Questions tagged [transition-metals]
For questions about the characteristic physical properties, chemical reactions, etc. of d-block elements, group 3-12, or their compounds. Do not use this tag if your questions is about general properties of metals, use [metal] instead. Also see [rare-earth-elements].
445
questions
-2
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0answers
51 views
Reason for there being no loss of exchange energy in d^6 configuration? [closed]
I have just read about exchange energy. But I got confused over a statement. This was the paragraph:
Exchange energy is approximately proportional to total number of possible pairs of parallel spins ...
0
votes
0answers
46 views
Is it necessary that all transition metal complexes with unpaired electrons will show color?
For example consider the complex ion $\ce{[Mn(CN)_6]^{3-}}$ , it is octahedral so its d orbitals will split like $\ce{t_{2g}^4e_g^0}$. I understand the basics of how complex compounds show color (that ...
-1
votes
1answer
59 views
What compounds given can oxidize Mn(2+) to MnO4(-)? [closed]
$$\ce{Mn^2+ Solution ->[reagent 'A'] MnO4^-}$$
The reagent '$\ce{A}$' can be
(A) $\ce{Pb2O3 + \text{conc.} HNO3}$
(B) $\ce{K2S2O8}$.
(C) $\ce{(NH4)2S2O8}$
(D) $\ce{K2SO4}$
All of the options can ...
2
votes
0answers
30 views
Ionic radius for tetrahedral metal–ligand complexes
The ionic radii for metal–ligand complexes that are in an octahedral coordination are easy to find. I understand that when the $\mathrm{e_g}$ orbital is filled, the ionic radius increases because the ...
4
votes
2answers
71 views
Transition metal chalcogenides
According to wikipedia, a chalcogenide is a chemical compound consisting of at least one chalcogen anion and at least one more electropositive element. In the same sense does transition metal ...
1
vote
0answers
20 views
The quartic electronic state of octahedral Fe(III): How make crystal field splitting diagram?
Using simple arguments from crystal field theory, how do I rationalize the quartic state of octahedral Fe(III)? I am not able to in a logical way distribute the 5 d electrons in such a a way as to end ...
1
vote
0answers
41 views
How can an element have two outermost shells incomplete? [closed]
As I read my book, I saw its written that the Transition metals have two outermost shells incomplete.
But , as I had read earlier, that shells are filled in stepwise manner.
So how is this possible?
...
1
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1answer
73 views
Why aren't solid pure transition metals colourful?
I understand that the compounds of transition metal are colourful because of the appropriate energy gap between different d orbitals. But why aren't they also colourful in their solid pure state? For ...
0
votes
0answers
25 views
How can t2g orbital account for extra stability in absence of ligands?
I have read in a book that t2g orbitals sometimes account for stability in 3d block transition elements. For example,
Chromium in 2+ oxidation state shows reducing properties because Chromium in 3+ ...
0
votes
1answer
59 views
Why does this ligand form 6-coordinate complexes with Transition elements and 8-coordinate complexes with Inner transition elements? [closed]
What change takes place in the denticity of this ligand if it is an inner-transition metal ion vs a common transition metal?
Primarily, why does the ligand behaves differently with the two situations ...
2
votes
0answers
39 views
Liquid storage of transition metal oxides?
Transition metal oxides (TMOs) have a lot of interesting properties, from ferroelectricity to battery applications. Often times you can change the properties with only slight changes of oxygen ...
1
vote
0answers
54 views
Manganese oxide reacts with tin(IV) hydroxide?
I have a problem on my chemistry summer homework in which it asks me to predict the product of “solid Manganese-Oxide when it reacts with tin(IV)-hydroxide in aqueous solution”. My issue is that there ...
2
votes
1answer
40 views
Determination of spinel structure by CFSE
$\ce{CuFe2O4}$ has inverse spinel structure, but $\ce{ZnFe2O4}$ has normal spinel structure. Explain.
I know that normal spinels have a structure like $\ce{(A^{II})^{tet}(B^{III})^{oct}_2O_4}$-like ...
6
votes
0answers
51 views
Are platinum metal whiskers very unusual?
Over 20 years ago I pulled my first set of platinum spark plugs out of a car because the engine was missing badly. Two of the six plugs each had one whisker in the gap between electrodes. One crossed ...
5
votes
1answer
69 views
What is the electron count in this nickel complex?
Our class has started learning about electron counting using the ionic method. I was having a little difficulty, especially when there are two metals in one complex, so I looked at Wikipedia for help.
...
1
vote
2answers
66 views
Octahedral Crystal Field Splitting Orbital Degeneracy
How are the $\mathrm{e_g}$ orbitals degenerate with each other?
