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2 electrons is the maximum number for an single orbital.

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Q: What is the maximum of electrons that can occupy one 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.

2 electrons is the maximum number for an single orbital.

The maximum number of electrons that can occupy the 5s orbital is 2. This is based on the Pauli exclusion principle, which states that each orbital can hold a maximum of two electrons with opposite spins.

The maximum number of electrons that can occupy the 2s orbital is 2. This is because the s orbital can hold a maximum of 2 electrons, following the Pauli exclusion principle which states that no two electrons in an atom can have the same set of quantum numbers.

Any orbital can hold a maximum of 2 electrons

Each orbital can hold a maximum of 2 electrons.

There can only be 2 electrons in each single orbital, and they will be on opposite sides of the electron cloud (orbital).

only if spins are opposite: one up one down.

The orbital notation for an orbital containing two electrons can be represented as follows: ↑↓. The arrows represent the two electrons with opposite spins in the same orbital.

In any orbital the maximum number of electrons is 2 of opposite spin. The following is a list of the different types of orbitals and the maximum nuber of electrons each type can contain. s-orbitals: one orbital, containing 2 electrons p-orbitals: three (px, py, pz) containing 6 in total d-orbitals: five, containing 10 f-orbitals: seven containing 14

2 ELECTRONS in one orbital. (An electron can only be in one orbital at once)

ten. because a d subshell corresponds to an l value of 2, m_l can be -2,-1,0,1,2. so that's 5 orbitals, and 2 electrons can fit into each one (one with a +1/2 spin and one with a -1/2 spin) so that's 10 electrons total.