Molar Volume

 STP?

• standard temperature (0°C) or (273.15 k) and pressure (1 atmosphere)  
• where one mole of gas occupies 22.4L 

Molar Volume?

• the volume occupied by one mole of gas

 How to find Molar Volume

Conversion from Moles to Molar Volume

Conversion from Molar Volume to Moles

Isn't that a simple task!?

Here is an online worksheet with some questions! don't look at the answers before you're finished so you can challenge yourself! (:

Molar Volume worksheet!

Do questions 6, 9, 10, 11 and 12

Here's a game you can play with Molar Volume!

FUN GAME! (:

Molar Mass

• The mass (grams) of 1 mole of a substance is called the molar mass
• It can be determined from the atomic mass on the periodic table
• Measured in g/mol

So what exactly is Molar Mass? 
 Molar mass is the atomic weight of an element expressed in grams is the mass of 1 mole of element.


How do you determine Molar Mass in a Compound?
To determine the molar mass of a compound you must ADD all the mass of the atoms together

Here's an explanation that will help you understand what Molar mass is:
 Follow these steps to find molar mass! What is the molar mass of H20? (water)

1. Identify how many atoms of each of the elements are in the chemical formula. In the example there are 2 atoms of Hydrogen and there is 1 atom of Oxygen.
2. Look at the periodic table and search for the elements given & then look at each of their atomic masses. The elements in H20 are Hydrogen and Oxygen. The atomic mass for Hydrogen is 1.0 amu and the atomic mass for Oxygen is 16.0 amu
3. Now multiply the number of atoms found in the chemical formula with the atomic mass.                        2 atoms of Hydrogen --->2(1.0) + 1atom of Oxygen-----> 16.0= 18.0 g/mol

So now that you have a basic foundation of what Molar Mass is now its YOUR TURN to do some practice problems! Answers will be provided at the bottom of the last question. ( but don't look straight into the answers you need to TRY some problems and then check if u understand it)  :)

• What is the molar mass of NO2?

• What is the molar mass of NaCl?

• What is the molar mass of FeO?

• What is the molar mass of NaNO3?

Answers:
NO2: 14.0 + 2(16.0)= 142.1 g/mol
NaCl: 23.0 + 35.5= 58.5 g/mol
FeO: 55.8 + 16.0= 71.8 g/mol
NaNO3: 23.0 + 14.0 + 3|(16.0)= 85 g/mol


Mole Conversions
To convert between moles & mass we use molar mass as the conversion factor. You must also be sure to cancel the appropriate units.

Here's an example: How many grams is there in 1.5 mol of 02?


1.5 Mol x     32.0   g   = 48.0 g
                     1 mol

Now you TRY!

How many moles are there in 115g of Fe203?


A sample of HCL contains 0.54 mol. How many grams of HCl is this?

Avagadro's Number and the Mole:

As we know, atoms and molecules are extremely small and microscopic objects contain too many of them to count or weigh individually. 

However, Amedeo Avogadro proposed a solution to this problem...

• the # of atoms in 12.00000 g of Carbon would be equal to a constant (this is = to 1 mole of carbon).
• this value is now called Avagadro's # and forms the basis of all quantitative chemistry

 So what is Avagadro's #?

1 Mole = 6.02 x 10^23


But What's a Mole?  

A mole is simply a multiple of things  

• 1 pair = 2
• 1 dozen = 12
• 1 century = 100  years
• So... 1 mole = 6.02 x 10^23              

How Big is a Mole?

• 1 mole of meters would cross the entire galaxy!
• $mole would be enough to give every person on earth 1 million billion dollars

You can also identify 1 mole as 602 000 000 000 000 000 000 000... 

                                                                             
Particle                                                                 
Atom:         Element            6.02 x 10^23
                                                 1 mole        Fe     
Molecule:   Covalent           6.02 x 10^23
                   Compound            1 mole        CO2  
Formula      Ionic                6.02 x 10^23
Unit:           Compound            1 mole        NaCl 

^ Example of using the mole:

• A sample of Carbon contains 3.78 x 10^24 atoms.  How many moles of carbon is this?

1. 3.78 x 10^24 atoms x 1 mole / 6.02 x 10^23 atoms
2. 3.78 x 10^24 / 6.02 x 10^23 (when doing this equation on your calculator you want to press "2nd ," which gives you EE.  This replaces the 10 and gives you a more precise answer)
3. this equation cancels out the unit atoms leaving us with the amount of moles...
4. thus your final answer is 6.28 moles

Another Example:

• Say you have 15.25 moles in a compound.  But you want to know the amount of molecules in the substance.  How would you solve this problem? 

