Tag Archives: revision

Get your Future-Proof VCE Chemistry Formula Book for just $55

James Kennedy's VCE Chemistry Formula Book 2017-2021Inspired by the formula booklets used by VCE Physics and VCE Maths Methods, here’s an 8-page Chemistry formula booklet you can use for your Year 11 and 12 Chemistry assignments. This custom-made booklet is a collection of reliable formulae that I have been using to answer VCE Chemistry questions while teaching and tutoring around Melbourne.

There are 76 formulae on 8 pages. At least 10 of these formulae aren’t in the three main chemistry textbooks. Orders are shipped in A4-sized booklet that resembles the VCAA Data Booklet.

Orders from schools, students and tutors are all welcome. Price includes free international delivery and a 10% voucher for the T-shirt store.

Order your copy now by clicking here

Learn from the best

James Kennedy achieved outstanding A-level results in 2006 in Maths, Chemistry, Physics and Biology. Those excellent grades (which equate to an ATAR of 99+) earned him a BA (Hons) degree and a Masters degree in Natural Sciences from the University of Cambridge.

Shortcut formulae were just one of the techniques James used to pass his A-level exams and get into Cambridge. Along with structured revision, revision guides, practice papers and study notes on wall-cards, James used shortcut formulae to save precious time in the examination hall. You can get your own copy of these original shortcut formulae – revised and updated for the 2017-2021 VCE Chemistry course – for just $55 including free international shipping. Click here to get your copy.

Here’s an preview of the inside

VCE Chemistry Formula Booklet, $55. Free, Fast Delivery Included.
VCE Chemistry Formula Booklet, $55. Free, Fast Delivery Included.

Click here to purchase your 8-page companion book with 76 formulae relevant for VCE Chemistry Units 1-4

We Lied To You

Click to download the book
click-here

This book contains 50 lies taught in the VCE Chemistry course.

These lies include well-meaning simplifications of the truth, mistakes in the textbook, and, in a few extreme cases, blatant falsehoods.

This book isn’t a criticism of the VCE Chemistry course at all. In fact, I just want to highlight the sheer complexity of Chemistry and the need to make sweeping generalisations at every level so it can be comprehensible to our students. This is a legitimate practice called constructivism in pedagogical circles. (Look that up.)

Many of these ‘lies’ taught at VCE level will be debunked by your first-year chemistry lecturers at university.

Here’s a preview of some of the lies mentioned in the book. Check out all 50 by clicking the download link at the bottom of the page.


lie-2


lie-15


lie-25


we-lied-to-you-cover-lightbulbs

click-here


SUVAT rearranged

SUVAT Rearranged. Traditional SUVAT equations are highlighted yellow. Copy this to your cheat sheet!
SUVAT Rearranged. Traditional SUVAT equations are highlighted yellow. Copy this to your cheat sheet!

There are just five traditional SUVAT equations:

Traditional set of five SUVAT equations

Save time in your examination by looking up the relevant equation from this table instead of rearranging them manually.

Click here to download free PDF to put on your Physics Cheat Sheet

Get my latest book here: Common VCE Chemistry Mistakes… and how to avoid them

Common VCE Chemistry Mistakes COVER.jpg

This book is a collection of common mistakes in VCE Chemistry and how to avoid them.

It comes from years of marking student SACs and exam papers, and from reading Examination Reports from the VCAA as well.

It’s free of charge, very informative, and very concise.

Click here to download the FREE book.

Redox Rules

Click to download REDOX RULES posters for VCE Chemistry
Click to download REDOX RULES posters for VCE Chemistry

What’s redox? We never learned that!

Yes, you did. I use the term “redox” to refer to all of the following chapters in Heinemann Chemistry 2, which you will have learned at the end of Term 3 (September).

