Oct. 9 – Review

Today we did an in class review to get ready for the test in the form of Jeopardy!

Here's a copy for you to play at home.  Try to answer all the questions to help you study.  The 1000 point questions are particularly challenging.

PowerPoint: Chemistry Review Jeopardy

Good luck in your studies!

Oct. 7 – Work Period

Today in Period 1 we had an anti-bullying assembly.  Here is a powerful video on the topic of bullying and how it affects people.

Video: To This Day Project - Shane Koyczan

Here's a live version where you can see the author reciting it in person.

Video: To This Day - Live version

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Then in class I handed back the Physical and Chemical Changes Investigation.  Have a look at TeachAssist for your updated marks.

Here are some notes on your responses:

• Clarity is either transparent, translucent or opaque.

• Dissolving is spelt D-I-S-S-O-L-V-I-N-G.  Breaking of a substance without affecting the particles.
  Wrong: the magnesium dissolved.
  Correct observation: I can no longer see the magnesium.
• Evaporation is a phase change from liquid to gass.
  Wrong: the magnesium evaporated.
  Correct observation: I can no longer see the magnesium.
• Both dissolving and evaporation are physical changes.

• "Cannot reverse" is not an observation.
• You can ONLY use your 5 senses to make observations.
• Use these observations to support "How do you know".

The rest of the period was for working on the element project and for studying.

Here are some review questions to help you study:

• Ch. 5, P. 202 #1, 2, 7, 10, 11, 12, 16, 17, 18, 19
• Ch. 6, P. 248 #1, 2, 4, 5, 6, 7, 10, 11, 13, 14, 19
• Ch. 7, P. 280 #1, 2, 3, 5, 6, 7, 8, 9

Oct. 4 – Naming Chemicals

Here are the solutions to yesterday's homework.

Here we go, the final topic before the test!

Naming compounds

Learning Goals: Understand the conventions in naming chemical compounds.

Success Criteria: Given the chemical formula for a certain compound, you can write down its chemical name.

Handout: Naming Compounds

There are a lot of rules, so take care in reading the handout carefully.

Element Project – Due Oct. 10

Handout: Element Project

In this project you will become an expert on one of the elements in the periodic table.  Use the handout as a guide to what information you should look for.  Then, once you've gather all the information, put it together into a pamphlet (or brochure) that describes that element.  You can do it by hand or typed, but make sure you print it if you use a computer.

Unit Test – Oct. 9

Handout: Topics to study

There will be no new topics between now and the unit test!  For those of you anxious to get started on studying, here are the relevant questions to try from each chapter:

Ch. 5, P. 202 #1, 2, 7, 10, 11, 12, 16, 17, 18, 19

Ch. 6, P. 248 #1, 2, 4, 5, 6, 7, 10, 11, 13, 14, 19

Ch. 7, P. 280 #1, 2, 3, 5, 6, 7, 8, 9

Oct. 3 – Ionic Formulas and Covalent Bonds

Learning Goals:

• Understand how ionic bonds form.
• Understand how covalent bonds form.

Success Criteria:

• You can write the formula for ionic compounds.
• You can explain how covalent bonds are formed between two non-metals.

Here's an interactive review of what we worked on yesterday:

http://www.bbc.co.uk/schools/gcsebitesize/science/add_edexcel/ionic_compounds/ionicact.shtml

Next we discussed the patters on the periodic table and how to figure out the ionic charges of each element.

Handout: Valence

Using these valences, we can figure out how many ions of each element are required to make an ionic compound.  I got some volunteers to come up and demonstrate using black and white beads as electrons and protons.  Then we discussed how you can use the crisscross method to figure out the same thing.

Handout: Writing formulas for ionic compounds

Finally we talked about covalent bonds.  Again, students came up to the front to demonstrate using beads as electrons.  In a covalent bond, the atoms don't lose or gain electrons, they share!

Handout: Covalent Bonds
Handout: Covalent Bonds Examples

If two hydrogen each share their electrons, then they will each have two, making a more stable molecule.  

Here's the example I showed in class of two oxygen forming a covalent bond with a carbon.

Homework: Complete the handouts.

Unit Test!

The Chemistry Unit Test will be on Wednesday Oct. 9.

We will wrap up the material this week and have a couple days of review before the test.  If there's anything in the unit so far that you are not sure about, please make sure to clarify with me before the test.

Handout: Topics to Study

Oct. 2 – Ionic Bonds

Learning Goals: Understand how ionic bonds are formed.

Success Criteria: You can draw the Bohr-Rutherford diagram for ions and show how they bond.

