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4f subshell has the highest energy. A f subshell has the highest energy among all the subshells in any shell.
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.
More or less. If you mean "orbital" in the sense "those things that can hold two electrons", then yes. A bound electron in an atom can be described by four quantum numbers, one of which is the spin and has two possible values, so any given "orbital" can be described by 3.The three are: n - Principal (shell), n > 0 l - azimuthal (subshell: s, p, d, f, g, h, etc.) n > l >= 0 m - magnetic (specific orbital within a subshell), -l <= m <= l
He did not receive any.
In an atom of any isotope of any element, there is a number of protons which is similar to the number of electrons.
Hund's Rule states that electrons will occupy orbitals of a subshell singly before any are doubly occupied. This is to maximize the total spin of the electrons in the subshell.
4f subshell has the highest energy. A f subshell has the highest energy among all the subshells in any shell.
To find this the equation is 2n2, while n being the shell number, so in this case 2*32 = 18
It depends on the particular atom in question. Any of those subshells can make up the outer shells of atoms. Examples: In Mg, the outer shell is the 2s subshell. In P, the outer shell is the 3p subshell. In Fe, the outer shell is the 3d subshell, etc.
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.
One orbital - 6s which can hold 2 electrons.
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.
It depends on which subshell you're speaking of.. remember the the Lewis Structures? Well the 1st subshell will have 2 electrons 2nd Subshell : 8 e- 3rd : 18 e- 4th : 32 e- Above that I've never had to do any structures with more than 4 subshells and even those are VERY rare and I'm doing Uni chem. Hope this helps a bit. peace
There isn't really some easy-to-understand explanation for why electrons behave like this, they just do.Electrons are fermions, and the definition of fermions includes the fact that no two of them in the same atom can have the same four quantum numbers. A "subshell" is defined by three quantum numbers, leaving only the fourth (spin) for them to be in different quantum states, and there are only two possible values for the spin quantum number, so there can only ever be two electrons in any given subshell.(Like a lot of things in science, it turns out that this is really lies-to-children; you can force electrons into the same quantum state if you overcome what's called electron degeneracy pressure, but it takes a LOT of force to do this, so unless you're actually inside a neutron star, assume that the electrons around you are following the Pauli exclusion principle.)
The 2p sub-level can hold a maximum of 6 electrons. The 2p sub-level is divided into 2px, 2py and 2pz. Each of those orbitals can hold a maximum of 2 electrons. There are 3 of them and thus 6 total for the 2p sub-level.
The number of electrons in the lowest electron shellis2 in the first or K shell (subshell 1s)---For other shells, the maximum is determined by the formula 2n2:2) 8 in the L shell (subshells 2s, 2p)3) 18 in the M shell (subshells 3s, 3p, 3d)4) 32 in the N shell (subshells 4s, 4p, 4d, 4f)5) 50 in the O shell (subshells 5s, 5p, 5d, 5f, 5g*)6) 72 in the P shell (subshells 6s, 6p, 6d, 6f, 6g, and an unnamed subshell)7) 98 in the Q shell (subshells 7s, 7p, 7d, 7f, 7g, and two unnamed subshells)* the highest existing subshells are 5f, 6d, and 7s* the highest currently predicted subshells are 7p and 8s* no existing element has more than 32 electrons in any shellThe maximum per subshell is determined by the formula 2(2L+1) (s is 0):s subshells can have 2 electronsp subshells can have 6 electronsd subshells can have 10 electronsf subshells can have 14 electronsg subshells can have 18 electrons*There are no elements with electrons past the f subshell, so the shells with 22 and 26 electrons have no name. The largest element created (Roentgenium, element 111) has 2 electrons in the 7s shell.
In the first column on the left of the table, the elements only have 1 valence electron. The next row over has 2, then 3 , etc. When you change rows, you start over from one. In the middle, after the 20th element, Calcium, there are a few elements that don't gain any more valence electrons as you move to the right. These have a subshell of electrons instead.