  • Chapter 26: Redox (revision of Year 11)
  • Chapter 27: Galvanic Cells
  • Chapter 28: Electrolytic Cells

Don’t underestimate redox

The VCAA has consistently used redox to discriminate which schools and students have the self-discipline required to keep studying at the end of the year. Studies show that redox is taught at a time when student motivation is at its minimum: energy levels are low, emotions are high, and graduation is just over the horizon. Many schools and students gloss over these topics because they’re running out of time, any many students think they’ve grasped the topic – when they’ve actually grasped misconceptions instead.

VCAA VCE Chemistry how difficult is each topic
Notice how chapters 26, 27 and 28 are consistently the most difficult and the most frequently askedClick to download PDF version

Here are some popular redox lies (misconceptions)

LIE #1: The polarities switch during recharge
Nope. The polarities never switch. It’s the labels of ‘anode’ and ‘cathode’ that switch because the electrons are flowing the other way through the external circuit. Polarity is permanent.

LIE #2: Hydrogen fuel cells don’t emit any greenhouse gases
Wrong. They emit H2O, which is a powerful greenhouse gas. If you don’t believe that the VCAA can be this pedantic, think again. Read their 2015 Examiners Report here.

LIE #3: Each mole of electrons forms 1 mol Ag, 2 mol Cu or 3 mol Al in a cell
Wrong again. If you look at the half-equations, you’ll see that each mole of electrons actually forms 1 mol Ag, 12 mol Cu or 13 mol Al. That’s why I teach “1, 12 and 13 moles” instead of the typical “1, 2, 3 moles” rule.

LIE #4: Temperature increases the rate of reaction in electroplating
Wrong! Remember that Faraday’s first law states that m ∝ Q. Because Q = I×t, only those two things – current and time – can affect the mass deposited at the cathode.

LIE #5: Electrons always leave the anode and go towards the cathode
Wrong again. Electrons go RACO: to see what that means, download the posters above. This question appears in recent versions of Chemistry Checkpoints. Give it a try.

LIE #6: The cathode is always positive
Ask your teacher.

LIE #7: Ions flow one way in the salt bridge
Nope. Anions always migrate to the anode; and cations always migrate to the cathode.

LIE #8: KOHES always works for balancing half-equations
KOHES only works for cells with acidic electrolytes. For cells with alkaline electrolytes, which sometimes appear in VCAA papers despite not being in the study design (see page 46 here), you’ll need to use KOHES(OH). Here’s KOHES(OH) explained:

  1. Do KOHES as normal
  2. Add the same number of OH(aq) ions to each side of the half-equation to balance out the H+(aq)
  3. Cancel and simplify. Remember that H+(aq) + OH(aq) makes H2O(l). Remember also to cancel out any remaining H2O(l).

LIE #9: I can balance an unbalanced redox equation by putting numbers in the equation
Don’t be fooled by this one! The ONLY way to balance an unbalanced redox equation successfully is to do the following:

  1. Separate it into two half equations
  2. Balance them using KOHES or KOHES(OH) as appropriate
  3. Multiply them and recombine
  4. Cancel and simplify
  5. Done!

That’s a lot of work but it’s the  only way to do it successfully. If you try to ‘cheat’ by just writing numbers (molar coefficients) in front of the reactants and products, you’ll find that the charges don’t add up, and you’ll get zero marks for the question.

LIE #10: I can break up polyatomic ions to make balancing half-equations easier
Nope! You’re only allowed to separate aqueous species in a half equation or an ionic equation. Because the Mn and O are actually bonded together in a polyatomic ion, you’ll need to write this:

  • MnO4(aq) + 8H+(aq) + 5e → Mn2+(aq) + 4H2O(l)  2/2 marks

Instead of this:

  • Mn7+(aq) + 5e → Mn2+(aq)  0/2 marks

If in doubt, keep it intact and it’ll cancel out by the end if it’s a spectator ion.

LIE #11: The two reactants that are closest together on the electrochemical series react
Not always true. Use SOC SRA instead, which is explained in the posters above. Still struggling? Ask your teacher or tutor for help.

