1. Chapter 1 The Organization of Matter
Related concepts: particles, atoms, molecules,

2. Matter and the Particle Model
Lesson 1.1
Matter and the Particle Model

3. Matter Matter is anything that has mass and volume 1
Mass means that it weighs something.
Be careful though, some things are so light we may think they have no weight, but they do!
Mass is usually measured in grams (g) or kilograms (kg)
Volume means that it takes up space.
Some things can expand and contract, but still take up space
Volume is usually measured in millilitres (mL) or litres (L)
1000 kg

4. Careful! Solids and Liquids are obviously made of matter.
They have easy-to-measure volume and mass
But so are gases!
Their mass is very low, so we often can’t measure it… It’s difficult, but not impossible, to weigh air!
Their volume can change easily, so it is difficult to measure the volume of a gas.
Matter
Matter
Matter
too!

5. Energy is NOT matter Electricity Heat Light Radiation Sound Motion

6. The Particle Model What is the particle model?
A scientific model that states:
“All matter is made of tiny particles”
Even science teachers are made of particles
The tiny particles include:
ATOMS and MOLECULES S O O S H H
Oxygen molecule
(O2) S
Sulfur molecule
(S8)
Water molecule
(H2O) H
Sulfur atom O C
Hydrogen atom O H H C
Carbon monoxide molecule
(CO)
Oxygen atom
Hydrogen molecule
(H2)
Carbon atom

7. How can matter be classified?
There are many ways to describe or classify matter.
By its phase or State.
By its Composition.
By its Properties
Gas
Solid
Liquid
Pure vs Mixture
Element - Compound – Solution - Colloid -Suspension
Density, melting/freezing point, boiling point, conductivity, characteristics

8. What are the phases or states of matter?
Gas
Solid
Gas
Liquid
The particles are close together
Very Strong Attraction
Little freedom to move
The particles are close together.
Fairly Strong Attraction
( a bit weaker than solid),
(much stronger than gas)
Some freedom to move.
The particles are far apart
Little or no attraction
Lots of freedom of movement

9. Summary Chart of Phases
State
Forces of Attraction of particles
Distance between Particles
Freedom of Movement of particles
Shape
(definite or indefinite)
Volume (definite or indefinite
SOLID
Very Strong
The bonds in a solid prevent the molecules from moving freely.
Close Together
Very Little Freedom of movement
(the particles can vibrate)
Definite
A solid keeps shape, even when you move it around
A solid keeps its volume, even when you move it around.
LIQUID
Fairly Strong Slightly weaker than a solid, but strong enough to keep the liquid together.
Close together
Some Freedom of movement
(particles slide & rotate)
Indefinite
Liquids take the shape of their container, but they may not fill it to the top.
Liquids keeps their volume, even if you pour them into a new container.
GAS
None
(or very weak)
The lack of bonds lets the molecules move anywhere
Far Apart
Lots of Freedom of movement
(particles move anywhere)
A gas takes the shape of its container, and fills it completely.
A gas fills its container completely, changing its volume to do so.

10. Classification: Everything that has a mass and volume is “matter”
Matter can also be classified this way:
Matter
Mixtures can be
physically separated
Pure Substances
Mixtures
Element
Compound
compounds can be
chemically separated
Homo-geneous Mixture
Hetero-geneous Mixture
eg. Gold
Or any of 117 other atoms of periodic table
eg.Water
Or any of thousands of compounds
Colloid
or emulsion
Solution
Suspension

11. Assignments on The Particle Model
Textbook: Read pp. 6 to 9
Workbook: Do pp. 1 and 2

12. Lesson 1.2 MIXTURES
A mixture contains at least two different substances.
Mixtures are not pure substances.

13. Mixture Homogeneous Solution Colloid Heterogeneous Suspension
A mixture is a type of matter.
A mixture is not Pure.
Matter
Pure Substance
Element
Compound
Mixture
Homogeneous
Solution
Colloid
Heterogeneous
Suspension
Homogeneous Mixtures include solutions and colloids.
Suspensions are heterogenous mixtures.

