All Questions
Tagged with periodic-trends electronic-configuration
19
questions
-2
votes
3
answers
169
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Why is there a non-uniformity in even the reasons that explain exceptions in the trends in chemistry? [closed]
I have been studying the periodic table and several properties of atoms like the Ionization Energy, Atomic Radii, Electron gain enthalpy, Electronegativity etc.
Now, each property has somewhat of a &...
- 120
-5
votes
1
answer
88
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Can halogens show -3 or -5 or -7 oxidation state. Why? [closed]
I mean can we think it like if the electrons get excited into the d orbitals and because there are now more than one unpaired electron, why does it only loose them and why don't they accept more than ...
- 7
-1
votes
3
answers
288
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Do Ions with less stability have less energy of ionization than those who are stable?
Problem. I've come up with the strange example of the third energy of ionization of both $\pu{Mg}$ and $\pu{Al}$, the standard logic that is to be applied on any problem of "which element has ...
- 133
-2
votes
1
answer
71
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Predict the valence configuration of this element using the first five ionization energies [closed]
If the first five ionization energies of an element are, respectively: $\pu{1.09 kJ/mol}$, $\pu{2.35 kJ/mol}$, $\pu{4.62 kJ/mol}$, $\pu{6.22 kJ/mol}$ and $\pu{37.83 kJ/mol}$, to which group of the ...
- 9
5
votes
1
answer
927
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Why aren't Boron and Aluminium assigned to group 3 of periodic table? What determines the group? [closed]
I've been curious about this 3D representation of the periodic table "Mendeleev's Flower" and was trying to study it, wondering if it reveals any regularities that are not obvious from classic ...
2
votes
2
answers
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, ...
- 121
0
votes
1
answer
1k
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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 ...
- 207
0
votes
1
answer
89
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Do the spins of outer orbitals block measurement of spin of inner orbitals?
Do the outermost s1 and s2 electrons block an outside observer from measuring the larger inner group orbitals for elements heavier than Nitrogen (for instance, would Chromium's 4s1 electron or ...
- 296
5
votes
0
answers
112
views
Trends in Slater's constant
I am aware of the various Slater rules to calculate the effective nuclear charge, $Z_\mathrm{eff}$
However, how can I decide the order in which the orbitals 2s, 3s, 3d, 3p, 4d, and 4f stand when ...
- 73
1
vote
1
answer
2k
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Last electron of a transition element
The electronic configuration of nickel is
Ni: [Ar] $3d^84s^2$
Here, while writing the configuration, we fill the 3d after 4s.Hence the 28th electron enters the d orbital.
But
$\ce{Ni+}$: [Ar] $...
- 73
4
votes
1
answer
357
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Finding electron configuration by following the Aufbau principle
In the question, "Electron Configuration of Tellurium", there is mention of the 'follow yellow brick road' method of finding electron configuration.
What I'd learned in the past was to find the ...
- 6,801
6
votes
2
answers
296
views
Why ground-state configuration is consistent ("additive") from one element to the next?
Ground-state configuration ("electron shells") is consistent throughout the periodic table, for example:
(source)
Why is it this way if the Hamiltonian of each atom is different? In other words, why ...
- 4,265
1
vote
1
answer
383
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Why does ionization increase from Li to Be? [duplicate]
If ionization energy decreases from $\ce{N}$ to $\ce{O}$ due to the pairing of electrons (causing electric repulsion and greater potential energy) in the $\mathrm{2p}$ orbital in the $\ce{O}$ atom, ...
- 1,529
5
votes
1
answer
9k
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Why ionic radii of Cu2+ is less than Zn2+?
Fully filled orbital has more effective nuclear charge than incompletely filled orbital. So atomic or ionic radii of elements or ions having fully filled orbitals should be less than that of elements ...
- 26.3k
1
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0
answers
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How does the electron configuration of platinum relate to its stability?
Does platinum's electron configuration, [Xe] 4f14 5d9 6s1, influence its reactivity and stability? Is the electron configuration the primary contributing factor to platinum's relative inertness?
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