LIE #12: Oxidants are all on the top of the electrochemical series
They’re actually on the left, and all the reductants can be found on the right side of each half equation in the electrochemical series. There is no top/bottom divide on the electrochemical series: only a left/right divide of oxidants/reductants.

Decorate your school/bedroom/hallway

Surround yourselves with truthful redox revision using these 17 free Redox posters. I’ve had these up around the whiteboard for a few weeks now – they’re a constant reminder to students that redox has many ideas that are always true.

One more tip: print and laminate an electrochemical series (available here) so you can annotate it during dozens of practice dozens without wasting paper. Good luck!

Let’s add nitrogen gas

elements110007
‘Nitrogen’ page from Theodore Gray’s amazing book, ‘The Elements’

Initial conditions

Recall from last week that our Periodic Table Smoothie contains the following species:

Substance Amount present (moles)
He(g) 1.00000
Be(s) 0.51435
LiH(s) 0.27670
Li2C2(s) 0.27165
B2H6(g) 0.23300
Be2C(s) 0.17470
H2(g) 0.14267
BeC2(s) 0.13625
CH4(g) 0.00949

Pressure: 718 kPa
Temperature: 350 °C

Reactions of nitrogen in our 10-litre vessel

Our freshly-added 1.00 mol of nitrogen gas, N2(g), reacts with hydrogen gas to make ammonia in the following reversible (equilibrium) reaction. We will assume that the interior metal surface of the vessel is a suitable catalyst for this reaction (e.g. iron). 

image130.png

There are three other reactions below that might have occurred at higher temperature, but I’ve chosen not to raise the temperature of the vessel at this point. Rather, we’ll keep it at 350 °C to keep things manageable.*

image020
image018
image024

*I was tempted at this point to elevate the temperature of our vessel to 500 °C so that the second reaction could take place as well. This would produce copious amounts of smelly ammonia gas, which would allow for larger quantities of interesting organic compounds to be produced later on. To keep our simulation safe and (relatively) simple, I’ve decided to keep the vessel at 350 °C. Interesting compounds organic will still form – only in smaller amounts.

Equilibria

The ammonia reaction above (the first equation) is actually an equilibrium reaction. That means that the reactants are never completely used up, and the yield is not 100%.

Recall from Le Châtelier’s principle that removing product from an equilibrium reaction causes the position of equilibrium to shift to the right, forming more product. This is because:

“If an equilibrium system is subjected to a change, the system will adjust itself to partially oppose the effect of the change.” – Le Châtelier’s principle

There are three reactions that will remove ammonia from our vessel while it’s being produced, and I’ve put all three of these into the simulation. One of these is the reverse of the reaction above (producing hydrogen and nitrogen gases) and the other two are described below. Let’s take a look at those other two reactions.

With what will the ammonia react in our vessel?

Ammonia can undergo the following reactions with the other things in our vessel**

image151
image153

**The ammonia does react with methane and beryllium as well, but only at temperatures of 1200 °C and 600 °C, respectively.

Two compounds will be formed: lithium amide and borazine.[1] Lithium amide reacts with nothing else in the vessel, so the reaction chain stops there. Borazine, on the other hand, is much more interesting.

We’ve made borazine!

Borazine is a colourless liquid at room at temperature. It boils at 53 °C and has a structure that resembles that of benzene.

200px-borazine-dimensions-2d
Borazine is isostructural with benzene
Because of the electronegativity difference of about 1.0 between the B and N atoms in the ring, borazine has a mesomer structure:

600px-borazin_mesomers

Like benzene, there is partial delocalisation of the lone pair of electrons on the nitrogen atoms.

Borazine polymerises into polyborazine!

