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What types of atomic orbitals are in the second principal energy level?
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∙ 11y ago
An s orbital
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∙ 12y ago
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∙ 14y agoThe s suborbital. Can contain only 2 electrons.
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∙ 11y agos and p orbitals. There is one s orbital (2s) and three p orbitals (2px, 2py, 2pz). Each orbital can hold two electrons of opposite spin, making 8 in all.
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∙ 11y agos, p, d, f orbitals. there is one s orbital, three p orbitals, five d orbitals, seven f orbitals.
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∙ 8y agoAnswer this queWhat is the only kind of orbital in the first energy level? stion…
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∙ 11y agothe s orbital
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∙ 10y ago1
Anonymous
s orbital
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What is the total number of electrons needed to completely fill all of the orbitals in an atoms second principal energy level?
8 electrons
How are orbitals and energy levels related?
The principal quantum number, n, designates the main energy levels occupied by electrons. The number of orbitals in an energy level is n2 (n squared), so that the first energy level, n = 1, contains 1 orbital; the second energy level, n = 2, contains 4 orbitals; the third energy level, n= 3, has 9 orbitals; and the fourth energy level, n=4, has 16 orbitals, and so on.
How many energy sublevels are there in the second principal level?
There are 2 energy sublevels in the second principal.
How many electrons can be placed in the second energy level?
8 electrons. The second energy level (n=2) has 4 orbitals. One s orbital and three p orbitals. Each orbital can hold 2 electrons of opposite spin.
What energy level can the s orbital be found in?
Each main energy level (1 to 7) has at least an s-orbital, p-orbitals are possible from the second level onwards (2 to 7) d-orbitals from 4th level f-orbitals from 6th level
What is the maximum number of dorbitals in a principal energy level?
1s orbital 3P, 5d, and 7f in discovered elements
What is the total number of electrons needed to completely fill all of the orbitals in an atoms second principal energy level?
8 electrons
How are orbitals and energy levels related?
The principal quantum number, n, designates the main energy levels occupied by electrons. The number of orbitals in an energy level is n2 (n squared), so that the first energy level, n = 1, contains 1 orbital; the second energy level, n = 2, contains 4 orbitals; the third energy level, n= 3, has 9 orbitals; and the fourth energy level, n=4, has 16 orbitals, and so on.
How many energy sublevels are there in the second principal level?
There are 2 energy sublevels in the second principal.
How many s orbitals are possible in the second principal level of an atom?
S sub-shell has only one orbital. So, the 2nd energy level has only one s orbital.
The total number of orbitals that can exist at the second main energy level is?
2 s and p orbital. 8 orbitals total
What is the total number of electrons in the second principal energy level of a calcium atom in the ground state?
The electron configuration of calcium is: 1s2 2s2 2p6 3s2 3p6 4s2 The "second principle energy level" refers in this case to the 2s and 2p orbitals, so it would be a total of 8 electrons.
How many electrons can be placed in the second energy level?
8 electrons. The second energy level (n=2) has 4 orbitals. One s orbital and three p orbitals. Each orbital can hold 2 electrons of opposite spin.
Which is the lowest energy that can have a s orbital?
Each main energy level (1 to 7) has at least an s-orbital, p-orbitals are possible from the second level onwards (2 to 7) d-orbitals from 4th level f-orbitals from 6th level
Why is second electron affinity for halogens is zero?
All of the halogens are one electron short of having all of their atomic orbitals filled to reach an atom's state of nirvana. This explains why, in general, halide chemistry is such that halogens so willingly literally accept one electron in their ionic formulations and formally accept one electron or share a pair of electrons in the vast majority of their predominately covalent compounds. Halogens have no affinity for accepting a second electron because once a halogen atom has accepted once electron, all of its atomic orbitals each contain two electrons and are thus full. Any element with all its atomic orbitals filled has the equivalent electronic configuration of a noble gas and is in its most stable electronic state.What follows is very important to understand. It appears that many chemistry students do not know this fact probably because most textbooks and instructors do not explicitly point it out or they do a poor job emphasizing it: Elements only possess the atomic orbitals defined by the row in which an element exists in the Periodic Table.In many compounds, a particular element may possess one or more empty atomic orbitals in its electronic ground state. Students who have completed the first semester of general chemistry were presented with, and expected to understand, what atomic orbitals each element has. They should also know the order in which a given element's orbitals are progressively occupied by electrons when that element is in its ground electronic state and that orbitals with the lowest energy are filled first. It is also important to understand that the theoretical order of atomic orbitals in elements heavier than argon may be in a different order. This effect, when it occurs, is due to electron-electron repulsions about the element's nucleus.Let's look at a 2nd row element as an example. How about nitrogen? Because it's a 2nd row element, nitrogen has two "shells" of atomic orbitals and a total of five orbitals; however only electrons in the outer shell of orbitals may participate in chemical bonding. The 1st shell of electrons consists only of the 1s orbital. Like all atomic orbitals, the 1s orbital can hold a maximum of two electrons, which is denoted by the superscript in the orbital's designation, as in 1s2. Starting from the 1st element in the 2nd row and counting each element up to and including nitrogen shows that the outer shell of orbitals on nitrogen contains five electrons. Assuming that no electron-electron interactions alter the respective theoretical energy levels of the five orbitals (This does not occur in any of the 2nd row elements), the atomic orbitals on nitrogen are, in increasing energy: [1s2], 2s2, 2px1, 2py1, 2pz1. The three 2p orbitals have the same energy and are filled with one electron first before any of them takes on a second electron. Note that the first p orbitals, and the ones lowest in energy, are the 2p orbitals. There is simply no such thing as a 1p orbital. The 2p orbitals could have been named 1p orbitals. Everyone who first applied quantum mechanics to the hydrogen atom in order to describe its atomic emission spectrum, and, not long thereafter, the number and energy levels of an atom's electrons, are no longer with us. Nevertheless, the reason for the seemingly strange numerical designations is almost certainly because the quantum numbers that are solutions to the wave equation corresponding to the number and shape of the atomic orbitals begin with "2" for the p orbitals, "3" for the d orbitals, etc., and perhaps the people who discovered and published all of these findings decided not to change the numerical designations.The point I hope I made is that the five atomic orbitals shown for nitrogen are all it has. In addition to s and p atomic orbitals, there exists d and f orbitals, but not for nitrogen or any other second-row element. Therefore, once the 2s and 2p orbitals are filled, nitrogen cannot accept or share another additional electron because there is no atomic orbital in which it can be placed.
How many orbitals are in second energy level?
There are two sublevels in the second principle energy level. The s sublevel has one orbital and the p sublevel has 3, for a total of 4 orbitals.
How many electrons does phosphorus have in its outermost principal energy level?
The total number of electrons in Phosphorus (P) is 15 (its atomic number). The first energy level contains 2, the second energy level contains 8, and the third energy level contains 5.
