For VCE Chemistry, you receive a data booklet for all your assessments. This is written by VCAA and contains formulas and information to aid you in answering questions.
It is very important to become familiar with what your data booklet includes and how to use it – you don’t want to lose any time in the exam!
This article will go through each page of the VCE Chemistry data booklet and discuss how you can effectively use what is provided.
Let’s dive in!
1. Electrochemical series
2. Chemical relationships
3. Physical constants and standard values
4. Unit conversions
5. Metric prefixes (including SI prefixes)
6. Acid-base indicators
7. Colours of selected conjugate redox reagents
8. Formulas and charges for selected ions
9. Solubility table
10, 11. Average bond enthalpies at 25°C – single and multiple bonds
12. Energy content of food groups
13. Molar enthalpies of combustion
14, 15. Heats of combustion of selected blended fuels and biofuels
16, 17. Periodic table of the elements and names of selected elements
18. Representations of organic molecules
19. Functional group nomenclature in organic chemistry
20. 2-amino acids
21. Formulas of selected fatty acids
22, 23, 24. Characteristic ranges for infrared absorption, 13C NMR data and 1H NMR data
25. Representation of selected biomolecules
26. Sustainability
1. Electrochemical series
This will be a point of reference for any questions referring to redox or electrolysis reactions. The electrochemical series uses double arrows to show both the reduction and oxidation reaction for each element, as well as its standard electrode potential.
Note: Remember that this standard electrode potential is calculated under Standard Laboratory Conditions
How do you use the electrochemical series?
To effectively use your electrochemical series in your VCE Chemistry data booklet, follow these steps to identify the half equations.
Firstly, circle all reactants that are present in the question – including water in aqueous solutions!
If the question is referring to a redox or spontaneous reaction, draw a backwards Z between the two reactants that gives the biggest gap. For example:
All reactants present are circled in green. Then, find the highest oxidant (on the left) and the lowest reductant (on the right). In other words, the strongest oxidant and the strongest reductant present.
In this example, Au+(aq) is the strongest oxidant and Cu(s) is the strongest reductant.
When we join the two, we can draw a backwards Z showing which direction each reaction occurs in. As a result, we find our two half equations:
Cu(s) → Cu2+(aq) + 2e–
Au+(aq) + e– → Au(s)
For electrolysis and spontaneous reactions, we go in the opposite direction. We draw a forward Z with the smallest gap. For example:
This time, we choose the oxidant and reductant that produce the smallest gap: H2O
From this Z, we can see the two half equations:
O2(g) + 2H2O(l) + 4e– → 4OH–(aq)
2H2O(l) → O2(g) + 4H+(aq) + 4e–
Once you have your half equations, you need to balance them to ensure they have the same number of electrons.
Cu(s) → Cu2+(aq) + 2e–
(Au+(aq) + e– → Au(s)) x 2 = 2Au+(aq) + 2e– → 2Au(s)
You can then combine them to get the overall equation, cancelling any atoms or electrons they have in common.
2Au+(aq) + Cu(s) → 2Au(s) + Cu2+(aq)
The other piece of information you may need to use from the electrochemical series is the standard electrode potential.
The voltage produced from a reaction is the standard electrode potential of the reductant minus the standard electrode potential of the oxidant. This is the formula:
E0 of cell = E0 (reductant) – E0 (oxidant)
If a question is referring to a reversible or secondary cell and asks you the required energy input, the answer is slightly more than [the E0 of the cell].
Make sure you familiarise yourself with these steps to ensure you can effectively use the electrochemical series in your VCE Chemistry data booklet to gather half equations. It is also important that you know the direction of increasing oxidant strength and increasing reductant strength.
2. Chemical relationships
This section of the VCE Chemistry data booklet gives you some key formulas. While this is very helpful as you don’t have to memorise these formulas, you do need to know what units each of them are in.
Formula Units
n = m/M n: mol, m: grams, M: relative atomic mass
n = V/Vm n: mol, V: litres, Vm: always 24.8L/mol
n = c x V n: mol, c: M (molarity), V: litres
Universal gas equation: p x V = n x R x T p: kPa, V: litres, n: mol, R: always 8.31 J/mol/K, T: Kelvins
Q = I x t Q: C (charge in Coulombs), I: amps, t: seconds
q = m x c x ∆T q: Joules, m: grams, c: specific heat capacity (will be given or if water: 4.18 J/g/K), ∆T: Kelvins
Chemical CF = E / ∆T E: Joules, ∆T: Kelvins
Electrical CF = (V x l x t) / ∆T V: Voltage, l: Amps, t: seconds, ∆T: Kelvins
Molar Enthalpy change: ∆H = q/n q: KJ/mol, n: mol
Amount of electrons: n =Q/F Q: C (charge in Coulombs), F: Faraday Constant
You also need to be comfortable rearranging each of the formulas, depending on what the question is asking you to find.
