Question #08502

1 Answer
Apr 16, 2015

Answer:

Here's what I get.

Explanation:

Question 1

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Both electrons in the #"3s"# orbital have the same spin.

This violates the Pauli Exclusion Principle: No two electrons in the same orbital can have the same spin.

Question 2

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You have no electrons in the #"2s"# orbital, which is between the #"1s"# and #"2p"# levels.

This violates the Aufbau Principle: When adding electrons to an atom, you put them in the lowest-energy orbitals available.

Question 3

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You have two electrons in one #"2p"# orbital, but none in the other #"2p"# orbitals.

This violates Hund's Rule: There must be one electron with the same spin in each orbital of the same energy before you can put two in the same orbital.

Question 4

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The electrons in the half-filled #"4d"# orbitals don't all have the same spin.

This violates Hund's Rule: There must be one electron with the same spin in each orbital of the same energy before you can put two in the same orbital.

Question 5

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You filled the #"4d"# orbitals before you filled the #"4p"# orbitals, which are lower in energy.

This violates the Aufbau Principle.

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