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sludger13
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I'm not sure why Chromium(VI) is reducing and Tungsten(VI) isn't. I also noticed their radius is quite similar. Is that related?
The stability of an element is determined by its electronic configuration. In the case of W(VI) and Cr(VI), the electronic configuration of W is [Xe]4f^14 5d^4 6s^2 while that of Cr is [Ar]3d^5 4s^1. The presence of filled d-orbitals in W makes it more stable compared to Cr which has only partially filled d-orbitals.
The size of the atom also plays a role in determining stability. W has a larger atomic size compared to Cr. This means that the electrons in the outermost shell of W experience less repulsion from the nucleus compared to those in Cr, making it more stable.
Apart from electronic configuration and atomic size, the oxidation state of an element also affects its stability. W has a higher oxidation state (+6) compared to Cr (+4) in their respective compounds, making it more stable.
Yes, the periodic table can be used to predict the stability of elements. Elements on the right side of the periodic table tend to have higher stability due to their electronic configuration and atomic size. W and Cr are both transition metals located on the right side of the periodic table.
The stability of an element can affect its reactivity in chemical reactions. In the case of W(VI) and Cr(VI), the higher stability of W makes it less reactive compared to Cr. This makes W more suitable for use in industrial processes where a stable and less reactive element is required.