1. 15.25 moles x 6.02 x 10^23/ 1 mole 

• But how did we figure our the ratio of molecules to moles?  You look at the chart above the first example!  Simple as that.  

    2.  15.25 moles x (6.02 x 10^23)... don't forget to use the "2nd ," instead of "x 10"
    3.  this equation cancels out the unit for moles and leaves you with the amount of molecules in the 
         substance 
    4.  your final answer is 9.1805 x 10^24 molecules 

Molecular Compounds

Naming Molecular Compounds

• Use the 1st name of the element
• 2 elements end in -ide
• 1 atom usually does not have a prefix. NO---> Nitrogen monoxide
• Hydrogen does not get a prefix

* Also be aware of the Latin prefixes. They are very important!!

Heres a link to a Molecular Compound Worksheet :)

thttp://www.docstoc.com/docs/2786822/Binary-Molecular-Compounds-Worksheet-1

Acids and Bases

Terms:

Acid:A solution that has an excess of H- ions. It comes from the Latin word acidus that means "sharp" or "sour". 

Base: A solution that has an excess of OH- ions. Another word for base is alkali

Acids & Bases have different properties...

Classical Names:

• Ferr- Iron
• Cupp-Copper
• Mercur-Mercury
• Stann- Tin
• Aunn- Gold
• Plumb- Lead

Naming acids
 *use the suffix- ic & or the prefix hydro
*Hydrogen appears first in the formula unless it is part of a polyatomic group

ex: sulfuric acid

      hydrochloric acid

• Hydrogen Compounds are acids
• HCl---->Hydrochloric acid

*IUPAC system was the aqeuous hydrogen compound

                                           Acids/ Bases to memorize

Naming Bases

*Use the cation name followed by hydroxide
- Sodium Hydroxide
- Barium Hydroxide

E.g: HI---> Iodic acid
       HBR---> Hydrobromic acid
       HOOCCOOH---> Oxalic acid

Here's a video that nay help you in Naming acids and Bases

            Hydrates

• These crystals contain water inside them which can be released by heating.

        Naming Hydrates

*These easy steps will help you ensure you get Hydrates right

1. Write the name of the chemical formula

2. ADD the prefix & # of water molecules

3. After the prefix add the hydrate

Here are some examples:

gfsgag

Electron Dot Diagrams

• The nucleus is represented by the atomic symbol
• For individual elements, you have to determine the number of valence electrons, which are represented by the dots around the atomic symbol
• To find the number of valence electrons is simple, look at the group number the element is in and that shows you the number of valence electrons
• There are four orbitals on each side of the nucleus holding a maximum of two electrons
• Each orbital gets 1 electron before they pair up, making a lone pair

 

Here are some examples of electron dot diagrams for sodium, magnesium and chlorine

Lewis diagrams for compounds and ions

• In covalent compounds, electrons are shared

Follow these two easy steps and learn how to draw a Lewis diagram for compounds and ions

1.       Determine the number of valence electrons for each atom in the molecule, which I explained above

2.       Place atoms so that valence electrons are shared to fill each orbital

This example shows the Lewis diagram for NF3

Double and triple bonds

Helpful Hint: Sometimes the only way covalent compounds can fill all their valence levels is if they share more than one electron

Lewis diagrams: Ionic compounds

• In ionic compounds electron transfer from one element to another
• Determine the number of valence electrons on the cation. Move these to the anion
• Draw [ ] around the metal and the non-metal
• Write the charges outside the brackets

Trends On the Periodic Table

Elements close to each other on the periodic table display similar characteristics.
- There are SEVEN important periodic trends:
1) Reactivity
2) Ion Charge
3) Melting point
4) Atomic Radius
5) Ionization Energy
6) Electronegativity
7) Density
We will only be talking about the first 6, today!

REACTIVITY:

•  metals and non-metals show different trends.
•  the most reactive metal is Francium; the most reactive non-metal is fluorine.

ION CHARGE:

• Elements ion charges depend on their group (column).

MELTING POINT:

• elements in the center of the table of the highest melting point.
• noble gases have the lowest melting points.
• starting from the left to right, melting point increases, until the middle
• carbon is an exception!

ATOMIC RADIUS:

• radius decreases to the up and the right.
• helium has the smallest atomic radius.
• Francium has the largest atomic radius.

