On the periodic table layout, Groups 1–2 on the left are the s-block. Groups 13–18 on the right form the p-block, and Groups 3–12 in the centre are the d-block. The f-block sits as two separate rows beneath, matching periods 6 and 7. Linking these group numbers to the blocks lets you locate any element quickly.
Drag each block name onto the shaded regions to test your new map-reading skill.
• Group 1 alkali metals have one valence electron. • Group 2 alkaline-earth metals have two valence electrons. • Soft, shiny metals that lose electrons to form +1 or +2 ions. • They react vigorously with water, releasing hydrogen gas. • Oxides are strongly basic; aqueous salts are usually colourless.
Recall these hallmark features to identify s-block elements quickly.
• Groups 13–18 span metals, metalloids and non-metals across each period.
• Moving right, metallic character drops while non-metallic nature rises.
• Atoms hold 3–8 outer p electrons, so oxidation states vary widely.
• Extremes range from B(+3) to Cl(–1).
• Down a group, size increases and metallic behaviour returns.
• Life-essential C, N and O showcase dominant covalent chemistry.
• Master these patterns to summarise any p-block trend quickly.
Quiz: Which p-block element shows both metallic and non-metallic forms?
• Inner transition rows sit beneath the main table.
• 4f series (lanthanides): shiny, soft, highly magnetic; Nd powers strong magnets.
• 5f series (actinides): largely radioactive; U and Pu fuel reactors.
• Predominant +3 state; weak f-electron shielding yields similar yet subtle chemistry.
After this slide, you can place these inner transition metals and cite their key uses.
Drag each element—Strontium, Bromine, Iron, Uranium—into its correct s, p, d or f block bucket.
Check your grasp of element identification and block recall.