Fascinatingly, borazine polymerises into polyborazine at temperatures above 70 °C, releasing an equal number of moles of hydrogen gas.[2] Polyborazine isn’t particularly well-understood or well-documented, but one recent paper suggested it might play a role in the creation of potential ceramics such as boron carbonitrides. Borazine can also be used as a precursor to grow boron nitride thin films on surfaces, such as the nanomesh structure which is formed on rhodium.[3]

Like several of the other compounds we’ve created in our Periodic Table Smoothie, polyborazine has also been proposed as a hydrogen storage medium for hydrogen cars, whereby polyborazine utilises a “single pot” process for digestion and reduction to recreate ammonia borane.

polyborazylene_polymer
Polyborazine’s chemical structure
The hydrogen released during the polymerisation process will then react further with a little bit of the remaining nitrogen to produce a little more NH3(g) – but not much. Recall from earlier that the ammonia reaction is an equilibrium one, and the yield of NH3(g) at pressures under 30 atmospheres is very low. Pressure in our vessel is still only around 7 atmospheres.

Simulation results

nitrogen smoothie.png

Once polymerised, this would form about 12 grams of polyborazine:

image104
image106

As far as I’m aware, no further reactions will take place in the vessel this week.

Conclusion after adding 1.00 mole of nitrogen gas

Substance Amount in mol
He(g) 1.000
Be(s) 0.514
LiH(s) 0.000
Li2C2(s) 0.272
B2H6(g) 0.000
Be2C(s) 0.175
H2(g) 0.007
BeC2(s) 0.136
CH4(g) 0.009
N2(g) 0.552
NH3(g) 0.154
LiNH2(s) 0.277
polyborazine 12.194 grams

Pressure: 891 kPa (higher than before due to the addition of nitrogen gas)
Temperature: 350 °C (vessel is still being maintained at constant temperature)

Next week, we’ll add a mole of oxygen gas to the vessel. Warning: it might explode.

References

  1. Stock, Alfred and Erich Pohland. “Borwasserstoffe, VIII. Zur Kenntnis Des B 2 H 6 Und Des B 5 H 11”. Berichte der deutschen chemischen Gesellschaft (A and B Series) 59.9 (1926): 2210-2215. Web.
  2. Mohammad, Faiz. Specialty Polymers. Tunbridge Wells: Anshan, 2007. Print.
  3. Toury, Berangere and Philippe Miele. “A New Polyborazine-Based Route To Boron Nitride Fibres”. Journal of Materials Chemistry 14.17 (2004): 2609. Web. 4 May 2016.

Last-Minute Tips for the VCE Chemistry Exam

exam-hall-empty
You’ll be sitting here tomorrow.

Only positively-charged fragments from mass spectrometers produce a peak on the spectrum. Uncharged free radical fragments are not detected because they lack a positive charge.

Weak acids with a lower Ka value are the weakest… this means that they ionise to a lesser extent when in aqueous solution, giving rise to a lower concentration of available H3O+(aq) and a higher pH.

The conversion of triglycerides (a type of ester) into biodiesel (another type of ester) is called transesterification.

The covalent bonds between deoxyribose and phosphate groups in DNA form a group of atoms called a phosphodiester group.

Ether bonds and glycosidc bonds are not the same. Ether bonds are C-O-C. Glycosidic bonds are a type of covalent bond that joins a carbohydrate (sugar) molecule to another group, which may or may not be another carbohydrate.

Amide groups and peptide groups are not the same, either. Amide groups are CONH. Peptide groups are CONH between amino acid residues in a polypeptide chain. Nylon, for example, has amide groups (CONH) which aren’t called peptide groups.

Ether: C-O-C
Ester: COO
Amine: NH2
Amide: CONH

The molar mass of any amino acid without its Z-group is 74 gmol-1.

The molar mass of glucose, fructose and galactose (all monosaccharides) is 180 gmol-1. By coincidence, aspirin is also 180 gmol-1.

The molar mass of sucrose is 342 gmol-1 because (180*2)-18=342.

In general, energy is required to break bonds. Energy is released when bonds are formed.

Use the formula C-(H/2) to find how many C=C are present in a fatty acid (only works for fatty acids).

