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Q: The maximum number of electrons that can occupy the s orbital at each level is?

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Each orbital can accommodate two electrons. There is one s orbital per principal quantum number, so for any Ns orbital level there are a maximum of two electrons.

An orbital can only occupy maximum of 2 electrons. As p orbital consist of 3 orbitals. And has 3 orientations. Px, Py, Pz. So as there are 3 orbitals so p orbital can occupy at the maximum 6 electrons regardless of principle quantum no.. In 4p 4 is principle quantum no. So it represent 4p represent the p orbital of 4th shell. So it also occupy at the maximum of 6 electrons.

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2 electrons is the maximum number for an single orbital.

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The maximum number of electrons that can occupy one orbital is 2: One with "Up" spin and one with "Down" spin.

2 electrons is the maximum number for an single orbital.

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of course they can. They have to be of opposite spin and two is the maximum number that can occupy one orbital.

Any s orbital can only hold 2 electrons maximum.

Each orbital can accommodate two electrons. There is one s orbital per principal quantum number, so for any Ns orbital level there are a maximum of two electrons.

An orbital can only occupy maximum of 2 electrons. As p orbital consist of 3 orbitals. And has 3 orientations. Px, Py, Pz. So as there are 3 orbitals so p orbital can occupy at the maximum 6 electrons regardless of principle quantum no.. In 4p 4 is principle quantum no. So it represent 4p represent the p orbital of 4th shell. So it also occupy at the maximum of 6 electrons.

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