1. Characteristic Properties of Matter
Characteristic that is UNIQUE to a particular substance. (melting point, boiling point, density)
Melting Point
When a substance goes from a solid state to a liquid state.
Ex: The melting point of water (ice) is 0̊ C
The melting point of aluminum is 660̊ C
Boiling Point
When a substance goes from a liquid state to a gaseous state.
Ex: The boiling point of water is 100̊ C
The boiling point of silver is 2162̊ C

2. Density
Measures the amount of matter in a given space
Measure of compactness
Measured in g/cm³ (or g/ml) *note: water has a density of 1 g/cm³ (or 1g/ml) *

3. Example
Calculate the density of 50 ml of a liquid having a mass of 63 g.

4. Formulas to remember: Density = mass ÷ volume Volume = mass ÷ density Mass = density x volume

5. Try This! What is: The melting point of a substance?
The boiling point of a substance?
2. Define density.
3. Give 3 examples of characteristic properties of matter.

6. Section 2: Transformation of Matter
Material World
Section 2: Transformation of Matter

7. Physical Changes
Physical Change: When the appearance of a substance changes but the nature of the substance remains the same.
Example: ice melting to liquid water, cutting a paper
No new substances are created.
The characteristic properties of the substance are preserved.
Changes in states of matter are physical changes.
Physical Changes are reversible.

8. Physical Changes: Reversible Transformations
Red Arrows: When the substance is heated Blue Arrows: When the substance is cooled

9. Changes of State and Particle Theory
See Changes of State and Particle Theory Worksheet

10. Try This! a) Name the three states of matter.
b) Name the six change in states of matter.
c) Give an example of each of these changes in states of matter.
2. What is a physical change?
3. Are new substances produced during a physical change? Explain.

11. Chemical Changes Chemical Changes:
Chemical changes occur when two or more substances called reactants, interact together to create entirely new substances called products.
Irreversible
New substances produced have their own unique properties that are different than those of the original substance(s).
Signs that a chemical change has occurred:
A gas is formed Heat/light is produced Color change occurs A residue is formed

12. Try This!
What is the difference between a chemical change and a physical change? Give some examples for each.
Are new substances produced during a chemical change?
What happens to the characteristic properties of a substance when a chemical change occurs?
What four signs indicate a chemical change?

13. Try This!
6. Indicate which of the statements below describe a physical change and which describe a chemical change:
Sugar dissolves in water.
The filament in a light bulb glows when an electric current runs through it.
A piece of chalk is crushed.
Snow melts.
Lime water (clear in color) becomes cloudy in color in the presence of carbon dioxide.

14. Conservation of Matter
“The mass of substances that undergo a transformation (whether a physical or chemical change) is ALWAYS equal to the mass of the resulting substances.”
Law of Conservation of Matter
Physical Change example: The mass of a can before being crushed is the same as the mass of the can after it is crushed.
Chemical Change example: The mass of a freshly eaten apple is the same as when it is left in contact with air and turns brown.

15. Pure Substances and Mixtures

16. Be Careful! Mixture Pure Substance (Homogeneous mixture)
Contains minerals in the water Pure water with no minerals

17. Homogenous Mixtures Contain two or more substances mixed together
The particles of each substance are evenly distributed in the mixture.
1 phase (no layers)
Also called solutions
Ex: Air, tap water, milk, apple juice
Out of the two substances present: - The one present in the larger quantity is called the SOLVENT (the stuff that does the dissolving)
- The one present in the smaller quantity is called the SOLUTE (the stuff being dissolved)

18. Try This!
Indicate what is the solute and what is the solvent in the following homogenous solutions:
Chocolate milk
Kool Aid
Tap water *

19. Try This!
Indicate whether each statement below describes a homogeneous or heterogeneous mixture:
Only displays one phase to the naked eye.
Displays an arrangement of particles that is not uniform.
Displays more than one phase to the naked eye or through a microscope.
Shows a uniform distribution of particles.
Noodle Soup
Vinegar
Milk

20. Note:
In a homogenous solution, there is only one solvent (the substance in largest quantity… the stuff that does the dissolving). However, there can be more than one solute! Ex: The air we breathe is an example of a homogenous mixture. It is composed of 78% nitrogen, 21% oxygen, 0.01% carbon dioxide and 1% other gases. Name the solvent and solutes.

21. Dissolution
Dissolution is the process of mixing two or more substances together (solvent and solute).

22. Separation of mixtures
Sedimentation
Letting a heterogeneous mixture sit and allowing the larger particles to settle at the bottom (they form a sediment)

23. Separation of mixtures
Decantation
Often used after sedimentation
Act of separating the layers by gradually
pouring out one layer at a time into another
container.

24. Separation of mixtures
3. Filtration
Separates different substances of a heterogeneous mixture.
Faster than the sedimentation process.
Uses filter paper which has tiny holes in it. The paper holds back the bigger particles (the residue) while the smaller particles (the filtrate) pass through.

