Y9-10 Acceleration Chemistry · Free Diagnostic Mock

🎁 FREE Diagnostic

15 questions to find exactly where your chemistry is strong — and where it's not

This is a free diagnostic for the Y9-10 Acceleration Chemistry course. 15 multiple-choice questions sample all eight Stage 5 knowledge areas, from chemical bonding to acids, rates and nuclear chemistry.

It's an exam: answer all the questions first (you can change any answer freely), then submit the whole exam to see your report. The worked solutions and hints unlock only after you submit. Use the jump menu at the top to move around.

At the end you get a knowledge-point report: a bar for every topic you attempted, your weak spots flagged, and the exact lessons to revise.

~15 minutes. No login needed. No marks deducted for a wrong answer — never leave one blank.
Self-paced, no time limit — but try to commit to an answer before you review, just like a real test.

Year 9–10 students working at NSW Stage 5. Calculator allowed.

⭐ Q1Y9-10 Stage 5Difficulty ★★Bonding › ionic vs covalent

The Problem

Which type of bond forms between a metal and a non-metal by the complete transfer of electrons?

Your answer

❓ Pick the best answer:

A Covalent bond
B Metallic bond
C Ionic bond
D Hydrogen bond
E Intermolecular force

🎯 Knowledge Point — what this tests

Metals lose electrons and non-metals gain them, forming oppositely charged ions that attract — an ionic bond. Covalent bonds share electrons between non-metals.

Identify whether the elements are metal+non-metal (transfer → ionic) or non-metal+non-metal (share → covalent).

💡 Hint 3 — set up the first step

Metal + non-metal → electrons transferred → ionic.
Two non-metals → electrons shared → covalent.

Metal loses electrons, non-metal gains them → ions attract = ionic bond.

✅ Answer: C — Ionic bond

Why this is the answer: electron transfer between a metal and a non-metal produces an ionic bond. Revise: Lessons 1–5.

⭐ Q2Y9-10 Stage 5Difficulty ★★Bonding › valency & ions

The Problem

A magnesium atom (Group 2) achieves a full outer shell by:

Your answer

❓ Pick the best answer:

A gaining 2 electrons
B losing 2 electrons
C sharing 2 electrons
D losing 6 electrons
E gaining 6 electrons

🎯 Knowledge Point — what this tests

Group 2 atoms have 2 outer electrons. Losing both gives a stable full shell and a 2+ ion (Mg²⁺).

Count outer-shell electrons from the group number, then choose the smallest change to reach 8 (or empty the shell).

💡 Hint 3 — set up the first step

Mg is Group 2 → 2 outer electrons.
Losing 2 is easier than gaining 6 → Mg²⁺.

Losing its 2 outer electrons gives Mg²⁺ with a full shell.

✅ Answer: B — losing 2 electrons

Why this is the answer: metals lose their few outer electrons to form positive ions; Mg loses 2 → Mg²⁺. Revise: Lessons 1–5.

⭐ Q3Y9-10 Stage 5Difficulty ★★Formulae › ionic formula

The Problem

What is the formula of the ionic compound made from Ca²⁺ and Cl⁻?

Your answer

❓ Pick the best answer:

A CaCl
B Ca₂Cl
C CaCl₂
D Ca₂Cl₃
E CaCl₃

🎯 Knowledge Point — what this tests

Ionic formulae balance total charge to zero. One Ca²⁺ (+2) needs two Cl⁻ (−1 each) to cancel.

Cross over / balance the charges so positives equal negatives.

💡 Hint 3 — set up the first step

Ca is +2, Cl is −1.
Need two Cl⁻ to balance one Ca²⁺.

+2 from Ca needs 2×(−1) from Cl → CaCl₂.

✅ Answer: C — CaCl₂

Why this is the answer: two chloride ions balance the 2+ calcium ion, giving a neutral compound. Revise: Lessons 6–8.