14. Heterogeneous Mixtures
Mixtures include:
the homogeneous types (solutions, colloids, and emulsions ) and…
the heterogeneous type. (suspensions)
Mixtures
Homogeneous Mixtures
Look like they are pure
(but they aren’t really pure)
Heterogeneous Mixtures
Don’t look pure
(because they aren’t)

15. Heterogeneous Mixtures (A.K.A. Suspensions) are unevenly mixed
Homogeneous Mixtures (Including solutions and colloids) are evenly mixed.
If they are liquid mixtures they are usually transparent and don’t settle. If they are solid mixtures they may be transparent, opaque, or metallic.
Examples: apple juice, kool-aid, sugar water, glass, bronze
Heterogeneous Mixtures (A.K.A. Suspensions) are unevenly mixed
They are usually cloudy and full of flakes, specks or grains.
Examples: mud, gravel, concrete,

16. COLLOIDS & EMULSIONS (the “nearly homogeneous” mixtures)
Colloids & emulsions appear homogeneous to the naked eye, but under a microscope the separate particles can be seen.
Colloids tend to look like jelly or mucilage (glue). They are thick, nearly clear liquids that can form semi-solid gels or pastes.
Emulsions tend to look milky. Homogenized milk is an example of an emulsion, so is paint,
Your textbook (incorrectly) refers to both types of “nearly homogeneous mixtures” as colloids, so we will consider them together and may use the word “colloid” for both of them.

17. Definition of a Solution
“A solution is a homogeneous mixture in which it is impossible to distinguish its constituent parts, even with an optical microscope”.
Solutions can exist as solids, liquids or gases:
Air = nitrogen(gas) + oxygen(gas) +other gases
Soda Water = water(liquid) + CO2(gas)
Wine = water(liquid) + alcohol(liquid) + flavours
Salt water = water(liquid) + salt(solid)
Steel = iron(solid) + carbon (solid)
Solution
Solvent
Solutes
Gaseous solution
Liquid solutions
Solid solution

18. AQUEOUS SOLUTIONS
The most important type of homogeneous mixture is the aqueous solution.
Aqueous solution means “a solution containing water”
An aqueous solution consists of…
Solute(s): the material(s) that is/are dissolved.
The solvent: The water (or liquid) that the solute(s) is/are dissolved in.
Solvent
Solution
Solute

19. Properties of Solutions
Concentration:
Concentration is the quantity of solute in a given amount of solution.
Concentration can be expressed a variety of ways:
Grams of solute per litre of solution (g/L)
Grams of solute per 100 mL of solution (% m/V)
Millilitres of solute per 100 mL of solution (% V/V)
Grams of solute per 100grams of solution (% m/m)
“Moles” of solute per litre of solution (mol/L or M.)

20. Concentration Formula
The formula for calculating concentration in grams per litre (the most common way we will express it) is:
Where:
C= concentration in g/L
m = mass of solute in grams
V = volume of solution in Litres.

21. Definition of Dilution
A concentrated solution can be made “weaker” by adding more solvent. This is called dilution.
“Dilution is a laboratory technique that involves decreasing the concentration of a solution by adding solvent.”
Definition of Dilution

22. The Dilution Formula The formula for calculating dilution is:
C1 V1 = C2 V2
Where:
C1 is the initial concentration (or concentration before dilution)
V1 is the initial volume (or volume before dilution)
C2 is the final concentration (or concentration after dilution)
V2 is the volume after dilution (or concentration after dilution)

23. Solubility
“Solubility is the maximum amount of solute that can be dissolved in a given amount of solvent”.
A saturated solution contains exactly the maximum amount of solute that can be dissolved in it.
An unsaturated solution contains less than the maximum amount
A supersaturated solution contains more than the maximum amount. Supersaturated solutions usually “precipitate” the excess solute.
Solubility can be expressed in the same units as concentration.

24. Separating Mixtures
Mixtures can be separated into the pure substances that they are made of.
We sometimes call the process of separating mixtures purification.
There are many methods of purifying mixtures, but we will list six of the most common.

