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].

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what possible reactions from chemistry will occur when water is added to water container? [closed]

cu has high reduction potential than water and hence will gain electrons from water but at the same time cu is not in charged state and so why it will gain electrons. 2)cupper being an active metal ...
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58 views

Why is HgI2 a colored complex?

Why is $\ce{HgI2}$ a colored complex it has fully filled d-orbits. According to the book, one which has fully filled d-orbital has no color in transition elements. So, why is this compound colored?
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Can someone help me figure out why I got this roman numeral wrong?

I am currently working on a Roman numeral practice in Chemistry and I am stuck on a question. I was wondering if someone could help me. The question: What is the chemical name of Fe2SO3? My answers: ...
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1answer
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Geometry of the transition metal complex in solid dipotassium bis(oxalato) copper(II) tetrahydrate

I was thinking of the geometry of the transition metal complex in solid $\ce{K2[Cu(ox)2] · 4 H2O}$ solid around the $\ce{Cu(II)}$ ion. At first I thought square planar, but is it possible or is there ...
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KMno4 is the strongest oxidizing agent. So why does it tend do have +2 oxidation state with reaction with acids? [closed]

Manganese has an oxidation state of +7 in potassium permanganate. When reacted with sulphuric acid, how does it tend to have +2 oxidation state by forming $\ce{MnSO4}$ along other products ? In acid, ...
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1answer
31 views

Bonding in d10 metals such as Zn

I recently learned about the MO bonding model in metals, where many metal atoms form lots of orbitals close in energy that form bands. However, I can't understand the bonding in d10 metals. It seems ...
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Molecular orbital diagram for carbene-metal and carbodiphosphorane-metal interaction

I am interested in understanding how carbenes and carbodiphosphoranes interact differently with a transition metals. I would like to use qualitative molecular orbital theory arguments (with an ...
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What type of bonding is there among d-block metals?

Metallic bond strength in $\mathrm{d}$-block elements increases up to the middle and then decreases. Why does pairing decrease the strength of metallic bond? What does pairing have to do with metallic ...
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2answers
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Density of d-block elements

Something that confuses me slightly is the trends in density when comparing periods 4, 5, and 6 in the d-block. Looking at periods 5 and 6, the density peaks at group 8, with ruthenium and osmium, ...
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1answer
679 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 ...
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2answers
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Understanding the Jahn–Teller elongation and compression for octahedral complexes (stabilisation/destabilisation of d orbitals)

I am currently learning about Jahn–Teller effect. For elongation I wondered why the d orbitals with $z$ component are stabilised when the metal–ligand bonds are getting longer? I thought a longer bond ...
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Beer Lambert law when complex is tetragonal (Jahn-Teller elongated)

I wondered what modifications there would be to the Beer Lambert law to find the molar extinction coefficients for the solution if the solvent contained the ligands which bind to the metal centre of a ...
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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 ...
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How does chromium behave in a carbonate solution? [closed]

I'm wondering how chromium (as a metal or as a salt) behaves in a concentrated carbonate solution. Will it form any, one or several carbonate specie(s)? Will the metal solubilize? How does it affect ...
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Does copper(III) nitrate exist?

I was balancing this reaction when I found an unusual compound had been formed. $$\ce{Cu(s) + HNO3(aq)-> Cu^{3+}(aq) + NO(g)}$$ My attempt: Balancing oxidation number: $$\ce{Cu -> Cu^{3+} +3e^-...
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How to make anhydrous or monohydrate FeSO4 from heptahydrate form?

I need the anhydrous form of $\ce{FeSO4}$ (7720-78-7). I have $\ce{FeSO4.7H2O}$, is there anyway it can be converted to anhydrous form, or at least to monohydrate? Do you know where I can purchase it? ...
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1answer
421 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 ...
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Why can mercury(I) exist, but not zinc(I)?

Mercury shows variable valency while zinc does not. Its electronic configuration is $\ce{[Xe]\:4f^14 5d^10 6s^2}$. So it can donate the $\ce{6s^2}$ electrons and should only be able to form $\ce{Hg^2+}...
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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 ...
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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 ...
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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 ...
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Why is it wrong to use the concept of hybridization for transition metal complexes?

I have asked a lot of questions on coordination chemistry here before and I have gone through a lot others here as well. Students, including me, attempt to answer those questions using the concept of ...
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Can one turn a nickel blue?

