Rust Protection & Electricity vs Iron — Student Pack (Age 14)

Two Mel Science experiments: A) Rust Protection — sacrificial anode idea, B) Electricity vs Iron — electric current accelerating iron corrosion. This pack includes: Cornell note-taking guide, printable student worksheets, step-by-step instructor scripts, ACARA v9-aligned standards and descriptors, scaffolded research questions for Year 8 and Year 9, and eight teacher analytic/scoring rubrics written in the style of Jane Austen for assessment.

Cornell Note-Taking System (Simple Guide for 14-year-olds)

Use Cornell notes during the lesson and your investigation to record observations, ideas, and conclusions.

• Prepare one page per experiment divided into three areas: a narrow left-hand column (cues/questions), a wide right-hand column (notes), and a 5-6 line space at the bottom (summary).
• During the lesson: write main ideas, observations, procedure steps and data in the right column.
• After the lesson: write keywords or questions in the left column that connect to the right-hand notes. At the bottom, write a brief summary (2–3 sentences) of what you learned.
• Use the notes to prepare your lab report and to answer scaffolded research questions.

Printable Cornell template (one page):

Experiment A — Rust Protection: "Did you know that one metal can sacrifice itself for another?"

Learning focus

Investigate how connecting a more reactive metal to iron can slow or prevent rusting by acting as a sacrificial anode (galvanic protection).

Materials (student worksheet)

• Iron nail or small iron strip (cleaned)
• Small zinc strip or galvanized nail (or magnesium if provided in kit)
• Copper wire or coin (for comparison)
• Beaker or small cups, water, salt (to make saltwater)
• Sandpaper, tissue, digital camera or phone for photos
• Labels and permanent marker
• Protective gloves, goggles

Safety

• Wear goggles and gloves.
• Work on a tray to contain drips.
• Wash hands after the experiment.

Procedure (Student Worksheet – printable)

1. Polish an iron nail/strip with sandpaper to remove rust and grease. Record initial appearance and mass if a balance is available.
2. Prepare three cup setups labeled A, B, C. Fill each with the same saltwater solution (e.g., 1 tsp salt in 200 mL water).
3. Setup A: Iron alone (suspended so it does not touch the cup bottom).
4. Setup B: Iron electrically connected (wired) to a piece of zinc so the metals touch and are joined by wire. Ensure metal-metal contact between iron and zinc. (Zinc should be exposed.)
5. Setup C: Iron electrically connected to copper (or a non-sacrificial metal) as a comparison.
6. Leave setups over several days; observe daily. Photograph and record changes in appearance, any gas, and if mass measurements are available, record them.
7. After the test period, describe which iron corroded most and which least, and write a short explanation.

Data table (printable)

Student Questions (Cornell cues & summary)

Use your Cornell notes to answer:

1. Which setup showed the least rusting? Why do you think that happened?
2. What is a sacrificial anode?
3. How would you explain this using the idea of metal reactivity?

Instructor script (simplified, step-by-step)

1. Introduce concept (5 minutes): Ask students what rust is and whether metals can protect each other.
2. Demonstrate how to prepare the nails/strips and how to make the connections (5 minutes).
3. Explain control variables: same saltwater, same temperature, same exposure time (2 minutes).
4. Students set up experiments in groups (10–15 minutes). Instructor checks safety and correct connections.
5. Students observe daily and record (homework or class starter for several days). Instructor prompts them to photograph changes.
6. After test period, lead class discussion (15–20 minutes) comparing results and guiding to explanation of galvanic protection.

Year-level Scaffolded Research Questions

Year 8 (simpler)

1. Make a hypothesis: Which setup will rust most? Explain in one sentence.
2. List three things you kept the same in every setup and explain why.
3. Describe what happened in one or two sentences when zinc was attached to iron.
4. Draw a simple diagram showing how electrons might move between the metals (label iron and zinc).

