S can hold no more than 2
P can hold up to 6
D can hold up to 10
F can hold up to 14
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.
There are four kinds of orbitals: s, p, d, and f. Each s orbital hold 2 electrons (1 pair). Each p orbital holds 6 (3 pairs), d orbitals hold 10 (5 pairs) and f orbitals hold 14 (7 pairs). The first orbit only has an s orbital. So it holds 2 electrons. The second and third orbits each have an s and a p orbital. So they each hold 8 electrons. The fourth and fifth orbits each have an s, a p, and a d orbital. So they each hold 18 electrons. The sixth and seventh orbits each have an s, a p, a d, and an f orbital. They each hold 32 electrons. To place the electrons in their orbitals: Start at Hydrogen and follow through the periodic table, adding one electron per element until you reach the one you're wondering about. You can also start at the previous noble gas and go towards the element in question. Add electrons to an s orbital if you are in group I or II (or He). Add electrons to a p orbital if you in group IIIA - Noble gases. Remember that the first p orbital is 2p. Add electrons to a d orbital if you are in the transition metals. Remember that the first d orbital is 3d. Add electrons to an f orbital if you are in the rare earth metals (the ones that are usually an insert at the bottom of the page). Remember that the first f orbital is 4f. Also, place all the electrons in the orbital unpaired, then pair them up after all the spots are full. Then progress on to the next type of orbital.
Yes, a stable atom can have an orbital with three electrons. An atomic orbital can hold a maximum of two electrons with opposite spins, following the Pauli exclusion principle. The third electron would go into a different orbital within the same energy level.
Two (2) electrons (s shell)Eight (8) electrons (2 in s, 6 in p)Eighteen (18) electrons (2 in s, 6 in p, 10 in d)The periodic table PDF at Los Alamos National Laboratory is pretty good and has the shell configurations. See related link.
The extra electron would go into a 4s orbital because 4s can hold up to 2 electrons before 3d can be filled.
Each orbital can hold a maximum of 2 electrons.
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.
There are four kinds of orbitals: s, p, d, and f. Each s orbital hold 2 electrons (1 pair). Each p orbital holds 6 (3 pairs), d orbitals hold 10 (5 pairs) and f orbitals hold 14 (7 pairs). The first orbit only has an s orbital. So it holds 2 electrons. The second and third orbits each have an s and a p orbital. So they each hold 8 electrons. The fourth and fifth orbits each have an s, a p, and a d orbital. So they each hold 18 electrons. The sixth and seventh orbits each have an s, a p, a d, and an f orbital. They each hold 32 electrons. To place the electrons in their orbitals: Start at Hydrogen and follow through the periodic table, adding one electron per element until you reach the one you're wondering about. You can also start at the previous noble gas and go towards the element in question. Add electrons to an s orbital if you are in group I or II (or He). Add electrons to a p orbital if you in group IIIA - Noble gases. Remember that the first p orbital is 2p. Add electrons to a d orbital if you are in the transition metals. Remember that the first d orbital is 3d. Add electrons to an f orbital if you are in the rare earth metals (the ones that are usually an insert at the bottom of the page). Remember that the first f orbital is 4f. Also, place all the electrons in the orbital unpaired, then pair them up after all the spots are full. Then progress on to the next type of orbital.
Yes, a stable atom can have an orbital with three electrons. An atomic orbital can hold a maximum of two electrons with opposite spins, following the Pauli exclusion principle. The third electron would go into a different orbital within the same energy level.
Yes. When electrons go from a higher energy orbital to a lower one, they release photons (ie: light).
Carbon is the sixth element with a total of 6 electrons. In writing the electron configuration for carbon the first two electrons will go in the 1s orbital. Since 1s can only hold two electrons the next 2 electrons for C goes in the 2s orbital. The remaining two electrons will go in the 2p orbital. Therefore the C electron configuration will be 1s2 2s2 2p2.
The maximum number of electrons that can occupy a 4d orbital is 10. This is because each orbital can hold a maximum of 2 electrons, and there are 5 4d orbitals available. Therefore, 2 electrons can occupy each of the 5 orbitals, giving a total of 10 electrons in the 4d orbital.
It has a lower energy level. All else being equal, electrons tend to go into the lowest energy orbital with space available.
Two (2) electrons (s shell)Eight (8) electrons (2 in s, 6 in p)Eighteen (18) electrons (2 in s, 6 in p, 10 in d)The periodic table PDF at Los Alamos National Laboratory is pretty good and has the shell configurations. See related link.
In chemistry, sub orbitals are the paths that electrons follow in the shells. They go in this order: s (x1) p(x6) d (x10) and f (x14) (It is very important that they are in lower case) There is only 1 's' orbital in each shell. Shell 1: 's': 2 electrons Shell 2: 's' and 'p': 8 electrons. etc Remember that electrons fill up the smaller sub orbitals first, so if electrons have to choose between 'f' and 's' they will always choose 's' . Hope that helps!
The extra electron would go into a 4s orbital because 4s can hold up to 2 electrons before 3d can be filled.
Electrons do not travel in pairs. An atomic or molecular orbital can hold a pair of electrons, which is probably what you're thinking of. The reason for this is that electrons are fermions: two electrons in an atom or molecule cannot have the exact same quantum state. Specifying the orbital uses up 3 of the 4 quantum numbers for describing an electron's quantum state; the last quantum number is the spin angular momentum which can either be +1/2 or -1/2, so two electrons per orbital. After that it's full and no more electrons can go into that orbital. Note that far from "traveling in pairs", fermions really don't like to be even that close to each other. If there are three orbitals at the same energy level, one electron will go into each before they start to "double up".