25. 1.Decantation
Decantation is used to separate two liquids that can form layers.
The top layer of liquid is poured off the top of the bottom layer, or
The bottom layer is drained away from the top layer.
Best For:
Heterogenous Mixtures
Mixtures of Liquids

26. 2. Filtration
Used to separate a solid suspension from a liquid using a filter.
The mixture is poured through a filter. The liquid passes through, but the solid stays in the filter.
Heterogenous Mixtures
Best For:
Solid and Liquid Mixture

27. 3. Evaporation
Best For:
Homogeneous Mixtures
Solid and Liquid
Used to separate a solid in solution from a liquid, such as water
The solution is set aside in a warm, dry place (such as a desiccator or a watch glass) and the liquid part evaporates leaving the solid part behind.

28. 4. Distillation
Distillation is used to separate two liquids that do not separate easily into layers, such as alcohol and water.
Homogeneous Mixtures
Mixtures of Liquids
Best For:

29. Centrifugation
Spinning a sample of mixture around at high speed may cause it to separate into layers that can then be decanted.
A machine called a “centrifuge” is used to spin the sample

30. Chromatography
To separate small samples, like ink or dyes, into their components we can cause them to spread out on a piece of special paper.

31. Assignments
Textbook: Read pages 10 to 20
Workbook pages 3 to 12

32. Lesson 1.3 PURE SUBSTANCES
A pure substance contains only one type of particle, once it has been purified or cleaned .
Elements and Compounds are Pure

33. Matter Pure Substance Compound Element
A Pure substance is a type of matter.
A Pure substance is not a mixture.
Matter
Pure Substance
Element
Metallic
Elements
Non-metallic
Compound
Ionic Compound
Covalent Compound
Mixture
Heterogeneous
Homogeneous
Pure substances include Elements and Compounds.

34. Compounds vs. Elements
Only compounds and elements can be called PURE substances
An Element
Can be made of individual atoms, or of molecules that have only 1 type of atom (ie. All the atoms in the molecule are the same)
A Compound
Its molecules must be made from at least 2 types of atom or element
Different atoms H Au H
One atom
All atoms the same

35. ELEMENTS
An ELEMENT is a pure substance that contains only one type of atom.
It is impossible to separate an element into other substances using chemical separation techniques
That’s because there are no other substances to separate it into… it only has one type of atom!

36. How Many Elements are There?
It depends on how you calculate it…
Periodic tables will show between 100 and 118 different elements
88 elements make up most of the universe.
94 elements exist naturally on Earth.
Including 6 that exist in only trace amounts
112 elements have been named.
Including 18 more that can only be produced artificially using nuclear reactions (very scarce)
118 elements have been detected.
Including six more that disintegrate so fast that we cannot study them. They have temporary designations instead of names.

37. More Metallic Elements
The Elements
rare or artificial elements
Non-metal
Elements
Metallic Elements
More Metallic Elements

38. The Periodic Table Metallic Elements Metallic Elements Non-Metallic
Review
The Periodic Table 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 I
Solid
Liquid
Gas
VIII H II
Synthetic
III IV V VI
VII He Li Be B C N O F Ne Na Mg
III B
IV B
V B
VI B
VII B
VIII B
I B
II B Al Si P S Cl Ar K Ca Sc Ti Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te Xe Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn
Uut
Uuq
Uup
Uuh
Uus
Uuo La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Non-Metallic
Elements
Metallic
Elements
↑ The properties and family associations of these elements are hypothetical ↑
Metallic Elements 38

39. A Few Elements by Name (with formula and particle— atom or most common molecule – shown)
Hydrogen H2 Silicon Si Germanium Ge
Helium He Phosphorus P4 Arsenic As
Lithium Li Sulphur S8 Selenium Se
Beryllium Be Chlorine Cl2 Bromine Br2
Boron B Argon Ar Krypton Kr
Carbon C Potassium K Silver Ag
Nitrogen N2 Calcium Ca Gold Au
Oxygen O2 Chromium Cr Platinum Pt
Fluorine F2 Iron Fe Lead Pb
Neon Ne Cobalt Co Mercury Hg
Sodium Na Nickel Ni Uranium U
Magnesium Mg Zinc Zn Plutonium Pu
Aluminum Al Copper Cu The Element Song Ge Si P As P Se Li S S S S Br Be Br Cl B Ar Kr K C Ag N N Ca Au Cr Pt O O Fe Pb F F Co Hg Ni U Na Zn Pu Cu Al

