Colour-Code the Periodic Table

periodic table shaded by block

Periodic table map coloured for s, p, d and f blocks

Four Blocks, Four Colours

Observe the periodic table map: four coloured zones immediately stand out.

Each zone represents a block whose location is set by the outer-electron subshell.

Key Points:

  • Left two columns → s-block
  • Right six columns → p-block
  • Middle ten columns → d-block (transition metals)
  • Detached bottom rows → f-block (lanthanides & actinides)

Explore the s-Block

s-Block Elements

These metals occupy Groups 1 and 2, filling the outermost \(ns^{1-2}\) subshell. They form the alkali and alkaline earth families.

Key Characteristics:

  • Soft, low-density metals with low melting points.
  • Large atomic and ionic radii; weak metallic bonding.
  • Highly reactive with water and oxygen.
  • Readily form +1 (Group 1) or +2 (Group 2) ions.
  • Excellent reducing agents.

Example:

Na → Na⁺ + e⁻ (Group 1); Ca → Ca²⁺ + 2e⁻ (Group 2)

Say Hello to the p-Block

p-Block Elements

The region (Groups 13–18) where the outermost electrons fill p-orbitals, giving configurations np¹–⁶ and broad chemical diversity.

Key Characteristics:

  • Occupies the right-side Groups 13–18 of the periodic table.
  • Hosts metals (Al), metalloids (Si), and non-metals (O, Cl).
  • Valence shell holds 3–8 electrons, enabling varied oxidation states.
  • Metallic character decreases and electronegativity rises across the block.
  • Reactivity spans from reactive halogens to inert noble gases.

Example:

Life-supporting O₂ and inert Ne both belong to the p-block.

Dive into the d-Block

d-Block Elements (Transition Metals)

d-Block elements fill an \( (n-1)d \) subshell. Sitting between s and p blocks, they are therefore called transition metals.

Key Characteristics:

  • Progressive filling of \( (n-1)d \) orbitals.
  • Variable oxidation states.
  • Form colourful ions and compounds.
  • Act as effective catalysts.

Example:

Fe transitions between Fe²⁺ and Fe³⁺, both coloured and industrially important.

Uncover the f-Block

f-Block (Inner Transition Metals)

Two rows of inner transition metals where electrons enter 4f or 5f subshells.

Key Characteristics:

  • Lanthanides: 4f filling, +3 common, used in bright LED phosphors.
  • Actinides: 5f filling, radioactive, show many oxidation states like +3 to +6.
  • Both rows lie below the table, dense, metallic, called inner transition metals.

Example:

Uranium-235 (actinide) fuels reactors; Europium(III) oxide (lanthanide) creates red light in TVs.

Sort the Elements!

Drag each element symbol into its s-, p-, d- or f-block. Click “Check” to see your classification.

Draggable Items

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Drop Zones

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Tip:

Recall: s-block ends with ns¹–²; p-block with np¹–⁶; d-block has (n−1)d; f-block has (n−2)f.

Key Takeaways

s-Block

Groups 1–2. Valence ns¹–². Soft, highly reactive metals giving +1/+2 ions.

p-Block

Groups 13–18. ns²np¹–⁶. Metals, non-metals, metalloids with variable oxidation states.

d-Block

Groups 3–12. Partially-filled (n-1)d. Coloured ions, many states; great catalysts.

f-Block

Lanthanides & actinides filling (n-2)f. Common +3 ions; actinides often radioactive. Keep this cheat-sheet handy.

Multiple Choice Question

Question

Which block does the element with configuration [Ar] 3d¹⁰ 4s² 4p⁵ belong to?

1
s-block
2
p-block
3
d-block
4
f-block

Hint:

Identify the subshell (s, p, d, or f) that receives the last electron.

Wrapping Up the Blocks

s-block: Groups 1–2, low electronegativity, form +1/+2 ions.

p-block: Groups 13–18, diverse properties, variable oxidation states.

d-block: Groups 3–12, transition metals, coloured ions, good catalysts.

f-block: Lanthanides & actinides, hidden rows, high atomic numbers.

Block location predicts metallic character, common oxidation states and general reactivity.

You can now recall these traits unaided—mission accomplished!

Thank You!

We hope you found this lesson informative and engaging.