Year 9 (more challenging)

1. Propose an explanation in terms of reactivity: why does zinc protect iron? Mention oxidation and reduction in one or two sentences.
2. Suggest an experiment variation to test how surface area of the zinc affects protection; include predicted results.
3. If you had to design a corrosion-protection system for a ship hull, what practical factors would you consider? (Cost, environmental effects, maintenance.)
4. Write a balanced word equation for the rusting of iron and discuss how connecting a more reactive metal changes which metal oxidises.

Experiment B — Electricity vs Iron: "Watch as electricity dismantles an iron strip!"

Learning focus

Observe how an electric current can drive chemical change (electrochemical corrosion or electrolysis) that will remove or change iron when connected in an electrolytic cell.

Materials (student worksheet)

• Small iron strip or nail
• Power source: low-voltage DC power supply or battery pack with adjustable current (teacher control)
• Graphite or inert electrode for the other terminal (e.g., carbon rod or copper but teacher must supervise)
• Saltwater electrolyte, beaker, wires with croc clips
• Multimeter (if available), sandpaper, goggles, gloves

Safety

• Teacher sets up power source or strictly supervises student use of low-voltage DC.
• Never exceed a small voltage/current. Keep current low (e.g., <1 A depending on setup) — follow kit guidance.
• Avoid direct skin contact with electrodes during current flow.

Procedure (Student Worksheet)

1. Prepare iron surface by cleaning with sandpaper. Record initial photo and mass if possible.
2. Set up an electrolytic cell: iron as one electrode, inert electrode as the other, both immersed in saltwater (do not let the electrodes touch).
3. Connect the iron to the positive terminal (anode) and the inert electrode to the negative terminal (cathode) of the DC source. NOTE: If iron is an anode it will oxidise (lose mass).
4. Switch on a small voltage for a set time (teacher determines safe voltage and time — e.g., 1.5–6 V for a few minutes depending on kit instructions).
5. Observe for bubbles, surface changes, and check for mass loss after drying (teacher supervised). Record current if multimeter is used.
6. Discuss what you observed and why current caused visible change to the iron.

Data table (printable)

Student Questions

1. Did the iron change? Describe the evidence (mass loss, surface changes, bubbles).
2. Which electrode lost mass and why?
3. How does electricity cause chemical change? Use the ideas of oxidation and reduction.

Instructor script (simplified)

1. Intro (5 minutes): Explain that electricity can push electrons and cause oxidation at one electrode.
2. Demonstrate safe setup and show how to connect the multimeter (5 minutes).
3. Students perform short trials under strict supervision (15–20 minutes). Instructor monitors currents and times.
4. Class discussion comparing results and linking to electrochemical principles (10–15 minutes).

Year-level Scaffolded Research Questions

Year 8

1. Predict what will happen to the iron when connected to the positive terminal and explain in one sentence.
2. Why do you need an electrolyte (saltwater) for changes to occur?
3. Make a simple diagram of the cell showing electrons leaving the iron.

Year 9

1. Explain how current and time would affect the mass loss of the iron. If you double the current but halve the time, what do you expect for total mass change? (Discuss conceptually.)
2. Discuss how this experiment relates to electroplating and industrial corrosion control.
3. Relate observations to redox reactions: write the half-reactions for iron oxidation and the likely reduction occurring at the cathode.

ACARA v9 Alignment (summary descriptors)

These experiments integrate Science Understanding and Science Inquiry Skills from the Australian Curriculum (ACARA v9). Below are the aligned descriptors in teacher-friendly language.

Year 8 alignment

• Chemical sciences: Chemical reactions involve rearrangement of atoms to form new substances; rusting is an example of oxidation of metals and can be affected by other metals (sacrificial protection).
• Science inquiry: Plan and conduct controlled investigations, including identifying variables, collecting and representing data, and using evidence to support explanations.

Year 9 alignment

• Chemical sciences and physical sciences: Chemical reactions can be represented by word and simple chemical equations; electricity can facilitate chemical changes (electrolysis), and energy transfer (electrical energy) can cause chemical change.
• Science inquiry: Analyse data, consider sources of uncertainty, and design improvements to experimental methods.