Today we reviewed som Bohr-Rutherford diagrams and I showed you what Lewis dot diagrams are.  These diagrams are only concerned with the outer shell of each atom.  Here are some examples:

We spent some time discussing the patterns that we see.  All group 1 atoms have one electron in the outer shell.  All nobel gases have complete outer shells.

Here are the handouts for today:

• Bohr-Rutherford and Lewis dot diagrams
• Putting atoms together
• How atoms combine (ionic bonds)
• Drawing Ions

Here's the main idea you should get out of these handouts: ionic bonds form when a metal loses one or more electrons and a non-metal gains the lost electrons.

The Bohr-Rutherford diagrams.

The Lewis dot structures.

Positive and negative ions attract each other and join together forming ionic compounds.

Homework: Complete the handout on Bohr-Rutherford diagrams for ions.

By popular demand, here are the lyrics to the periodic table song!

Video: Periodic Table Song

Written, Directed, Produced, Edited and Sung by Mitchell Moffit.

Based on the "Can-Can" music, by Offenbach. 

LYRICS:

There's Hydrogen and Helium

Then Lithium, Beryllium

Boron, Carbon everywhere

Nitrogen all through the air

With Oxygen so you can breathe

And Fluorine for your pretty teeth

Neon to light up the signs

Sodium for salty times

Magnesium, Aluminium, Silicon

Phosphorus, then Sulfur, Chlorine and Argon

Potassium, and Calcium so you'll grow strong

Scandium, Titanium, Vanadium and Chromium and Manganese

CHORUS

This is the Periodic Table

Noble gas is stable

Halogens and Alkali react aggressively

Each period will see new outer shells

While electrons are added moving to the right

Iron is the 26th

Then Cobalt, Nickel coins you get

Copper, Zinc and Gallium

Germanium and Arsenic

Selenium and Bromine film

While Krypton helps light up your room

Rubidium and Strontium then Yttrium, Zirconium

Niobium, Molybdenum, Technetium

Ruthenium, Rhodium, Palladium

Silver-ware then Cadmium and Indium

Tin-cans, Antimony then Tellurium and Iodine and Xenon and then Caesium and...

Barium is 56 and this is where the table splits

Where Lanthanides have just begun

Lanthanum, Cerium and Praseodymium

Neodymium's next too

Promethium, then 62's

Samarium, Europium, Gadolinium and Terbium

Dysprosium, Holmium, Erbium, Thulium

Ytterbium, Lutetium

Hafnium, Tantalum, Tungsten then we're on to

Rhenium, Osmium and Iridium

Platinum, Gold to make you rich till you grow old

Mercury to tell you when it's really cold

Thallium and Lead then Bismuth for your tummy

Polonium, Astatine would not be yummy

Radon, Francium will last a little time

Radium then Actinides at 89

REPEAT CHORUS

Actinium, Thorium, Protactinium

Uranium, Neptunium, Plutonium

Americium, Curium, Berkelium

Californium, Einsteinium, Fermium

Mendelevium, Nobelium, Lawrencium

Rutherfordium, Dubnium, Seaborgium

Bohrium, Hassium then Meitnerium

Darmstadtium, Roentgenium, Copernicium

Ununtrium, Flerovium

Ununpentium, Livermorium

Ununseptium, Ununoctium

And then we're done!!

Oct. 1 - Bohr-Rutherford Diagrams

I handed back the Density Quiz today.  Here are the solutions:

• Density Quiz Solutions (Period 1)
• Density Quiz Solutions (Period 4)

Next we discussed an interesting element: carbon.  Carbon can come in may different forms, each with vastly different properties.

Handout: Graphite to Diamonds

Bohr-Rutherford Diagrams

Learning Goals: Understand the structure of atoms.

Success Criteria: You can draw the Bohr-Rutherford diagrams for the first 20 atoms on the periodic table.

First you must know how to find the number of protons, neutrons and electrons in each atom.  Here's a worksheet for you to practice:

Handout: Subatomic Particles Worksheet

Next we went over how to draw Bohr-Rutherford diagrams.  Here are the steps:

1. Determine the number of protons and neutrons.
2. Write it in the middle (nucleus.)
3. Determine the number of electrons.
4. Put the electrons in concentric shells (orbitals)

• First orbital can hold up to 2 electrons.
• Second orbital can hold up to 8 electrons.
• Third orbital can hold up to 8 electrons.
• Fourth orbital can hold up to 8 electrons.

Handout: Bohr-Rutherford Diagrams

Here's an example: http://www.youtube.com/watch?v=wy83UlGQpWw

Here are the solutions:

Homework: Complete the handouts and answer the questions to find patterns with these diagrams.

Dr. Manhattan from Watchmen has a Bohr-Rutherford diagram of hydrogen on his forehead!