Note: This isn't a homework question. After the semester ended (I don't go to MIT), I ended up on MIT open course-ware to watch some ...
0
votes
2answers
83 views
Why are chelating ligands often used to treat poisoning by heavy metals (e.g. mercury, lead)?
Why are chelating ligands such as EDTA often used to treat poisoning by heavy metals (e.g., mercury, lead)?
I have a vibe that it has something to do with the lone pairs of electrons that are able to ...
0
votes
1answer
36 views
Octahedral Crystal Field Splitting Orbital Energy Levels [closed]
(image source)
In the above diagram, where do the 3/5 and 2/5 come from? Also, how are the $\ce{e_g}$ orbitals degenerate with each other?
7
votes
2answers
517 views
Can aqua regia work with sources of chloride and nitrate other than hydrochloric acid and nitric acid?
According to Professor Poliakov and a question on Chemistry Stackexchange here, gold dissolves in aqua regia because the nitrate ion oxidizes the gold into $\ce{Au^3+}$, and the chloride bonds to the ...
3
votes
1answer
39 views
Similarities between Co and Ni [closed]
Elements $\ce{Co}$ and $\ce{Ni}$ share many similar/same properties and usually if one of them is an example of some group (e.g., ferromagnetism, same possible oxidation states, packing fraction and ...
2
votes
1answer
35 views
Nickel salts from hypochlorites
(JUST A HEADS UP I’m 15 years old and new to chemistry) So I was recently looking around the house looking for products that I can extract chemicals from and I found a bottle of cleaning Vinegar ( 5% ...
-1
votes
1answer
32 views
Are inner transition metals also part of the transition group? [closed]
My book doesn't say anything about this and leaves it ambiguous. The periodic table they gave colored the inner transition metals as "transition metals". So, are inner transition metals also part of ...
3
votes
1answer
43 views
Order of filling electrons in Jahn-Teller energy diagram
When filling electrons in atomic or molecular orbitals we fill first the lower energy orbitals and then the higher, according to Pauli and Hund's rule. But this seem not to be the case when ...
-6
votes
1answer
56 views
what catalyst to use for the reaction between AgNO3 and NaCl? [closed]
What is the best catalyst to use for the reaction between AgNO3 and NaCl that would result in a change in activation of energy so therefore more precipitate formed. Please give me the ways I can ...
28
votes
3answers
8k views
Why isn't the American nickel magnetic?
I never thought that modern American nickels actually contained nickel anymore. However, according to this wiki article, the coins actually do contain 25% nickel, the rest being copper. And yet, no US ...
1
vote
0answers
40 views
Effect of optical isomerism on colour of transition metal complexes
I know that different stereoisomers of a given transition metal complex (cis- and trans- forms) have different colours. But do different optical isomers (non-superimposable mirror images) have ...
-1
votes
1answer
71 views
Does tris(ethylenediamine)iron(III) exhibit optical isomerism? [closed]
I'm studying 12th. In my book they mentioned that $\ce{[Co(en)3]^3+}$ exhibits optical isomerism.
But in that same book, there is a question
Which of this doesn't exhibit isomerism?
and the ...
1
vote
2answers
85 views
Indicators of Cu(I) or Cu(II)
We performed an experiment in class where we placed a piece of copper wire in a solution of silver nitrate, we were tasked with predicted the mass of copper that should react and the mass of silver ...
10
votes
0answers
191 views
What is d-orbital collapse?
When I was perusing the works of Schwarz on atomic structure, I came across the unfamiliar term of d-orbital collapse.
He describes it as a variation in energetic sequence from group 1 to 3 elements ...
1
vote
1answer
75 views
Only valence shell electrons participate in bonding then how is Cr in H2CrO4 forming 6 covalent bonds although it has only 1 valence electron?
The structure of $\ce{H2CrO4}$ is as follows:
Shell configuration of chromium is 2,8,13,1 i.e. it has only 1 valence electron and only valence electron participate in bonding but Chromium in the ...
4
votes
1answer
86 views
Fractional index in a chemical formula of metal oxide
I have just read an article in which they used $\ce{WO3}$ and $\ce{WO_{2.9}}$ as precursors, whose objective was to form $\ce{WS2}$, in an atmosphere of argon by CVD. In one boat there is the powder ...
4
votes
2answers
563 views
Why Zn has highest ionisation enthalpy in 3d series?
Zn which has the highest ionisation enthalpy in 3d series.The reason given in my textbook is:
The value of zinc is higher because it represent ionisation from 4s level.
This is not correct because ...
3
votes
1answer
510 views
Reorganization during ionisation for d block elements
This is a quote from my textbook:
The irregular trend in the first ionisation enthalpy of 3d lmetals,can be accounted for by considering that the removal of one electron alters the relative ...
