HSC Chemistry Data Sheet the best annotated guide

The HSC Chemistry data sheet can be overwhelming to look at and confusing to follow, that why we have created this guide to help you navigate it.

  • Access the original version from NESA here

Want more top tier HSC chemistry resources? Our open access HSC Chemistry digital textbook is available here

Page 1

HSC chemistry data sheet - the formulas within it.

n is the number of moles (moles)

c is the concentration in (moles/L)

V is the volume (L)

T is the temperature in kelvin (K)

q is the molar heat (J/mol)

delta G is the change in free energy (kJ/K⋅mol)

delta H is the the amount of heat released or absorbed in a reaction carried out at constant pressure (kj/mol)

delta S is the change in disorder of a system (kJ⋅K-1mol-1)

[H+] is the concentration of protons (M or mol/L)

pH is the -log[H+] and is unitless

ka is disassociation constant /[reactant]

pKa is unitless

A is the absorbance and is unitless

l is the pathlength (cm)

Na is Avogadro’s constant is the number of molecules in a mole, this is a constant

This part of page 1 on the HSC Chemistry Data Sheet is useful for determining what salts are are going to be insoluble. Additionally, there will be questions which require you to use the solubility constant (Ksp), usually these are from module 5 – equilibrium or module 8 – applying chemical ideas.

Reference for the solubility constants.

Page 2

This data is valuable for analysing the infrared absorption spectra, C NMR spectra and UV-vis absorption spectra. This will be used for module 8 questions. Often you will be given a graph/s of unknown compounds and be required to identify the features, correlate them to the known characteristics on page 2. As a result, you can identify the unknown chemical compound.

HSC chemistry data sheet reference for the module 8 data.

Page 3

Arguably this page is more important for year 11 HSC chemistry as opposed to year 12. It tells us the standard potentials with formation of hydrogen gas being our reference. Remember, OIL-RIG, oxidation is loss of electrons, reduction is gain of electrons. So the potentials given are reduction potentials. If we reverse the equation and take the negative of the reduction potential, we will have the oxidation standard potentials, e.g Pb(s) <–> Pb2+ + 2 e is 0.13 V

Reference for the standard potentials.

Page 4

This is the periodic table of elements as found in the HSC Chemistry Data Sheet.

  • Electronegativity increases as you approach the top right corner of the periodic table, with Fluorine being the most electronegative
  • As you go down the periodic table, the atoms get bigger
HSC chemistry periodic table.

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