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djinnidew

The number of orbitals that are completely full is 5.

The reason you may have thought it was 3 is because you're confusing orbitals with subshells.

In this electron configuration, the sub shells are:  1s^2, 2s^2, 2p^6, 3s^1

So, we have four sub shells.

Each sub shell consists of a specific number of orbitals. s subshells have one orbital, p subshells have three orbitals, d subshells have five orbitals, and f subshells have seven orbitals. Knowing this, we can look back at the electron configuration we were given and determine how many orbitals are filled.

1s^2 has one orbital, 2s^2 has one orbital, 2p^6 has three orbitals, and 3s^1 has one orbital. The first three subshells are completely full, so a total of five orbitals are full.

Eduard22sly

The number of orbitals that are completely filled in an atom whose electronic configuration is 1s²2s²2p⁶3s¹ is 5

Electronic configuration can simply be defined as the arrangement of electrons around the nucleus of an atom.

The electrons in an atom are arranged in orbital. These orbitals includes: s-orbital, p-orbital, d-orbital and f-orbital

S-orbital has 1 subshell = maximum of 2 electrons

P-orbital has 3 subshells = maximum of 6 electons

D-orbital has 5 subshells = maximum of 10 electrons

F-orbital has 7 subshells = maximum of 14 electrons

With the above information in mind, we can determine the number of orbitals that are completely filled in the atom given in the question above. This can be obtained as follow:

Electronic configuration => 1s²2s²2p⁶3s¹

1st shell => 1s² = 1 subshell = 2 electrons (complete)

2nd shell => 2s²2p⁶ => 4 subshells = 2 + 6 = 8 electrons (complete)

3rd shell => 3s¹ => 1 subshellsubshells => 1 electron (incomplete)

From the above illustration, we can see clearly that only 5 orbitals are completely filled.

Thus, we can conclude that the number of orbitals that are completely filled in an atom whose electronic configuration is 1s²2s²2p⁶3s¹ is 5

Learn more: https://brainly.com/question/10291893

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