Use the shortcut formula (Ka/[acid])^0.5 to find % ionisation of a weak acid.

Use -log(Ka) to find the exact pH at the end point of an indicator.

Use the quick titration formula for rapid multi-choice titration questions: c1v1/ratio1 = c2v2/ratio2

A hydrogen bond is an intermolecular bond that forms between O-H groups. The covalent bond between the O and the H is not a hydrogen bond.

Can you write the half-equation for the reaction occurring at the anode in an ethanol-oxygen fuel cell with an alkaline electrolyte? Tip: start by writing the known reactants and products then use KOHES(OH) to balance your equation.

The products of a titration determine the pH at the equivalence point. For example, the the pH at the equivalence point in a titration between CH3COOH(aq) and NaOH(aq) is around 8.5 because at equivalence point, only products are present: Na+(aq) and CH3COO(aq). The ethanoate ion (CH3COO(aq)) is a weak base, which makes the solution produced slightly basic.

If you have absolutely no clue in the multiple choice sections, pick C. In the last 4 years of VCE Chemistry examinations, C has been correct 50% more of the time than B.

The multiple choice questions really do get harder towards the end. I’ve done the statistics.

Use your reading time wisely. During reading time, read all the questions with the following idea in mind: “how would I do this question?” without actually doing the question.

Bring sharp pencils.

Sleep early tonight (before 9pm). At this stage, getting enough sleep is far more important than revising those tiny details that may or may not come up in the examination.

All the best tomorrow.

Test Yourself Here on the Hardest VCE Chemistry Questions Ever Asked

VCE Chemistry Hardest Multiple Choice Questions Ever Asked Great Revision Tool
Click the image to begin Quiz 1

Great revision tools are available here. All the questions in these quizzes are real VCAA Chemistry questions extracted from Section A of past Chemistry papers.

Quiz 1
Answers

Quiz 2
Answers

Quiz 3 (long)
Answers

Revise What’s HARD: Focus on Electrolysis

VCAA VCE Chemistry how difficult is each topic
Click to download PDF version. Numbers in parentheses denote Chapter numbers.

The VCE Chemistry examination is only 22 days away. As you complete at least one practice paper each day and correct them ccording to your revision timetable, you’ll be finding that you’ve already mastered certain topics while others remain difficult.

Patterns emerge in student readiness: each year, electrolysis is the worst-studied topic on the course. Because VCAA has a reputation for asking questions on topics that students repeatedly got wrong in previous years; I decided to test this hypothesis by getting real data from recent examination reports and displaying it on a scatterplot of:

  • how difficult each topic is (% of marks lost) on the x-axis
  • how often the topic is asked (marks per paper) on the y-axis

The results were fascinating. While it’s impossible to say with any certainty which topics will be on the examination this year, previous years’ examination papers have placed more emphasis on the difficult topics (electrolysis, Ka, redox and biofuels). Focus your revision on these topics again this year.

Conclusion: Focus your Chemistry revision this week on your least favourite topics… those topics will probably be worth more marks in the examination!

Chapter 25: Essential Calorimetry Formulae

Chapter 25 Essential Calorimetry Formulae VCE Chemistry
Click to download PDF version

Calorimetry can be a confusing topic. Avoid common errors by following these essential tips:

  1. Always label the units of E (kJ or J) above the E. This is the most common source of error in calorimetry calculations. Try this quick way to remember the required units of E: If there’s ΔH in the equation, the units are kJ; otherwise, the units are J.
  2. In E=mcΔT, all the variables refer to the mass of water being heated. A common error among students is to use the mass of limiting reactant instead of the mass of water. Generally, m in this equation is 100 g or a similar round number.
  3. Never convert ΔT to kelvin. Temperature changes are the same in kelvin and celcius… never add 273 when finding ΔT.
  4. No calibration step? Use m×c instead. Because E=mcΔT and E=CfΔT, it therefore follows that Cf ≡ m×c. For example, if we’re heating a 100.0 g of water without a Cf, we should use Cf = 100×4.18 = 418 J K-1 instead.
  5. In ΔH = E/n, n denotes the number of moles of limiting reactant. Never add up the number of moles of reactants: use the number of moles of limiting reagent only.
  6. Calculate twice. Students most often make mistakes when converting hours or days into seconds. Many answers are therefore wrong by a factor of 60. Do your calculations twice: once while doing the question and again when you check over your answers at the end of the SAC or examination.
  7. Know a ballpark figure. Neutralisation and solubility reactions tend to have 2-digit ΔH values; combustion reactions tend to have a 3-digit ΔH and explosive reactions tend to have a 4-digit  ΔH. If you get a 5-digit ΔH value, you’ve probably forgotten to convert your answer into kilojoules!
  8. Remember the ‘+’ or ‘-‘ sign! The calculator doesn’t know whether the answer should be positive or negative. Think about it yourself instead: endothermic reactions need a ‘+’ sign and exothermic need a ‘-‘ sign. VCAA awards a whole mark for getting the ‘+’ or ‘-‘ sign correct! It’s possibly the easiest mark in the whole paper.

Consider getting a home tutor who can answer your questions and explain difficult concepts to you. Students learn much faster with a tutor than on their own.

For more Study Tools for Year 12 students, click here.

Free VCE Chemistry Progress Tracker Wall Chart

Chemistry LADDER progress chart for VCE students
Click to download PDF version (A3 size)

Track your progress in VCE Chemistry with this A3 size progress tracker. Cross out or colour in each box as you complete it, and write your scores in . Start at the bottom (highlighted) and work your way upwards.

A ‘minimum expected level of examination preparation’ of 26 examination papers is labelled on the chart. Write your percentage scores in each of the boxes as you mark each paper. When you’re achieving past/practice examination scores concordantly above 90%, you’re ready to sit the VCE Chemistry examination.

For more Study Tools for Year 12 students, click here.

How they did it: Tips from 99.95 students

Tips from Izabella Bratek at Academyplus.com.au

1. Develop excellent study skills. Cultivate ideal study habits such as waking up early, reading your notes before school, doing all homework on time and studying even when there’s no homework set.

2. Stay committed and know what you want and WHY. People who know why they do what they do are far more likely to persist and put in the huge number of hours required to excel at that particular skill. All successful people were driven by a higher. Find your why and you’ll feel more motivated to study VCE.

3. Keep motivation levels high and consistent throughout the year. Remind yourself constantly why you’re studying the VCE subjcets you’ve chosen.

4. Do not “over-indulge” in VCE tutoring. Your tutors and teachers can only take you so far. The highest-achieving students are those who are self-motivated: they push themselves and study even when nobody asked them to. Become self-motivated and use your tutoring time wisely to maximise your performance in VCE exams.

Tips from Alastair Weng at Cloudninetutoring.com

1. Maintain good study habits. Get more information on study habits here.

2. Keep a balanced life. Stay healthy by socialising and exercising regularly. Don’t sacrifice health for your ATAR: a healthy body helps maintain a healthy mind.

3. No regrets. Remember that the sacrifices you make today will pay off in the future.

Tips from Akhil on the BoredofStudies.org forum

1. Stay a whole module ahead.

2. There are two things you need to do: make great notes and do practice questions. 

3. Build on your notes from external sources (other people’s notes and the textbook)

4. Mark your questions – or get them marked! Akhil says that while it’s an excellent learning exercise to practice marking questions by yourself, it’s also necessary to get your practice papers and Checkpoints questions marked by a teacher or tutor because they’ll be more vigilant with sticking to the marking scheme and can pick up slight errors in wording that are easy to miss if you mark your own work.

Want more? Try How to Get Ahead in VCE Chemistry

Do you know of any more study tips? Are there any crucial tips missing from this list? Post them into the comments section below.