40. Information from the Periodic Table11 Na
Sodium
23.0
Atomic Number
(# of protons)
Sodium has 11 protons.
Chemical Symbol
( abrev. of Latin name)
Eg. The Latin name of sodium is Natrium
Element Name
(English name)
Atomic Mass (weight)
(approx. # of protons + neutrons)
Sodium always has 11 protons, and usually 12 neutrons.
Metals
Non-metals Li
 Element is normally a solid metal Ne
 Element is normally a gas and a Non-metal Br
 Element is normally a liquid and a Non-metal Pu
 Element is a synthetic metal (not found in nature)

41. COMPOUNDS
A COMPOUND is a pure substance that contains two or more types of atoms that are chemically combined (ie. tightly bonded together).
It is possible to separate compounds into elements, but only by using chemical separation techniques (eg. Electrolysis, reduction)
There are thousands of different compounds known to exist.

42. Some Common Compounds with formulas and diagrams of their molecules
Water (H2O) Baking Soda (NaHCO3)
Salt (NaCl) Vinegar (CH3COOH)
Alcohol (C2H5OH) Sugar (C12H22O11)
Methane (CH4) Glucose (C6H12O6)
Ammonia (NH3) Gasoline (C8H18)
Carbon dioxide (CO2) H Na O C H H O Na Cl H C C O H H C C o H H H H H C H H H H N H H C C C C O C O

43. A Molecule

44. Why are Compounds Called “Pure”?
Because they can be purified.
When purified all their molecules are the same.
Pure
Pure
Mixture H H O H O H H O H
All particles the same
All particles the same
Two different particle types

45. Textbook: read pages 20 to 22
Workbook: pages 13 and 14

46. Characteristic Properties Lesson 1.4

47. Characteristic Properties
“A Characteristic property is one that helps us identify a pure substance, or a group to which the pure substance belongs”.
The concept of characteristic properties applies mainly to pure substances, ie. Elements & compounds, although chemical properties may show constituents.
Characteristic properties are of two types
Characteristic Physical Properties (pure substances only)
Characteristic Chemical Properties (possible constituents)
Non-characteristic properties are ones that are not much help in identifying what a pure substance is, or what it is made of.

48. Examples of Physical Characteristic Properties
Physical Property
Description
Examples
Melting Point
(or Freezing Point)
Temperature at which a solid becomes a liquid (vice versa), expressed in °C
Water: 0°C
Ethanol: -117°C
Salt: 801°C
Boiling Point
(or Condensation Point)
Temperature at which a liquid becomes a gas (vice versa) expressed in °C
Water: 100°C
Ethanol: 79°C
Salt: 1465°C
Density
The mass per unit of volume, expressed in g/mL
Water : 1.0 g/mL
Ethanol: 0.79 g/mL
Gold: 19.3 g/mL
Solubility
(at standard temperature of 25C)
The maximum amount of solute that can be dissolved in a given amount of solvent. Can be expressed in g/L or %v/v, %m/m , mol/L etc.
Salt* 357 g/L
CO2* 3.48 g/L
Sugar* 1792 g/L
* Dissolved in water
You Don’t need to copy this whole table. A copy of it is found on page 23 of your text book. Just list the names of the physical characteristic properties

49. Characteristic vs. Non-characteristic
Mass is a non-characteristic property.
Why? Because a material can have any mass. You could have a kilogram of lead, or a kilogram of water, or a kilogram of Styrofoam. The mass of material does not help identify it.
Volume is a non-characteristic property.
Why? You could have a litre of water or a litre of alcohol or a litre of gasoline. A material can have any volume.
Density, calculated from mass and volume, is a characteristic property
Why? Because each different substance has its own density. You can use density to help identify a substance.

