Sep 30, 2011

Physical & Chemical Change

Different States of Matter:
Solid, liquid, and gases are the three states of matter and their particles within the substance act differently according to their different states.
Solid                             Liquid                        Gas

Chemical Changes: Chemical changes take place on the molecular level. A chemical change produces a new substance. Examples of chemical changes include combustion (burning), cooking an egg, rusting of an iron pan, and mixing hydrochloric acid and sodium hydroxide to make salt and water.

Physical Changes: Physical changes are concerned with energy and states of matter. A physical change does not produce a new substance. Changes in state or phase (melting, freezing, vaporization, condensation, sublimation) are physical changes. Examples of physical changes include crushing a can, melting an ice cube, and breaking a bottle.

Difference: A chemical change makes a substance that wasn't there before. There may be clues that a chemical reaction took place, such as light, heat, color change, gas production, odor, or sound. The starting and ending materials of a physical change are the same, even though they may look different.


Examples of Chemical Changes

  • burning wood
  • dissolving salt in water
  • mixing acid and base
  • digesting food

Examples of Physical Changes

  • crumpling a sheet of paper
  • melting an ice cube
  • casting silver in a mold
  • breaking a bottle

Sep 26, 2011

Scientific Notation

Scientific Notation: used to express very large or very small numbers.
Any number will be between 1 and 10,  multiplied by a power of 10.

Ex/ 3489=3.489×103 When you move decimal to the left - positive exponent (examples: 106)
    0.3489=3.489×10-2

When move decimal to the right - negative exponent  (example: 10-4)


Ex/ 465          4.65 x 102

                    = 465
 3489=3.489
0.3489=3.489                    =4.65 x 10-2
                                                        
                    = 0.0465


Adding / Subtracting
When adding or subtracting, change the scientifc notations into standard form and add or subtract
                       ( 5 x 102 ) + ( 1 x 103 )
                    = 500 + 1000
                    = 1500
Then, change the number back into scientific notation
                    = 1.5 x 103

Or, change the power of 10 so that they are the same and add or subtract the number (between 1-10) and keep the power of 10 the same

Example: (7×106) + (3×105)
              = (7×106) + (0.3×106)
              = 7.3×106
Multiplying / Dividing
Multiply or divide the number between 1-10 first, then multiply or divide the power of 10 
                   
                       
( 2 x 103÷(8 x 102 )
                    =  2÷8= 0.25
                    =  103÷102
                    =  0.25×101
                    =  2.5



Rounding: Avoid rounding in the middle of a question. Round ONLY at the final answer.

Scientific Notation on Calculator
If we want to express 2×106 on the calculator, then we can press 2 then the EXP or ×10x button and then 6. This button will save time and avoid making mistakes.

Matter
Matter is anything that has mass and occupies space.

This is a simple matter chart to show the different sub-categories of matter.

Pure Substances:
Here is the chart in more detail about pure substances
 Examples of elements include metals, non-metals, and metalloids.
 Ionic and covalent compounds fall are also examples of pure substances

Mixtures:




Examples of homogeneous mixtures: milk (colloid), oil, or coffee
Examples of heterogeneous mixtures: granola bar (mechanical mixture), chicken soup, or chocolate chip cookies 


Sep 20, 2011

Two Step Unit Conversions


Two Step Conversions:
For conversions that skip the base unit, convert to the 100 prefix first.
Example: Convert 0.112km to cm = 0.112km×1000m/km×100cm/m = 0.112×1000×100cm
The kilometers and meters cancel each other out and so it becomes 11200cm
0.112km= 11200cm or 1.12×104cm
By including units in the calculations, the conversion factors set up nicely so that they cancel each other out as they multiply.
Do not put the same units on the numerator or denominator because they will not cancel
Example: Convert 12cm into meters
12cm×100cm/1m
The above is wrong because this would get you 1200cm2                          

Derived Quantity Conversions:
Derived quantity is a quantity that has more than one SI base unit
Examples: m/s or cm2
To convert derived quantities: Convert one unit first, and then the other
Example: Convert 150m/s into km/h
150m/s×1km/1000m×3600s/1h =  (150×3600)/1000 = 540km/hour

Now let's look at some funny unit conversion jokes!
1. 52 cards = 1 decacards
2. How much time do you have between slipping on a peel and smacking on the pavement?
    1 bananosecond
3. 453.6 graham crackers = 1 pound cake
4. 2,000 pounds of Chinese soup = Won ton

We will end with a video that teaches about multiple step conversions.



Sep 16, 2011

Quantities and Unit Conversions


l  Any measurement is always a multiple of some basic units.

