Periodic Trends: Chemical (DP IB Chemistry: SL)

• Periodic trends can also be seen in the typical properties of metals and non-metals which are summarised below:

The typical properties of metals and non-metals

• The typically properties of metals and non-metals can be explained by reference to their trends in atomic radius, ionic radius, ionisation energy, electron affinity and electronegativity
• The low ionisation energies and low electronegativities of metals can account for the ability of their valence electrons to move away from the nucleus
  • This is known as 'delocalisation' of the electrons

• These properties increase from left to right as you transition from metal to metalloid to non-metal
• The high electronegativity and electron affinity of non-metals can be related to their tendency to share electrons and form covalent bonds, either with themselves or other non-metal elements
• The similarities in electronegativities of the diagonal band of metalloids which divides the metals from the non-metals explains the behaviour of metalloids

Test yourself on the trends in the periodic table:

Answer:

The correct option is D

• • Across a period atomic radius decreases, electronegativity and ionisation energy increase and ionic radius increases then decreases