50. Examples of Characteristic Chemical Properties
Chemical Property
Indications
Changes
Reaction of Litmus Paper
Indicates if the substance is an acid or a base
Turns Red = Acid (pH<7)
Turns Blue=Base (pH>7)
No change = neutral (pH7)
Reaction of Cobalt Chloride paper.
Indicates if the substance contains water
Turns pink, white or greenish = substance contains some water
Reaction of Limewater (to a gas)
Indicates if the substance contains carbon dioxide
Turns milky = contains some CO2
Reaction of Glowing wooden splint (to a gas)
Indicates if the substance supports combustion (usually oxygen)
Splint reignites = contains substance that supports combustion (eg. Oxygen)
Reaction of a burning wooden splint (to a gas)
Indicates an explosive gas (usually hydrogen)
If a “pop” or small explosion occurs, there is an explosive gas
Reaction to an open flame
The colour of the flame may indicate certain substances.
Purple = potassium
Green = barium or copper
Red = strontium
Table also found on page 24

51. Textbook
Workbook: pages 15 to 22

52. Chapter 1 Questions (Answers)
How do we define matter? Matter is anything that has mass (or weight) and takes up space (or volume)
What holds the particles of a solid together? The particles of a solid are held together by strong forces of attraction.
Using the particle model, describe two differences between a solid, a liquid, and a gas. In a solid the particles are close together & bound by strong forces. In a liquid the particles are also close together, but bound by weak forces. In a gas, the particles are far apart and not bound by forces of attraction.

53. Can you confirm that this is a solid?
The particles of a sample of matter are very close together.
Can you confirm that this is a solid?
No, both solids and liquids have particles close together.
What other information would confirm that it is a solid?
If the particles are held together by strong forces of attraction, then it must be a solid.
The smallest particle of matter that can be chemically divided is:
the molecule. It can be divided into atoms.
In the photo, the materials are...
Homogeneous: the liquid (a solution), the glass, the steel (an alloy) in the spoon, and the ceramic of the dishes
Heterogeneous: The cereal, the bamboo mat, and the paper tablecloth.

54. What type of mixture is each of these?
Handful of earth. Heterogeneous
Air Homogeneous (solution)
Smog Heterogeneous*
Stainless steel fork Homogeneous (alloy)
Seawater Homogeneous*(if filtered)
Whipping cream Heterogeneous*
Raisin muffin Heterogeneous
*Debatable. Depends on exact conditions
Definitions
Solvent (a substance that can dissolve another)
Solute (substance that dissolves into another)
Solution (homogeneous mixture)

55. The concentration is determined by the amount of solute dissolved in a certain amount of solution, as shown by the formula:
A patient receives a prescription from a doctor for a medication that needs to be dissolved in water at a concentration of 2 g/L. The dosage is the following: one teaspoon (5mL) three times a day for 10 days.
What is the minimum volume of medication that the patient will need?
Dose: 5mL total volume needed
3 time /day 5 x 3 x 10 = 150
10 days 150 mL of the medication solution is needed
If you were the pharmacist, how would you prepare the medication from a powder?
Data
C= 2 g/L formula:
V= 150 mL = 0.15 L
m = ? So: x = 2 g/L x 0.15 L
x = 0.30 g
The pharmacist would have to dissolve 0.30 g of the powder in enough water to make 0.15 L (or 150mL)

56. The hairdresser uses a hydrogen peroxide solution at 3% to lighten (a woman’s) hair. He needs to prepare 100 mL of this solution by diluting a concentrate at 30%. How should he do it?
After
After
Before
Data:
C1= 30%
V1= v
C2= 3%
V2= 100 mL
Formula: C1V1 = C2V2
Substution: % v = 3% 100mL
Or v = 300
So: v = 300 / 30
So: v= 10 mL
Answer: The hairdresser should prepare the solution by measuring 10 mL of the concentrated (30%) solution, and adding it to 90 mL of water (enough water to make 100 mL of the weaker solution).

