Question

note taking guide: episode 304
name
quantum numbers
used to describe an electron in an atom
n
represents ____ energy level of ____
____ # of ____ in an
example: what is the maximum number of electrons that can be in the
______ main energy level?
l
the ______
describes the ____ within an ____
____ of orbital __ possible in ____
______=
orbital shapes
designated ______
level 1: ______
level 2: ______
level 3: ______
level 4: ______
how many electrons can each sublevel hold?
s = 1 orbital x 2 e/orbital = ______e-
p = 3 orbitals x 2 e/orbital = ______e-
d = 5 orbitals x 2 e/orbital = ______e-
f = 7 orbitals x 2 e/orbital = ______e-

Explanation:

Step1: Recall quantum - number concepts

Quantum numbers describe electrons in an atom. The principal quantum number $n$ represents the main energy level of an electron. The number of electrons in a main energy level is $2n^{2}$.

Step2: Analyze angular - momentum quantum number

The angular - momentum quantum number $l$ describes the shape of the orbital within a shell. The number of orbitals for a given $l$ is $2l + 1$.

Step3: Calculate electrons per sublevel

For $s$ sublevel ($l = 0$), $1$ orbital $\times2$ electrons/orbital $= 2$ electrons. For $p$ sublevel ($l = 1$), $3$ orbitals $\times2$ electrons/orbital $= 6$ electrons. For $d$ sublevel ($l = 2$), $5$ orbitals $\times2$ electrons/orbital $= 10$ electrons. For $f$ sublevel ($l = 3$), $7$ orbitals $\times2$ electrons/orbital $= 14$ electrons.

Answer:

$n$: main, electron; $2n^{2}$; $l$: angular - momentum, shape, shell; $2l + 1$; $s$: 2, $p$: 6, $d$: 10, $f$: 14