Problem: Explain why vanadium (radius = 134 pm) and copper (radius = 128 pm) have nearly identical atomic radii, even though the atomic number of copper is about 25% higher than that of vanadium.

FREE Expert Solution

We have to explain why vanadium and copper have nearly the same atomic radius although the atomic number of copper is higher than that of vanadium.


The size of an atom (atomic radius) depends upon:

  • The number of energy levels (shells)
  • The strength of attractive forces between the nucleus and the valence electrons
  • Shielding that results due to inner electrons.

 

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Problem Details

Explain why vanadium (radius = 134 pm) and copper (radius = 128 pm) have nearly identical atomic radii, even though the atomic number of copper is about 25% higher than that of vanadium.

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Our tutors have indicated that to solve this problem you will need to apply the Periodic Trends: Atomic Radius concept. You can view video lessons to learn Periodic Trends: Atomic Radius. Or if you need more Periodic Trends: Atomic Radius practice, you can also practice Periodic Trends: Atomic Radius practice problems.