Why transition metals are less reactive than s block elements?
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The compounds that transition metals form with other elements are often very colorful.Compared with the alkali metals in group 1 and the alkaline Earth metals in group 2, the transition metals are much less reactive. They don't react quickly with water or oxygen, which explains why they resist corrosion.
Answer:
Concept:
In free elements and cations, transition metals are distinguished by partially filled d subshells. Because the energies of the ns and (n 1)d subshells are similar, minor impacts can cause electron configurations to differ from the general sequence in which the subshells are filled. Such abnormalities can be difficult to predict in second- and third-row transition metals, especially in the third row, which has very close 4f, 5d, and 6s orbitals. Because of the lanthanide contraction, the rise in atomic radius between the 3d and 4d metals is larger than the 4d and 5d metals. Ionization energies and electronegativities, as well as densities and electrical and thermal conductivities, grow slowly throughout a row, whereas hydration enthalpies decrease.
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Why transition metals are less reactive than s block elements?
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find the answer for the given question
Answer:
Transition metals are less reactive than elements in the s block. This is because their ions have higher sublimation heats, higher ionization energies, and lower hydration energies. Transition metals are less reactive because they do not "give away" their electrons as easily as other metals during a reaction (as shown in the video above). Alkali metals (Group 1), on the other hand, readily give up their electrons and are hence regarded more reactive.
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