Quantum Numbers and Orbitals: Flashcards

Quantum Numbers and Orbitals: Flashcards

1. Question

   Name the four quantum numbers and their symbols.

   Answer

   Principal $n$, angular momentum $l$, magnetic $m_l$, spin $m_s$.

2. Question

   What values can $l$ take for a given $n$?

   Answer

   0, 1, 2, ..., $n - 1$

3. Question

   What letters stand for $l$ = 0, 1, 2 and 3?

   Answer

   s, p, d, f

4. Question

   What values can $m_l$ take?

   Answer

   Whole numbers from $-l$ to $+l$: $2l + 1$ values.

5. Question

   How many orbitals are in an s, p, d and f subshell?

   Answer

   1, 3, 5 and 7

6. Question

   How many orbitals and electrons fit in shell $n$?

   Answer

   $n^2$ orbitals and $2n^2$ electrons (e.g. n = 3: 9 orbitals, 18 electrons).

7. Question

   State the Pauli exclusion principle.

   Answer

   No two electrons in an atom can have the same four quantum numbers, so an orbital holds at most two electrons, with opposite spins.

8. Question

   Describe the shapes of s and p orbitals.

   Answer

   s: spherical. p: two lobes (dumbbell) along the x, y or z axis.

9. Question

   Is the set $(2, 2, 0, +\tfrac{1}{2})$ allowed?

   Answer

   No: $l$ cannot equal $n$ (maximum $l$ for $n = 2$ is 1).

10. Question

    How many radial and angular nodes does a 3p orbital have?

    Answer

    Angular: $l = 1$. Radial: $n - l - 1 = 1$. Total: $n - 1 = 2$.

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