Monthly Archives: February 2016

Class of: 12-Feb-2016.

Today we covered Section 7.3: Ionic Compounds: Chemical Formulas and Naming (p. 183).

Learning Objectives:

• Students will be able to produce the chemical formula of an ionic compound given its component elements or polyatomic ions.
• Students will be able to write the name for an ionic compound given its chemical formula.

Two interesting things today: pure, distilled water does not conduct electricity very well at all! This is because water is a molecular compound. In general, you rarely find pure water. Most water has ions dissolved in it that are harmless to drink, but do conduct electricity.

A lightning strike will disperse about 6 metres in water. It doesn’t travel very far because the electrical energy disperses in all directions very rapidly. If you think about it, 6 metres in all directions is a lot of water! Almost as dangerous as the electric shock is the sound that is created: as much as 300 decibels as far away as 100 metres, which is enough to kill fish and make humans lose their hearing in one shot.

Please work through the following review problems:
p. 191 #2-5

Class of: 11-Feb-2016.

Today we covered Section 7.2: Chemical Bonding (p. 176).

Learning Objectives:

• Students will be able to classify bonds as either ionic or covalent.
• Students will be able to describe the properties of ionic and molecular compounds.

Lead poisoning is also known as plumbism! It’s symptoms include pain, cramps, constipation, insomnia, headaches, irritability, loss of appetite, fatigue, high blood pressure, numbness, amnesia, anaemia, kidney dysfunction, and finally death. So, don’t eat the lead!

Please work through the following review problems:
p. 182 #1-11

Class of: 10-Feb-2016.

Today we covered Section 7.1: 7.1: Compounds, Atoms, and Ions (p. 169).

Learning Objectives:

• Students will be able to write the ionic form of atoms.
• Students will be able to combine ions into compounds using electron transfer.

Compounds have very different properties than the elements that make them up! NaCl is made up of sodium, which we saw to be very reactive in water, and chlorine, which is a deadly gas. But combined they are… delicious!

Please work through the following review problems:
p. 174 #1-12

Class of 09-Feb-2016.

We did a mini-lab today on Classifying Elements! Please take a look at the marking checklist (in another post) to see the instructions and how I will be marking it.

We will be having a quiz tomorrow morning on Chapter 6. You will need to know how to do the following things:

Given an element, determine atomic number, # protons, # electrons, # electrons, mass number, atomic mass, chemical symbol, chemical formula, and chemical family. You will also need to know how to classify a material as a pure substance, element, compound, or mixture. You will have to know how to draw a Bohr diagram.

You WILL be given a periodic table.

As an interesting fact, helium is one of the rarest elements on the planet. Helium accounts for 0.00052% of the atmosphere, which is almost nothing! Most of it is instead extracted from minerals and natural gas deposits in the ground, both of which are finite resources. People keep using helium for balloons, making it even more rare and expensive to buy for scientific research. There is now talk about banning helium balloons because of this! Helium is selected because it is very unreactive. Which other elements could be used to fill balloons based on this quality?

Check out the marking checklist for the Classifying Elements lab here:

Sci-10-6.L-Checklist

This report is due Monday, 15-Feb-2016.

Class of: 05-Feb-2016.

Today we went over Section 6.3: Classifying Elements with the Periodic Table (p. 157).

Learning Objectives:

• Students will be able to classify elements as metals, non-metals, or metalloids.
• Students will be able to show how related elements are grouped into families on the periodic table and know the properties of those families.
• Students will be able to read data about electron configuration and other atomic data from elements on the periodic table.

Sodium metal (Na) reacts violently with water and should be kept away from it! The oily substance around it is actually kerosene, which it sits submerged into prevent it from reacting with moisture in the air.

As a reminder we will have a short quiz on Chapter 6 at the beginning of class on Wednesday, 10 February. Be prepared!

Please work through the following review problems:
#1-12 on p. 161.

Class of: 04-Feb-2016.

Today we went over Section 6.2: Atomic Theory (p. 153).

Learning Objectives:

• Students will be able to represent atoms using Bohr diagrams, labelling the parts of the diagrams.
• Students will be able to understand and determine an atom’s mass based on the subatomic particles that make it up.

For your interesting factoid of the day, a proton has a mass of 1 u, which is 1.6726219 × 10^-27 kilograms. That means it would take 597,863,750,000,000,000,000,000,000 protons to weight one kilogram. That’s a lot of protons!

Please work through the following review problems:
#1-7 on p. 156.

Class of: 03-Feb-2016.

Today we started Chapter 6: Elements, Compounds, and the Atomic Theory.

We began with Section 6.1: Properties Are Used to Identify Matter (p. 149).

Learning Objectives:

• Students will be able to classify substances as mixtures or pure substances using their physical and chemical properties.
• Students will be able to classify pure substances as elements or compounds again based on their properties.
• Students will be able to write the chemical symbol and chemical formula for any element on the periodic table.

As an interesting fact about physical properties, osmium (atomic number 76, chemical symbol Os) is the densest substance on the planet. It is also, therefore, the densest metal (including any alloys). Unfortunately it forms an extremely toxic compound with oxygen when exposed to the air, and it is also a pyrophoric substance, meaning that is bursts into flames spontaneously at room temperature. So, you probably won’t find it being used as cutlery any time soon!

Also, in case you were wondering, when you want to give an example you use “e.g.” because it stands for “exempli gratia” in Latin, which translates to “for the sake of the example.” This is different than when you use “i.e.” to indicate only one specific thing, which stands for “id est,” meaning “that is”

Please work through the following review problems:
#1-11 on p. 152.

We have now started Chemistry! Specifically we are on Unit B: Elements, Compounds, and Reactions.

The topics of the unit and assessments will be like so (things might change a little as we get closer):

Chapter 6: Elements, Atoms and the Atomic Theory (p. 148)
– Quiz & Classifying Elements Lab

Chapter 7: Compounds, Ions, and Molecules (p. 168)
– Quiz & Ionic vs. Molecular Lab

Chapter 8: Classifying Chemical Compounds (p. 200)
– Quiz & pH Lab & Organic Debate Project

Chapter 9: Investigating Chemical Reactions (p. 230)
– Quiz & Reaction Investigation Lab & Reaction Rate Lab

Check out the marking checklist here:

Sci 10 S.1 P Checklist