IONIZATION ENERGY:

• ionization energy is the energy needed to completely remove an electron from an atom.
• it increases going up and to the right.
• all noble gases have high ionization energy.
• helium has the highest ionization energy.
• francium has the lowest ionization energy.
• opposite trend from atomic radius.

ELECTRONEGATIVITY:

• refers to how much atoms want to gain elections.
• same trend as ionization energy.

Isotopes & Atoms

Scientists discovered that an atom contains 3 fundamental particles: Protons, neutrons, & electrons. All atoms of a given element are identical because they have they same number of protons & electrons. However, it does not mean that all atoms have the same number of neutrons.

   

Since all elements have different properties, scientists refer to the periodic table





 Each element is listed in squares in the periodic table which provides information about a particular element. Scientists know where to specifically look when they are trying to identify an element.







Scientists look for:
A= Atomic # (protons & electrons)
B=Ion charges
C= Abbreviation of element
D=Element
 E=Atomic mass

The only subatomic particle that does not appear on the Periodic Table is the Neutron. But it's no big deal since the Neutron can be easily found by using this simple formula. Atomic mass- Atomic Number = # of Neutrons.


And since ATOMS do NOT have the same number of Neutrons they are called Isotopes. Hydrogen has isotopes...



Same with Lithium...


Mass Spectrometers are used to determine the abundance & mass if the isotopes of elements.
 Or you can simply just use the formula:  mass x abundance = atomic mass. THIS video will give a Clear understanding of how to find atomic masses. Enjoy!

Quantum Mechanics

Bohr Theory

• The electron is a particle that must be in orbital in the atom

Quantum Theory

• The electron is the cloud of negative charge in a wave function
• Orbitals are areas in 3D space where the electrons most probably are
• The energy of the electrons is in it's vibrational nodes
• Photons are produced when high energy modes change into lower energy modes

Determining an elements chemical properties is it's electron configuration, particularly the valence shell electrons. The type of orbital the atom's outermost electrons reside determines the 'block' and the number of valence shell electrons determine the 'group'.

The total number of electron shells detemines the period it belongs and each shell is divided into sub-shells

Subshell:	S	G	F	D	P
Period
1	1s
2	2s				2p
3	3s				3p
4	4s			3d	4p
5	5s			4d	5p
6	6s		4f	5d	6p
7	7s		5f	6d	7p
8	8s	5g	6f	7d	8p

Through a group of lightest element to heaviest element, the outer shell electrons are all in the same orbital, with a very similar shape, but increasingly higher energy and distance from the nucleus. The outer shell, for instance, all have one electron in an s-orbital. In hydrogen, the s-orbital is the lowest possible energy state of any atom, the first.



 The different regions of the atomic table are named according to the sub-shell in which the last electron is...

S-Orbital
- Each Orbital holds two electrons
- Spherically symmetric around the nucleus
- Only has one orbital

P-Orbital
- There are 3 sub-orbitals
- Each Orbital contain 2 electrons
- In total, there are 6 electrons

D-Orbital
- There are 5 sub-orbitals
- Each orbital contains 2 electrons
- In total, there are 20 electrons

F-Orbital
- There are 7 sub-orbitals
- Each contain 2 electrons
-In total, there are 14 electrons

Here's a really helpful video to help understand electron configuration

Lets see if you can do some! (:

1. What is the electronic configuration for nickel?
2. What is the electronic configuration for Gold?
3 What is the electronic configuration for Zinc?

Answers
1. 1s2 2s2 2p6 3s2 3p6 3d8 4s2
2. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s1 4f14 5d10
3. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰

Bohr's Model

The Bohr model: was introduced my Neils Bohr in 1913. He introduced that surronding the positively charged nucleus was electrons. His idea is somewhat similar to the solar system with the exception that electrostatic forces provide attraction not gravity. At some point Bohr and Rutherford's models were "combined" since Bohr's model is like a quantum physics based modification of Rutherford's model; people called it the "Bohr-Rutherford model. "

-Rutherford's model was inherently unstable

• Protons and Electrons should attract eachother

-Matter emits light when it is heated (backbody radiation)

•   Light travels as a photon

 . Energy photons carry depends on their wavelength
   e.g: radio stations such as the beat 94.5 <---- the 94.5 actually represents frequency radio waves
         (FM has more energy than AM)

These lines in the emission spectrum are unique set of lines for each element. Each line represents a Photon of light emitted from the excited atom. Bohr based his model on the energy (light) emitted by different atoms. Each atom has a specific spectra of light. To explain this emission spectra, he suggested that electrons occupy Shells or Orbitals

Bohr's Theory

- Electrons exist in orbits
- when they absorb energy they move to a higher orbital
- As they fall from a higher orbital to a lower one they release energy as a photon of light.


