Questions regarding elements between Group 3 and Group 12 (inclusive), or also referred to as d-block.
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1answer
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Transition Metals' Charges
I came across a compound $\ce{[FeO4]^{2-}}$ but $\ce{Fe}$ has +6 charge according to my calculations. How this is possible ? Or it is possible but my periodic table is kind of non-detailed one. (On ...
2
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1answer
31 views
Strongest chloride complex as perdicted by HSAB theory
Why won't $\ce{Ni^2+}$ form a complex with $\ce{Cl-}$, while the ions $\ce{Cu^2+}$ and $\ce{Co^2+}$ form the complexes $\ce{[CuCl4]^2-}$ and $\ce{[CoCl4]^2-}$?
According to the HSAB theory, ...
1
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1answer
76 views
Bonding in a bridged metal carbonyl
Can someone please explain the bonding in a bridged metal carbonyl (like diiron nonacarbonyl)?
I cannot understand what kind of bonds (sigma/pi) exist between the bridging carbonyls and the metals.
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1answer
61 views
Why do transition elements make colored compounds?
Why do transition metals element make colored compound both in solid form and in solution? Is it related with their electrons or something else?
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0answers
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Are Zn, Cd & Hg transition elements? [closed]
My textbook describes that Zn, Cd & Hg are not transition elements. Whereas, on wikipedia it is said that they should be studied under transition elements. Are they?
9
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1answer
1k views
Why are some salt solutions coloured?
I notice that salt solutions of $\ce{NaCl}$ and $\ce{KCl}$ are colourless while those of $\ce{CuSO4}$ and $\ce{FeSO4}$ are coloured.
I got as far as figuring that it has to do with the transition ...
3
votes
1answer
73 views
Brittle d-block metal trend
I remember seeing a periodic table that had the top-left corner of the d-block shaded and marked as "brittle". If I recall correctly, the elements were $\ce{Sc,Ti,V,Cr,Mn,Y,Zr,Nb,La}$. I think (Sorry, ...
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5answers
642 views
Why do elements in columns 6 and 11 assume 'abnormal' electron configurations?
When I look around for why copper and chromium only have one electron in their outermost s orbital and 5/10 in their outermost d orbital, I'm bombarded with the fact that they are more stable with a ...
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2answers
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How is Vanadium's 3+ ion paramagnetic?
"Both Vanadium and its 3+ ion are paramagnetic. Use electron configuration to explain why this is so"
The electron configuration of Vanadium is [Ar] 4s2 3d3.
If drawn in a box diagram, it would ...