Chemistry Task Words

Chemistry VCE task words verbs for Chemistry education and instruction
Click for a PDF version of these task words

RTQ! This is one of the most common sources of errors in Chemistry examinations. When I sat 2014’s VCE Chemistry examination, I lost 5 marks in the paper for not reading the question! Your teachers will have told you to ‘read the question’ or ‘RTQ’ as well.

Task word errors can be avoided in two ways. First, learn the exact meanings of each task word. This is particularly important for EAL Chemistry students. Second, highlight the task words in a question (just as you would highlight the important information in a complicated titration question).

For example: “Explain how the different intermolecular forces in butane and butan-1-ol give these two compounds different boiling points. 3 marks

In your answer, you will need to explain the effect of intermolecular forces. This means you’ll need to write why the butan-1-ol forms hydrogen bonds (due to the polar nature of the hydroxyl group) whereas butane forms only dispersion forces with its surrounding molecules (due to the non-polar nature of the molecule). You’ll also need to make some kind of comparison (which is hinted at by the word, ‘different’) in order to get all 3 marks.

Example 3-mark answer: “Butan-1-ol forms intermolecular hydrogen bonds with the surrounding molecules due to the polar nature of the hydroxyl group (O-H bond). Butane forms only dispersion forces with its surrounding molecules due to the non-polar nature of the molecule. Hydrogen bonds are stronger than dispersion forces and thus require more energy to break. This results in a higher boiling point for butan-1-ol than for butane”.

One mark would be awarded for each of:

  • Explaining the intermolecular bonding of butan-1-ol
  • Explaining the intermolecular bonding of butane
  • Comparing the relative strengths of the two and relating this to boiling points

In a 2-mark answer, the student might omit the comparison step:

Example 2-mark answer: “Butan-1-ol forms intermolecular hydrogen bonds with the surrounding molecules due to the polar nature of the hydroxyl group (O-H bond). Butane forms only dispersion forces with its surrounding molecules due to the non-polar nature of the molecule.”

In a 1-mark answer, the student might only mention one of the two molecules, or might only make a comparison without explaining why these two compounds display different types of intermolecular forces.

Example 1-mark answer: “Hydrogen bonds formed by butan-1-ol are stronger than dispersion forces formed by butane and thus require more energy to break. This results in a higher boiling point for butan-1-ol than for butane”.

In that latter example, the student didn’t explain the reasons for the differences in intermolecular bonding – they merely stated them.

Task word Chinese Description
Calculate 计算 Write the value of a number (include equations)
Compare 比较 Write the similarities and differences between
Evaluate 评价 Write arguments for and against
Define 确定 Write the exact meaning of
Describe 描述 Write details about (a thing or a process)
Discuss 讨论 Write reasons for and against
Distinguish 区分 Write the differences between two or more things
Explain 讲解 Write details to give the reader an understanding of
Find/State Write (sometimes by doing calculations)
Identify 鉴定 Write which one
Illustrate 说明 Write something and draw a labelled diagram as well
Indicate 表明 Write which one (usually on a given diagram)
List 列出 Write a list
Outline 轮廓 Write a summary
Suggest 建议 Write a reason for a phenomenon
To what extent 到什么程度 Write whether a reaction is complete (→) or incomplete (↔).

Watch task words in the examination… and make sure you answer the question!

3 Things You Take With You from Year 12

1) Friendships

Memories and connections are some of the most valuable things you’ll take with you from Year 12. Keep in touch with as many people as possible both officially (using alumni networks) and unofficially (using social media). People move in different directions after graduation and you’ll be surprised at how your friendships evolve, too: classmates who were mere acquaintances during school might become very close friends in five years’ time. Keep in touch with all your classmates to make sure you don’t miss out on these future business connections, too. You might even meet again one day sitting opposite each other at a job interview!