57. 12. A wine contains 12% (vol/vol

60. Workbook Answers. Page 1 Matter is anything that has mass and volume
The Particle model is a scientific model based on the idea that matter is made of small particles
An atom is the smallest particle of matter, it cannot be divided chemically.
A molecule is two or more atoms held together by chemical bonds
The particle mode states that matter is made of small particles in constant movement.
Organization
Solid
Liquid
Gas
Distance between particles
Very close
Far apart
Forces of attraction
Very Strong
Fairly Strong
None (or very weak)
Movement of particles
Vibrate (little)
Slide around (more)
Move all over
Shape of matter
Definite shape
Indefinite shape
Volume of matter
Definite volume
Indefinite volume

61. Workbook Answers Page 2 Indicate the phase
Solid (definite structure and shape)
Gas (particles have freedom of movement)
Gas (takes up all the space it is given)
Liquid (definite volume but indefinite form)
How does the arrangement explain...
Gas particles are far apart (so gases are invisible)
Liquid particles can slide around (so liquids spread out)
Solids particles have strong forces of attraction (so they are rigid)
Gas particles move in all directions (so container must be closed)
Liquid particles can slide around (so they take the container’s shape)
a) gas b) solid
Molecule, chemical bond, atom

62. Workbook Answers, Page 3
A mixture consists of at least two different substances. It contains two different types of particle.
A heterogeneous mixture is made of two substances which can be distinguished with the naked eye
A homogeneous mixture is made up of two substances which cannot be distinguished with the naked eye.
A colloid is a homogeneous mixture with substances which can be distinguished under a microscope.
A solution is a homogeneous mixture in which it is impossible to distinguish its parts, even under a microscope.
A solute is a substance that dissolves in another substance
A solvent is a substance that can dissolve in another substance.
The missing words are “homogeneous mixtures” and “colloids”

63. Workbook page 4
The substances in a homogeneous mixture cannot be distinguished with the naked eye, but in a heterogeneous mixture they can be.
Indicate if it is homogenous or heterogeneous
Heterogeneous (orange juice with pulp)
Homogeneous (perfume)
Homogeneous (vinegar)
Heterogeneous (oatmeal)
Homogeneous (milk)
Homogeneous (air)
True or false Why?
False (you don’t need a microscope to see a heterogeneous)
True (a solution does contain at least two substances)
False (some solutions don’t contain liquids)
True (it is possible to have a solid solution, like steel)

64. The parts of a colloid can be distinguished under a microscope, but the parts of a solution can not.
You will see nothing different. The particles of a solution are too small to see with a microscope.
All three are colloids (you can see their parts in the microscope photos)
Possible answers:
Example
Solute
Solvent
a) Apple juice
Sugar, malic acid (apple flavour)
Water
b) Sparkling water
Carbon dioxide (CO2)
c) Energy drink
Sugar, caffeine, colour, flavour, etc.
d) Air
Oxygen
Nitrogen
e) Steel
Carbon
Iron

65. Some possible answers (see drawing)
The distilled water is the only one that is not a mixture. It is pure, since all the impurities have been removed from it by distillation.
Some possible answers (see drawing)
Heterogeneous Mixtures
Homogeneous Mixtures
Tree
Blood
Mud or ground
Sweat
T-shirt
Water
Soccer Ball
Steel (in the goal post)
Grass
Cloud

66. Workbook Answers, Page 7 C1V1=C2V2
Definitions:
The concentration corresponds to the quantity of dissolved solute in a given quantity of solution
Dilution is a laboratory technique that involves decreasing the concentration by adding solvent.
Solubility is the maximum amount of solute that can be dissolved in a given amount of solvent
A saturated solution is one that contains exactly the maximum amount of solute that can be dissolved in it.
Mathematical Formulas: C is the concentration
m is the mass of solute
V is the volume of solution
C1 is initial concentration
V1 is initial volume
C2 is final concentration
V2 is final volume
C1V1=C2V2

