Which of the following orbital designations is (are) not correct? a. 1 p b. 3 d c. 3 f d. 2 p e.

step 1 looking at quantum numbers. So the number one indicates the principal energy level n equals one.

Which of the following orbital designations is (are) not...

Key Concepts

Principal Quantum Number

The principal quantum number (n) indicates the energy level or shell of an electron in an atom. It must be a positive integer and sets the scale of the orbital size. The value of n determines the overall energy of the electron and, together with the angular momentum quantum number, defines the orbital's possible shapes and positions. In orbital notation, the number preceding the letter corresponds to n.

Angular Momentum Quantum Number

The angular momentum quantum number (l) defines the shape of an orbital and has permissible integer values ranging from 0 to n-1 for a given principal quantum number n. Each value of l is associated with a specific orbital type: 0 is s, 1 is p, 2 is d, 3 is f, and so on. This quantum number determines the number of angular nodes within the orbital.

Orbital Designation Conventions

Orbital designations combine the principal quantum number (n) with a letter that corresponds to the angular momentum quantum number (l). According to the rules, the orbital designation is valid only if the principal quantum number is greater than the angular momentum quantum number (n > l). For instance, a p orbital (l=1) is not possible when n=1, because n must be at least 2, and similarly a f orbital (l=3) requires n to be at least 4.

Allowed Combinations of Quantum Numbers

In electron configurations, the combination of quantum numbers must follow the rule that the principal quantum number n is always greater than the angular momentum quantum number l (n > l). This rule is critical for validating orbital designations. Hence, orbital labels such as '1p' (where n=1, l=1) and '3f' (where n=3, l=3) are not allowed, while labels that satisfy this condition, such as '3d', '2p', '5f', and '6s', are valid.

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