⭐ Q4Y9-10 Stage 5Difficulty ★★Formulae › polyatomic ions

The Problem

Sodium carbonate is made from Na⁺ and the carbonate ion CO₃²⁻. Its formula is:

Your answer

❓ Pick the best answer:

A NaCO₃
B Na₂CO₃
C Na(CO₃)₂
D Na₃CO₃
E Na₂(CO₃)₃

🎯 Knowledge Point — what this tests

The carbonate ion CO₃²⁻ carries a 2− charge, so two Na⁺ are needed to balance it. The polyatomic ion stays as one unit.

Treat CO₃²⁻ as a single 2− ion and balance with Na⁺.

💡 Hint 3 — set up the first step

CO₃ is 2−; Na is 1+.
Two Na⁺ balance one CO₃²⁻.

Two Na⁺ balance one CO₃²⁻ → Na₂CO₃.

✅ Answer: B — Na₂CO₃

Why this is the answer: two sodium ions are needed to balance the 2− carbonate ion. Revise: Lessons 6–8.

⭐ Q5Y9-10 Stage 5Difficulty ★Organic › alkanes

The Problem

What is the general formula of an alkane?

Your answer

❓ Pick the best answer:

A CₙH₂ₙ
B CₙH₂ₙ₊₂
C CₙHₙ
D CₙH₂ₙ₋₂
E CₙH₂ₙ₊₁

🎯 Knowledge Point — what this tests

Alkanes are saturated hydrocarbons (only single bonds). Each has the formula CₙH₂ₙ₊₂ — e.g. methane CH₄, ethane C₂H₆.

Check against a known alkane: methane is CH₄, so n=1 must give 4 hydrogens.

💡 Hint 3 — set up the first step

Methane CH₄: n=1 → 2(1)+2 = 4 H. ✓
Ethane C₂H₆: n=2 → 2(2)+2 = 6 H. ✓

Saturated chains follow CₙH₂ₙ₊₂.

✅ Answer: B — CₙH₂ₙ₊₂

Why this is the answer: the saturated alkane formula gives CH₄, C₂H₆, C₃H₈… Revise: Lessons 9–11.

⭐ Q6Y9-10 Stage 5Difficulty ★Organic › combustion

The Problem

Complete combustion of a hydrocarbon in plenty of oxygen produces:

Your answer

❓ Pick the best answer:

A carbon monoxide + water
B carbon (soot) + water
C carbon dioxide + water
D hydrogen + carbon dioxide
E carbon dioxide only

🎯 Knowledge Point — what this tests

With enough oxygen, every carbon becomes CO₂ and every hydrogen becomes H₂O. Limited oxygen gives CO or soot (incomplete combustion).

Plenty of O₂ = complete → the fully oxidised products.

💡 Hint 3 — set up the first step

Enough O₂ → complete combustion.
Carbon → CO₂, hydrogen → H₂O.

Complete combustion fully oxidises C→CO₂ and H→H₂O.

✅ Answer: C — carbon dioxide + water

Why this is the answer: complete combustion gives the fully oxidised products CO₂ and H₂O. Revise: Lessons 9–11.

⭐ Q7Y9-10 Stage 5Difficulty ★Polymers › monomers

The Problem

A polymer is best described as:

Your answer

❓ Pick the best answer:

A a single small molecule
B a long chain made of many repeating monomer units
C a mixture of gases
D an ionic compound
E a metal alloy

🎯 Knowledge Point — what this tests

Polymers are giant molecules built by joining many small repeating units called monomers (e.g. ethene → polyethene).

‘Poly’ = many, ‘mer’ = unit. Find the option meaning many repeating units.

💡 Hint 3 — set up the first step

Monomer = one small unit.
Many monomers joined = a polymer chain.

Many monomers join into a long repeating chain = a polymer.

✅ Answer: B — a long chain of repeating monomer units

Why this is the answer: polymers are long chains built from many repeating monomers. Revise: Lessons 12–13.

⭐ Q8Y9-10 Stage 5Difficulty ★★Equations › balancing

The Problem

Which is the correctly balanced equation for hydrogen burning in oxygen?