67. Workbook Answers, Pages 8 to 10
Alcohol
Rubbing alcohol
Isopropyl alcohol
Water
70% vol/vol
Effect on concentration
Decrease
Increase
Lemonade
10 g/L
Concentration will increase (it goes up to 30 g/L)
Concentration will decrease (it goes down to 2.5 g/L)

68. What True or false What does it represent? See table
A saturated solution
Heat the solution
True or false
False
True
What does it represent?
The concentration of protein in the drink
125 g of protein
See table
a) 10g 2L
5 g/L
b) 450 g
1.5 L
300 g/L
c) 625 g
2.5 L
25% mass/vol
d) 0.5 g
250 mL
2 g/L

69. 8. Solution step Procedure 1. Determine what we are looking for.
What is the concentration of the fat?
2. Determine the variables and their values
C=?
m= 3 g
V = 250 g or 0.25 L
3. Choose the formula
C= m V
4. Replace variables and calculate
C = g = 3 ÷ g/L = 12 g/L
0.25 L
5. Check solution and answer the question.
The fat concentration is 12 g/L

70. 9. a) the probable phase is solid, because the solubility increases with temperature. b) the solubility at 60°C is 375 g/L c) the solution will be supersaturated, because the amount of solute exceeds the amount of solute that can be dissolved in this much water. 10.
Step
Procedure
1. Determine what we are looking for.
What volume of concentrated ice tea do I need to use?
2. Determine the variables and their values.
C1= 1500 g/L C2= 100 g/L
V1= ? V2= 300 mL
3. Choose the formula
C1V1 = C2V2
4. Replace the variables and identify the unknown
V1= 20 mL
5. Check the solution and answer the question.
I must use 20 mL of the concentrated iced tea.

71. Workbook, Page 11
Mixture separation techniques are used to obtain pure substances.
Technique
Description
Decantation
When a mixture’s constituents have different densities they separate into different layers. Each layer can be poured out individually.
Centrifugation
Centrifugation accelerates the decantation process using an instrument that can spin a mixture at high speeds.
Filtration
Filtration involves passing a solid-liquid or solid-gas mixture through a filter. The solids stay on the surface of the filter.
Evaporation
Evaporation lets you collect a solid that was dissolved. The liquid in the mixture evaporates, leaving behind the solid.
Distillation
Distillation uses the different boiling points of a mixture’s constituents. They boil off at different temperatures.
Chromatography
This separates a mixture using porous paper and a solvent. The different rates they travel on the paper separates them.

72. Workbook, Page 12. 1. a) filtration c) Decantation e) Evaporation
b) Chromatography
d) Distillation
f) Centrifugation 2.
Examples
Similarity
Difference
a) Evaporation and distillation
Both involve evaporation of a liquid
In distillation, the evaporated liquid is collected and condensed. In evaporation it escapes. (other answers OK)
b) Decantation and Centrifugation
Both separate a mixture by its densities.
Centrifugation separates the mixture more rapidly. 3.
a) You want to get sugar from sugar cane juice
Evaporation
b) You want to get pure water from tap water
Distillation
c) You want to get orange juice without pulp
Filtration
d) You want to separate the colours in a drop of ink
Chromatography

73. Workbook, Page 13
A pure substance contains only one substance, in other words, only one type of particle.
An element is a pure substance that contains only one type of atom. It is impossible to separate an element into other substances using chemical separation techniques.
A compound is a pure substance that contains at least two types of atoms chemically combined. It can be separated using chemical separation techniques.
The periodic table is a list that groups together elements with similar properties. 79 Au
Gold
197
Chemical Symbol
Atomic number
Element Name
Atomic weight
Pure Substances
either order
Elements
Compounds