Often, the best way to ensure you are using the formula correctly is to copy it out from the data booklet and then substitute the information that the question has given you (in the correct units). Then, rearrange to find the unknown.
Check out our tips to effectively using the VCE Physics Formula Sheet !
3. Physical constants and standard values
These are constants that may appear in your calculations and always have the same value.
For this section, you really just need to know which formula each of the constants appear in and make sure to substitute them in correctly.
4. Unit conversions
These conversions are especially important when the formula you need to use requires a different unit to the one the question has provided. An effective way to do conversions is shown below:
First, write the ratio given to you. Then write the value you are trying to convert below the number with the same unit. Divide by the number above, and then multiply by the number next to it. This will give you the converted value.
5. Metric (including SI prefixes)
This table helps if you are ever unsure as to what a prefix means in numbers. For example, you may come across nanometres and micrometres in your exam. This table in the VCE Chemistry data booklet can help you convert between units.
6. Acid-base indicators
You will need to use this table to decide which indicator to use in titrations and volumetric analysis.
To use this effectively you need to first figure out the range of values which the equivalent point occurs in. This will lead you to a certain indicator from the list.
Next, you may need to determine which direction the colour change occurs. It is important to note that the colour changes listed in your data booklet occur when the solution starts from a lower pH and becomes higher. This isn’t always the case so you need to double check.
Read our comprehensive guide on ‘Everything You Need to Know about VCE Chem’ !
7. Colours of selected conjugate redox reagents
In some VCE Chemistry questions, the brief will state the a certain colour appears or is present in a substance or reaction. When the question takes note of a specific colour, look at this table, because it’ll inform you of what conjugate redox reagants are present.
Please note that you can also use the conjugate redox reagents to determine what colour a substance or reaction will be.
8. Formulas and charges for selected ions
Pretty self explanatory, this table just guides you as to what charge particular ions have. Note that there is a table for cations (positive charge) and anions (negative charge)!
You’ll use this in questions like cells and electrolysis, where the charge of particular compounds and elements are necessary.
9. Solubility table
This table outlines which salts are soluble and insoluble.
Soluble things dissolve, while insoluble things do no dissolve. So, the purpose of the solubility table is to determine whether a substance will dissolve or not in water. This content will typically be used in fuels and electrolysis!
10, 11. Average bond enthalpies at 25°C – single and multiple bonds
Bond enthalpies display the amount of energy required to break a bond. These two tables display the bond enthalpies for single and multiple bonds between various elements.
These tables will be used to determine whether a reaction will take place and whether there is any bond between elements at all.
12. Energy content of food groups
This table is useful when calculating the energy content of a food based on its components. The formula is quite simple: you multiply the amount of the food group (grams) by its corresponding energy content value in the table.
The one thing to remember is that cellulose cannot be broken down by the human body as we lack the enzyme, so we cannot include it in our calculations. If the question indicates that cellulose is included as a subcategory of carbohydrates, we must take away the amount of cellulose from the total amount of carbohydrates before multiplying.
13. Molar enthalpies of combustion
The Molar enthalpy of combustion is the heat energy given out when one mole of a substance burns completely in oxygen.
Please note that these are calculated in standard laboratory conditions, with the standard combustion products (water and oxygen gas). Also, the molar enthalpies are negative because of the exothermic nature of combustion reactions.
You’ll use this table in the fuels topic, while looking at combustion reactions.
14, 15. Heats of combustion of selected blended fuels and biofuels
You will need to use the values in this table when determining thermochemical equations. Just keep in mind mole ratios; these values are calculated based on one mole of the fuel.
The values are all positive because they represent the amount of heat energy released, however, it is important to remember that when you deal with enthalpy of combustion (∆H) your value could be positive or negative depending on whether the reaction is endothermic or exothermic.
Also, it is important to note that we need to use heat of combustion kJ/g instead of molar heat of combustion when dealing with mixtures, as we cannot determine the molar mass of a mixture. In saying this, section 12 gives you the heat combustion of three common blended fuels.
16, 17. Periodic table of the elements and names of selected elements
The first page of your VCE Chemistry data booklet contains the periodic table of the elements.
By the time you reach VCE Chemistry, you will be familiar with some of the information that this table offers like the atomic number, element name and symbol, and relative atomic mass of each element.