(Ex. 5g = 1g × 5 ... 5g is a multiple of 1g)

l  Measurements can be described in a different unit.

(Ex. 1km = 1000m = 100000cm)



Quantities

Measurements have two parts- the number and the unit. Number and unit together= quantity. In Canada, we use SI (Système International) unit system to describe a measurement.


l SI System

 SI system is a French system, that dates back to the early 1800`s using power of 10.


lSI Base Units

<><><><><><><><><><><><><><><><><> 

Measurement
Unit
Abbreviation
length
metre
m
time
second
s
mass
gram
g
amount of substance
mole
mol
luminous intensity
candela
cd
temperature
Kelvin
K
electric current
ampere
A



Conversions

When converting the two units, use “MAGIC ONE”!!!

l  Big unit to small unit :

(original measurement+its unit)x
(power of 10 for measurement+ unit converting to)/1+its unit

l  Ex. Converting 2Gg to g
  

  2Gg×109g/1Gg = 2×109g


l  Small unit to big unit:

(original measurement+its unit)x(1+unit converting into)/(power of 10 for measurement+original unit

l  Ex. Converting 2ns to s

2ns×1s/109ns= 2×10-9s



Here is a video that talks more about measurements!




Sep 12, 2011

WHMIS and Safety Lab Rules

WHMIS labels will help identify the product and alert users of the hazards, and how to properly use the product.
The Material Safety Data Sheet will provide more information about each dangerous substance.
The label will include:
l Name of chemical
l The WHMIS hazard symbols
l Risks and precautions
l First aid instructions
l Supplier’s name and address
l Reference to the matching Material Safety Data Sheet

Labels and hazards
Class A- Compressed Gas
Compressed gases are hazardous because they are under high pressure and the gas itself can be hazardous too. The bottle may explode if it is dropped or hit strongly.
These containers should be kept away from heat and store in designated areas.
Examples of compressed gas: steel cylinders of ethylene oxide, propane, oxygen, etc.

Class B- Flammable and Combustible Materials
These are items that will burn at a low temperature (Flammable = >37.8 degrees Celsius and Combustible = between 37.8 – 93.3 degrees Celsius).
If these materials come into contact with water or air, it could also cause them to burn.
Sub divisions:
Division 1: Flammable Gas – hydrogen, methane
Division 2: Flammable Liquid – gasoline, ethanol, methanol
Division 3: Combustible Liquid – diesel fuel
Division 4: Flammable Solid – sodium, magnesium
Division 5: Flammable Aerosol – butane, propane
Division 6: Reactive Flammable Material – lithium (in air), sodium (in water)



Class C- Oxidizing Materials
Has a risk of fire or explosion when near flammable and combustible material.
Wear protective equipment when handling these items.
Examples: Hydrogen peroxide, bleach

                                       
 Class D- Poisonous and Infectious Material
These materials have are poisonous and could be fatal. It can also cause permanent damage if inhaled, swallowed or absorbed through skin.
Division 1: Immediate and Serious Toxic Effects
Contain materials that can have immediate impact on life and health
Examples: Formaldehyde, carbon monoxide, cyanide






Division 2: Other Toxic Effects
These materials are poisonous but will not cause immediate damages. Repeated exposure can result in death or permanent damage.
 Examples: Examples: Asbestos, lead, mercury




Division 3: Biohazardous Infectious Material
Organisms like bacteria and viruses and toxins that may cause diseases fall under this category.
Examples: salmonella, AIDS virus,






Class E: Corrosive Material
Acids or caustic materials that will corrode metal and eat through skin are corrosive materials.
Examples: household cleaners, sulfuric acid, hydrogen chloride






Class F: Dangerous Reactive Materials
These substances will react dangerous when heated, pressured, or come into contact with water.
Examples: Ethylene oxide, ozone
International Safety Symbols:

International Safety Symbol

An octagon represents DANGER and indicates very harmful substances
A diamond means a moderate level of danger or “warning.”
A triangle indicates caution and represents the least dangerous materials.

Safety Rules For Labs:
l  Do not begin the experiment without the teachers permission
l Read instructions carefully and make sure you understand everything before starting the experiment
l Always wear safety goggles and keep them on at all times
l Do not eat or drink in the lab
l Waft substances to smell them, don’t inhale
l Report spills and other injuries to teacher
l Make sure hands are dry when handling electric materials
l Always wash hands after the experiment and clean up

What to do with Injuries:
Burns – run under cold water for 15 minutes
Cuts – put pressure on cut
Faints – keep the person lying down
Chemicals in eye – Wash with running water for 15 minutes
Poisoning – identify the poison
Chemical on skin – wash in water for 15 minutes