CHEM1011 · Fundamentals Of Chemistry 1a
The Complete Exam Bible · S1 2026Fundamentals of Chemistry 1A
Fundamentals of Chemistry 1A builds the language and quantitative core of chemistry — atoms, the mole and stoichiometry, periodic trends, bonding and molecular shape, organic structure, thermodynamics, equilibrium, and acids and bases. The final exam is 55% of your grade and is closed-book, and the laboratory is a separate hurdle you must pass to pass the unit, so this guide teaches each topic to exam standard: the method examiners reward, the formula they expect, and the calculation steps that earn the marks.
What CHEM1011 covers
Thirteen weeks of foundational chemistry → one exam-ready map. Each topic links to its free chapter guide.
How CHEM1011 is assessed
| Component | Weight | Format |
|---|---|---|
| Final exam | 55% | Supervised closed-book exam · 130 min · ~1/3 MCQ + 2/3 short answer · datasheet & periodic table provided |
| Laboratory · hurdle | 25% | Labtorials, logbook, technique competency & major assessment — must be passed to pass the unit |
| Weekly quizzes | 14% | Online Canvas quizzes from Week 2; best 9 marks count |
| Checkpoint quiz | 5% | Week 7, 40-minute online open-book quiz |
| Early feedback task | 1% | Week 1 online quiz (due Week 2) |
Limiting reagent & mass of product — the workhorse calculation
- +1Convert each mass to moles: n(H2) = 6.00 / 2.016 = 2.98 mol; n(Cl2) = 35.0 / 70.90 = 0.494 mol.
- +1Compare moles ÷ coefficient (the ratio is 1:1): 0.494 < 2.98, so Cl2 is the limiting reagent.
- +1Scale to product by the mole ratio: n(HCl) = 2 × 0.494 = 0.988 mol.
- +1Convert to mass: m = n × M = 0.988 × 36.46 = 36.0 g HCl.
Key terms
- Mole (n)
- The amount of substance containing Avogadro's number (6.022 × 1023) of particles; linked to mass by n = m/M, where M is the molar mass in g mol−1.
- Limiting reagent
- The reactant that runs out first; it caps the amount of product. Found by comparing each reactant's moles divided by its stoichiometric coefficient.
- Electronegativity
- The ability of a bonded atom to attract the shared electrons; it rises across a period and falls down a group, and a large difference (ΔEN) signals ionic rather than covalent bonding.
- Enthalpy change (ΔH)
- The heat absorbed or released at constant pressure; a negative ΔH is exothermic, a positive ΔH endothermic. It is path-independent (Hess's Law).
- Equilibrium constant (K)
- The ratio of product to reactant activities at equilibrium for aA + bB ⇌ cC + dD: K = [C]c[D]d / [A]a[B]b; pure solids and liquids are omitted.
- pH
- A measure of acidity: pH = −log10[H3O+]; pH + pOH = 14 at 25 °C, and at the half-equivalence point of a weak-acid titration pH = pKa.
CHEM1011 FAQ
Is CHEM1011 hard?
It is concept-broad and calculation-dense rather than conceptually deep: most marks come from applying a standard method (moles, Lewis structures, ICE tables, pH) accurately and to the right number of significant figures. Because the final exam is 55% and closed-book and the laboratory is a separate hurdle, the difficulty is precision under exam conditions.
How is CHEM1011 assessed?
The final exam is 55% and closed-book; the laboratory is 25% and a hurdle you must pass to pass the unit; weekly online quizzes are 14% (best nine count), a Week 7 checkpoint quiz is 5%, and an early-feedback task is 1%. Confirm the current weights in your own unit outline.
What is on the CHEM1011 final exam?
About one-third multiple choice (30 questions) and two-thirds short answer over 130 minutes. It covers the whole lecture course: atoms and the mole, stoichiometry, periodic trends, Lewis structures and VSEPR, organic structure and isomers, thermodynamics, equilibrium, and acids and bases. A datasheet and periodic table are provided.
Do I have to memorise the constants and the periodic table?
No — a datasheet of constants and a periodic table are provided in the exam. What you must bring is the methods: how to set up a mole calculation, build a Lewis structure, run an ICE table, and work a titration. This guide drills exactly those workflows.
Is using AskSia for CHEM1011 cheating?
No. AskSia is a study reference written in our own words — we host none of your lecturer's files, and Sia teaches you the method to earn the marks; it does not complete or sit your assessments.
How to study for the exam
Treat chemistry as a set of repeatable calculation workflows. For every topic, practise the method from a blank page: the mole map (n = m/M), the limiting-reagent comparison, the five-step Lewis build, the VSEPR angle table, the two routes to ΔH, the ICE table, and the titration region map. Memorise the methods, not the constants — the datasheet and periodic table are provided. Because the final is 55% and closed-book and the laboratory is a hurdle, banked, well-practised calculation marks are the safest marks in the unit.
