Elements of which block of the periodic table shows variable oxidation state?
Correct answer: C. The d and f block elements
- A. The s-block elements
- B. The p-block elements
- C. The d and f block elements
- D. None of the blocks
Explanation
In the case of d-block elements due to the presence of electrons at d orbitals, is closer to the outermost shell of the metal. They show variable oxidation states. With increasing the number of electrons of the d orbitals (up to 5 electrons), the number of oxidation states increases. In the case of d electrons due to a lower effective nuclear charge of attraction, the electrons can be removed to form different oxidation states.Actinides are F-block elements(atomic number 89 to103) with the general electronic configuration of the outermost shell being [Rn]5f1,146d0,17s2. Where the last electron enters the inner 5f-orbital of the actinides. Actinides are also known as rare earth metals. Now according to the Aufbau principle(L+S value), the energy order of the orbitals should be 5f<6d<7s but due to the more diffuse orbitals, their energy becomes more or less the same. As a result, electrons can be excited easily. Due to this reason, actinides show a greater range of oxidation states. But if we consider lanthanides due to their comparatively small size of 4f orbital they have a limited number of oxidation states.
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About Periodic Properties and Trends
Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.
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