74. Atoms, subatomic particles, and the particle model (Not Examined)
ENRICHMENT
Atoms, subatomic particles, and the particle model
(Not Examined)
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75. up Li p+ O O C O String Theory Quarks Joining Quarks
There are those who believe that all particles are made up of tiny vibrating bundles of energy. That’s right, at the smallest levels of existence, matter and energy may be the same stuff.
Quarks
These “strings” of energy wrap around on themselves to form the smallest of particles, called Quarks. There are six main types of quarks: up, down, top, bottom, strange and charm. Quarks can also have three different charges, named after colours: red, blue and green
Joining Quarks
Three quarks of different colour-charge can join together to form a subatomic particle. In this case, two up-quarks and a down quark are joining together to form a proton. If it was two down quarks and an up quark, then a neutron would form instead. up Li O
Subatomic Particles
This proton is made up of quarks, as are neutrons and some other subatomic particles. O e- C
The Atomic Nucleus
The nucleus of an atom is made out of subatomic particles: protons and neutrons to be precise. The protons have a positive electric charge, but the neutrons have no charge. e- p+ n0 n0 n0 p+ p+ n0 p+ H O up dn up e-
Strings  Quarks Subatomic Particles  Atoms Molecules  Macromolecules

76. Particle model: Atoms and Molecules
Parts of an atom
Forming molecules
Valence electrons
Compounds vs. Elements

77. The Atom
The diagram you see is magnified approximately 10,000,000,000,000 times (10 trillion times)
Three parts of an atom
Electrons
Negative charge
Protons
Positive charge, found in nucleus
Neutrons
neutral charge, found in nucleus

78. Forming molecules Atoms nearly never stay alone.
Noble gases are exceptions
A group of two or more ATOMS is called a MOLECULE
Sharing/trading electrons enables formation of molecules
Atoms group together to stabilize their electrons

79. Valence Electrons
Electrons are grouped in concentric layers around the nucleus
These are called shells
The outermost shell is called the valence shell
The valence shell contains the valence electrons
Atoms are stable when the outermost shell is full
by either filling or emptying the valence shell

80. Compounds vs. Elements Rn
BOTH compounds and elements are made from ATOMS and MOLECULES
Elements (one type of atom)
have a unique number of protons in their nuclei (about 112 types)
Have one or more ATOMS of the SAME element per MOLECULE.
six elements are stable as single atoms
These are called the noble gases, their outer shells are full to begin with.
Seven elements are stable in groups of two. These are diatomic.
A few are stable in larger groups
The rest are metals, where the atoms overlap. We treat metals as if they had individual atoms Rn Ar Kr Xe Ne He I Br O Cl F N H N Br O Cl F I H S S
“I Have No Bright Or Clever Friends” P C C S S C C P S S P P C C S S Al Al Al Al ? ? ?

81. Molecules and Compounds
Two or more ATOMS bond together to form MOLECULES
If the atoms in the molecules are Different, then the molecules are COMPOUNDS.
If the atoms are all the same then they are still elements.
Element Molecules
Compound Molecules

82. Where do things fit in? Level of organization examples
Don’t study this year
Where do things fit in?
In this chapter
In another chapter.
Level of organization
examples
Strings (not studied)
Vibrating bundles of energy
Quarks (not studied)
Up, down, top, bottom, charm, strange
Sub-atomic particles
Protons, neutrons, electrons
Atoms (and elements)
117 types (eg. H, He, O,…)
Molecules (& compounds)
Millions of types (eg. H2O, CO2)
Macromolecules
DNA, proteins, carbohydrates, etc.
Cells
Skin cell, muscle cell, nerve cell, etc.
Tissues
Epithelial, muscular, etc.
Organs
Kidney, Lung, Heart, eye, etc.
Systems
Respiratory, Skeletal, etc.
The Human Organism
Larger Smaller

83. Level of organization examples The Ecosystem The Biosphere
The Human Organism
Us. Individual human beings
The Ecosystem
The things around us that we interact with
The Biosphere
All the water, animals, plants, and other life that cover our world
The Planet Earth
Our planet and its moon
The Solar System
The Sun, 8 planets, their moons, 5 dwarf planets, comets & asteroids
Our Galaxy
The Local Group
About a dozen galaxies closest to us
The Virgo Supercluster
A cluster of thousands of galaxies
The Universe

84. Bunches of particles… Mixture vs. Pure substance
Heterogeneous/Homogeneous
Elements vs Compounds

85. Mixture vs. Pure Substance
At least two different types
can be lots more
Pure substance
A bunch of exactly the same molecules