1. Chemistry:Review
SNC1P

2. Safe Lab Techniques
When lighting a Bunsen Burner, ensure all long hair and loose clothing is out of the way
When smelling a chemical waft it towards you. DO NOT SMELL it directly
Put broken glass in the designated bin
When something is spilled. Notify Mr. Hoover immediately
If something breaks. Notify Mr. Hoover immediately

3. Safe Lab Techniques Never eat or drink in the lab
Wash hands after handling chemicals
When performing a lab, always stay standing, do not sit down.
Never leave a Bunsen burner unattended
Always use appropriate equipment
Always wear safety goggles
Never wear open toed shoes in the lab

4. WHMIS
The Workplace Hazardous Materials Information System (WHMIS) is Canada's national hazard communication standard.
The key elements of the system are cautionary labelling of containers of WHMIS "controlled products", the provision of material safety data sheets (MSDSs) and worker education programs

5. WHMIS Symbols CLASS A: COMPRESSED GAS
This class includes compressed gases, dissolved gases, and gases liquefied by compression or refrigeration.

6. WHMIS Symbols CLASS B: FLAMMABLE AND COMBUSTIBLE MATERIAL
This class includes solids, liquids, and gases capable of catching fire in the presence of a spark or open flame under normal working conditions.

7. WHMIS Symbols CLASS C: OXIDIZING MATERIAL
These materials increase the risk of fire if they come in contact with flammable or combustible materials.

8. WHMIS Symbols
CLASS D: POISONOUS AND INFECTIOUS MATERIAL Division 1: Materials Causing Immediate and Serious Toxic Effects
These materials can cause death or immediate injury when a person is exposed to small amounts. Examples: sodium cyanide, hydrogen sulphide

9. WHMIS Symbols
CLASS D: POISONOUS AND INFECTIOUS MATERIAL Division 2: Materials Causing Other Toxic EFFECTS
These materials can cause life-threatening and serious long-term health problems as well as less severe but immediate reactions in a person who is repeatedly exposed to small amounts.

10. WHMIS Symbols
CLASS D: POISONOUS AND INFECTIOUS MATERIAL Division 3: Biohazardous Infectious MATERIAL
These materials contain harmful micro- organisms that have been classified into Risk Groups 2, 3, and 4 as determined by the World Health Organization (WHO) or the Medical Research Council of Canada.

11. WHMIS Symbols CLASS E: CORROSIVE MATERIAL
This class includes caustic and acid materials that can destroy the skin or eat through metals. Examples: sodium hydroxide, hydrochloric acid, nitric acid

12. Matter has many forms Matter – anything that has mass and volume.
Mass is a measure of the quantity of an object. (g, kg,)
Volume is a measure of space taken up (mL, L)
Matter can be found as a solid, liquid or gas. (or even a combination of these)

13. Changes of State
There are 3 states of matter
Solid
Liquid
gas

14. Terms for changes of state
Melting – Change from a solid to a liquid
Evaporation - Change from a liquid to a gas
Condensation - Change from a gas to a liquid
Freezing - Change from a liquid to a solid
Sublimation - Change from a solid to a gas
Deposition - Change from a gas to a solid

15. Terms for changes of state

16. The Particle Theory of Matter (4 points)
Way of describing matter.
All matter is composed of very tiny objects called particles.
Each Pure substance has its own kind of particles, different from the particles of other pure substances.

17. The Particle Theory of Matter (4 points)
3. Particles present in matter are always in motion. They may be vibrating back and forth, as in a solid, or moving in all directions, as in a gas. In a liquid, particles stay close together but can slide past one another.
4. The particles in a substance attract each other. The amount of attraction is different for different kinds of particles. All particles have spaces between them.

18. The Particle Theory of Matter (4 points)
The distances between the particles change for different states of matter.

19. Classification Of Matter
Pure Substances
Element
Compound
Mixture
Mechanical Mixture
Suspension
Solution

20. Pure Substances (2)
A pure substance is made up of only one kind of matter
unique set of properties
colour, hardness, boiling point, and melting point.
A pure substance is either an element (gold) or a compound (sugar).

21. Element
A pure substance that cannot be broken down into any simpler substance by chemical means.
Each element has its own name and symbol. Example: Gold (Au)

22. Compound
A pure substance that is made from two or more elements that are combined together chemically.
Example, water (H2O) is a compound containing the elements hydrogen and oxygen.

23. Mixtures (3) A mixture is a combination of pure substances.
Each substance remains in its original, pure form, although each is not always easy to see distinctly once the mixture is made.

24. Mechanical Mixture (heterogeneous mixture)
Different substances that make up the mixture are visible
Hetero = different

25. Suspension
A cloudy mixture in which tiny particles of one substance are held within another.
Can be separated out when the mixture is poured through filter paper.
A suspension is also a heterogeneous mixture.

26. Solution (homogeneous mixture)
Different substances that make it up are not individually visible
One substance is dissolved in another
The prefix “homo-” means same, and all parts of a homogeneous mixture look the same.

27. Physical Properties
-A physical property describes a characteristic of a substance that can be observed or measured without changing the composition of matter.
Example: Melting Point, Boiling Point

28. Observing Physical Properties
Property
Description
Examples
What it looks like
Colour and lustre
The light the substance reflects gives it colour and lustre (shine)
The names for some
substances, such as gold,
are also the names of colours. Gold has lustre; concrete is dull
Conductivity
Conductivity is the ability
of a substance to conduct electricity or heat. A
substance that conducts
electricity or heat is called a conductor. A substance with little or no conductivity is an insulator.
Most metals are good conductors. Copper is a very good conductor of electricity and so is used to make electric wires. Styrofoam® and glass are insulators.