I've heard of artificial coin toning, but haven't been able to find a recipe for creating a blue (or blue-ish) nickel coin. While not a metallurgist, I work with one. She tried nitric acid, which ...
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Why are palladium and platinum carbonyls unstable at room temperature?

By palladium and platinum carbonyls, I mean the mononuclear, homoleptic, charge-neutral, binary carbonyl complexes of the form $\ce{M(CO)_n}$ and not any heteroleptic complexes like $\ce{Pd(CO)(PPh3)3}...
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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 ...
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6answers
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Colour of Nickel thiocyanate

What is the colour of $\ce{C2N2NiS2}$ (Nickel thiocyanate)? In most of the web sites it only molecular weight,formula and other specifications but its colour is missing every where.
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1answer
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Compare stability of transition metal cations in aqueous solution

I have to compare the stability of the following transition metal cations: $\ce{Co^3+, Fe^3+, Cr^3+, Sc^3+}$ in aqueous solution. (Source: Joint Entrance Exam (JEE) 2013 Mains India) The first thing ...
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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? ...
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2answers
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Is palladium on carbon acting as an oxidising or reducing agent?

In the conversion of piperidine to pyridine, palladium on carbon (Pd/C) is used. But it is reducing agent. Clear the confusion, please.
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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 ...
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1answer
153 views

precipitation reaction - cellulose in schweizer reagent reacts with acid

In the regeneration of dissolved cellulose (in a cuprammonium solution) in an acid bath, say sulphuric acid, what is the chemical reaction? There is a lot about the chemistry of the production of the ...
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1answer
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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 ...
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Is scandium considered a transition metal?

I have seen so many conflicting answers to this question in various places so I wanted to ask it again. IUPAC defines a transition element as an element whose atom has a partially filled d sub-...
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Mixing cobalt(III) hydroxide and thallium(III) hydroxide

A simple question on solutions is driving me crazy. At this point, I think the textbook's wrong. Here's the question: A saturated solution of cobalt(III) hydroxide $(K_\mathrm{sp} = \pu{1.6e-44})$ ...
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1answer
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Can metals have a net negative charge

Normal metals like sodium or Calcium have a positive charge as $\ce{Na}^+$ or $\ce{Ca}^{2+}$. Transition metals have a loot of variable oxidation states. Yesterday I read about Iridium in Wikipedia ...
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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+ ...
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1answer
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Regular decrease in the atomic radius of 3d series

While comparing atomic radius, two factors are important: A. Decrease in size due to increase in effective nuclear charge B. Increase in size due to increase in shielding effect I was surprised to ...
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1answer
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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 ...
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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 ...
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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 ...
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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 ...
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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 ...
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2answers
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Why is Cr²⁺ is a good reducing agent but Mn³⁺ is a good oxidising agent? [duplicate]

The question is the same as the title states. In my textbook,[NCERT Chemistry I for Class 12 , pg no 217.] the following is written $\ce{Cr^{2+}}$ gets converted to $\ce{Cr^{3+}}$ as the +3 oxidation ...
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What is the lattice structure of manganese?

A transition element is defined as the one which has incompletely filled d orbital in its ground state or in any one of its oxidation state. Zinc , cadmium and mercury are not typical transition ...
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What is CuCl · CO · 2 H₂O?

What is the chemical $\ce{CuCl.CO.2H2O},$ formed via the reaction of copper chloride and carbon monoxide? Does this compound have any use or appear in any noteworthy reaction?
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Why is anhydrous copper(II) sulfate white while the pentahydrate is blue, even though both have one unpaired electron?

We all know that $\ce{CuSO4.5H2O}$ is blue and it turns to $\ce{CuSO4}$ on heating which is white. I also learnt about coordination complexes and d–d transitions and how transition metal compounds are ...
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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. ...
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How to know dichromate is being reduced from Cr⁶⁺ to Cr³⁺?

When potassium dichromate is being used as an oxidising agent, it gets reduced from chromium(VI) to chromium(III). Is there any way to know that or calculate that other than being familiar with ...
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2answers
92 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 ...
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How to determine the oxidation states of the metal atoms when both cation and anion are coordination complexes?

How to determine the oxidation states of the metal atoms when both cation and anion are coordination complexes? For example, how to determine the oxidation states of $\ce{Pt}$ in the following ...

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