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Which of the following states that no more than two electrons can occupy an atomic orbital and that two electrons in the same orbital must have opposite spins?
a. Hund's rule
b. Dalton's theory
c. the Aufbau principle
d. the Pauli exclusion principle

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The correct answer is D. The statement that no more than two electrons can occupy an atomic orbital and that two electrons in the same orbital must have opposite spins is from the Pauli Exclusion Principle. If one is in the +1/2 up-spin the other should be in the -1/2 down-spin. From this principle, no two electrons can have the same quantum numbers. 

Answer:

a) Hund's rule

Explanation:

The given statement is in accordance with the Hund's Rule  of maximum multiplicity.

It states that if more than one orbital of the same energy are available, then the each of these orbitals will be first singly filled with electrons before becoming doubly occupied. In addition, the electrons filling the subshells will each have parallel spins (i.e. S = +1/2) to begin with. Once all the degenerate orbitals are singly filled, the subsequent electrons will be oriented with antiparallel spins (i.e. S = -1/2). Multiplicity is expressed as 2S+1 where S is the total spin angular momentum. Therefore, the Hund's rule ensures that there are maximum unpaired electrons which results in maximum multiplicity.

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