributed equally – diffusion

13. Gas vs. Vapor
Gas – a substance that is naturally in the gaseous state at room temperature
EXAMPLE: Helium
Vapor – the gaseous state of a substance that is a solid or liquid at room temperature
EXAMPLE: Steam

14. PLASMA Plasma is the most common state of matter in the universe
A state of matter that does not have a definite shape or volume and whose particles have broken apart
Consists of + and – charged particles (electrons are knocked off due to collisions)
A plasma is a very good conductor of electricity and is affected by magnetic fields.
Plasma is the most common state of matter in the universe

16. STATES OF MATTER SOLID LIQUID GAS PLASMA
Tightly packed, in a regular pattern
Vibrate, but do not move from place to place, definite shape and volume
Close together with no regular arrangement.
Move about, flow and slide past each other. Definite volume, no definite shape takes shape of its container.
Well separated with no regular arrangement.
Move freely at high speeds. No definite shape or volume. Easily compressible.
Has no definite volume or shape and is composed of electrical charged particles
PLC-Unit 1B

17. 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

18. A transition of matter from one state to another.
Phase Change
A transition of matter from one state to another.

20. Some phase changes are more common and easier for us to visualize
Some phase changes are more common and easier for us to visualize. For example, you have probably witnessed freezing, melting, and vaporization just by making ice, melting ice, and boiling water.

21. Condensation often occurs on the outside of cold beverage containers
Condensation often occurs on the outside of cold beverage containers. This is when the humid air changes directly to a liquid on the surface of the container.

22. Sublimation Dry ice is actually solid carbon dioxide
Sublimation Dry ice is actually solid carbon dioxide. When it sits in the open or is placed in water it rapidly changes directly from solid to gas creating a foggy cloud.

23. Deposition Frozen patterns of ice on your car windshield is an example
Deposition Frozen patterns of ice on your car windshield is an example. Deposition involves a gas changing to a solid. This occurs during winter months when the humid air directly freezes into solid ice.

24. Physical properties
Characteristics that can be observed without changing the makeup or identity of the matter
Examples: color, size, state of matter, density, ductility, malleability, boiling point, melting point, freezing point, electrical conductivity, solubility, reaction to light

25. Density The ratio of the mass of an object to its volume
Formula: d = m/V
Units: g/mL or g/cm3

26. Ductility
The ability to be pulled into a thin strand
EX: wire

27. Malleability The ability to be pressed or pounded into a thin sheet
EX: aluminum foil, sheet metal

28. Boiling Point
The temp at which a substance changes from a liquid to a gas
EX: the boiling point of water = 1000C

29. Melting Point
The temp at which a substance changes from a solid to a liquid
EX: the melting point of chocolate is 340C

30. Freezing Point
The temp at which a substance changes from a liquid to a solid
EX: the freezing point of water = 00C

31. Electrical Conductivity
How well a substance allows electricity to flow through it
EX: copper wires,
electrical lines

32. Solubility The ability to dissolve in another substance
EX: sugar in water

33. Reaction to Light Reflection – to bounce off ( mirror)
Refraction – to bend (water)
Absorption – to take in (leaf)

34. Reaction to Light Transmission – allow to pass through
Opaque – little to no light passes through (blanket)
Translucent – some light passes through (sunglasses)
Transparent- most light passes through ( glass window)

35. Chemical properties
The ability of matter to undergo a specific chemical change, creating a different type of matter with new properties
Examples: flammability, decomposition, oxidation

36. Flammibility To burn Must occur in the presence of oxygen
EX: Flame tests help to identify metals by their characteristic flame color

37. Decomposition To rot or breakdown
Complex compounds breakdown to simpler substances
EX: CO2 breaks down to Carbon and Oxygen

38. Oxidation The process of losing electrons
EX: iron rusts when exposed to oxygen

39. Physical Changes
A process where a substance’s chemical properties have not changed
Can be a change in size, color, shape, state of matter
EX: ice melting, salt dissolving in water, glass breaking

40. Chemical Change
Occurs when new substances or materials are produced to have different chemical properties from the reactants
EX: rust is the product
of iron and oxygen,
wood burning

41. Democritus Greek philosopher in 440 bc
Was the first to proposed the existence of atoms
“Atomos” meaning “not to be cut”

42. John Dalton British chemist 1803
Atomic Theory – He came up with the theory that all substances were made of atoms
Atoms were small, hard, dense spheres that could not be created, destroyed, or altered

43. Dmitri Mendeleev Known as the father of the present day periodic table
Organized the elements (each type of atom) by similar properties in 1869

44. J. J. Thomson British scientist 1898
Proposed that atoms themselves were made of smaller particles .
He discovered that atoms contained negatively charged particles, but did not know their location

45. J. J. Thomson
Theorized the negatively charged particles were spread evenly throughout the positively charged material
Thomson’s model of the atom was called the “plum-pudding” model

46. Ernest Rutherford 1911 a former student of Thomson's
Proposed that atoms had a dense, positively charged nucleus surrounded by electrons

47. Niels Bohr 1913 Danish scientist
Said that electrons revolve around the nucleus in circular paths, called orbits
And that electrons could only exist in certain orbits and at certain energy levels

48. Today’s model electron cloud model
Bohr’s model was an important stepping stone to today’s, which was developed in the 1920’s
Electrons surround the nucleus, traveling not in prescribed paths but in regions of various thicknesses called clouds

49. Bohr Model Electrons orbit the nucleus of an atom in set energy levels
P = 20
N = 20

50. Energy Level The specific energies an electron in an atom can have
In the Bohr model used to describe the different orbits or shells that the electrons travel in around the nucleus

51. Valence Electrons
The electrons in the highest or outermost energy level

52. Polarity
When electrons are not shared equally in a covalent bond, causing one end of the water molecule to have a positive charge while the other has a negative charge

53. Each end of a water molecule is attracted to the opposite charged end of another water molecule. Water's polarity is responsible for the "stickiness" or cohesion between the molecules.

54. States of Matter
The only known substance to naturally exist on Earth in all three states of matter is water
Solid - Ice
Gas - Clouds
Liquid - Lakes

55. pH
The measure of how acidic or basic water is
Rainwater

56. Universal Solvent
More substances dissolve in water than in any other liquid

57. Cohesion
Water molecules are attracted to more water molecules so they stick to each other
Water ↔ Water

58. Adhesion
Water molecules are attracted to and stick to other substance
Water ↔ Other

59. Surface Tension
Water molecules have a stronger attraction to each other than to the air above, so the water molecules cling tightly to each other forming what’s like a skin at the surface

60. Capillary Action
Movement of water within the spaces of a porous material due to the forces of adhesion, cohesion and surface tension

61. High Specific Heat
The amount of energy required to raise the temperature of water by one degree Celsius is quite large, causing the temperature of water to change slowly

62. Heat of Vaporization
Water absorbs heat as it changes from a liquid to a gas