1. Chemistry Lesson 3 - Matter and Energy Mrs. Eline
Bordentown Regional High School

2. Section 3.1 Properties of matter

3. Matter-anything that has mass and takes up space.
3.1States of matter
Definitions
Matter-anything that has mass and takes up space.
Substance – matter with a uniform and unchanging composition.
SOLID-a form of matter that has its own definite shape and volume. Particles of matter tightly packed.
LIQUID-a form of matter that flows, has constant volume and takes up the shape of its container. Particles of matter are able to move past one another.
GAS-a form of matter that not only flows to conform to the shape of its container but also fills the entire volume of its container.

24. States of matter: SOLID

25. States of matter :LIQUID

26. States of matter: GAS

28. The Amazing H2O- the substance that the Celsius Scale was built upon!
Freezes at 0C
Boils at 100 C
0C
100C

29. Physical Properties-a characteristic of matter that can be observed or measured without changing the sample’s composition.
Density, color, odor, hardness, melting point and boiling point.
Extensive property-dependent upon amount of substance ex: Mass
Intensive property-independent of amount of substance ex:Density.

30. Chemical Properties-the ability or inability of a substance to combine with another.
Ex. Iron combines with O2 to make rust. Iron combined with N2 no reaction.
O > +

31. Properties of Copper Physical Properties Chemical Properties
Reddish brown, shiny
Forms green copper carbonate compound when in contact with moist air
Easily shaped into sheets(malleable) and drawn into wire(ductile)
Reacts with Nitric Acid and sulfuric Acid
Good conductor of heat and electricity.
Forms a deep-blue solution when in contact with ammonia.
Density = 8.96 g/cm3, Melting point =1085C boiling point 2562C

32. Properties and States of Matter are dependent on the conditions.
It is important to state the specific conditions-temperature, pressure as the physical and chemical properties depend on those conditions.
Liquid water has a density of 1.00 g/cm 3
As a gas H2O has a density of g/cm 3

33. Section 3.2 Changes in Matter

34. Changes in Matter
Chemical Change

35. Changes in Matter
Physical Change

36. massreactants = massproducts
Our First LAW of Chemistry :CONSERVATION of Mass
massreactants = massproducts

37. Section 3.3 Mixtures of Matter

38. Mixtures of Matter
Heterogeneous- a mixture that does not blend smoothly. Ex. Salad dressing
Homogeneous- a mixture that does blend smoothly. Ex. Lemonade mix. Also referred to as a solution.

39. Types of Solution Systems
Example
Gas-Gas
Air in a scuba tank. O2 N2 & Ar gas
Gas-liquid
O2 and CO2 in seawater.
Liquid-gas
Moist air exhaled by Scuba Diver
Liquid-liquid
When it is raining, freshwater mixes with salt water
Solid-liquid
Solid salts dissolved in Sea water
Solid-solid
The air tank is made of alloy-a mixture of 2 metals.

40. Separating Mixtures of Matter
Based on the physical properties of the component substances in a mixture they can be separated.
Inquiry 1 - If we had a mixture of sand, iron filings and small pebbles what could we use to separate the 3 substances?
Inquiry 2 – how could we get the salt out of a salt water solution?

41. Methods for Separating Mixtures of Matter
Filtration- a porous barrier can separate a solid from a liquid, solids of different particle sizes.
2. Distillation-based on the different boiling points of the substances involved.
3. Crystallization-when the solution contains as much of the dissolved substance it can hold, the addition of a tiny amount more causes the dissolved substance to come out in a crystalized form.
4. Sublimation-the process by which a substance goes from the solid phase to the gaseous phase without melting.
5. Chromatography-separates the components of a mixture dissolved in either a gas or a liquid (called the mobile phase) based on the ability of the component to travel across the stationary phase.

42. Filtration

43. Distillation

44. Crystallization
How to make Rock Candy!!

45. Sublimation
Dry Ice CO2 (solid)->CO2(gas)

46. Chromatography
Sample of 2 substances loaded on to the top of the column of porous particles such as ion-exchange resin. step a
Solvent runs through the system and different substances travel through the column at different rates. steps b-d
The scientist collects the different fractions of the 2 substances. step e and f

47. Section 3.4 Classes of Matter