CHEM10007: pass the exams, not just read the notes
Your complete guide to University of Melbourne's fundamentals of chemistry unit. See where the marks are, work real practice questions, and study with an AI tutor that knows CHEM10007.
Sia generates CHEM10007 practice questions, works through them step by step, and quizzes you on the material the exam weights most heavily.
Worked example
How many moles of water are there in 36 g of water? (Molar mass of H2O = 18 g/mol.)
The mole relationship is amount (mol) = mass (g) / molar mass (g/mol).
n = 2 mol.
So 36 g of water is 2 moles (and contains 2 × Avogadro's number of molecules).
The trap: Multiplying mass by molar mass (36 × 18 = 648) instead of dividing. Moles are mass divided by molar mass; multiplying gives a meaningless number far larger than any real amount here. classic slip!
One exam decides 60% of your grade. This whole page is built around that.
Overview
What CHEM10007 is, and where it sits
CHEM10007 Fundamentals of Chemistry is the University of Melbourne's foundational first-year chemistry subject, taught in the School of Chemistry and designed for students who need core chemistry without assuming a strong prior background. It covers atomic structure and periodicity, chemical bonding and molecular structure, stoichiometry and the mole concept, states of matter, chemical equilibrium and acids and bases, energetics, and an introduction to organic chemistry, supported by a substantial laboratory program.
Assessment blends a 60% end-of-semester exam with continuous work: online feedback quizzes, pre-laboratory quizzes, a sustainability learning task, and hands-on practical work. The recurring quantitative skill is the mole-based reasoning that connects masses, amounts and concentrations, alongside the conceptual understanding of bonding and equilibrium the exam tests.
Official outline: handbook.unimelb.edu.au · CHEM10007 outline. Always treat the official outline and the exam timetable as authoritative.
Difficulty & time commitment
Is CHEM10007 hard, and how much time does it take?
CHEM10007 is manageable if you keep a weekly rhythm and treat the back half as the main event. The pattern is consistent: it starts gently and steepens, and the heaviest assessment is the part that separates grades.
The difficulty curve and the assessment weighting point the same way: the back half is harder and worth more. Front-loading effort there is the highest-return decision in the unit.
Is this unit for you
Who tends to do well, and who tends to struggle
You will likely do well if
- You are comfortable with mole-based arithmetic and unit conversions and practise stoichiometry until it is automatic.
- You keep up with the continuous quiz and laboratory work rather than relying only on the final.
- You build genuine understanding of bonding and equilibrium concepts, not just memorised facts.
You may struggle if
- You are shaky on the mole concept, which underpins most quantitative questions.
- You treat the labs and pre-lab quizzes as optional, losing continuous marks.
- You memorise without understanding equilibrium and bonding, which the exam probes conceptually.
- Make mole conversions (mass to moles to particles to concentration) completely automatic.
- Prepare thoroughly for each practical with the pre-lab quiz so lab time is productive.
- Practise equilibrium and acid-base problems, common exam material that rewards understanding over recall.
Syllabus
The 11 topics, topic by topic
The exam-weight marker on each topic shows where the marks concentrate. The amber topics carry the highest exam weight.
T1 · Atoms, the Periodic Table & Electronic Structure
Matter, isotopes, atomic mass, the Bohr & quantum-mechanical models, electron configuration and periodic trends (Wks 1-2)
T2 · Chemical Bonding, Lewis Structures & Shape
Ionic, covalent and metallic bonding; common ions; naming; drawing Lewis structures and molecular shape (Wk 2)
T3 · Intermolecular Forces, Chemical Reactions & the Mole
Polarity & IMF, balancing equations, precipitation/net-ionic reactions, the mole concept, molar mass and empirical formula (Wks 3-4)
T4 · Stoichiometry, Solutions & Gases
Mass-mass stoichiometry, limiting reagents, percentage yield, significant figures, molarity, the gas laws and ideal-gas calculations (Wks 4-5)
T5 · Thermochemistry, Calorimetry & Hess's Law
Energy, heat and work; enthalpy; calorimetry (q = mcDeltaT) and Hess's Law (Wks 5-6)
T6 · Redox & Electrochemistry
Oxidation numbers, balancing redox half-equations, galvanic cells and EMF, and electrolysis (Wks 6-7)
T7 · Reaction Kinetics
Reaction rate, factors affecting rate, activation energy and catalysts (Wk 7)
T8 · Chemical Equilibrium
Dynamic equilibrium, Kc, the reaction quotient Q and Le Chatelier's Principle (Wk 8)
T9 · Acids, Bases & Aqueous Equilibria
Bronsted-Lowry acids/bases, pH/pOH, weak-acid equilibria with ICE tables, buffers and solubility (Ksp) (Wks 8-9)
T10 · Organic Chemistry I: Alkanes, Isomerism & Stereochemistry
Alkane structure and IUPAC naming, structural isomers, Newman conformations, chirality and R/S, and the functional-group map (Wk 10)
T11 · Organic Chemistry II: Alkenes, Alkynes & Aromatics
Cycloalkanes, cis-trans and E/Z isomerism, alkenes and alkynes, polyenes and benzene (Wk 11)
How it's assessed
Assessment structure
| Component | Weight | Format & timing |
|---|---|---|
| Online Feedback Quizzes (FBQ-1 to FBQ-5) | 10% | 5 quizzes (2% each), 30-min online MCQ, open across the relevant weeks. |
| Sustainability Independent Learning Task (ILT) | 5% | Online interactive quiz on sustainability (content not covered in lectures), due Week 12. |
| Practical work (laboratory) | 20% | 6 experiments F1–F6; 6 lab worksheets/reports; report cannot be submitted without doing the experiment. YES. |
| Pre-Laboratory Quizzes | 5% | 5 online quizzes, each completed before its practical class (no quiz = no lab entry). |
| Exam | 60% | On-campus, closed-book, 2 h writing + 15 min reading; Section A MCQ (60 marks) + Section B extended written (60 marks); appendices booklet provided. |
- Pass on a weighted average of at least 50%. No single-component hurdle unless noted; confirm against the official subject page.