Note: Use these descriptors as guidance for Australian state curriculum expectations for Years 8 and 9 under ACARA v9. Teachers should cross-check with their local detailed curriculum documents for exact code numbers and required achievement standards.

Teacher Analytic and Scoring Rubrics (Eight rubrics, presented in Jane Austen prose)

For each experiment we provide two rubrics per year level: an Analytic rubric focusing on practical investigation skills, and a Content/Scoring rubric focusing on scientific understanding. Each is written in genteel Jane Austen prose for a touch of delight in assessment.

Experiment A — Rust Protection

Year 8 — Analytic Rubric (Jane Austen prose)

It is herein observed, with both candour and the gentlest scrutiny, that the student who attains the highest commendation arranges their apparatus with such neatness and care that an observer is at once sensible of method and prudence. Their notes are full and punctual; their observations are described with clarity; and their adherence to safety evinces most laudable attention to duty. At the middle rank, the pupil shows adequate order, records pertinent observations, and keeps to the principal safety rules, though some small omissions may be discovered. The lesser degree demonstrates an attempt at procedure but with careless layout, incomplete notes, and occasional disregard for measured controls; thus improvement is recommended.

• Excellent (4): Apparatus correct and tidy, daily observations complete, variables controlled, safety followed.
• Proficient (3): Apparatus mostly correct, regular observations, most variables controlled, safety mostly followed.
• Developing (2): Apparatus incomplete or untidy, observations irregular, controls not consistent, some safety lapses.
• Beginning (1): Apparatus poorly set, insufficient observations, no control of variables, safety procedures ignored.

Year 8 — Content / Scoring Rubric (Jane Austen prose)

With respect to the explanation of protection afforded by a sacrificial metal, the student of superior merit expounds the cause with a felicitous use of terms, including the notion that one metal succumbs to change so that its companion remains unaltered. The explanation shall embrace the idea of reactivity and of electron transfer in a manner both succinct and accurate. A middling account shall reveal partial understanding; while the humble account shall scarce rise above mere observation.

• Excellent (4): Clear explanation linking reactivity and sacrificial protection; uses terms such as 'oxidation' correctly; predicts results sensibly.
• Proficient (3): Reasonable explanation, some correct vocabulary, minor inaccuracies.
• Developing (2): Limited explanation, basic vocabulary, misunderstanding of cause and effect.
• Beginning (1): Minimal explanation, largely observational with incorrect reasoning.

Year 9 — Analytic Rubric (Jane Austen prose)

The student of distinguished application plans and conducts the inquiry with artful exactness: measurements and photographs are employed, controls are defended, and data are presented with suitable tables and commentary. Those of fairer exertion furnish a competent experiment yet may omit the finer points of uncertainty or replication. Those of scanter endeavour exhibit hurried work and little analytical commentary.

• Excellent (4): Thoughtful experimental design, replicates or discusses replication, analyses uncertainty, clear data presentation.
• Proficient (3): Sound design and data, limited discussion of uncertainty or replication.
• Developing (2): Partial design with incomplete data analysis, little consideration of uncertainty.
• Beginning (1): Poorly designed, data missing or uninterpretable, no analysis of reliability.

Year 9 — Content / Scoring Rubric (Jane Austen prose)

In the matter of chemical explanation, the most commendable pupil relates sacrificial protection to the relative reactivity of metals and employs the terms 'oxidation' and 'reduction' with proper decorum. They shall also suggest a reasonable improvement to the experiment. Lesser accounts may show acquaintance with reactivity but falter in precise reasoning or in the proposing of improvements.

• Excellent (4): Accurate redox explanation, links to reactivity series, proposes valid experimental improvements.
• Proficient (3): Good explanation; some minor omissions in linking concepts or improvements.
• Developing (2): Partial conceptual understanding; suggested improvements are weak.
• Beginning (1): Misconceptions about redox and no sensible improvements.

