Why do the transition elements exhibit higher enthalpies of atomisation?
The transition element exhibit higher enthalpies of atomisation because the atoms in these elements are closely packed and held together by strong metallic bonds. The metallic bond is formed as a result of the interaction of electrons in the outermost shell. Greater the number of valence electrons, stronger is the metallic bond.
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Why is the following electronic configuration not correct for the ground state of Mo atom? (at. no. = 42). 1s2 2s2 2p6 3s23p63d10 4s2 4p6 4d4 5s2.
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Name a transition element which does not exhibit variable oxidation states.
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Why does Zr and Hf exhibit similar properties?
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Why is the enthalpy of atomisation increases upto the middle of the transition series and then decreases?
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Why Pd is not called a transition elements?
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Why is the density of Zn lower than that of Cu?
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Why are Zn, Cd and Hg softer and volatile metals?
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Explain why iron is a transition element but sodium is not?
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Atomic radius in a transition series does not vary much while that of s and p-block does. Why?
