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Atom sublevels fill according to the Aufbau principle which states that electron levels are filled according to their energy, the lowest are filled first, then followed by higher energies. To answer your question, 4s has a lower energy level than 3d.
A full electron configuration:
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s6 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6
Actually the above answer is incorrect and so is the question.
Contrary to what is stated in the vast majority of textbooks, the 4s orbital does not fill before the 3d, and nor does it have lower energy.
If you have access to the Journal of Chemical Education look for the article by Eugen Schwarz. April 2010, p. 444.
eric scerri PhD
UCLA
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Why does the 4S orbital begin to fill before the 3D orbital?
Electrons occupy orbitals in a definite sequence, filling orbitals with lower energies first. Generally, orbitals in a lower energy level have lower energies than those in a higher energy level. But, in the third level the energy ranges of the principal energy levels begin to overlap. As a result, the 4s sublevel is lower in energy than the 3d sublevel, so it fills first.
Why do electrons enter the 4s orbital before entering the 3d orbital?
because its energy level is lower
When comparing the energy of an electron in the 3d sub-level to that of an electron in the 4s sublevel of the same atom?
They are both capable of holding a maximum of 10
Why does an element lose 4S electrons before 3D electrons?
Because 4s is a lower energy level and 3d is higher. In fact, s levels should, strictly, be written first before d levels when writing electron configurations.
How many orientations can s orbital have about the nucleus?
The orbital orientations that are possible in each sub level are:S-1p-3d-5f-7
How many electrons can 3d hold?
There are a maximum of 10 electrons in the 3d sub-level.
Which orbital should fill first 4s or 3d orbital?
4s will fill first because it is at a lower energy level than the 3d level.
What is the element filling a 3d sub level in group 6?
Chromium
Why is 2d1 not possible?
A break down of 2d1:2 = the quantum energy level or electron shell denoted as 'n'd = the sub-shell of the energy level (known as a degenerate level)1 = the number of electrons occupying the sub-shell.Through extensive research by scientists, no known element has a d sub-shell in the second (n=2) energy level. In fact, the d sub-shell does not appear until the fourth period (fourth row).The first d sub-shell is known to be in the third energy level (therefore the first energy level with this sub-shell is 3d, but not 2d).Transition metals are the elements known to fill the d sub-shells. The first transition metal in the periodic table is scandium (Sc) with the electron configuration of [Ar]4s23d1.The reasons for the formation of sub-shell of d is beyond my knowledge and the scope of basic chemistry.
3d electrons on Fe?
The 3d sub-level has 5 orbitals, and therefore space for a total of 10 electrons. Excluding certain hyper-valent bonding scenarios, the first element with electrons to occupy the 3d sub-level is scandium (Sc).
How are the orbitals different in sublevels of the same principal energy level?
In every atom there are principle energy levels, sub-levels and atomic orbitals. The principle energy levels are often those first taught when studying chemistry. They correspond to how close the electrons are to the nucleus. The first principle energy level is closest to the nucleus and can hold a maximum of two electrons. The second principle energy level is slightly further away from the nucleus and can hold a maximum of eight electrons. The third energy level is even further away and can hold a maximum of ten electrons. Each principle energy level is comprised of different sub-levels: s, p, d and f. The s sub-level can hold a maximum of two electrons; , p a maximum of 6; d, a maximum of 10 and f, a maximum of 14 (although the f sub-level is only present in the lanthanide and actanide series). Sub-levels all have different energies and electrons fill sub-levels in order of lowest energy to highest. The first principle energy level has one sub-level, the 1s sub-level. The second principle energy level has two sub-levels, 2s and 2p. The third principle energy level has three sub-levels, 3s 3p and 3d. (However, the 4s sub-level is filled before the 3d sub-level, which is a different matter which cannot be explained quite so simply.) Now, each sub-level is comprised of atomic orbitals which define the approximate boundaries of the electron orbit. Each orbital can hold up to two electrons, so a s sub-level has one orbital; a p sub-level has three orbitals; a d sub-level has five orbitals and a f sub-level has seven. This explanation is really quite brief as there is so much more information concerned with principle energy levels, sub-levels and atomic orbitals.
What is the shorthand configuration of copper?
Atomic shorthand uses the noble gas before the element in questionAnswer: Cu: [Ar]4s[1]3d[10]Explanation: Copper Cu is an anomaly. Logically we would write 4s[2]3d[9] but for Cu, having the d sub level full is more stable than having the s sub-shell full and the d sub-shell less than full. Chromium also has this anomaly, and is written [Ar]4s[1]3d[5]
How many total orbitals are within the 3s 3p and 3d sub levels of the third energy level?
There are one 3s orbital, three 3p orbitals, and five 3d sublevels.
Why does the 4S orbital begin to fill before the 3D orbital?
Electrons occupy orbitals in a definite sequence, filling orbitals with lower energies first. Generally, orbitals in a lower energy level have lower energies than those in a higher energy level. But, in the third level the energy ranges of the principal energy levels begin to overlap. As a result, the 4s sublevel is lower in energy than the 3d sublevel, so it fills first.
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When phosphorous is excited what will its electronic configuration be and Will the excited electron go to 4s orbital as per energy level diagram or 3d orbital and why?
In the case of excited phosphorus, the electron will bump up to the 3d level. This is the next closest location (in terms of energy) that the electron can go. Even though ground state phosphorus has no electrons in 3d, the atom can still access that sub-level because the principal quantum numbers for 3p (where its valence electrons are anyway) and 3d are the same.
How do you make a 3d level on Littlebigplanet?
There is a glitch to do this. Just consult the level '3D level glitch' for more info