In VCE, you will learn several trends that you can identify from the periodic table such as electronegativity, atomic radius, and electron shell configuration.
The most common piece of information you will need from the periodic table is the relative atomic mass.
You will often need to use the relative atomic mass in calculations, such as calculating the amount of a substance, so it is important that you can identify elements by both their names and symbols; in your exam the question may only refer to an element by symbol.
The names of selected elements just provides the same information as the periodic table but in an easier to read format, so if you get stuck with the periodic table, make sure to use it!
18. Representations of organic molecules
This table is a friendly reminder of the different ways you may be asked to demonstrate an organic molecule in VCE chemistry. If you are ever unsure in the exam, especially with skeletal formula as this can be tricky, consult this page.
19. Functional group nomenclature in organic chemistry
This table shows the priority functional groups when naming organic compounds. Remember, the suffix group with the highest priority determines the suffix of the compound.
When studying organic chemistry, this table is your best friend. Make sure to become really familiar with it before your SACs and exam!
20. 2-amino acids
This table of amino acids contains their full name, symbol and simplified structure.
You may be asked to identify the products of hydrolysis of a protein, or conversely, you may be asked to draw a section of a polypeptide chain. Either way, you need to know how to ‘open’ the bonds of an amino acid. Like so:
You will also need to know how to draw a zwitterion. Always check what pH the question is referring to — if it is very low or very high, you will need to check whether you can ionise the side chain.
The best way to use this section of the VCE Chemistry data booklet is to draw the full structure of the amino acid, while keeping the side chain semi-structural. This will make it easier to break or form bonds between amino acids, as you can visualise what is happening.
Do not worry about trying to memorise what each amino acid looks like, however, some common ones to become familiar with are alanine, glycine, glutamine and aspartic acid. Just make sure that you check the side chains very carefully in your assessments, as some amino acids are very similar.
21. Formulas of selected fatty acids
The main thing to keep in mind with these fatty acids is paying attention to the bonds when drawing them, as there are many repeats in the fatty acid tails. If you draw them in semi-structural form, you can put brackets around a section that is repeated, ensuring that the bonds extend past the bracket. Like so:
22, 23, 24. Characteristic ranges for infrared absorption, 13C NMR data, 1H NMR data
The next three sections of the data booklet are vital for determining a molecule from spectra data.
Firstly, you can determine the type of bonds present from analysing an infra-red spectrum. Find the range of wavelength values where the absorption peak(s) occur and consult the data booklet’s table to figure out which type of bond is therefore present in the molecule.
Then, the 13C NMR and 1H NMR data will help you identify the types of carbon and hydrogen environments present.
The NMR spectra will show you the number of carbon/hydrogen environments (based on the number of peaks), the ratio of atoms in each environment (based on peak area), and the type of environment present (based on chemical shift) — this is what the data booklet’s table is based off.
Using the chemical shift (ppm away from TSM) of a peak, you can identify the carbon or hydrogen environment.
Note: For the 1H NMR data, the H that is bolded is the hydrogen atom that the chemical shift corresponds to.
For these types of questions, you will need to collect all of these pieces of information and then put it all together to determine the unknown molecule.
Read our guide on what to do the night before the VCE Chemistry exam!
25. Representation of selected biomolecules
This section just displays how glycerol, alpha glucose, amylose (starch) and amylopectin (starch) is structured in visual diagrams.
You will need to understand how to use these diagrams to identify he selected biomolecules and even redraw them under different contexts!
These diagrams will become important when you study organic chemistry in Unit 4.
26. Sustainability
This section outlines sustainable goals, green chemistry principles, and sustainable economic processes in a chemistry context.
Sustainability is a new topic that will be explored in Unit 3 and 4. You will tackle questions that require you to assess the sustainability of various chemical processes that you study throughout the year.
The principles outlined in the Chemistry Data Booklet can help guide your answers and provide points for you to address.
There you have it!
Now that you have some tips and tricks for using your data booklet, make sure to practise these techniques when you complete practice questions and some VCE Chemistry past papers.
Becoming familiar with your data booklet early on will save you a lot of time in the exam and ensure that you make the most of what VCAA is giving you!
Follow our steps to acing your end of year VCE Chemistry exam!
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Narisha Ford is an avid student who loves all things from studying the immune system, to analysing poetry, and learning how to differentiate logarithms. She graduated in 2021 with a 99+ ATAR and is thrilled to be a part of the AOS Content Writing team to support students through their VCE journey. She hopes to one day work in the international security field, but is still figuring everything in life out!