Your answer

❓ Pick the best answer:

A H₂ + O₂ → H₂O
B 2H₂ + O₂ → 2H₂O
C H₂ + 2O₂ → H₂O
D 2H₂ + 2O₂ → 2H₂O
E H₂ + O₂ → 2H₂O

🎯 Knowledge Point — what this tests

A balanced equation has equal atoms of each element on both sides. 2H₂ + O₂ → 2H₂O gives 4 H and 2 O on each side.

Count atoms of each element on both sides; adjust whole-number coefficients only.

💡 Hint 3 — set up the first step

Left of B: 4 H, 2 O.
Right of B: 2×H₂O = 4 H, 2 O. ✓

2H₂ + O₂ → 2H₂O balances 4 H and 2 O on each side.

✅ Answer: B — 2H₂ + O₂ → 2H₂O

Why this is the answer: only B has equal numbers of H and O atoms on both sides. Revise: Lessons 16–18.

⭐ Q9Y9-10 Stage 5Difficulty ★★Equations › conservation of mass

The Problem

In a sealed container, 10 g of fuel reacts completely with 32 g of oxygen. What is the total mass of the products?

Your answer

❓ Pick the best answer:

A 10 g
B 32 g
C 22 g
D 42 g
E cannot be determined

🎯 Knowledge Point — what this tests

The law of conservation of mass: in a closed system, total mass of products = total mass of reactants. 10 g + 32 g = 42 g.

Add the masses of all reactants — in a sealed system nothing escapes.

💡 Hint 3 — set up the first step

Mass is conserved in a closed system.
10 g + 32 g = 42 g.

Products mass = reactants mass = 10 + 32 = 42 g.

✅ Answer: D — 42 g

Why this is the answer: mass is conserved, so products weigh the same as the reactants (10 + 32 = 42 g). Revise: Lessons 16–18.

⭐ Q10Y9-10 Stage 5Difficulty ★★Reaction types › displacement

The Problem

A more reactive metal displaces a less reactive one from its salt solution. Which mixture will react?

Your answer

❓ Pick the best answer:

A copper + zinc sulfate
B zinc + copper sulfate
C silver + copper nitrate
D copper + magnesium chloride
E gold + iron sulfate

🎯 Knowledge Point — what this tests

Use the activity series: zinc is more reactive than copper, so zinc displaces copper from copper sulfate. The reverse (copper into a zinc salt) does not happen.

Check whether the free metal is ABOVE the metal in the salt on the activity series.

💡 Hint 3 — set up the first step

Zinc is more reactive than copper → reaction.
Copper/silver/gold are below the salt metals in A, C, D, E → no reaction.

Zn (more reactive) displaces Cu from CuSO₄.

✅ Answer: B — zinc + copper sulfate

Why this is the answer: only here is the free metal more reactive than the metal in the salt. Revise: Lessons 19–21.

⭐ Q11Y9-10 Stage 5Difficulty ★★Reaction types › precipitation

The Problem

Mixing solutions of silver nitrate and sodium chloride forms a white precipitate of:

Your answer

❓ Pick the best answer:

A sodium nitrate
B silver chloride
C silver sodium
D sodium silver nitrate
E no precipitate forms

🎯 Knowledge Point — what this tests

Swap the ions: Ag⁺ pairs with Cl⁻ and Na⁺ with NO₃⁻. Silver chloride (AgCl) is insoluble, so it precipitates; sodium nitrate stays dissolved.

Cross-pair the ions and recall that most silver salts (except nitrate) are insoluble.

💡 Hint 3 — set up the first step

Ag⁺ + Cl⁻ → AgCl (insoluble).
Na⁺ + NO₃⁻ → stays in solution.

AgCl is insoluble → it is the white precipitate.

✅ Answer: B — silver chloride

Why this is the answer: silver chloride is insoluble and forms the white solid; sodium nitrate remains dissolved. Revise: Lessons 19–21.

⭐ Q12Y9-10 Stage 5Difficulty ★Acids › the pH scale

The Problem

A solution with pH 2 is:

Your answer

❓ Pick the best answer:

A strongly basic
B neutral
C weakly basic
D strongly acidic
E a neutral salt

🎯 Knowledge Point — what this tests

On the pH scale, 7 is neutral, below 7 is acidic and above 7 is basic. The further from 7, the stronger. pH 2 is well below 7 → strongly acidic.

Compare the pH to 7 and judge how far away it is.

💡 Hint 3 — set up the first step

pH < 7 → acidic.
pH 2 is far below 7 → strongly acidic.

pH 2 is well below neutral 7 → strongly acidic.

✅ Answer: D — strongly acidic

Why this is the answer: a pH of 2 is far below 7, so the solution is strongly acidic. Revise: Lessons 22–24.

⭐ Q13Y9-10 Stage 5Difficulty ★Acids › neutralisation

The Problem

In the reaction acid + base → ______ + water, the other product is a:

Your answer

❓ Pick the best answer:

A gas
B metal
C salt
D polymer
E precipitate in every case

🎯 Knowledge Point — what this tests

Neutralisation of an acid by a base always produces a salt and water. The salt's metal comes from the base and the non-metal part from the acid.

Recall the standard neutralisation pattern: acid + base → salt + water.

💡 Hint 3 — set up the first step

Acid + base → salt + water.
The non-water product is a salt.

Neutralisation always gives a salt plus water.

✅ Answer: C — salt

Why this is the answer: acid + base neutralisation produces a salt and water. Revise: Lessons 22–24.

⭐ Q14Y9-10 Stage 5Difficulty ★Rate › factors

The Problem

Which change would increase the rate of a reaction?

Your answer

❓ Pick the best answer:

A lowering the temperature
B using larger lumps instead of powder
C increasing the concentration of a reactant
D removing the catalyst
E cooling the mixture

🎯 Knowledge Point — what this tests

Reaction rate rises with more frequent successful collisions — higher temperature, higher concentration, larger surface area (powder), or a catalyst. Increasing concentration packs more particles in to collide.

Pick the change that makes particles collide more often or with more energy.

💡 Hint 3 — set up the first step

Higher concentration → more particles → more collisions → faster.
A, B, D, E all slow the reaction down.

More concentrated reactant → more frequent collisions → faster reaction.

✅ Answer: C — increasing the concentration

Why this is the answer: more particles per volume means more collisions per second, so the rate increases. Revise: Lessons 25–28.

⭐ Q15Y9-10 Stage 5Difficulty ★★Nuclear › radiation types

The Problem

An alpha particle is:

Your answer

❓ Pick the best answer:

A a high-energy electron
B a helium nucleus (2 protons + 2 neutrons)
C a high-energy photon
D a single proton
E a single neutron

🎯 Knowledge Point — what this tests

Alpha radiation is a helium nucleus: 2 protons and 2 neutrons (charge 2+, mass 4). A beta particle is a fast electron; gamma is a high-energy photon.

Recall the three radiation types: alpha = He nucleus, beta = electron, gamma = photon.

💡 Hint 3 — set up the first step

Alpha = 2 protons + 2 neutrons (He nucleus).
Beta = electron; gamma = photon.

An alpha particle is a helium-4 nucleus (2 p + 2 n).

✅ Answer: B — a helium nucleus

Why this is the answer: alpha radiation is a helium nucleus of 2 protons and 2 neutrons. Revise: Lessons 25–28.

🏁 Finish

That's the end of the exam

Go back and change any answers you like. When you're ready, submit the whole exam to lock it in and see your knowledge report — then you can revisit every question to read the full worked solution.

The report stays locked until you submit — you can't open it early.

📊 Diagnostic Report

Your knowledge-point report

Here is how you performed on every knowledge area you attempted. Bars show your accuracy per topic — green is strong, amber is shaky, red needs work. Only questions you answered are scored.

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