Alongside  Mr Nicol's Videos I found this on very helpful


http://www.youtube.com/watch?feature=player_embedded&v=HACQtNdQKj8

Oxidation Numbers

The notes for this are on pp59-60 in Beginning Chemistry.

Markovnikov's Rule

The "rish" (more H's) get "richer".

Oxidation-Reduction Introduction

Here is a quick overview of the content of the Oxidation-Reduction topic that we will be working on in Term Four.

Review of Organic Chemistry

Alcohols Revision

Our groups overview of Alcohol's. 

Lucas Reagent

Lucas Reagent provides a high concentration of chloride ions. These ions can replace the hydroxy (-OH) groups of secondary and tertiary alcohols.

Alcohols. Part Deux

• Solubility of Alcohols
• pH of Alcohols
• Oxidation of Alcohols

Alcohols Introduction

The video below outlines the functional group, general formula, physical properties and classification of alcohols.

Addition Polymers

Reactions of Alkenes

Introduction to Alkenes

Alkenes are unsaturated hydrocarbons.

Reactions of Alkanes

Alkanes

INTRODUCTION TO ALKANES

• general formula
• nomenclature

STRUCTURAL ISOMERISM IN ALKANES

Acidic/Alkaline Salts

Some salts are not truly neutral, despite being made in a neutralisation reaction (acid + base). How can we determine whether a salt is acidic or alkaline? How can we justify this?

pH Calculations

It is important to be able to calculate the pH of strong acids and strong bases this year:

Acids and Bases Introduction

Dynamic Equilibrium and le Chatelier's Principle

A dynamic equilibrium is a reaction which is reversible and the rate of reaction in the forward direction is the same as the rate of reaction in the reverse direction.

le Chatelier's Principle says that this equilibrium will shift (in the forward or reverse direction) to overcome any change made to the system. For example, if more reagent is added, the equilibrium shifts in the forward direction to decrease this amount of reagent. As a consequence, more product is made. The "aim" is to re-establish dynamic equilibrium.

Bond Enthalpies

pp143-144 Beginning Chemistry

This is also a pretty good website which could help: http://www.kentchemistry.com/links/Kinetics/BondEnergy.htm

Bond Enthalpies feat. special talents

Calculating Enthalpy Change

Endothermic vs. Exothermic

Today, we did four simple experiments to see that some reactions absorb heat energy (feel cold) while others release heat energy (feel warm/hot).

1. NaOH + water = increase in temperature (exothermic)
2. Ammonium chloride + water = decrease in temperature (endothermic)
3. HCl + NaOH solutions = increase in temperature
4. Ammonium thiocyanate + barium hydroxide = decrease in temperature

Determining Molecular Polarity

Molecules

Shapes of Molecules

The shapes of molecules are the last clue for helping determine molecular polarity:

Lewis Diagrams

Lewis Diagrams and Structures are very useful for helping us predict molecular polarity.

Answers to today's examples:

NOTE: Some of the dots/crosses representing electrons are unclear. Please save the image onto your computer and enlarge it to see the details.

Introduction to Molecules

Substance Type Overview

It is very important to understand that "Matt" is not an attractive force, so please do not use it as an answer in assessments.

Chart - Type of Solid, Type of Particle, Attractive Forces Between Particles

http://chemicalminds.wikispaces.com/file/view/solidsANSWERS.pdf

This is a fully answered chart for multiple types of solids, same type of question from one of the question sheets from today.

Molecular Solids

Molecular Solids have some characteristic properties:

• low m.p./b.p.
• electrical and thermal insulators
• often brittle

These properties need to be explained in terms of the forces between the molecules (particles). These forces are called van der Waal's forces. Before we can understand these, we need to understand molecular polarity, which requires us to understand intra-molecular bonding (covalent), shapes and electron cloud size.

Covalent Networks

With Mr Nicoll away, we had to make our own summary about the structure and characteristic properties of covalent network solids. This group includes diamond, graphite and silica (glass).

Diamond

Silica: Red = Oxygen; Blue = Silicon

Metallic Solids

Most elements are metals. Metals have some characteristic properties which can be explained by the metallic bond and the structure of metals in their solid state:

1. Electrical Conductivity
2. Thermal Conductivity
3. Malleability/Ductility
4. Relatively High m.p (except Hg)

Ionic Solids

Photo of Ionic Solids Video

Structure and Bonding Introduction

Next term, we will be starting our next topic. Structure and Bonding is part of a bigger topic including Enthalpy Changes (Thermochemistry) and is assessed by AS91164.

Here is a brief overview of what we will be covering in the Structure and Bonding section:

Thank you to Macca for the camera work.

Introduction to Solids

Titration Calculations

Titration Introduction

Standard Solutions

How to make a standard solution and calculate its precise concentration:

Thank you to Po for the camera work.

Percentage Composition

Water of Crystallisation

Many ionic crystals have water molecules withing their structure. We call these hydrated salts. We can drive the water off by heating the salts strongly, creating anhydrous salts (salts with no water inside their crystal structure).

This can be easily seen in substances such as copper (II) sulfate:

Hydrated Copper(II) Sulfate is a blue crystal.

A crucible is placed on a pipe-clay triangle to heat the hydrated copper(II) sulfate strongly.

Anhydrous copper (II) sulfate is a finer powder and is white (left).

However, not all hydrated salts will change colour when dehydrated. Instead, we record the mass of the hydrated salt, then heat it strongly, then record the mass again. If the mass has changed, we can infer that water of crystallisation has been removed by the heating.

The change in mass is the water removed. As we know the molar mass of water (18.0 g mol^-1), we can then calculate the amount of water removed. Once we calculate the amount of the anhydrous salt we have left, we can calculate the formula of the hydrated salt:

EXAMPLE

5.96g of hydrated BaCl₂ was heated strongly for 5 minutes, weighed (5.08g), then heated again for another 2 minutes and reweighed (5.08g).

As the ratio is 1:2, the formula is BaCl₂.2H₂O

In the table, we are always trying to get the ionic crystal to be "1" in the ratio. The value in the ratio for the water molecules should be rounded to the nearest whole number.

The Mole

Today we learnt about the mole. The mathematical relationship between automic mass and molar mass.

Quantitative Analysis

Today, the class wanted an overview of the topic and to see how the different concepts were linked. Here are the video of this overview and a close-up of the diagram drawn on the whiteboard:

The video is is a bit rough as this was an impromptu teaching moment...

Mol(e)

What we are going to be learning in our new topic 2.1

Identifying Cations

This link should take you to the youtube video of Mr Nicoll teaching us about Identifying Cations

Complex Ions

You need to memorise these :)

What we need to know from the Periodic table

This video was from last week when Mr. Niccol was showing us what we do and don't need from the periodic table. He explains how the columns are related to the charge of each ion. He goes over the most common ones of which we need to know e.g. Na, H, and Al. But also some awkward ones in the middle e.g. Pb, Ag. 

Cards

What you need to write on you cards that we got today :)

Outline

Talking about all this! Cheers! Your friendly neighbourhood blogger.

Sir!

Start of the lesson