0
Orbitals having the same first two quantum numbers are degenerate ... they have the same energy ... in the absence of a magnetic field.
So all 1s orbitals in a given atom have the same energy, all 3d orbitals in a given atom have the same energy, etc.
In a magnetic field, the spin degeneracy is removed, so that "spin up" and "spin down" electrons have different energies, even if they're in the same orbital.
Wiki User
∙ 12y ago
Add your answer:
Earn +20 pts
How many orbitals are in the following sublevel 4s sublevel?
All p sublevels contain three orbitals, including the 4p sublevel.
Why transition metals are colored?
The 5 orbitals within the 3d subshell have different energies and electrons within the 3d subshell can move up and down these orbitals. The energy transitions within the orbitals of the 3d subshell correspond to the energy of visible light.
What is the maximum number of spdf in chemistry?
The number of orbitals in electron shells are: One s orbital three p orbitals 5 d orbitals 7 f orbitals every shell has an s orbital, only shells 2 and above have p orbitals, only shells 3 and above have d orbitals only shells 4 and above have f orbitals. Each orbital can hold a maximum of 2 electrons. Level by level the orbitals 1s (one) 2s, 2p(three) 3s, 3p, 3d (five) 4s, 4p, 4d 4f(seven) In a shell where they are possible, all three p orbitals have the same energy, all 5 d orbitals have the same energy and all seven f orbitals have the same energy. I do not like the idea of saying there is a maximum-- an orbital is a solution to the energy levels in a hydrogen atom. You simply cannot have less than 3 p orbitals for instance.
What is a degenerate d-orbital?
"Degenerate" in this sense means "indistinguishable" or more specifically "having the same energy." Properly speaking, the word shouldn't be used for a single orbital; it refers to the relationship between two or more orbitals. For example, in an isolated atom, the three p orbitals in a given shell are said to be degenerate, since they all have the same energy level.
According to Hunds' rule when electrons occupy orbitals of equal energy one electron enters each orbit until?
All the orbitals contain one electron, with the same spins.
Does an electron have the same amount of enery in all orbitals?
All of the orbitals in the same energy sublevel (s, p, d, f) have the same amount of energy. For example, each of the 3p orbitals have the same energy and all of the electrons in the 3p orbitals have the same energy.
What subshell have the higher energy 4s4p4dor 4f?
4f subshell has the highest energy. A f subshell has the highest energy among all the subshells in any shell.
If Assuming all orbitals are the same in energy level which type of orbital has the lowest energy?
The s orbital has the lowest energy level.
How many orbitals are in the following sublevel 4s sublevel?
All p sublevels contain three orbitals, including the 4p sublevel.
Why 2 electrons are present in s orbital?
It is not the orbital that holds more electrons. All orbitals can hold a maximum of 2 electrons.However, the p-subshell can hold more electrons than the s-subshell. This is because the s-subshell is only made of 1 orbital, and 1 x 2 = 2, therefore it can only hold 2 electrons. The p-subshell is made of 3 orbitals, and 3 x 2 = 6, so it can hold a maximum of 6 electrons.So, a p-subshell can hold more electrons than an s-subshell because it is made up of more orbitals. It is not the orbitals that hold more electrons.
Why transition metals are colored?
The 5 orbitals within the 3d subshell have different energies and electrons within the 3d subshell can move up and down these orbitals. The energy transitions within the orbitals of the 3d subshell correspond to the energy of visible light.
What is the maximum number of spdf in chemistry?
The number of orbitals in electron shells are: One s orbital three p orbitals 5 d orbitals 7 f orbitals every shell has an s orbital, only shells 2 and above have p orbitals, only shells 3 and above have d orbitals only shells 4 and above have f orbitals. Each orbital can hold a maximum of 2 electrons. Level by level the orbitals 1s (one) 2s, 2p(three) 3s, 3p, 3d (five) 4s, 4p, 4d 4f(seven) In a shell where they are possible, all three p orbitals have the same energy, all 5 d orbitals have the same energy and all seven f orbitals have the same energy. I do not like the idea of saying there is a maximum-- an orbital is a solution to the energy levels in a hydrogen atom. You simply cannot have less than 3 p orbitals for instance.
What is a degenerate d-orbital?
"Degenerate" in this sense means "indistinguishable" or more specifically "having the same energy." Properly speaking, the word shouldn't be used for a single orbital; it refers to the relationship between two or more orbitals. For example, in an isolated atom, the three p orbitals in a given shell are said to be degenerate, since they all have the same energy level.
According to Hunds' rule when electrons occupy orbitals of equal energy one electron enters each orbit until?
All the orbitals contain one electron, with the same spins.
What is energy of electron when it is closest to the nucleus?
The energy level closest to the nucleus is the 1s orbital and can hold 2 electrons as do all s orbitals. Every electron orbital has a distinct shape and number. The 1s orbital has the same shape the 2s orbital and the 3s orbital and so forth. There are other orbital shapes such as p, d, and f. Regardless of the number or level of the orbital, all p orbitals are the same shape and all d orbitals are the same shape. Orbitals differ in distance from the nucleus and the distance is indicated by the number before the orbital shape.
How do you calculate LFSE value?
The difference between (1) the total energy of a coordination complex with the electron configuration resulting from ligand field splitting of the orbitals and (2) the total energy for the same complex with all the d orbitals equally populated is called the ligand field stabilization energy, or LFSE.
What are the different principles that govern the building of an electron configuration?
Pauli's Exclusion Pricipal.A single orbital can only hold 2 electrons.Hund's Rule.The most stable arrangement of electrons is that with the maximum number of unpaired electrons,all with the same spin direction.Aufbau Principle.Electrons fill the lowest energy subshell first before moving to the next subshell.