Here is an educational video that explains a bit more about Bohr's theory. :)

Chaper 1 Chemistry test!

Today in Chemistry 11, we had a test on Chapter 1 and it was great! (:

Atomic Theories

Today in Chem 11, we had an in depth lesson on something we learnt about in grade 10, Atomic theories!

There are many people, concepts and features that are important to know when learning Atomic theories, so here are a few important ones to learn:

Four Element Theory (Arostotal)
- Matter is made up of water, wind, earth and fire
- This theory of Arototal's lasted for 2000 years!
- But, isn't a scientific theory because is couldn't be tested against observation

Democritus (4000 BC)
- First mentioned Atoms, and said they were indivisible partices
- This theory was not a testable one though, it was a conceptional one
- There were not any mention of atomic neucleus or it constituients and can't be used to explain chemical reactions

Lavoiser (Late 1700's)
- Introduced the law of conservation of mass and the law of definite proportions
- Water is always 11 % Hydrogen and 89 % Oxygen

Proust (1799)
- Claimed that if a compound is broken down into it's constituients, the products exist in the same ratio as in the compound

Dalton (Early 1800's)
- Aoms are solid, indestructable spheres, just like billiard balls!
- Provides for differet elements
- Explains chemical reactions
- Does not explain isotopes, electricity, attraction, compulsion, etc..

JJ Thompson (1850's)
- Proposed the raisin bun model
- Solid, positive spheres with negative particles embedded in them
- First atomic theory to have positive (protons) and negative (electrons) charges
- Demonstrated existance of electrons using cathode ray tubes

Rutherford (1905)
- Showed that atoms have a positive, dense, centre with electrons outside it which resulted in a planetary model
- Suggested that atoms are mostly empty space

Density & Graphing

What is Density?

• The Density of an object is it's mass divided by it's volume 

Ex.  d = m/v (density = mass in kg divided by volume in L)

• Is usually expressed in Kg/L, Kg/m^3, or g/cm^3

Ex.  135Kg/65L = 2.077 ~ 2.01
                           = 2.01 Kg/L

Well, what about Graphing...? 

Graphing is pretty straight forward but we need to remember 5 very important things when faced with the task of putting one together:

1. Label axis' 
2. Create an appropreate scale
3. Don't forget the title!
4. Plot the data points
5. And finally use a line of best fit

• Three things can be done when working with a graphs.  #1, reading the graph.  #2, finding the slope.  #3, Finding the best fit line. 

Here's a video that will give you a good idea of what graphing in physics 11 is all about :)  

What's good about that video is that it gives you information about how to find slope AND area.  But just to recap...

Slope = Rise / Run or Y2-Y1 / X2-X1
Area of a triangle =1/2 (bh)
Area of a rectangle = l x w
 

WHAT is Dimensional Analysis!?

Dimensional Analysis: is the technique of converting between units! There are only 4 basic steps to solving a problem using Dimensional Analysis
Steps:

• Find the unit equality
• Find the conversion factor
• Apply conversion factor
• Cancel units    

Now FOLLOW these easy steps to solve the problems. Here are step-by-step examples :)

• How many inches are in 250 centimeters?

                1 in= 2.54cm

         d= 250cm x   1 in   
                              2.54cm
    
         d= 98.4 in

• How many dollars is E35.00? 

                   1E=$1.4

       35E x $   1.4  =$49.00

                       1

• What is 100 km/h in miles/hour?                 

     100  km   x   1mi    = 62.5 mi/h

               h        1.6km

If u still don't understand this concept... Here's a quick video that will show how to do Dimensional Analysis..  :)

Unit Equality is also very important... Unit equality is the starting point for solving the problem. A unit equality is an equation that shows how different units are related.

Significant Digits and Scientific Notation

In our last Chem 11 class, we learnt about Significant Digits and Scientific Notation!

The concept of significant digits and scientific notation is pretty simple to grasp, so here are a few notes for you

A Significant Digit is a digit in a measurement that is certain, plus one digit that is an estimate

• Here's an example, there are three significant digits in the number 34.5. Two of which are certain, 3 and 4; and one which is estimated, 5.

