All Questions
Tagged with periodic-trends transition-metals
33 questions
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Anomaly in boiling point as compared to melting point in d-block [duplicate]
Consider the following graph:-
In the above graph, it can be observed that the melting point of Chromium is higher than that of Vanadium (though there's not much greater difference despite the fact ...
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1
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Why does the 1st ionisation energy decrease from the 9th period to the 10th period
I’m currently looking at the ionisation energy chart within my chemistry textbook and while I know that there are not really meaningful periodic trends within transition metals, generally the ...
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2
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Why do heavier transition metals show higher oxidation states?
In p-block elements, higher oxidation states are less stable down the group due to the inert pair effect. This is not the case for transition metals.
Why do heavier transition metals show higher ...
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1
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Why does Cr have higher melting point in the 4 period among the transition metal? [duplicate]
There is a lot of answer stating that the low enthalpy of atomisation in Cr is due to the reason of partially filled d orbital, thus having extra stability. This makes the orbital more attracted ...
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Trend in formation enthalpy of metal fluorides
Please see below for the data I am referring to. I don't really understand why the trend in Cr ceases and reverses.
I think I understand what the logic for WFn is - while the cost of forming Mn+ ...
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Why do the successive ionisation energies of Ni and Pt diverge?
The data I am referring to is below on the graph. The explanation I have found is that the 5d orbital of Pt is more diffuse than the 3d orbital of Ni, so is less sensitive to the increases in Zeff as ...
4
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1
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610
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Lower melting points of zinc, cadmium and mercury
I am aware of the fact that d-block elements like zinc, cadmium and mercury have lower melting points than other d-block elements. Also I am aware that these three metals have a fully filled d shell.
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Melting and boiling points of transition elements
The melting and boiling points of transition elements increase from scandium ($1530~\mathrm{^\circ C}$) to vanadium ($1917~\mathrm{^\circ C}$). They increase because as we go across the group, we have ...
- 22.9k
2
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Atomization enthalpies of transition elements
So, my book says that transition elements have higher enthalpies of atomization than other elements (say s- or p- block) because of stronger metallic bonding, primarily due to large number of unpaired ...
- 408
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69
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Why middle elements of transition series show more number of oxidation states [duplicate]
Why do the elements in the middle of the transition series show more number of common oxidation states than others?
- 38.5k
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Is there regular decrease in atomic radii of 3d series?
The following fragment of the table of atomic radii from CrystalMaker — Elements, Atomic Radii and the Periodic Table shows a regular decrease in the atomic radius of 3d series:
Table of Atomic Radii
...
- 38.5k
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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 ...
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1
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752
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Why is copper a better conductor of electricity than calcium?
How would we compare the electrical conductivity between copper and calcium? I understand that electrical conductivity of a metal is dependent on the number of delocalized electrons for that metal. ...
- 14.3k
5
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What determines the kind of Bravais lattice structure (body-centred cubic, hexagonal, etc) a transition metal shows?
With the exception of Zn, Hg, Cd and Mn transition metals most transition metals have only one kind of lattice structure at room temperature. Another trend I noticed was that Groups 3 and 4 have ...
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Exchange energy of d6 configuration
In NCERT Chemistry book, it is given as:
Exchange energy is responsible for the stabilization of energy state. Exchange energy is approximately proportional to the total number of possible pairs of ...
2
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2
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10k
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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, ...
CommunityBot
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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 ...
CommunityBot
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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 ...
- 436
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561
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Why are the Covalent Radii of Ruthenium and Osmium So Similar?
Osmium and Ruthenium have covalent radii 144 and 146 respectively (according to Wikipedia).
How are these values so similar when Osmium has 32 more electrons, with another filled p, s, and f orbital ...
- 147
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628
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Rationalising the trend of standard electrode potentials between the +II and +III oxidation state of first-row transition metals
Trends in standard electrode potentials of d block elements:
An examination ofthe $E^0 (\ce{M^3+}/\ce{M^2+})$ values (Table 8.2) shows the varying trends. The low value for Sc reflects the ...
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Why does cobalt have no negative charge?
I would like to know why cobalt cannot have a negative charge (or at least why a negative charge for cobalt isn't typical). I am not sure where I have gone wrong in my reasoning.
The electronic ...
- 1,623
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Why does density decrease across the period 4 and 5 transition metals?
I know that density decreases across period 4 because the last two elements are liquids and gases which means that their densities are less but why are the densities increasing and then decreasing ...
6
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Variation in atomic sizes in the transition elements
From left to right across a period, effective nuclear charge increases in the transition series, just like in the p block, and so atomic size decreases. Here the electrons are being added to the d ...
- 68.7k
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Why are there peaks in electronegativities in d-block elements?
Looking at the Pauling electronegativities in the Periodic Table (below, from ChemWiki):
Asides from the overall trend of increasing electronegativity across and up the Periodic Table (towards ...
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143
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Relative orbital energies of Mn and Ni
In this MO diagram, why are the atomic Mn $3d$ orbitals higher in energy than the Ni $3d$ orbitals?
- 38.5k
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Why the ionization energy of Au is more than that of Cu?
As we go down the group from 3d to 5
d, size increases.
Vanderwaal radius of Cu and Au is 140pm and 166pm respectively. Since Cu is smaller in size, ionization energy of Cu must be greater.
Then ...
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1
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1
answer
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Pattern to determine the maximum ionic charge for transition elements?
According to my textbook, main group elements follow a simple pattern when determining their maximum ionic charge. The maximum cationic charge is always equivalent to their main group number (group ...
- 68.7k
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The most variant groups of periodic table
Is it okay to call group 11 (formerly 1B) a "group"? I meant that according to my knowledge "A group is a horizontal column consisting of elements with similar valencies and a continuous gradation in ...
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Melting temperature and electronegativity trends in transition metals [duplicate]
So I know that generally the melting temperature increases across the row (let's look at just the first row for now) but what are the deviations? And why do they occur? I've looked everywhere online ...
- 19.1k
2
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714
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Trends in the covalency of bonding across the transition metals
I am under the impression that the covalent character in the bonding of transition metal compounds increases across a group; in fact I think this is why they're called transition metals (a transition ...
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Why is Iron (Fe) difficult to reduce?
$\ce{Fe^3+ + e- -> Fe^2+} \quad +0.77$
$\ce{Fe^3+ + 3e- -> Fe} \quad -0.04$
$\ce{Fe^2+ + 2e- -> Fe} \quad -0.41$
$\ce{Zn^2+ + 2e- -> Zn} \quad -0.76$
$\ce{Co^2+ + 2e- -> Co} \quad -0.29$...
- 68.7k
7
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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, ...
- 15.5k
5
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How to rationalise the trend in the covalent radii of the transition metals?
Why do the covalent radii of transition series decrease at the start rapidly, then become almost constant and at the end of series begin to increase from left to right in periodic table?
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