29. Observing Physical Properties
Property
Description
Examples
What it looks like
Density
Density is the amount of
mass in a given volume of
a substance.
D = m/v
The density of pure water is 1 g/mL.
The density of gold is 19 g/mL.
Water is denser than oil, but gold is denser than water.
Ductility
Any solid that can be
stretched into a long wire is said to be ductile.
Copper is a common
example of a ductile material.

30. Observing Physical Properties
Property
Description
Examples
What it looks like
Hardness
Hardness is a substance’s
ability to resist being scratched. Hardness is
usually measured on the Mohs hardness scale from
1 to 10.
The mineral talc is the softest substance on the Mohs hardness scale (1). Emerald is quite hard (7.5). Diamond is the hardest
(10).
Malleability
A substance that can be
pounded or rolled into
sheets is said to be malleable.
Aluminum foil is an example of a malleable substance.
Metals such as gold and tin are also malleable.

31. Observing Physical Properties
Property
Description
Examples
What it looks like
Viscosity
Viscosity is the resistance of a fluid to flow.
Honey has a high viscosity
Compared to water.

32. Observing Chemical Properties
A chemical property describes the ability of a substance to change into a new substance or substances.
In order to view a chemical property a chemical change must occur.
Chemical change - the formation of a new substance or substances with new properties.
A chemical reaction is a process in which a chemical change occurs.

33. Chemical Properties
1. Combustibility is the ability of a substance to burn. In order to burn a substance requires Oxygen

34. Chemical Properties
2. Light sensitivity is a chemical property of that can cause new substances to form when light hits it.

35. Chemical Properties
3. Reacting with an acid is a chemical property where when acid is poured on a substance it produces a gas and bubbles.

36. Clues that a chemical change has occurred
Evidence
Change in colour
Final product(s) may have a different colour than the colours of the starting material(s).
Formation of a solid (precipitate)
Final materials may include a substance in a state that differs from the staring material(s): Precipitate

37. Clues that a chemical change has occurred
Evidence
Formation of a gas
Final materials may include a substance in a state that differs from the staring material(s); commonly, a gas
Release / absorption of heat or light
Energy (light, electricity, sound or most commonly heat) is given off or absorbed.
The change is difficult to reverse
The change cannot be reversed or it is difficult to.

38. Atoms are composed of three subatomic particles
Protons- Heavy positively charged found in the nucleus
Neutrons -are neutral particles that have the same mass as protons and are located in the nucleus
Electrons- Negatively charged particles with almost no mass. They circle the nucleus at different energy levels.

39. Atoms are composed of three subatomic particles
Atoms are electronically neutral so the number of electrons = the number of protons

40. Metals Found on the Left side of the periodic table
The majority of elements on the periodic table are metals. All metals, except for mercury are solids at room temperature. Metals have the following properties.
Malleable: The ability to be hammered or bent into a shape.

41. Metals Lustre: They are shiny in appearance.
Ductile: They can be pulled into a wire.
Conductor of electricity: Electricity can travel through the metal.

42. Metals
A mixture of two or more metals is called an alloy. The process of alloying different metals together can enhance the properties of the metal.

43. Non-Metals Non-metals generally have these properties:
Non-conductor of electricity in its solid form
At room temperature most are gasses (11) or solids (5) and only one is liquid.
Solids are brittle and lack the lustre of metals

44. Metalloids Found in the middle-right of the periodic table
Some elements do not fit as metals or non- metals. These fit on either side of the staircase that divides the metals and the non-metals.
They have some properties of metals and some properties of non-metals. They are called semiconductors because they do not conduct electricity well.

45. Atomic Number (Z)
Atomic number - the number of protons in an atom of an element.
Each element has a set number of protons and every atom from that element will have that many protons.
The pattern for increasing protons moves from left to right and then down to the next row just like reading a book.

46. Atomic Mass (A) Atomic mass - the average mass of an element’s atoms.
Atomic mass is given in atomic mass units (amu).
H has a mass of 1.01 amu. This means that iron atoms are about times heavier than hydrogen atoms.
Atomic masses are always expressed as decimal fractions. One reason that they do not have whole number values is that, except for fluorine, atoms of the same element have different numbers of neutrons.

47. Ion Charge
Ion charge - the electric charge that an atom takes on when it loses or gains electrons.
An atom or group of atoms that has lost or gained electrons is called an ion.
Electrons have a negative charge, and so an atom that loses electrons becomes a positive ion. An atom that gains electrons becomes a negative ion.
Metal atoms can lose electrons in certain situations. (positive ions)
Non-metals can gain electrons in certain situations. (negative ions)

48. Ion Charge
Elements with atoms that can form similar ions are grouped together in the periodic table. Metals generally lose electrons and become positive ions.
Many non-metals can gain electrons and so become negative ions.

49. Calculations Determining the number of neutrons
Subtract the atomic number (# of protons) from the Atomic mass (# of protons and neutrons)
Atomic mass – atomic number (A – Z = N)
Example: Iron
55.85 – 26 = 30 neutrons

50. Orbit # # of Electrons 1 2 8 3 4 18 Bohr Diagrams
To represent electron arrangements at various orbits we use Bohr diagrams. Each orbit has a set number of electrons.
Orbit #
# of Electrons 1 2 8 3 4 18

51. Every row in the period contains a shell
Every row in the period contains a shell. The farther you move down the table the more shells you added to the diagram. H = 1 shell, Li = 2 shells, K = 3 shells.

52. Moving left to right on the periodic table adds valence electrons to the shells of that row. Na has 1 valence e-, Mg has 2 valence e-, Al has 3 valence e-, etc.