This is an exam-cram unit. With the exams at 60% of the grade and the exam alone at 60%, your result is overwhelmingly decided by how well you perform under time pressure.
How to actually pass it
A weekly rhythm, two checklists, and the traps to avoid
The unit rewards consistency over cramming, and practice over re-reading. Here is the loop that works, then what to have nailed before each exam.
The weekly loop
Before the mid-semester checklist
Before the final heaviest topics
- Drill stoichiometry and mole conversions until they are automatic.
- Revise chemical bonding and molecular structure at the concept level.
- Practise equilibrium and acid-base calculations, common exam topics.
- Review the energetics and introductory organic material for the 60% final.
The mistakes that cost marks
Confusing multiply and divide for moles. Moles equal mass divided by molar mass. Multiplying instead is the classic stoichiometry error and derails any calculation that builds on it.
Neglecting the labs. Practical work and pre-lab quizzes are continuous marks and reinforce concepts; skipping them costs marks and understanding.
Memorising over understanding. The exam probes why bonding and equilibrium behave as they do; rote facts without reasoning cap the achievable mark.
Teaching team
Who teaches CHEM10007
The bios below are factual. We do not rate lecturers; any star ratings are submitted by students who have taken CHEM10007.
Dr Sonia Horvat
Director of First-Year Studies in the School of Chemistry, University of Melbourne, and a CHEM10007 lecturer.
Mr Mick Moylan
Lecturer for CHEM10007 in the School of Chemistry, University of Melbourne.
Dr Patricia Jackson
Lecturer for CHEM10007 in the School of Chemistry, University of Melbourne.
Associate Professor Lars Goerigk
Deputy Director of First-Year Studies in the School of Chemistry, University of Melbourne.
Teaching team as listed in the unit materials reviewed. AskSia does not rate lecturers; star ratings are submitted by students who have taken CHEM10007.
Formula & concept sheet
The vocabulary and formulas you must own
- Mole (amount of substance)
- n = mass / molar mass (n = m / M). One mole contains Avogadro's number (about 6.022 × 10^23) of particles.
- Concentration
- c = n / V: moles of solute per litre of solution (mol/L). Central to solution and titration calculations.
- Stoichiometric ratio
- The mole ratio from a balanced equation that links reactants and products; the basis of limiting-reagent and yield calculations.
- Equilibrium constant
- K expresses the ratio of product to reactant activities at equilibrium; its size indicates how far a reaction proceeds.
- pH
- pH = -log10[H+]: a measure of the hydrogen-ion concentration and hence acidity of a solution.
Common acronyms: mol · M · K · pH · STP.
Where it fits
Prerequisites, related units & why it matters
Foundational first-year chemistry subject; designed for students without a strong prior chemistry background. Check the UniMelb Handbook for the sequence into mainstream chemistry.
Your CHEM10007 study toolkit
Study the unit with Sia, not just read about it
Each tool already knows CHEM10007: your syllabus, your texts, and where the marks are. Grouped by how you study, from first contact to exam week.
FAQ
Frequently asked questions
Is CHEM10007 hard?
It is a moderate first-year subject. The chemistry is foundational rather than advanced, but the 60% exam and the continuous lab and quiz work reward consistent understanding of mole-based reasoning and bonding and equilibrium concepts.
How is CHEM10007 assessed?
A 60% end-of-semester exam, 20% laboratory practical work, online feedback quizzes (10%), pre-laboratory quizzes (5%) and a sustainability independent learning task (5%). The components sum to 100%.
Do I need prior chemistry?
It is designed as a foundational subject for students who need core chemistry without a strong prior background, building the mole concept and bonding from the ground up.
How much maths is involved?
Foundational quantitative work: stoichiometry, moles, concentration and equilibrium calculations. It is arithmetic and algebra rather than heavy calculus.
Is there a lab?
Yes, a substantial laboratory program worth 20% with pre-laboratory quizzes; hands-on practical work is a continuous part of the subject.
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