SCIENCE 1206 – UNIT 2CHEMISTRY

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

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!

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.

CHEMISTRY TERMINOLOGY

● MASS– The amount of matter an object contains,

measured in grams, g.

3 STATES OF MATTER

● SOLID– Definite volume and shape

● LIQUID– Definite volume, indefinite shape

● GAS– Indefinite volume, indefinite shape

3 STATES OF MATTER

● Chemistry Subscripts– (s) - solid

– (l) - liquid

– (g) - gas– (aq) – aqueous, dissolved in water

3 STATES OF MATTER

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

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.

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– Odor– Solubility– Brittleness– Conductivity– Melting Point and Boiling Point

PHYSICAL PROPERTY

Examples of Physical Properties● Odor● Solubility● Brittleness● Conductivity● Melting and Boiling Pointng Point

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)

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.

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)

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.

CHEMICAL CHANGE INDICATORS

● COLOUR CHANGE

CHEMICAL CHANGE INDICATORS

● BUBBLES OF GAS

CHEMICAL CHANGE INDICATORS

● SOLID (PRECIPITATE) FORMATION

CHEMICAL CHANGE INDICATORS

● HEAT/LIGHT GIVEN OFF

MATTER FLOW CHART

PURE SUBSTANCE● Made up of only ONE TYPE OF ATOM or

ATOM COMBINATION

● Stays the same in response to a physical change

PURE SUBSTANCE● Example:

– O2

– H2O

● TWO TYPES:– Element– Compound

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.

ELEMENT

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

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.

COMPOUND

– Examples:

● NaCl● C

12H

22O

11

● CH4

● H2O

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

MIXTURE

● HETEROGENEOUS MIXTURE– Contains 2 or more visible phases

throughout– Examples:

● Soil, soup, fruitcake

DIATOMIC MOLECULES● There are 7 elements that are diatomic, or found in

pairs, in their natural state.● These are:

– H2 (g) Also P

4 (s) and S

8 (s)

– O2 (g)

– F2 (g) Memory tool: P.S., HOFBrINCl

– Br2 (g)

– I2 (g)

– N2 (g)

– Cl2 (g)

● 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) + O2(g) CO

2(g)

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

WHMIS Symbols

MSDS – MATERIAL SAFETY DATA SHEET