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the first orbital to be filled is 1s because in this orbital the negatively charged electron is closer to the positively charged nucleus than in any other orbital
Quoted directly from my Chenistry Text Book ( World of Chemisty Zumdahl/Zumdahl/DeCoste , p377 McDougal Littell 2007)
What else can I help you with?
How many electrons tan fit in the 1st orbila shell?
Two electrons can fit into the first orbital shell of any atom.
How many electrons can go into a orbital?
In an atom, electrons are in "shells", the first shell is around the center of the atom and holds a maximum of 2 electrons. Each subsequent shell out, will hold a maximum of 8 electrons. there is no maximum number of shells.
Can 3f orbital be exist?
no because f orbitals are not energetically available until the n=4 quantum state
How is an unoccupied orbital represented in orbital notation?
An unoccupied orbital is represented by an empty box in orbital notation. It does not have any electrons present in it but is available to accept electrons if needed.
How many orbitals are in a 1s sublevel?
Sub level is also called orbital.It does not have any degenerate orbital.
What is the difference between a filled and an unfilled orbital?
A filled orbital has either 2 electrons (if it is the first shell of an atom) or 8 electrons. This is the highest number of electrons these shell can hold Every orbital tends to complete itself to form a stable element. A filled orbital could be any orbital, either 1st, 2nd, second last or last shell of the atom. An unfilled orbital always has atleast one less electron than the shell can hold. It is always the last shell of an atom and always makes the atom unstable as atom tends to acquire inertness by trying to get this unfilled oribital filled.
In an atom the first orbital is complete when it has how many electrons?
Any orbital is complete when it contains 2 electrons.
How many electrons tan fit in the 1st orbila shell?
Two electrons can fit into the first orbital shell of any atom.
Is The 9i orbital permitted?
There is technically a 9i orbital, but no atom in the ground state has any electrons in this orbital (in fact, no known element has any electrons in even the 8s orbital, and there are quite a few energy levels between that and 9i). In an excited state ... sure, it could happen.
What orbital is being filled when fluorine accepts one electron from sodium?
When fluorine (F) takes an electron from sodium (or from any element in an ionic bonding scenario), the 2p6 sub-orbital is filled, which allows fluorine to achieve the electron configuration of nearby neon (Ne).
What is the lowest level having f orbital?
The lowest energy level that has F orbitals is the fourth energy level. The Atomic orbital of any atom only contains 2 electrons.
How do you arrange the electron in energy level in all atom?
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.
How many p electrons are possible in any orbital?
6 electrons can ocupy the 2p, 3p, 4p, and so on. each p subshell has 3 orbitals, and each orbital can hold up to 2 electrons, so each p subshell can hold up to 6 electrons total.
Why all atom have 2 electron in first shell not more or less?
Actually, there is only one electron in a hydrogen atom, which has the atomic number 1. The existance of exactly two electrons in the innermost shell can be described by Shrodinger's Wave Equation. According to the Wave Equation, there is only one atomic orbital existing in the principal quantum number 1 energy level which is also known as 1s. Any atomic orbital can hold 2 electrons at most and it is the reason that every atom other than hydrogen have exactly 2 electrons in their innermost energy level.
What is the electron filling rule that states that any electronic orbital must be filled by 2 electrons of opposite spin?
the pauli exclusion principle
Why helium exist in the form of he not he2?
he2 is a fatty. He atom is a inert gas. so it can not react with any other atom or molecules to form any compounds.so He2 can't exist. ANOTHER ANSWER: Helium atom has only one shell i-e K-shell which can accommodate a maximum of two electrons which it already has. therefore Helium atom does not need any more electrons to become stable as it is already stable by duplet rule. Thus helium atom does not combine with another helium atom and hence exists as He and not He2.
How many electrons must an atom lose or share to become stable?
As long as the valence shell is filled, it can be any number.
