d and f BLOCK ELEMENTS Quiz

• It causes a steeper increase in ionisation enthalpies
• It leads to a more gradual increase in ionisation enthalpies across the transition series
• It makes the atoms larger
• It decreases the nuclear charge

• The second electron is always a d-electron
• Removing the second electron involves overcoming the increased effective nuclear charge experienced by the remaining electrons
• The atomic radius increases after the first ionisation
• The second electron is farther from the nucleus

• Transition metals have weaker metallic bonds
• Transition metals utilise both ns and (n-1)d electrons for delocalisation, leading to stronger bonds
• S-block metals utilise d-electrons for bonding
• There is no difference in metallic bonding

• It is the least stable configuration
• It represents a particularly stable electron arrangement that can cause breaks in ionisation enthalpy trends
• It is only stable for chromium
• It has no special significance

• Due to weak van der Waals forces
• Due to the strong metallic bonding involving a large number of delocalised electrons from both ns and (n-1)d orbitals
• Due to the formation of covalent networks
• Due to the presence of ionic bonds