1. Characteristics of Matter

2. Matter Matter is anything that has mass and takes up space.
Mass – the amount of matter in something
Volume – the amount of space something occupies
Every element/compound is unique in some way from all others.
If you know enough about a substance, you can figure out what it is (meaning you can identify it).
If you know what a substance is, you can know all types of things about it.

4. Try it out

5. Elements and Compounds are Pure Substances
Figure 1.10 – Page 36

6. Matter
All matter has 2 types of properties: Physical properties and chemical properties.
Property: a characteristic of a substance that can be observed

7. Physical properties
A physical property is a characteristic of a substance that can be observed without changing the substance into another substance.
(You can see it without changing what you’re looking at into something else.)

8. Physical Properties Physical properties can be extensive or intensive:
Extensive properties depend on the amount of a substance that you have.
Intensive properties don’t depend on how much you have (they are independent of the quantity).

9. Physical Properties - Examples
Examples of extensive physical properties include:
Volume
Mass
Weight
Size

10. Physical Properties - Examples
Examples of intensive physical properties include:
Density— is the amount of mass per unit of volume. The density of water is 1.0g/mL
Melting point—the temperature at which a substance changes from a solid to a liquid at a given pressure
water = 0oC
Boiling point—the temperature at which a substance changes from a liquid to a gas at a given pressure
water = 100oC

11. Physical Properties - Examples
Other physical properties include:
Color
Odor
Taste
Texture
Luster (shine)
Flexibility
Heat conductivity
Electrical conductivity
State of matter (liquid, gas or solid)
Solubility (ability to dissolve in water)
Hardness (how easily it can be scratched)
Shape
Viscosity (how easily it flows)
Ductility (that it can be pulled into a wire)
Malleability (it can be hammered into a sheet)
Magnetism

12. Physical properties
List as many physical properties as you can for this item

13. Chemical properties
A Chemical property is a characteristic of a substance that can only be observed by changing it into a different substance.

14. Chemical properties - Examples
Examples of chemical properties include:
The ability to burn
Ability to tarnish
Ability to rust
Ability to decompose
Ability to react with other chemicals
Instability
Ability to do acid/base reactions

15. Chemical properties
List as many chemical properties as you can for this item.

16. Chemical and physical properties – So what?
Titanium is very strong and doesn’t rust, so it is often used in jet engines.
Titanium is also nonallergenic. This, combined with the fact that it is rust proof makes it great for artificial joints as well as piercings.

17. Chemical and physical properties – So what?
Tungsten is usually used as the filament in lightbulbs because it has the highest melting point of any metal.
It glows red hot when electricity runs through it, and it gives off both heat and light.

18. Chemical and physical properties – So what?
Vanadium is heavier and harder than titanium, so mixing a tiny bit of vanadium with steel can make cheap tools that are still very strong.

19. Chemical and physical properties – So what?
Helium is almost completely nonreactive (inert).
It is lighter than air, so it’s great for floating balloons (or making funny voices.)
When electricity runs through helium, it glows a creamy pale peach color.

20. Chemical and physical properties – So what?
In 1943, all US pennies were made of zinc plated steel because copper was being used in the war. The pennies had to be coated with zinc because steel will rust, but zinc won’t.

21. Chemical and physical properties – So what?
Sulfur smells awful. Rotten eggs, onions, and garlic all have sulfur in them. Stink bombs use sulfur to create a bad smell.
Sulfur is also flammable, and it is one of the 3 main ingredients in gun powder.

22. Chemical and physical properties – So what?
Chromium is famous for its intense luster. Chrome plated tools, jewlery, silverware, or car parts are very popular.

23. Chemical and physical properties – So what?
Most bullets are made of lead because lead is a very dense metal. These bullets are required, by international law, to be coated with a different metal because lead has such a low melting point and is so malleable.