When trying to tell how many digits are significant, remember when a zero is not significant. place holder zeroes in a measurement are not significant

• An example is 1040, how many significant digits are there? Well, to start off the 1 and the 0 are are exact and the 4 is an estimation. Therefore, there are only three significant digits. The final zero is a place holder zero and isn't significant.

When we add or subtract numbers, we determine the number of significant digits by depending on the number with the largest uncertianty

• Here's an example,  951.0 + 1407 + 23.911 + 158.18 = 2540., the decimal place is there to show that the final zero is not a place holder, but significant.

When we multiply or divide two numbers, we determine the number of significant digits by choosing the smallest number in the equation.

• An example is, 3.052 x 2.10 x 0.75 = 4.8, which means that there are two significant digits and we only use two digits because the smallest number of significant digits in the equation is 2.

Scientists have developed a shorter method of experssing large numbers, this method is called scientific notation, which is based on powers of the base number 10

The number 123, 000,000,000 is written as 1.23 x 10^11

Writing a number in scientific notation is easy!

Put the decimal after the first digit and drop the zeros. To find the exponent count the number of places from the decimal to the end of the number

So, in 123,000,000,000 there are 11 places after the decimal place which determines the exponent, which is 11.

That wasnt so hard, now was it?

Try out some examples to perfect your knowledge of Significant digits and Scientific Notation
Scientific Notation
6.34 x 10^5 =
4.89 x 10^-6 =
Significant Digits
0.0026701 =
19.0550 =

to end off the lesson, heres a mind boggling video on the relative size of things in the universe. (:

  

Uncertainty in Measurements

As a recap form the previous lesson "Mixtures" There are many methods to seperate mixtures, depending on the type of mixture.
  - By hand
  - Filtration <------ heterogeneous mixtures only
  - Distillation
  - Crystallization
  - Chromatography

Here is an example of the process filtration ^

Now something new we learned last class was uncertainty in measurements. Here are some few notes:

Accuracy: Degree of closeness of measurements
Precision:  Repeated measurements that show the same results

The image of a dartboard is an excellent example of both Accuracy and Precision.

 Measurements are uncertain for 2 reasons: Measuring instruments are never completely free of flaws & measuring always involves some estimation. We use a plus or minus symbol like this one ----> ±

to show uncertainty of a measurement. 

There is also a metric system called International System of Units, abbreviated SI (after the French System International d'Unites) which had streamlined at an international conference in 1960. The SI is built upon a set of 7 metric units, which are called base units of the SI

But the base SI units are not always convenient to use. There is a convenient way of writing the measurement by using the metric prefix. Metric prefixes are attached to the base unit.

 

 A very important note from the lesson was Percent Error.

 Error as you all may know is an inescapable part of science. One may think that error is a BAD thing in an experiment but it is actually wrong!! In many ways Scientists need error in an experiment in order for the experiment to be succesful. Successful?!? How can this be you may ask well... Error actually helps scientists with experiments because when an experiment ends up not functioning properly, scientists can learn from their mistakes of the FAIL experiment and new measures can be taken up to improve the mistakes.

Here is the equation:

Percent error= measure value-accepted value

                         ------------------------------------     x 100=

                                  accepted value

Classification of Matter:

Yesterday in Chem11 we learned about the classifications of Matter...

Here are some notes

We can divide matter into two main types of Substances:

 Homogeneous
- One type of substance that we can see (ex. Distilled Water, Milk, Oxygen, Graphite)

Heterogeneous
- Contains more than one visible component (ex. Sand, Blood, Granite, Chocolate chip cookie)

Below is a chart that helps describe how Matter is classified:

From the branch "Homogeneous Substances" comes two other branches.  

1. The first is labeled Pure Substances. There are 2 types of pure substances...

•  Elements - substances that cannot be broken down into simpler substances by chemical reactions (ex. Oxygen, Iron, Magnesium).
• Compounds - Substances that are made up of 2 or more elements and can be changed into elements (or other compounds) by chemical reactions (ex. Sugar, Water).

* How do you tell the difference?  

• Often VERY difficult to tell the difference between Elements and Compounds (their differences are only 'visible' on the atomic level). 
• However you can use Electrolysis to help you.  

Pretty cool right?! :)

     2.  The second branch is labeled Homogeneous Mixtures. 

• in Homogeneous Mixtures, the different parts are not visible. 
• a Solution is a homogeneous mixture of 2 or more substances.
• Solutions usually involve liquids but don't necessarily have to (ex. Fog, Steel). 
• The component of a solution which is present in greater amount is the Solvent (Water = most common solvent). 

