Y11 REVIEW

Chemistry is different to/sometimes more difficult than many other courses for various reasons, but one of those is because almost every aspect of the Year 11 course (except small pieces here and there, and electrochemistry) is revisited as the basis for Year 12 work, and therefore examinable.

Study for this subject absolutely requires that you solidly understand Year 11 work. The tutorials and videos on this page take you back through the Preliminary Course to ensure that you have a sound foundation for the HSC. This will help the pieces fall together.

You are strongly encouraged to review one per day / night to consolidate your learning.

CHEMISTRY OVERVIEW

Videos:

Intro to Chemistry, Basic Concepts - Periodic Table, Elements, Metric System & Unit Conversion https://www.youtube.com/watch?v=bka20Q9TN6M [3.01.40 hours]

1. MEASUREMENT

Tutorials and Problems links:

Videos:

(Skim through these, you don't need to watch all in depth)

Scientific Notation https://www.youtube.com/watch?v=_BtzXojuM1o&index=2&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS [42.30 mins]
Significant Figures Made Easy https://www.youtube.com/watch?v=9WFxkxFXb20 [1.36.01 hours]

PROPERTIES AND STRUCTURE OF MATTER

2. CLASSIFICATION OF MATTER

Tutorials and Problems links:

Videos:

Elements, Compounds, Pure Substances and Mixtures https://www.youtube.com/watch?v=OHhnm2p5G3o&index=9&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS [19.12 mins]
Physical and Chemical Changes https://www.youtube.com/watch?v=YE2xaMsoGFU&index=11&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS [11.07 mins]
Physical and Chemical Properties https://www.youtube.com/watch?v=gH1R87ahFvA&index=12&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS [10.34 mins]
PSM1 https://www.youtube.com/watch?v=EWyeCtbECqg&index=1&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [4.57]
PSM2 https://www.youtube.com/watch?v=f8_X4t85CQM&index=2&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [4.59]
PSM3 https://www.youtube.com/watch?v=ncugEdbIAWw&index=6&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [4.57]
PSM5 https://www.youtube.com/watch?v=PrUH2XGyafI&index=4&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [5.02]
PSM6 https://www.youtube.com/watch?v=CIzt0pUDq7A&index=7&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [5.14]

3. ATOMIC STRUCTURE

Tutorials and Problems:

Videos:

PSM7 https://www.youtube.com/watch?v=rwn427EPBR0&index=13&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [5.17]
Protons, Neutrons, Electrons... https://www.youtube.com/watch?v=tW_ItPxFwvY&index=16&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS [19.33 mins]
What are Isotopes? https://www.youtube.com/watch?v=bagegEZBtOs&index=20&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS [12.42 mins]
PSM8 https://www.youtube.com/watch?v=kTcGkLR9dQ0&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP&index=12 [5.19]
PSM9 https://www.youtube.com/watch?v=Gso_eNAIJdc&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP&index=11 [5.15]
PSM14 https://www.youtube.com/watch?v=ok63ZzUQbx4&index=20&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [5.09]
PSM15 https://www.youtube.com/watch?v=0FSG4-wCQYs&index=19&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [5.05]
PSM16 https://www.youtube.com/watch?v=HhsgpMDEKs8&index=18&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [5.06]
PSM11 https://www.youtube.com/watch?v=KymWeZ6mNd8&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP&index=9 [5.03]
Average Atomic Mass Practice Problems https://www.youtube.com/watch?v=rgixSP7PxS0&index=17&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS [10.19 mins]

4. ELECTRONS IN ATOMS

Tutorials and Problems links:

Videos:

5. PERIODIC TABLE

Tutorials and Problems links:

Videos:

6. FORMING COMPOUNDS

Tutorials and Problems links:

7. BONDING: INTRA-MOLECULAR FORCES

Tutorials and Problems links:

IONIC BONDS

METALLIC BONDS

COVALENT BONDS

Chemical Bond

Covalent Bond

Molecular Compounds

Energy and Covalent Bond Formation

Lewis Electron Dot Structures

Single Covalent Bonds

Multiple Covalent Bonds

Bond Energy

VSEPR Theory

Molecular Shapes: No Lone Pairs on Central Atom

Molecular Shapes: Lone Pair(s) on Central Atom

Bond Polarity

Polar Molecules

Videos:

