Chemistry Form 4 Work — Experiment 4.2

While memorizing the reactivity series (Potassium > Sodium > Calcium > Magnesium > Aluminium > Carbon > Zinc > Iron > Tin > Lead > Hydrogen > Copper > Silver > Gold) is essential, provides the visual evidence that makes these rankings stick. This article will break down the objective, hypothesis, variables, apparatus, procedure, results, and common mistakes to ensure you score an 'A' in your lab report.

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During the experiment, students should follow proper safety protocols to ensure their safety and the safety of others: experiment 4.2 chemistry form 4

: A small amount of each oxide is added to a test tube containing distilled water. The mixture is shaken, and the pH is measured using a pH meter or universal indicator.

I’ve written two versions: one for (most common) and one for Group 17 . Choose the one that fits your syllabus. The mixture is shaken, and the pH is

Here is the expected outcome table for . We look at whether a reaction occurs ( ✓ = Yes, ✗ = No).

: Test tubes, stoppers, pH meter or universal indicator, Bunsen burner, and spatulas. 3. Experimental Procedure Here is the expected outcome table for

Metals like Magnesium and Aluminium form a thin, inert oxide layer (MgO, ZnO) when exposed to air. This layer prevents the metal from contacting the solution. Sandpaper removes this barrier, allowing the true reactivity to show.

Before stepping into the lab, you must understand the principle behind Experiment 4.2.

If you do the opposite—put Copper into Magnesium Sulphate solution— because Copper is less reactive.

Place a conical flask on a white paper marked with a black cross. The Base Mixture: sodium thiosulphate into the flask. Start the Reaction: Quickly add 5 of sulphuric acid and start the stopwatch immediately. The Observation: