how much of\rbits electrons have for example Fe56 atom? In on place I read that on each orbit can't be more than 2 electrons. And in wikipedia read that electrons orbits can be up to 10 and maybe more... So who is right? So according to textbooks Iron 26/56 not jonizated have 13 electrons orbits.
The number of orbitals is infinite in any atom. But electrons use a finite number of them.
At most 2 electrons per orbital, but then one should say properly that atoms have three orbitals 2p ans so on. That's just a matter of vocabulary, people tend to say "the" 2p orbital has 6 places because the three 2p are identical, just rotated one from another.
Beware that electrons won't fill the orbitals in a simple sequence. This is especially true for so-called transition elements (like iron! Couldn't you pick a simpler example, like nitrogen?). And they won't pair unless necessary.
At most 2 electrons per orbital, but then one should say properly that atoms have three orbitals 2p ans so on. That's just a matter of vocabulary, people tend to say "the" 2p orbital has 6 places because the three 2p are identical, just rotated one from another.
Beware that electrons won't fill the orbitals in a simple sequence. This is especially true for so-called transition elements (like iron! Couldn't you pick a simpler example, like nitrogen?). And they won't pair unless necessary.
QUOTE (Enthalpy+May 11 2008, 04:34 PM)
At most 2 electrons per orbital,
That's what I want to hear. And another metaphors and metaprhrase curently don't interesting to me... So in each orbit at maximum 2 electrons and in final orbit can be one electron and in all lower exactly 2
That's what I want to hear. And another metaphors and metaprhrase curently don't interesting to me... So in each orbit at maximum 2 electrons and in final orbit can be one electron and in all lower exactly 2
As I said, the sequence of filling the orbitals isn't that simple.
One reason for it is that as a first electron fill an orbital, it repels electrically the second electron, which finds a better place alone on another orbital.
For instance, in a nitrogen atom (which is something very unusual), the three outer electrons fill on 2p orbital each, instead of grouping in pairs.
With heavier atoms, where many orbitals have similar energies, electrons don't fill a shelve before beginning a new one. These are transition elements - though more elements behave in a complicated manner as well.
Also, the common assertion that full shelves are chemically inert is false. For instance, beryllium is chemically quite active, though its 2s shelve is full. Just as carbon also has the valence 4 in addition to 2. Or xenon builds stable molecules with fluor.
In this field, beware of simple ideas.
One reason for it is that as a first electron fill an orbital, it repels electrically the second electron, which finds a better place alone on another orbital.
For instance, in a nitrogen atom (which is something very unusual), the three outer electrons fill on 2p orbital each, instead of grouping in pairs.
With heavier atoms, where many orbitals have similar energies, electrons don't fill a shelve before beginning a new one. These are transition elements - though more elements behave in a complicated manner as well.
Also, the common assertion that full shelves are chemically inert is false. For instance, beryllium is chemically quite active, though its 2s shelve is full. Just as carbon also has the valence 4 in addition to 2. Or xenon builds stable molecules with fluor.
In this field, beware of simple ideas.
You want to say, that electron either ocuping place according to charge rules, either by shrodinger equation. But still never can be more than 2 electrons in one orbit. And one electron can be only on outer-last orbit. I guess those 2p, 2s and so on was gotten frrom shrodginer equation and was veried with experiment... But how according to them judge about properties of matter? Still need simulate it and what you will understand from it? Density of atoms in g/cm^3 ? What's more? Somthing in combustion engine, biology? How it is important? Not very much...
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