25. Separation of mixtures
4. Distillation: Separating homogeneous mixtures
Relies on the boiling point of the substance you want to separate from the rest of the mixture.
Ex: You are stranded on a deserted island and only have the salt water from the ocean to survive on (homogeneous mixture). You need to find a way of separating the salt from the water to be able to drink it. You can do this by distilling the water.

26. Distillation (Set-Up)

27. Distillation Process
Heat the salt water solution in the distillation flask to 100 ̊C (boiling point of water).
Only the water (not the salt and minerals) will start to boil and evaporate up the distillation flask and into the condenser. The salt, minerals and any other impurities will stay in the flask.
Once in the condenser, the water vapor is cooled and condenses back into liquid water.
The liquid water drops down into the receiving flask. You now have pure water (called distilled water).

28. Try This! a) Provide an example of a heterogeneous mixture.
b) Provide an example of a homogeneous mixture.
2. What is the difference between a pure substance and a homogeneous mixture?
3. Is tap water a pure substance or a homogeneous mixture? What about distilled water?
4. In filtration plants, the water to be treated passes through a layer of sand. Is this sedimentation or filtration? Explain your answer.

29. Try This!
Name the filtration process you would use in the following scenarios:
Beaker A contains a heterogeneous mixture. You can clearly see brown particles suspended in it and you can also see a deposit at the bottom of the beaker.
b) Beaker B contains a blue solution. There are no visible particles in the liquid.
c) Beaker C contains a heterogeneous mixture. The suspended particles are very fine. There is not visible deposit at the bottom of the beaker.

30. Section 3: Organization of Matter
Material World
Section 3: Organization of Matter

31. The Atom
The particles of matter we have been talking about are actually atoms.
Atoms are the smallest component of matter.
Everything is made up of atoms!
There are 120 different kinds of atoms.
When two or more atoms attach together with a chemical bond, a molecule is formed
The atom is made up of three components: protons, neutrons and electrons.

32. The Atom An atom looks like this:
In the center of the atom we have a nucleus.
Inside the nucleus, we have protons (positively charged
particles) and neutrons (neutral particles, they have no charge).
Floating around the nucleus are electrons (negatively charged particles) which move around the nucleus in orbits (like planets moving around the sun)

33. In reality, the atom actually looks like this:

34. Try This! What is an atom? What holds atoms in molecules together?
Which particle(s) is/are found in the nucleus?
Where are electrons located?
What charge do protons, neutrons and electrons each have?

35. The Elements: Different Kinds of Atoms
Atoms that have the same number of protons (positively charged particles in the nucleus) are considered to be the same “type” of atom.
*** THE NUMBER OF PROTONS OF AN ATOM IS THEREFORE A CHARACTERISTIC PROPERTY OF ELEMENTS ***
The different “types” of atoms are called elements.
There are 120 different elements.
Elements are organized in a table called The Periodic Table of Elements

36. The Periodic Table of Elements

37. The Periodic Table of Elements
& number of protons

38. The Periodic Table of Elements
The periodic table contains all natural and artificial elements known to date.
These elements form all of the visible and invisible matter around us.

39. The Periodic Table of Elements
The elements are laid out in rows and columns.
Rows are in ascending order of atomic number (# protons the element has).
The rows are called periods.
The columns are called families or groups.
Each family contains elements with similar properties.

40. Try This! What do atoms of the same element have in common?
Elements are classified in a table called…
The rows of the periodic table are called…
The columns in the periodic table are called…

41. The molecule = A group of atoms
When 2 or more atoms attach together with chemical bonds, they form a molecule.
The molecule can be made up of many atoms of one element.
Ex:
Or the element can be made up of many atoms of different elements.

42. Chemical Formulas Elements are represented by chemical symbols.
Molecules are represented by chemical formulas.
Chemical formulas indicate which elements the molecules contain.
Ex:
Molecule
Chemical formula
Molecular Model
Atomic Composition
Silica (Sand)
SiO2
1 atom of silicon
2 atoms of oxygen
Glucose (Sugar)
C6H12O6
6 atoms of carbon
12 atoms of hydrogen
6 atoms of oxygen

43. Chemical Formulas
The chemical formula for water

44. Try This!
Determine the different elements that make up the following molecules. In addition, determine how many atoms there are of each element:
CH4
CO2 O3 N2
C6H12O6
H2O2
NaCl
HNO3

45. The Atomic Theory
All matter us made up of tiny particles called atoms.
Atoms are made up of even smaller particles called protons, neutrons and electrons.
Atoms can be distinguished from each other by their number of protons, neutrons and electrons.
Atoms with the same amount of protons are called elements.
Atoms combine to form molecules (2 or more atoms bound together form a molecule)

46. Try This! How are atoms like letters of the alphabet?
How are molecules like words?
What 3 particles atoms composed of? Where are the 3 particles located in the atom?
What is the name of a group of atoms that have the same number of protons?
The periodic table groups together elements by families and periods. What do the elements of the same family have in common?