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Science lesson plan · 9th grade (Year 10 in England) · 45 minutes

Electron shells and the periodic table

Atoms, elements and the periodic table

CCSS NGSS.HS-PS1-1England: KS4 Combined Science: Atomic structure and the periodic table

Objective and success criteria

Students will: Electron shells and the periodic table.

  • I can answer questions on today's skill on my own, without help.
  • I can explain each step and say why it works.
  • I can check my answer and spot a mistake.

Before and after

Needs first: Atomic number, mass number and isotopes

Leads to: Ionic, covalent and metallic bonding; Predict ion charges from the periodic table

Materials: Periodic tables, Atom model kits, Mini whiteboards, A diagram or short video clip of the idea, Printed student sheet (below).

Warm-up · 5 min

  • 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 beryllium is written ⁹₄Be (mass number 9, atomic number 4). How many neutrons does it have? → 5Prompt: Atomic number = number of protons (= electrons in a neutral atom).
  2. Oxygen has atomic number 8. How many neutrons are in the isotope oxygen-18? → 10Prompt: The number after the name is the mass number.
  3. A sodium atom loses one electron to become a sodium ion. What is its charge? (−1 / +11 / 0 / +1) → +1Prompt: It now has one more proton than electrons.

Hook · 5 min

  • Show the periodic table and ask what patterns students can see before anything is explained.
  • Share the objective: Electron shells and the periodic table. Read the success criteria together.

I do: model it · 10 min

  • Work through the example out loud, saying why you do each step, not just what you do.
  • Example: How many electrons does an atom of neon (atomic number 10) have in its outer shell?
  • Step 1: 2,8
  • Step 2: So the answer is: 8
  • Answer: 8
  • Pause after each step and ask a student to say what comes next.

We do: guided practice · 10 min

  • Do these together. Students try each step on whiteboards before you reveal it.
  • Use the hints as prompts rather than giving the answer.
  1. How many electrons does an atom of lithium (atomic number 3) have in its outer shell? → 1Prompt: Fill the shells 2, 8, 8 in order.
  2. Why do elements in the same group react in similar ways? (They have the same number of electrons in their outer shell / They have the same mass / They have the same number of neutrons / They were discovered at the same time) → They have the same number of electrons in their outer shellPrompt: Reactions involve the outer electrons.

You do: independent practice · 10 min

  • 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 8 questions are on the student sheet below, with answers in the key.

Exit ticket · 5 min

  • Two questions on their own. Sort answers into got it / nearly / not yet to plan the next lesson.
  1. Why do elements in the same group react in similar ways? (They were discovered at the same time / They have the same number of electrons in their outer shell / They have the same number of neutrons / They have the same mass) → They have the same number of electrons in their outer shellPrompt: Reactions involve the outer electrons.
  2. How many electrons does an atom of sulfur (atomic number 16) have in its outer shell? → 6Prompt: Fill the shells 2, 8, 8 in order.

Watch out for

  • Everyday meanings of words getting in the way of the science meaning: define key words explicitly.
  • Remembering facts without the reason: ask "why?" and "what is the evidence?"

Support and stretch

Support

  • Review first: Atomic number, mass number and isotopes.
  • Use concrete materials: periodic tables.
  • Give the first step of each question, or a partly worked example to finish.
  • Pair with a confident partner for the guided practice.

Stretch

  • Move on to: Ionic, covalent and metallic bonding; Predict ion charges from the periodic table.
  • Explain a common mistake in writing and how to fix it.
  • Write a word problem that uses today's skill, then solve a partner's.

Homework and more practice

Free online practice with hints and printable worksheets for this skill: eurekami.com/science/grade-9.

Free lesson plan from eurekami.com/lesson-plan-builder

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Electron shells and the periodic table

Name

Date

Score/ 8

  1. Question 1

    Fluorine has atomic number 9. What is its electronic structure?

    +++++++++F

    coral + = proton · grey = neutron · purple − = electron

    • A. 2,8
    • B. 2,7
    • C. 9
    • D. 1,8

  2. Question 2

    How many electrons does an atom of neon (atomic number 10) have in its outer shell?

    Answer

  3. Question 3

    Who arranged the elements in an early periodic table and left gaps for undiscovered elements?

    • A. Charles Darwin
    • B. Marie Curie
    • C. Isaac Newton
    • D. Dmitri Mendeleev

  4. Question 4

    Argon has atomic number 18. What is its electronic structure?

    18 p22 nAr

    coral + = proton · grey = neutron · purple − = electron

    • A. 2,8,8
    • B. 2,8,9
    • C. 2,16
    • D. 18

  5. Question 5

    How many electrons does an atom of carbon (atomic number 6) have in its outer shell?

    Answer

  6. Question 6

    Oxygen has atomic number 8. What is its electronic structure?

    ++++++++O

    coral + = proton · grey = neutron · purple − = electron

    • A. 2,6
    • B. 2,7
    • C. 8
    • D. 1,7

  7. Question 7

    How many electrons does an atom of helium (atomic number 2) have in its outer shell?

    Answer

  8. Question 8

    Why are noble gases so unreactive?

    • A. Their outer shell is full
    • B. They have no electrons
    • C. They are liquids
    • D. They are very heavy

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Answer key: Electron shells and the periodic table

  1. 1. B. 2,7

  2. 2. 8

  3. 3. D. Dmitri Mendeleev

  4. 4. A. 2,8,8

  5. 5. 4

  6. 6. A. 2,6

  7. 7. 2

  8. 8. A. Their outer shell is full