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How can you tell the doffermce between 2s subshell and 2p subshell?
You can tell the difference between a 2s sub-shell and 2p sub-shell from their energy levels, because a 2p sub-shell is a higher energy level than a 2s sub-shell.
What is the n value for sub level 6g?
The n value for the 6g sublevel is 6. The principal quantum number (n) represents the energy level or shell in the electron configuration. In this case, the electron is in the 6th energy level.
How many electrons can be held in the first 4 energy levels?
== Answer== Generally, each sub-shell has its own energy. The sub-shells, listed in order of energy with the number of orbitals in that sub-shell, with the number of electrons each one occupies, are:1s: 1 orbital, 2 electrons2s: 1 orbital, 2 electrons2p: 3 orbitals, 6 electrons3s: 1 orbital, 2 electrons3p: 3 orbitals, 6 electrons4s: 1 orbital, 2 electrons3d: 5 orbitals, 10 electrons4p: 3 orbitals, 6 electronsetc.So, in the first four separate energy levels or sub-shell (1s, 2s, 2p, and 3s) there are 2 + 2+ 6 + 2 = 12 electrons. Note that in these first four sub-shells there are 6 orbitals (with 2 electrons each).
How many sub-shell are there in second shell?
The second shell of an atom has two sub-shells: the 2s and 2p sub-shells. The 2s sub-shell can hold a maximum of 2 electrons, while the 2p sub-shell can hold a maximum of 6 electrons, allowing the second shell to accommodate a total of 8 electrons.
Are the highest energy levels in shells always filled first?
No, the highest energy levels in shells are not always filled first. Electrons fill atomic orbitals starting from the lowest energy level and move to higher energy levels according to the Aufbau principle. This means that within a shell, sub-levels with lower energy (e.g., s before p, p before d) are filled before those with higher energy. Therefore, the filling order is determined by energy levels and sub-levels rather than simply by shell numbers.
How can you tell the doffermce between 2s subshell and 2p subshell?
You can tell the difference between a 2s sub-shell and 2p sub-shell from their energy levels, because a 2p sub-shell is a higher energy level than a 2s sub-shell.
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.
What happens when a 3s electron becomes a 2s electron?
Any electron is not fixed to any sub-shell or orbital. If you provide sufficient energy to an electron, it would make transition to any of the higher energy orbitals and then come back to the lower orbitals radiating energy.
What is the sub energy level of boron?
The atomic no of Boron is 5 , so two electrons in ist shell the last three electrons are divided in two sub energy levels two in lower level 's' and one in higher level 'p'
What is the n value for sub level 6g?
The n value for the 6g sublevel is 6. The principal quantum number (n) represents the energy level or shell in the electron configuration. In this case, the electron is in the 6th energy level.
What is energy levels sub-levels?
Sub energy pretty much explains itself: It is below energy level
Which quantum number is also called sub-shell quantum number?
The azimuthal quantum number (l) is also known as the sub-shell quantum number. It represents the sub-shell of an electron within a given energy level. The value of l determines the shape of the orbital (s, p, d, f).
What number on the periodic table indicates the energy level of an atoms valence electrons?
The number beside the letter represents the energy level. The letter represents the sub level. The exponent represents the number of electrons in the sub level. So in the case of: 1s^2 1 is the energy level; S is the sub level; ^2 is the number of electrons in the sub level.
How many electrons can be held in the first 4 energy levels?
== Answer== Generally, each sub-shell has its own energy. The sub-shells, listed in order of energy with the number of orbitals in that sub-shell, with the number of electrons each one occupies, are:1s: 1 orbital, 2 electrons2s: 1 orbital, 2 electrons2p: 3 orbitals, 6 electrons3s: 1 orbital, 2 electrons3p: 3 orbitals, 6 electrons4s: 1 orbital, 2 electrons3d: 5 orbitals, 10 electrons4p: 3 orbitals, 6 electronsetc.So, in the first four separate energy levels or sub-shell (1s, 2s, 2p, and 3s) there are 2 + 2+ 6 + 2 = 12 electrons. Note that in these first four sub-shells there are 6 orbitals (with 2 electrons each).
How many sub-shell are there in second shell?
The second shell of an atom has two sub-shells: the 2s and 2p sub-shells. The 2s sub-shell can hold a maximum of 2 electrons, while the 2p sub-shell can hold a maximum of 6 electrons, allowing the second shell to accommodate a total of 8 electrons.
How many different sub levels are second energy level?
2
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.
