Year 9 is the awkward bridge year: still Key Stage 3 in school life, but already starting GCSE habits. This page gives free Year 9 Chemistry practice from GradeNinja's own bank - 61 auto-marked questions across 2 Year 9 topic sets.
The aim is not to cram GCSE papers early. It is to make the first GCSE topics feel normal: short retrieval practice, clear corrections, and enough repetition that classwork sticks before Year 10 gets busy.
Use these as ten-minute checks after a lesson or before homework. If you miss one, read the explanation, then come back tomorrow and answer it cold.
Year 9 questions are pulled from late Key Stage 3 and foundation GCSE bridge material. They should feel harder than Year 8, but they are not meant to be full Year 11 exam questions.
Answer first, then reveal. The useful bit is the retrieval attempt, not reading the answer. If a topic keeps going wrong, paste the homework or Google Classroom text into GradeNinja's Classroom import tool and turn it into a focused pack.
Real questions from GradeNinja's own bank, with the answer and the explanation the app gives. Tap to reveal.
18
Mr of H₂O = (2 × 1) + 16 = 18. You add up the relative atomic masses of all atoms in the formula: two hydrogen atoms (2 × 1 = 2) plus one oxygen atom (16).
Charge +1, mass 1
Protons are found in the nucleus and have a relative charge of +1 and a relative mass of 1. Neutrons have charge 0 and mass 1. Electrons have charge -1 and negligible mass (1/1836 of a proton). The number of protons = atomic number = number of electrons in a neutral atom.
Decreasing concentration of reactants
Decreasing the concentration of reactants reduces the number of particles available for collisions, which slows down the rate of reaction. A higher concentration typically leads to more frequent collisions, increasing the reaction rate. Remember that concentration affects how often particles collide.
7
pH 7 is neutral (eg pure water). Below 7 is acidic; above 7 is alkaline. The scale runs from 0 (very strong acid) to 14 (very strong alkali).
A) 20.0 g
The balanced equation is 2Mg + O₂ → 2MgO. Moles of Mg = 12.0 ÷ 24 = 0.50 mol. Moles of O₂ = 10.0 ÷ 32 = 0.3125 mol. The stoichiometric ratio requires 2 mol Mg per 1 mol O₂, so 0.50 mol Mg needs 0.25 mol O₂. Since 0.3125 mol O₂ is available, oxygen is in excess and magnesium is the limiting reagent. 0.50 mol Mg produces 0.50 mol MgO (Mr = 40), giving 20.0 g. Mass is conserved, so 12.0 g + 8.0 g O₂ reacted = 20.0 g MgO.
Sharing of electrons between non-metals
Covalent bonds form when two non-metal atoms share electrons. Each atom contributes one (or more) electrons to a shared pair. Both atoms are attracted to the shared electrons, holding them together. Examples: H₂O, CO₂, CH₄. Metallic bonding involves a sea of delocalised electrons.
It decreases and the melting range broadens
Impurities lower the melting point and broaden the melting range. A pure substance melts sharply at one temperature; an impure mixture melts over a range of temperatures. This is used to check purity in the lab.
Filtration
Filtration traps the insoluble solid in the filter paper and lets the liquid pass through.
Carbon dioxide and water vapour
Early Earth's atmosphere was similar to Venus and Mars today: mainly CO₂ and water vapour, with small amounts of methane and ammonia. Over billions of years, photosynthesis by early organisms (cyanobacteria) released oxygen. CO₂ dissolved in oceans and formed carbonate rocks.
Fractional distillation
Fractional distillation separates crude oil by exploiting the different boiling points of its components. The oil is heated, vapours rise up a fractionating column, and fractions condense at different heights according to their boiling points.
32S2-, mass number 32, charge 2-
The number of protons, 16, identifies sulfur. Mass number is protons + neutrons = 16 + 16 = 32. It has two more electrons than protons, so the charge is 2-.
A substance made of only one element or compound, with a fixed melting/boiling point
A pure substance in chemistry is defined as a material made up of only one element or compound, which has a fixed melting or boiling point. Understanding purity is essential for distinguishing between different substances in chemistry. Remember that pure substances have consistent physical properties.
Igneous rock
Igneous rocks form when magma (underground) or lava (at the surface) cools and solidifies. Examples include granite (slow cooling underground, large crystals) and basalt (fast cooling at surface, small crystals). The slower the cooling, the larger the crystals formed.
Electron
Electrons are negatively charged. Protons are positive and neutrons are neutral.
Burette
A burette delivers precise, variable volumes of liquid (usually acid in a titration). It is read from the bottom of the meniscus to 0.05 cm³ accuracy.
6
Number of neutrons = mass number − atomic number = 12 − 6 = 6. The atomic number equals the number of protons. In a neutral atom, the number of electrons equals the number of protons. Neutrons and protons are both in the nucleus.
55,718 questions across 28 subjects, XP, boss battles and friend challenges. No card needed.
Start revising free →They are bridge questions: harder than early Key Stage 3, but not pitched as full Year 11 GCSE exam papers. The point is to prepare the habits and core knowledge early.
Yes. Use Classroom import in the app: paste the Google Classroom post, homework email or assignment brief and it turns the topics into practice questions and flashcards.
Short and often. Ten minutes after a lesson or a few times a week is more useful than one long session before a test.
Yes, signing up is free. GradeNinja has Year 9 bridge content plus the wider question bank across 28 subjects.