SCIENCE 1206 UNIT 2 CHEMISTRY - Home of the Titans! · PDF fileUNIT OUTLINE CHEMISTRY ... at the base of your locker or bookbag ... The amount of matter an object contains, measured

SCIENCE 1206 – UNIT 2

CHEMISTRYNovember – January 2010

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!

In other words, do not leave it in a crumpled mess at the base of your locker or bookbag

LINK

LINK 2

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.

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

Chemistry Subscripts◦ (s) - solid

◦ (l) - liquid

◦ (g) - gas

◦ (aq) – aqueous, dissolved in water

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 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) 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

HOMEWORK!!!1. Identify the following as a PHYSICAL PROPERTY or

a CHEMICAL PROPERTY.1. Burns in air when heated.

2. Melts at 98 degrees Celsius.

3. Reacts violently with water.

4. Can be cut with a knife.

5. Conducts electricity.

2. Identify the following as a PHYSICAL CHANGE or a CHEMICAL CHANGE.

1. Digesting a meal.

2. Butter melting in a pan.

3. Burning gasoline.

4. Wood rotting.

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MATTER FLOW CHART-Draw

MATTER

PURE SUBSTANCE

COMPOUND

ELEMENT

ATOM

MIXTURE

HOMOGENEOUS MIXTURE

(SOLUTION)

HETEROGENEOUS MIXTURE

PURE SUBSTANCE

Made up of only ONE TYPE OF ATOM or ATOM COMBINATION

Stays the same in response to a physical change

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.

◦ Examples: Na

Li

Ar

W

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 elements are chemically joined together in fixed proportions.

◦ Examples:

NaCl

C6H12O6

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

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,

◦ O2,

◦ F2,

◦ Br2,

◦ I2,

◦ N2,

◦ Cl2,

◦ Also P4 and S8

Memory tool: P.S., HOFBrINCl

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) CO2(g)

HOMEWORK . . . 1. Name the type of pure substance that is

found on the periodic table.

2. Give an example of each of the following:

1. Pure substance

2. Heterogeneous mixture

3. Homogeneous mixture

LINK

MSDS – MATERIAL SAFETY DATA SHEET