igcse model questions vol1 2023 chemistry | Practical

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Question 1 View Details
You are given a solid piece of an unknown metal. Using a balance and a graduated cylinder, you determine its mass and its volume by water displacement. Mass of the metal = 2.00 g (to 3 s.f.) Initial water level in the cylinder = 25.00 mL Final water level after immersion = 26.20 mL
Question Parts
(a)
Calculate the density of the metal in g·cm⁻³. Show all steps.
(b)
Using the density you have obtained, identify the metal by comparing with the following known densities (to 2 d.p.): Magnesium – 1.74 g·cm⁻³ Aluminium – 2.70 g·cm⁻³ Lithium – 0.53 g·cm⁻³ Zinc – 7.14 g·cm⁻³ State the name and chemical symbol of the metal.
(c)
For the metal you have identified, use the periodic table values: atomic number = 12, relative atomic mass = 24.31 u. (i) Write the number of protons, neutrons and electrons in a neutral atom of this metal. (ii) Calculate the total number of neutrons present in the 2.00 g sample. Express your answer in scientific notation to two significant figures.
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Question 2 View Details
Three unknown solid salts (labelled Sample 1, Sample 2 and Sample 3) are subjected to a flame test using a clean platinum wire. The observed flame colours are recorded as follows: Sample 1 – bright yellow flame Sample 2 – lilac (pale violet) flame Sample 3 – deep red flame
Question Parts
(a)
Identify the metal cation present in each sample by matching the observed flame colour with the standard flame‑test colours given below: Na⁺ – yellow K⁺ – lilac Rb⁺ – deep red State the metal name and its chemical symbol for each sample.
(b)
Write the ground‑state electron configuration for each identified metal ion (use the noble‑gas shorthand).
(c)
Explain, using periodic trends, why the flame colour changes from yellow (Na⁺) to lilac (K⁺) to deep red (Rb⁺) as you move down Group 1.
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Question 3 View Details
You are given four solid compounds labelled A, B, C and D. Their identities are unknown to you. The compounds are: sodium chloride (NaCl), copper(II) sulphate pentahydrate (CuSO₄·5H₂O), glucose (C₆H₁₂O₆) and ammonia solution (NH₃(aq)). Using the apparatus listed, you will investigate the electrical conductivity of each compound in aqueous solution and, where possible, in the molten state. Apparatus: conductivity meter with cell constant 1.0 cm⁻¹, beakers (250 mL), distilled water, Bunsen burner, crucible, tongs, thermometer, balance (0.01 g), safety goggles and lab coat. Procedure (summarised): 1. Weigh 2.00 g of each solid (A–D) and record the masses. 2. Dissolve each solid in 100 mL of distilled water in separate beakers, stirring until completely dissolved. 3. Rinse the conductivity probe with distilled water and blot dry before each measurement. 4. Record the conductivity (µS cm⁻¹) of each solution. 5. For the solids that melt on heating (A and B), transfer a small amount to a clean crucible, heat gently over the Bunsen burner until a clear melt is obtained, and immediately insert the probe to record the conductivity of the molten material. 6. Clean the probe between measurements to avoid cross‑contamination. Answer the following questions:
Question Parts
(a)
Record the conductivity of each aqueous solution and, where applicable, of each molten sample in the table provided.
(b)
Based on the observations, classify each compound as predominantly ionic or covalent and justify your classification.
(c)
Explain why glucose, although it dissolves in water, shows very low conductivity.
(d)
Suggest one precaution that should be taken to minimise error caused by electrode contamination during the experiment.
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Question 4 View Details
A piece of magnesium ribbon is used to prepare magnesium oxide by combustion in air. The experiment is carried out as follows: 1. A clean, dry crucible with lid is weighed and the mass recorded (M₁). 2. Approximately 0.50 g of magnesium ribbon is placed in the crucible and the mass of the crucible with the magnesium is recorded (M₂). 3. The crucible is covered with the lid and gently heated over a Bunsen burner. The magnesium is allowed to burn completely, forming magnesium oxide. 4. After cooling, the crucible with the product is weighed (M₃). The recorded masses are: M₁ = 12.340 g M₂ = 12.845 g M₃ = 13.115 g Answer the following questions:
Question Parts
(a)
Calculate the mass of magnesium that reacted.
(b)
Determine the mass of oxygen that combined with the magnesium to give magnesium oxide.
(c)
Calculate the number of moles of magnesium and oxygen and deduce the empirical formula of the product.
(d)
Identify two possible sources of error in this experiment and suggest a method to reduce each error.
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