On the other side of the diagram is the category "Heterogeneous Substances" which links the last branch. 

1. The last branch we talked about was called Mechanical Mixtures.  We didn't go into too much detail about it but it's basically this...

•  a mixture whose components can be separated by mechanical means.

This leads us to our last topic which is Separating Mixtures.   There are many ways to do this but it depends on the type of mixture.  For example, Filtration is used for Heterogeneous mixtures only.  The other four listed in our notes are "by hand, distillation, crystallization, and chromatography.  All of these are 'Physical Changes.'

Here's a video on some of the different ways you can separate mixtures:

 Have a great day!

Physcial or Chemical Change?

For many of us Physical and Chemical Changes were just a review of what we learned from grade 8, 9 & 10...but for some of us who don't, Physical and Chemical Changes are easier than you may actually think!
Here are some key notes from Mr. Doktor that will give you ideas and insight on what Physical and Chemical Changes are all about:

 

Physical Change:

- Involves changing shape or a state of matter
    Examples: Crushing, Tearing, etc..

- No new substances are formed
    Examples: Cutting wood, Boiling water, etc...

Chemical Change:

- New substances are formed
- Properties of the matter changes

    - Conductivity, Audicity, Colour, etc...
      Examples: Iron rusting, Burning wood,
                        Digesting food

Now that you are a bit familiar with Chemical & Physical Changes, can you identify some of the things in this video that is either chemical or physical?

We also did some review on writing and balancing chemical equations

Here are some examples, try them!

1. A solution of aluminum chloride, carbon dioxide and water can be prepared mixing pure aluminum carbonate with a solution of hydrochloric acid

2. Write a balanced equation for the reaction of aqueous barium hydroxide neutralizing a solution of phosphoric acid if solid baruim phosphate and water are produced

To finish off, here's a funny video for you to watch but NEVER try at home

 

Word Equations & Balancing

Yesterday, we learned about Word Equations & Balancing in chem11.  However, because we were already taught this topic throughout Science 10 (last year), it was a review for most of us.  But it was still a much needed review and the class was really thankful to get some practice in before going on to the "real" topics of chem11! Here are some helpful notes and reminders that Mr. Doktor gave us that day...

Phase Symbols: they indicate the phase of a chemical.  So they are either solid (s), liquid (l), gas (g), or an aqueous solution which means dissolved in water (aq).

Chemical Equations from Word Equations:  the main objective of this class was to learn how to understand the meaning of chemical equations, to change chemical equations into words, and finally to balance them!  So, we were reminded of the diatomic seven (H, N, O, F, Cl, Br, and I) which all end with the subscript 2 when placed alone in a chemical reaction.  Another good trick to remember them is that the start at the atomic # 7 and form the shape of a seven when you look at them on the periodic table, minus hydrogen.  Also, we similarly learned about the polyatomic molecules found on the periodic table which are P with the subscript 4, and S with the subscript 8.  The final thing that we got from that section of notes was that in chem11, a solution means something is dissolved in water.  Therefore the phase is aqueous.  

After we wrote down those notes, we immediately got into practicing!  We went over basic balancing and analyzing word equations until the very end of the class.  We were also given some more homework to do at home regarding balancing and word equations from our textbook.  SO, over all Tuesday was a very productive day for Mr. Doktor's chem11 students! 

Here's a helpful video on the basics of Balancing:

Have a great day! :D

First day of survival! Safety TIPS

Today's topic was Safety; to start off the class we went into groups and discussed things that could be hazardous in a science class when doing an experiment. After listening to the other group's ideas we split into groups of 3 or 4 and had to look inside Lab drawers to see if we could find any lab equipment from a previous handout. Given that it was Friday the classes were shortened so for homework we had to find out what each WHMIS symbol meant. For fun and lab safety tips we watched a FUNNY lab safety video :)

                                                              
Here are 10 smart safety tips we learned from the funny video and from our text book:

1. Wear the proper safety equipment
2. Don't forget to tie long hair back!
3. If something bad/dangerous happens, warn your teacher imediately
4. No open toed shoes
5. No horseplay
6. Listen to the teacher's instructions and follow them very carefully
7. Don't mix chemicals unless asked to do so
8. Waft, don't inhale
9. Don't ever leave an open flame
10. Know the locations of the safety materials in your lab

If you'd like to watch the video yourself here's the link ^

Welcome!

We hope that you will find this blog informative and learn to enjoy Chemistry 11! (: