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Physical properties of transition metals versus Group 1

Atomic structure and the periodic table • Properties of transition metals

Key concepts

What you'll likely be quizzed about

  • Metallic bonding occurs between positive metal ions and a sea of delocalised electrons.
  • Transition elements possess partly filled d-orbitals, providing additional delocalised electrons and stronger overlap of orbitals.
  • In contrast, Group 1 metals contain a single outer s-electron that delocalises, leading to weaker metallic bonds.
  • Therefore, transition elements exhibit increased cohesion between atoms, which results in greater hardness, enhanced strength, higher melting points, and larger densities compared to Group 1 metals.

Flashcards

Test your knowledge with interactive flashcards

Explain how delocalised electrons affect melting point.

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More delocalised electrons increase cohesive forces between atoms, necessitating more thermal energy to break interactions and elevate the melting point.

Key notes

Important points to keep in mind

Hardness is resistance to indentation; strength is resistance to deformation.

Transition elements possess stronger metallic bonds from d-electrons; Group 1 metals exhibit weaker bonding due to a single s-electron.

Stronger metallic bonding correlates with higher melting points, increased hardness, and enhanced strength.

Transition elements show greater densities due to higher atomic mass and tighter packing.

Alloying, impurities, and defects may alter hardness, strength, and melting points.

Group 1 metals are soft, have low densities, and exhibit low melting points compared to transition metals.

Conditions such as purity and temperature can alter observed property values.

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