2) ATAR

Remember that your ATAR is only a means to a much more meaningful goal: it’s the key to a university course of your choice. Strive for an ATAR that’s high enough: there’s no need to stess yourself out by aiming for a ‘perfect’ score of 99.95. Your ATAR is like a disposable key: it gets you into university but doesn’t help you while you’re there. Nobody asked me what my A-level results were throughout my undergraduate years at Cambridge. High-school results simply weren’t important.

3) A Relentless Work Ethic

You’ve worked harder in Year 12 than you’ve ever worked in your life. If you want to be successful, you’ll have to maintain this level of hard work – or even increase it – to accomplish your goals in life. You’ve learned the difficult way that in Year 12, going to school and doing all the required homework isn’t enough. You’ve figured out in Year 12 that you have to spend hours reading the textbook by yourself, doing practice question sets that aren’t on the course, and making summary notes that your teacher will probably never see in order to get a high grade.

The relentless work ethic you’ve garnered will help you to conquer bigger obstacles in the years that follow. Give every major event in your life at least as much passion, dedication and preparation that you gave to your VCE examinations and you’ll be sufficiently prepared for the challenges that await you in the future. VCE is pre-season training for life.

Is there anything I’ve missed from this list? Is an ATAR more than just a “key to a university course”? Let us know in the comments section below.

Make Your Own 2015 VCE Revision Timetable

Click to download by Sample 2015 VCE Revision Timetable
Click to download by Sample 2015 VCE Revision Timetable

You’ve got 100 days until your English examination and full-time revision should begin from today.

How to Make a Revision Timetable

First, print my 2015 wall calendar in A3 size or larger. The left, middle and right of each day-box represents each of three study sessions:

  • Morning session: 8am to 12pm (make a dot to the left)
  • Afternoon session: 1pm to 5pm (make a dot in the middle)
  • Evening session: 6pm to 9:30pm (make a dot to the right)

Next, use coloured stickers from Officeworks (or coloured markers) to label your examinations. Use a different colour for each subject. Working backwards from those examinations, put more stickers on the chart to denote which subjects you’ll study in each study session.

Rules when filling your timetable:

  • Plan 100 revision sessions in the 100 days before your first examination
  • Try not to plan revision sessions on school days – save that time for homework!
  • Adjust the number of sessions you will have for each subject: you might want to focus more on some subjects than on others, or prepare for them all equally. It’s up to you.
  • Revise for 12 sessions each week that you’re not in school
  • Revise for no more than two sessions in a day
  • Avoid the evening session when possible.
  • Use your free time to relax or get some exercise.
  • You may move a study session but you are not allowed to cancel it

Make Your Own Revision Timetable

Blank 2015 calendar
Click to download a printable 2015 calendar

This strategy worked extraordinarily well for me during my A-level studies. I studied this much (48 hours per week) and achieved an equivalent ATAR of over 99. What’s your revision strategy? Leave your ideas in the comments section below.

How to Deal with Exam Stress

How to Deal with Exam Stress Infographic from StopProcrastinatingApp.com
Source: StopProcrastinatingApp.com

It’s that time of year when students are starting to plan their exam revision. Getting to grips and memorising all you have learn over the past year is only half the battle, as new research from productivity website Stop Procrastinating has found that 64% of students believe that exam stress and anxiety is affecting them so much that it will lower their performance and affect their grades.

The poll of 2000 undergraduates heading into their final exams found that 66% of students believe their stress levels are greater than in the past due to modern day problems, such as the difficult jobs market. They feel that a lower grade could affect the rest of their lives, closing doors to opportunities and causing them to miss out on jobs.

The survey found that procrastination was a major cause of stress. Students today have more opportunities for distraction with the rise of the Internet, smart phone and social media. A massive 45% of students surveyed said they wasted time on the Internet or social media instead of revising.

There is good news, however. The survey also found the strategies and solutions that students find most effective. By using Internet blockers while revising, taking more exercise, and by breaking down revision into manageable, bite sized-chunks, students are finding ways to cope and succeed.

The full list of effective revision strategies is available at Stop Procrastinating’s website here.