The d sublevel always contains 5 orbitals. Therefore the d sublevel can accommodate 10 electrons just the same as 3d and 4d orbitals.
Each of the 5 separate d orbitals can only contain two electrons.
there are five 5d orbitals
each orbital can accomodate 2 electrons maximum
so ten electrons (maximum) can be accommodated in 5d orbitals
[Xe] 4f^14 5d^8
Any orbital can only contain a maximum of 2 electrons. The 5d energy level contains 5 orbitals - 5dxy 5dxz 5dyz 5d(x2-y2) and 5(dz2) each of which can contain a maximum of two electrons, so there are 10 total electrons in the set of 5 d orbitals.
1s orbital 3P, 5d, and 7f in discovered elements
The subshells of 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 4f act like core orbitals. This understanding of the configuration of the atom helps us to understand why electrons and atoms behave the way they do.
Assuming the electron is in the lowest states and the atom is neutrally charged, it will fill an orbital before extending the next one. 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p H and He fill 1s as it holds two electrons. Li and Be fill 2s as it holds two electrons. B, C, N, O, F, and Ne will fill the 2p orbital as it holds 6 electrons (2p1, 2p2, and 2p3 orbitals). However, nitrogen will have one electron in each 2p1, 2p2, and 2p3 orbitals as an electron will not go two to an orbital until each orbital is filled. Neon completes the 2p orbital and is very stable (considered an inert gas--electrons are neither attracted nor want to leave the completed 2p orbital). Fluorine is the most electronegative element, as it wants to rip any electron it can to fill its 2p orbital. All noble gasses (right most on the periodic table) will complete a p-orbital. Periods 3-12 will fill a d-orbital. Lanthanoids and actinoids will fill the f-orbitals. So, for instance, Calcium (Ca) has an atomic number 20. You look up Ca on the periodic table. As it comes after He, it will have a 1p orbital filled. As it comes after Be, it will have a 2s orbital filled. As it comes after Ne, it will have a 2p orbital filled. And Ca will have a 3s orbital filled. Therefore, you note that Ca has electrons in the following orbitals: 1s, 2s, 2p, 3s. Another example is Fluorine (F), which would be: 1s, 2s, 2p1(2), 2p2(2), 2p3(1) where the parenthetical numbers note the number of electrons in each orbital.
5d
In any shell excluding shell1, there is only 1 s orbital and 1 p orbital. Subshells and the Orbitals are same. Orbital g is known as subshell 5. g orbital is present shell 6. But till today no element is discovered with an electron in g orbital.
[Xe] 4f^14 5d^8
They are further away from the nucleus and easier to remove (requires less energy), i.e. first ionization is less.
Any orbital can only contain a maximum of 2 electrons. The 5d energy level contains 5 orbitals - 5dxy 5dxz 5dyz 5d(x2-y2) and 5(dz2) each of which can contain a maximum of two electrons, so there are 10 total electrons in the set of 5 d orbitals.
Yes, it exists. If you write the orbitals in order of increasing energy, then you get it. The order is:- 1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p..................... Here, you get the 3s orbital at the 4th place.
There are 5 total 4 d orbitals. (4dy, 4dx, 4dz, 4dz2, 4dx2-y2) Each of these can fit 2 electrons. This rule is known as the Pauli Exclusion Principal. 2X5 = 10. 10 total electrons. This is the same for all d orbitals. 1d, 2d, 3d, 4d, 5d, etc.
There are four (4) source: http://en.wikipedia.org/wiki/Electron_shell (if you go down a little way on the above website then it lists all of the electrons, which is very helpful!)
1s orbital 3P, 5d, and 7f in discovered elements
The subshells of 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 4f act like core orbitals. This understanding of the configuration of the atom helps us to understand why electrons and atoms behave the way they do.
You mean this form of the electron configuration. [Xe] 4f^14 6s^2 5d^10 6p^3 This is Bismuth and it is in the 5A nitrogen group and it has 5 valance electrons and needs three electrons to complete its valance octet.
Assuming the electron is in the lowest states and the atom is neutrally charged, it will fill an orbital before extending the next one. 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p H and He fill 1s as it holds two electrons. Li and Be fill 2s as it holds two electrons. B, C, N, O, F, and Ne will fill the 2p orbital as it holds 6 electrons (2p1, 2p2, and 2p3 orbitals). However, nitrogen will have one electron in each 2p1, 2p2, and 2p3 orbitals as an electron will not go two to an orbital until each orbital is filled. Neon completes the 2p orbital and is very stable (considered an inert gas--electrons are neither attracted nor want to leave the completed 2p orbital). Fluorine is the most electronegative element, as it wants to rip any electron it can to fill its 2p orbital. All noble gasses (right most on the periodic table) will complete a p-orbital. Periods 3-12 will fill a d-orbital. Lanthanoids and actinoids will fill the f-orbitals. So, for instance, Calcium (Ca) has an atomic number 20. You look up Ca on the periodic table. As it comes after He, it will have a 1p orbital filled. As it comes after Be, it will have a 2s orbital filled. As it comes after Ne, it will have a 2p orbital filled. And Ca will have a 3s orbital filled. Therefore, you note that Ca has electrons in the following orbitals: 1s, 2s, 2p, 3s. Another example is Fluorine (F), which would be: 1s, 2s, 2p1(2), 2p2(2), 2p3(1) where the parenthetical numbers note the number of electrons in each orbital.