1
vote
0answers
44 views
Why is Cadmium so carcinogenic compared to other heavy metals?
This free article as well as this article do a good job highlighting the carcinogenic effects of Cadmium and the mechanisms by which they occur. However, my question is why is Cadmium so carcinogenic ...
0
votes
1answer
86 views
How to precipitate Chloroplatinic acid? [closed]
For the precipitation reaction, I have to react $\ce{H2PtCl6}$ with $\ce{(NH4)2CO3}$ while maintaining the $\ce{pH}$ in the range of 7-8 at 60 °C. But the problem is Chloroplatinic acid is not ...
-4
votes
1answer
28 views
Why n-Butane has high B. p than iso-Pentane although both have equal no. of carbon atoms along the chain length? [closed]
n-Butane =B. p =-1 oC
iso pentane =b. p= 28 oC
0
votes
1answer
209 views
Why does 2+ oxidation state become more stable relative to 3+ oxidation state for first row of transition metals? [duplicate]
I viewed an image showing all the possible oxidation states of each element in the first row of transition metals, and the main oxidation states highlighted in a different colour.
I noticed all ...
2
votes
0answers
106 views
Colour of VO3^-?
To aquire the yellow colour of vanadium ion, it must be present in a 5+ oxdiation state.
This can be acheived (according to my textbook) by adding dilute sulfuric acid to $\ce{NH4VO3}$, then followed ...
0
votes
1answer
72 views
Can the 5+ and 4+ oxidation state of Vanadium ion exist independently?
From my class text book:
The oxidation states of Vanadium ions 5+ and 4+ are shown in the compounds $\ce{VO2^{+}}$ and $\ce{VO^{2+}}$ respectively, whereas $\ce{V^{3+}}$ and $\ce{V^{2+}}$ are ...
-1
votes
1answer
1k views
The second Ionisation energy of the Zn, Cd, and Hg follows the order?
It is observed that the order of second ionisation energy of these three elements is $\ce{Zn > Cd < Hg}$.
Why is there an anomaly in the observation?
0
votes
1answer
156 views
Why is chromate coloured but tungstate colourless?
I have to try and work this out using the tetrahedral molecular orbital diagram for $\ce{[WO4]^2-}$ but I am confused as both are $\mathrm d^0$ right?
1
vote
1answer
249 views
The number of transition elements
I searched in the internet but most of them said that there are 38 transition metals. But our text book says that group 12 or the group of zinc CAN'T BE COUNTED as transition metals. Which already ...
-4
votes
2answers
215 views
Oxidation state of Manganese [closed]
We know that Mn shows variable oxidation states ranging from +2 to +7 but why is +1 oxidation state of Manganese(Mn) not stable?
The +1 oxidation state of Mn would have a configuration of 4s1 3d5.
...
-1
votes
1answer
51 views
Transition metals and their ability to form coloured ions [closed]
I understand that in solution. transition metals form coloured ions, but what about the transition metals in solid compounds that are coloured- is this also due to d-d transition?
can you give any ...
2
votes
1answer
112 views
Effective Bohr Radius in Transition Metal Complexes?
I am playing around with a toy model of a transition metal complex where the HOMO are $d$-electron states of predominantly transition metal character. Let's say this is a $d^1$ (or $d^9$) system and ...
2
votes
1answer
60 views
Flame test for copper salts
I have read from sources here, here and even in my textbook that Copper (specifically $\ce{CuCl2}$ ) burns with a bluish green flame. All the sources mention that this is due to electron excitation ...
1
vote
1answer
357 views
Does pure iron not rust?
In my school science textbook, written more than twenty years ago, it said that pure iron does not rust. Accompanying was a photograph of an ancient iron statue situated outside, which had not rusted.
...
0
votes
0answers
115 views
Why does manganese have lower enthalpy of atomisation and melting point than chromium? [duplicate]
We know that due to stable half filled 3d5 config of Mn(3d5 4s2) it deviates from the general trend of melting points. However, Cr(3d5 4s1) also has stable half filled d-orbitals yet it has higher ...
1
vote
2answers
1k views
How is Zn not a transition metal? [duplicate]
A transition metal can be defined as an element that possesses an incomplete sub-level in one or more of its oxidization states. In the textbook I'm reading, it claims that zinc is not a transition ...
2
votes
1answer
359 views
What happens when ferric chloride is dissolved in water?
Ferric chloride can be prepared by dissolving hematite in hydrochloric acid:
$$\ce{Fe2O3 + 6HCl -> 2FeCl3 + 3H2O }\tag{1}$$
But the resulting ferric chloride will be exposed from its formation to ...