Experiment B — Electricity vs Iron

Year 8 — Analytic Rubric (Jane Austen prose)

The pupil who conducts their task with genteel industry observes the simple rigour needed for an electrical inquiry. Connections are firm; durations and settings are recorded; and observations are noted with decorum. The less methodical often forget to report times or to ensure safe connection, thereby detracting from the merit of their work.

• Excellent (4): Safe, correct connections; times and voltages recorded; clear observations; supervised appropriately.
• Proficient (3): Mostly correct setup; most data recorded; safe practice usually followed.
• Developing (2): Setup incomplete or inconsistent; missing data; some safety lapses.
• Beginning (1): Unsafe or incorrect setup; insufficient data; no regard for safety.

Year 8 — Content / Scoring Rubric (Jane Austen prose)

On the matter of explanation, the superior student will describe how electrical energy causes a metal to undergo change, making reference to the loss of electrons at the anode in language fitting a junior chemist. A lesser attempt may correctly note change but fail to associate it with the flow of electric charge.

• Excellent (4): Correctly explains that current causes oxidation at the anode; uses 'electrons' and 'oxidation' suitably.
• Proficient (3): Good explanation with minor gaps in linking electricity and chemical change.
• Developing (2): Vague explanation, limited linking to electricity.
• Beginning (1): Incorrect or absent explanation.

Year 9 — Analytic Rubric (Jane Austen prose)

Inquiries of a higher order are those in which the student measures and records voltage and current and appraises their influence upon the chemical change with a most reasonable analysis; attention to sources of error and to improvement bespeaks scholarly care. The middling student attends to data but neglects judicious commentary on uncertainty.

• Excellent (4): Records voltage/current, quantifies effect, analyses error sources, suggests improvements.
• Proficient (3): Records essential data, some analysis of effects, limited error discussion.
• Developing (2): Data incomplete or analysis weak, little consideration of uncertainty.
• Beginning (1): Negligible data and no analysis.

Year 9 — Content / Scoring Rubric (Jane Austen prose)

Of theoretical exposition, the student most worthy shall present the half-equations for the oxidation of iron and for the reduction at the cathode with clarity and balance. He or she shall further discuss the relationship between charge passed and the mass of metal altered, in terms fit for the level. Lesser efforts may state observed facts but fail to set them within the framework of redox half-reactions.

• Excellent (4): Correct half-equations, conceptually links current/time to mass change, uses redox vocabulary correctly.
• Proficient (3): Good use of half-reactions with small inaccuracies; acknowledges current/time relationship.
• Developing (2): Partial or incorrect half-reactions; weak link to current/time.
• Beginning (1): Misunderstanding of redox and no connection to electrical quantities.

Printable Student Worksheet Pack (Concise Print-Friendly Format)

Below are compact printable versions: students should print one worksheet per experiment and one Cornell note page.

Worksheet — Experiment A (Rust Protection)

Worksheet — Experiment B (Electricity vs Iron)

Teaching Tips & Differentiation

• Provide printed Cornell sheet and model a filled-in example for the first 5 minutes of class.
• For students who need more support, provide partially completed data tables and sentence starters for conclusions.
• For advanced students, ask them to calculate percent mass change, propose improvements, or explore the electrochemical series further.

Suggested Sequence & Timing (One 60–90 minute lesson + follow-up observations)

1. Hook & Cornell mini-lesson (10 minutes)
2. Demonstrate experiment setup & safety (10 minutes)
3. Students set up in groups (20 minutes)
4. Immediate observations & data entry (10 minutes)
5. Assign daily observations for 1 week (short home/class entries)
6. Final analysis & discussion (class session after week — 30–45 minutes)

Final Notes

This pack blends practical investigation, ACARA-aligned learning intentions, inquiry skill development, and assessment rubrics expressed in charming Jane Austen prose to enliven reporting. Teachers should adapt voltages, chemical concentrations, and experimental durations to the specific Mel Science kit instructions and local safety rules. Always supervise students with electrical setups and provide pre-briefing on safety.

If you would like this pack exported as a ready-to-print PDF (worksheets + Cornell templates + rubric sheets), tell me and I will prepare a printer-ready layout.