SCIENCE 1206 UNIT 2 CHEMISTRY

Transcription

1 SCIENCE 1206 UNIT 2 CHEMISTRY

2 UNIT OUTLINE CHEMISTRY TERMINOLOGY GENERAL TERMS PERIODIC TABLE BOHR DIAGRAMS ATOMS versus IONS NAMING COMPOUNDS IONIC, MOLECULAR, ACIDS CHEMICAL REACTIONS BALANCING CHEMICAL EQUATIONS 5 TYPES of REACTIONS

3 IMPORTANT TO KNOW... You will get a PERIODIC TABLE!!! It is your best friend for this unit! You will need it each and every day. Take care of it, cherish it, appreciate it!

4 CHEMISTRY TERMINOLOGY MATTER DEFINITION: Anything that has mass and volume (takes up space). What is not matter? Energy In chemistry, we often discuss microscopic matter, such as atoms, ions, elements, and compounds.

5 CHEMISTRY TERMINOLOGY MASS The amount of matter an object contains, measured in grams, g.

6 3 STATES OF MATTER SOLID Definite volume and shape LIQUID Definite volume, indefinite shape GAS Indefinite volume, indefinite shape

7 3 STATES OF MATTER Chemistry Subscripts (s) - solid (l) - liquid (g) - gas (aq) aqueous, dissolved in water

8 3 STATES OF MATTER

9 WHAT IS CHEMISTRY? DEFINITION: The study of the properties and chemical changes/reactions of matter. So, chemistry matters Examples of chemical reactions: Rusting Burning/Combustion

10 TWO TYPES OF CHEMISTRY PURE CHEMISTRY Theoretical work that involves DESCRIBING known substances and DISCOVERING new compounds for research purposes. APPLIED CHEMISTRY Practical work that involves searching for USES for known substances.

11 PHYSICAL PROPERTY A QUALITY or CHARACTERISTIC of a substance that can be observed WITHOUT a chemical reaction. Examples of Physical Properties State of matter Hardness Colour Malleability Ductility

12 PHYSICAL PROPERTY Examples of Physical Properties Odor Solubility Brittleness Conductivity Melting and Boiling Pointng Point

13 PHYSICAL CHANGE A change in state of matter of a substance. Examples of Physical Changes: Melting/fusion SOLID to LIQUID Freezing LIQUID to SOLID Evaporation LIQUID to GAS Condensation GAS to LIQUID Sublimation SOLID to GAS Deposition GAS to SOLID Ex: H2O(s) H2O(l)

14 CHEMICAL PROPERTY A BEHAVIOUR of a substance that can only be observed when a CHEMICAL CHANGE is taking place. Example: Magnesium ribbon burning 2 Mg(s) + O2(g) 2 MgO(s) + light energy The chemical property is that light is given off when magnesium is burned.

15 CHEMICAL CHANGE A change in which ONE OR MORE NEW SUBSTANCES is formed. Example: Iron Rusting 4 Fe(s) + 3 O2(g) 2 Fe2O3(s)

16 INDICATORS OF A CHEMICAL CHANGE Basically, a chemical change has occurred if the change is DIFFICULT TO REVERSE. However, there are many good indicators of a chemical change. Observe the following pictures, and take a guess at what is happening to indicate a CHEMICAL CHANGE.

17 CHEMICAL CHANGE INDICATORS COLOUR CHANGE

18 CHEMICAL CHANGE INDICATORS BUBBLES OF GAS

19 CHEMICAL CHANGE INDICATORS SOLID (PRECIPITATE) FORMATION

20 CHEMICAL CHANGE INDICATORS HEAT/LIGHT GIVEN OFF

21 MATTER FLOW CHART

22 PURE SUBSTANCE Made up of only ONE TYPE OF ATOM or ATOM COMBINATION Stays the same in response to a physical change

23 PURE SUBSTANCE Example: O 2 H 2 O TWO TYPES: Element Compound

24 TYPES OF PURE SUBSTANCES ELEMENT A pure substance that CANNOT be broken down into a simpler substance by a CHEMICAL CHANGE. It is made up of 1 TYPE OF ATOM. Element SYMBOLS are always written with the first letter UPPERCASE and the second letter LOWERCASE. Element NAMES are always written in LOWERCASE letters.

25 ELEMENT Examples: Na - sodium Li - lithium Ar - argon W tungsten K potassium C carbon Ag - silver

26 TYPES OF PURE SUBSTANCES COMPOUND A pure substance that CAN be broken down into its elements with a CHEMICAL CHANGE. It is made up of two or more different elements are chemically joined together in fixed proportions.

27 COMPOUND Examples: NaCl C 12 H 22 O 11 CH 4 H 2 O

28 MIXTURE Contains 2 or more pure substances TWO TYPES: HOMOGENEOUS MIXTURE AKA SOLUTION Have only one visible phase throughout Examples: air, apple juice, salt water

29 MIXTURE HETEROGENEOUS MIXTURE Contains 2 or more visible phases throughout Examples: Soil, soup, fruitcake

30 DIATOMIC MOLECULES There are 7 elements that are diatomic, or found in pairs, in their natural state. These are: H 2 (g) Also P 4 (s) and S 8 (s) O 2 (g) F 2 (g) Memory tool: P.S., HOFBrINCl Br 2 (g) I 2 (g) N 2 (g) Cl 2 (g)

31 REACTANTS Starting Materials in a chemical reaction PRODUCTS New substances formed in a chemical reaction CHEMICAL REACTION Reactants go to form Products Example: C(s) + O 2 (g) CO 2 (g)

32 WHMIS Workplace Hazardous Materials Information System Canada's hazard communication standard Requires that all containers of WHMIS controlled products must have: A Label illustrating the effects of the product Material Safety Data Sheet (MSDS) Sheet

33 WHMIS Symbols

34 MSDS MATERIAL SAFETY DATA SHEET