Elements, Atoms, Molecules, Ions, Ionic and Molecular Compounds https://www.youtube.com/watch?v=pSJeMJaCkVU&index=18&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS [13.53 mins]
Introduction to Ionic and Covalent Bonding https://www.youtube.com/watch?v=S_k0kr2eZSQ&index=19&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS [12.50 mins]
What is an Ion? https://www.youtube.com/watch?v=ALNSIAnm-EQ&index=21&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS [10.31 mins]
PSM21 https://www.youtube.com/watch?v=DUI4JlmtmX8&index=22&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [6.05]
PSM22 https://www.youtube.com/watch?v=xXqWdw7f1qY&index=21&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [6.56]
PSM23 https://www.youtube.com/watch?v=JColWVL-tuQ&index=24&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [6.10]
Ionic Bonds, Polar Covalent Bonds and... https://www.youtube.com/watch?v=8NQzcpWvq4g [11.00 mins]
Which Bond is More Polar? https://www.youtube.com/watch?v=o0-a5HzSzdE [11.35 mins]
PSM24 https://www.youtube.com/watch?v=6xhNopMp64M&index=23&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP [6.47]
PSM#25 Allotropy https://www.youtube.com/watch?v=cz0jU6Cf4l0&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP&index=25 [4.41]
PSM#26 Ionic networks https://www.youtube.com/watch?v=4pA37Bpk3rQ&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP&index=26 [5.27]
PSM#27 Covalent networks https://www.youtube.com/watch?v=sWpfAKfDLSU&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP&index=27 [5.16]
PSM#29 Metallic networks https://www.youtube.com/watch?v=M6Oxq-9Ucsk&list=PLeFSFSJ9WqSARl70FH6vBJCVfhtu4JjKP&index=29 [5.23]

8. INTER-MOLECULAR FORCES

Please note: When considering an increase in the size of molecules (e.g. methane to ethane), you will see some texts and websites that use the term "stronger forces" rather than "more attractions".

Rather than the force "getting stronger" (like a volume knob being turned up), there are more points of interaction, leading to an increased number of attractive forces.When moving from a smaller to a larger molecule, the fundamental mechanism of a single temporary dipole attraction doesn't change, but the number of simultaneous interactive forces increases.

It's not an issue until you are comparing intermolecular forces, as we will later.

Increasing mass and geometry of an organic homologous series.

Methane: One Shift in Electron Density

A single methane molecule (CH4) is a small, symmetrical sphere: the 10 electrons of methane, its electron cloud, essentially form a tiny ball. When two methane electron clouds approach, they can only ever make interact at one single point. Because methane has no length or 'surface area,' it physically doesn't have the shape to line up against another molecule at multiple places at the same time.

For a split second, that distribution can fluctuate, leaving a slight negative charge on one side of the molecule and a slight positive charge on the opposite side. This instantaneous dipole creates a single electrostatic attraction with a neighbouring molecule.

Because it is just one single, fleeting interaction over a tiny surface area, it is incredibly easy to separate the molecules. Methane boils at -161.5C.

Ethane: Multiple Shifts in Electron Density

Because the ethane molecule is longer and has more electrons, its electron cloud is larger, electron distribution can fluctuate in multiple places independently.

For a split second, you can get multiple shifting positive and negative zones along its length, all at the same time.

When two ethane molecules line up, they don't just form one point of attraction. These multiple temporary dipoles create a greater number of simultaneous attractive interaction points between the two electron clouds.

The type of force at each point is still just as weak as it was in methane, but because you have more interaction points acting at once, it takes significantly more energy to separate them.

And more so for propane and beyond.

Down a group of the Periodic Table

As we move down a group on the periodic table, the atoms get much larger and their electron clouds become vastly more spread out with many more electrons. Because these large electron clouds are so far from the attractive force of the nucleus, the electron distribution can fluctuate wildly and independently in many different areas at once.

This means a larger molecule's massive cloud allows for a much higher number of simultaneous interaction points with a neighbouring molecule. Just like moving from methane to ethane, there's no change to the type of force at each point—they are still just temporary positive and negative fluctuations—but the number of interaction points acting at the exact same time is vastly higher. This is why boiling points steadily increase as you go down a group.

Tutorials and Problems links:

Videos: