Heating and Cooling Curve of a Pure Substance

• Solid-closely packed in an orderly manner-strong bonds, vibrates at a fixed position.
• Heat energy converts to kinetic energy (K.E.) K.E. goes up, vibrate a little faster, temperature goes higher.
• Solid to liquid-temperature remains constant because heat is used to overcome forces of attracton that hold the particles together-melting point-heat released is called latent heat of fusion.
• Liquid (All solid has melted)
• Temperature goes higher, particles move faster, K.E. up.
• Some molecules start to move freely. Starts changing from liquid to gas.
• Liquid to gas.Temperature stays same. Heat is used to overcome the forces of attraction that hold the particles together. Boiling point.
• Particles move faster -Temperature increase as heating continues.

Gas Particles have high energy, move quickly.
Vaperization: KE down, particles are getting closer together.
Start to form intermolecular bonds
condensation begins
liquid satrts to form
Freezing; particles arranged in an ofdered manner. Freezing point.
Solid.


Liquid to solid: Freezing
Solid to liquid: Melting
Solid to gas: Sublimation
Gas to solid: Deposition
Liquid to gas: Vaperization
Gas to liquid: Condensation

Separation Techniques

Separating Mixtures

• Basis for separation: different components and different properties.
• Strategy: Create a process that distinguishes between components with different properties.
  high/ low density polar/ non polar

Separation

• Components in the mixture retain their identities.
• The more similar the properties, the more difficult it is to separate them.

Basic Techniques

• Filtration
• Floatation
• Crystallization and Extraction
• Distillation
• Chromatography

Hand Separation

• Mechanical mixture/ heterogeneous mixture can be separated by using a magnet or sieve.

Evaporation

• Boil away the liquid and the solid remains

Filtration

• Mixture passes through a porous filter.
• Residue left in filter paper and filtrate goes through filter paper.

Crystallization

• Aspect of precipitation.
• Solids are separated by filtration or floatation.
• Saturated solution of desired solid
• Evaporate cool -> solid -> crystal (pure).
• Crystals are then filtered

Gravity Separation

• Centrifoge (machine that separates mixtures) whirls test tube around at high speed forcing denswer materials at the bottom.

Solvent Extraction

• Mechanical mixture - use liquid to dissolve a solid but not the other so the desired solid is left behind or dissolved.
• Solution - Solvent = insoluble with solvent already present

Distillation

• Heating mixture can cause low boiling component to vapourize.
• Then collect and condense vapourized components.

Chromatography

• Mixture flows over material that attracts some components more than the others, so different components flow over the material at different speeds.
• A mobile phase sweeps sample over a stationary phase.

Sheet Chromatography (Paper chromatography)

• Stationary phase is liquid soaked into sheet or strip of paper.
• Components appear as separate spots.

Thin layer chromatography (TLC)

• Stationary phase = thin layer of absorbent coating a sheet of plastic or glass.
• Some components attract to absorbent strongly; others weakly.

Scientific Notation

Definition: To express any large or small number.

In scientific notation, any number will be between 1 and 10 and multiplied by a number of 10.

Adding and Subtracting

In order to add and subtract using scientific notation, solve the equation first and then change to scientific notation.

32000+ 4000= 36000 (change to number)
= 3.6 x 10^4 (change to scientific notation)

Multiplying and Dividing

In order to multiply and divide,

1. Use the law of exponents.
2. Combine the "like" terms.

Rounding - Avoid rounding in the middle of the question. Round only at the final answer.


(3.2 x 10^2)(2.0 x 10^3) = 6.4(multiply) x 10^5(law of exponents.

Matter

• Matter : Anything that has a mass and takes up space
• Mass : A property of matter that causes it to have weight, mass measures the resistance of an object to a change in its state of motion

PROPERTY :
Matter includes 3 states :

Solid

Liquid

Gas

There are 2 kinds of matter:

I. MIXTURE

1. More than one set of property
2. Physically combined
3. More than 1 kind of substance
- Homogeneous

+ Uniform throughout

+ Appears to have only one component

* Solution

*Colloid

- Heterogeneous

+ Non uniform

+ Have more than 1 component

* Suspension

* Mechanical mixture

II. Pure substances

1. 1 set of property

2. 1 kind of particle

- Element

+ Simplest form of metal

+ Can't be decomposed

+ Made up of atoms :

* Metals

* Metalloids

* Non-metals

- Compound

+ Made up of element

+ Smallest particle is called a molecule

* Covalent ( between 2 non metal )

* Ionic ( between metal and non metal )

Quantities and Unit Conversions

All measurements are always a multiple of some basic unit.

Quantities

• There are 2 parts in measurements: the number and the unit.
• The number + the unit = quantities.
• SI (Systeme Internationale) - a French system that uses powers of 10.

SI Base Units

Conversions

• Use the "magic one" to convert between units.

EXAMPLE:

5cm x (1m/ 100cm) = 0.05m

Note: You need to keep track of what you're doing. Don't skip steps because that may lead to careless mistakes.

SI Prefixes and Conversion factors

On a test, this chart will not be provided.

WHMIS

So, what's WHMIS?

WHMIS is Workplace Hazardous Materials Information System. WHMIS is used by students and workers to inform them (using special labels and symbols) of the safety and health hazards of the substance they're working with.

WHMIS LABELS

All products that students or workers work with MUST HAVE WHMIS labels. This label tells the handlers the name of the product, what hazards this product is responsible for and how to work with it. YOU MUST READ THE LABEL BEFORE USING THE PRODUCT.

WHMIS SYMBOLS

These symbols are separated into 7 classes; class A, B, C, D, E, F.

Class A
Compressed Gas

• Gas kept under pressure.
• Adding heat or dropping it may cause it to explode. You must handle it with care.
• If the gas itself is dangerous, it will have another hazard sign along with this sign.
• Examples are fire extinguishers, argon, neon, and etc.

Class B

Flammable and Combustible Materials

• The material is a potential fire hazard.
• It may burn at a relatively low temperature.
• May burst into flame spontaneously in air or release a flammable gas on contact with water.

Class C

Oxidizing Materials

• The material is a fire or explosion risk near flammable or combustible material. This can potentially burn theskin or eyes on contact.
• This material may not burn by itself, but it can release oxygen or other oxidizing gases which could have the potential of being flammable.

Class D

Poisonous and Infectious Material

• A potentially fatal poisonous substance.
• Can cause permanent damage if it in inhaled, ingested, or absorbed through skin.
• May burn skin or eyes on contact
• May burn skin or eyes on contact

Materials Causing other Toxic Effects

• The material is poisonous but not immediately dangerous to health.
• Repeated exposure may cause death or permanent damage.
• This includes materials that cause immediate irritation.

Biohazardous Infectious Material

• This includes any organisms and the toxins they may produce that believed to cause disease.

Class E

Corrosive Material

• Caustic or acid materials that can eat through the skin or corrode metals like aluminum or steel.
• This also includes corrosive gases, such as ammonia and the acids hydrogen fluoride.

Class F

Dangerously Reactive Material

• Products undergo dangerous reactions such as polymerization, decomposition, or condensation.
• Subject to heat, pressure, shock, or allowed to contact water.

 

Sources : http://www.youtube.com/watch?v=yclOrqEv7kw&feature=related

http://www.youtube.com/watch?v=qOGUjPn6764&feature=related

Test post for chemistry 11

hi chemistry is amazing