24. Chemical and physical properties – So what?
The most dense elements are Iridium and osmium which have a density of about 22.6 g/cm3

25. Element abundance
The most common element in the universe is Hydrogen (about 75%), and Helium (about 25%).
The most common element on Earth is Oxygen (46.6%), and Silicon (27.7%).
The most common element in your body is Oxygen (65%), and Carbon (18%)

26. Separating Mixtures Separating Heterogenous Mixtures
Filtration — Solid particles can be removed from liquids this way.

27. Density – Density is the ratio of mass to volume of a substance
Density – Density is the ratio of mass to volume of a substance. If two substances have different densities, the less dense material will be on the top, and the more dense will be on the bottom.
Magnets - if one component of a mixture is a magnetic solid such as iron.

28. Separating Homogenous Mixtures/Solutions
Recrystallization — Evaporate or boil off the liquid to leave the solid. (example: evaporating water from salt water to recover the salt).
Chromatography —Allowing a solution to flow through a stationary substance. Different components will have a different attraction for the stationary phase and the mobile phase (usually water).
Example – Ink on paper

29. Distillation
– used to separate a mixture of two liquids with different boiling points. The one with the lower boiling point boils off first leaving the liquid with the higher boiling point behind.

30. Chemical and physical changes

31. Physical Change
A Physical change is a change in a substance that does not change what the substance is.

32. Physical Change - examples
Examples of physical change include:
Change in shape
Change in size
Change in phase
Melting (solid to liquid)
Boiling (liquid to gas)
Evaporation (liquid to gas)
Condensation (gas to liquid)
Freezing (liquid to solid)
Sublimation (solid to gas)
Deposition (gas to solid)

33. Physical Change Physical changes might be caused by: Grinding Cutting
Crushing
Bending
Breaking
Heating/cooling
(change in phase)
Squishing
dissolving something

34. Physical Change
Evidence that a physical change has occurred might include:
Change in shape
Change in form
Change in size
Change in phase (This is always a physical change!)
Physical changes are usually reversible

35. Physical change
What could you do to these items to cause a physical change to occur?

36. Chemical change
A chemical change is a change in which a substance is changed into a different substance. (You’ve changed what it is.)

37. Chemical change Examples of chemical changes include: Burning Rusting
Tarnishing
Decomposing
Polymerization

38. Chemical change
Chemical changes occur when a chemical reaction causes bonds between atoms to break or to form.

39. Chemical change – Chemical reactions
There are 5 types of chemical reactions that cause chemical changes to occur.

40. Chemical change – Chemical reactions
1- Composition reactions (also called Synthesis)
Two things come together to form something new
A + B = AB
2H2 + O2  2H2O

41. Chemical change – Chemical reactions
2- Decomposition reactions
1 thing breaks apart to form 2 or more things.
AB = A + B
2H2O  2H2 + O2

42. Chemical change – Chemical reactions
3- Single replacement reactions
One atom replaces another atom
A + BC = AC + B or A + BC = AB + C
Mg + 2HCl  H2 + MgCl2

43. Chemical change – Chemical reactions
4- Double replacement reactions
Two chemicals switch places
AX + BY = AY + BX
2KI + Pb(NO3)2  PbI2 + 2KNO3

44. Chemical change – Chemical reactions
5- Combustion reaction
A substance combines with oxygen and releases energy.
C3H8 (propane) + 5O2  3CO2 + 4H2O

45. Chemical Change: Evidence
Evidence that a chemical change has occurred might include:
A color change
An odor change
Formation of a precipitate (you mix two liquids and make a solid)
Gas is formed (bubbles)
Changes in physical properties
Light is emitted
Change in temperature

46. Physical and Chemical change
During a chemical change energy can be released in the form of:
Heat
Light

47. Chemical change – Chemical reactions
When a chemical change occurs, energy is either released or absorbed.

48. Physical and Chemical change - heat
A chemical reaction that releases energy in the form of heat is called exothermic.
Heat comes OUT
Exo = out
Thermic = heat
It will feel HOT.

49. Physical and Chemical change - heat
A chemical reaction that absorbs energy in the form of heat is called endothermic.
Heat goes IN
Endo = in
Thermic = heat
It will feel COLD