• Quick retrieval from earlier learning (Atomic number, mass number and isotopes). Students answer on mini whiteboards.
• Show answers together and note who needs support in the main task.

1. An atom of sodium is written ²³₁₁Na (mass number 23, atomic number 11). How many electrons does it have? → 11Prompt: Atomic number = number of protons (= electrons in a neutral atom).
2. Uranium has atomic number 92. How many neutrons are in the isotope uranium-235? → 143Prompt: The number after the name is the mass number.
3. Which number is the same for all isotopes of an element? (the mass number / the number of neutrons / the relative mass / the atomic number) → the atomic numberPrompt: Isotopes differ only in their neutrons.

• Show the periodic table and ask what patterns students can see before anything is explained.
• Share the objective: Relative atomic mass from isotope abundances. Read the success criteria together.

• Work through the example out loud, saying why you do each step, not just what you do.
• Example: Natural boron contains 20 % of mass 10 and 80 % of mass 11. Calculate its relative atomic mass to 1 decimal place.
• Step 1: 10 × 20 + 11 × 80 = 1080
• Step 2: 1080 ÷ 100 = 10.8
• Step 3: So the answer is: 10.8
• Answer: 10.8
• Pause after each step and ask a student to say what comes next.

• Do these together. Students try each step on whiteboards before you reveal it.
• Use the hints as prompts rather than giving the answer.

1. Natural copper contains 69 % of mass 63 and 31 % of mass 65. Calculate its relative atomic mass to 1 decimal place. → 63.6Prompt: Multiply each mass by its percentage abundance.
2. An element has two isotopes: mass 73 (10 %) and mass 75 (90 %). What is its relative atomic mass? Give 1 decimal place. → 74.8Prompt: The answer must lie between the two isotope masses.

• Students work on the student sheet. Circulate and check the first two answers of every student early.
• Students who finish: write a question of their own for a partner, with the answer.

The 6 questions are on the student sheet below, with answers in the key.

• Two questions on their own. Sort answers into got it / nearly / not yet to plan the next lesson.

1. An element has two isotopes: mass 56 (25 %) and mass 58 (75 %). What is its relative atomic mass? Give 1 decimal place. → 57.5Prompt: The answer must lie between the two isotope masses.
2. Do isotopes of the same element react differently in chemical reactions? (Yes: they have different numbers of protons / Yes: heavier isotopes are always more reactive / No: they have the same electron arrangement, so their chemistry is the same / No: isotopes never react) → No: they have the same electron arrangement, so their chemistry is the samePrompt: Chemistry depends on electrons.

Free online practice with hints and printable worksheets for this skill: eurekami.com/science/grade-10.