For the table below, write which orbital goes with the quantum numbers. Don't worry about x, y,

For the table below, write which orbital goes with the...

Key Concepts

Magnetic Quantum Number (m)

The magnetic quantum number, denoted as m (often represented as m?), specifies the orientation of an orbital in space relative to an external magnetic field. Its values range from -l to +l, including zero, and provide further detail about the electron's orbital position.

Angular Momentum Quantum Number (l)

The angular momentum quantum number, denoted as l, determines the shape of the orbital. Its possible values range from 0 to n-1, where each value corresponds to a specific orbital type (e.g., 0 for s orbitals, 1 for p orbitals, 2 for d orbitals, etc.).

Allowed Quantum Number Combinations

Allowed combinations of quantum numbers are governed by selection rules and restrictions, such as the range of l being from 0 to n-1 and m being between -l and +l. These rules ensure that each electron in an atom occupies a unique quantum state, and any combination falling outside these restrictions is not allowed.

Quantum Numbers

Quantum numbers are a set of numerical values that describe the properties and behaviors of electrons in atoms. They include values that determine an electron's energy level, orbital shape, orbital orientation, and spin, and they help define the unique quantum state of an electron in an atom.

Principal Quantum Number (n)

The principal quantum number, denoted as n, indicates the main energy level or shell in which the electron is found. It is a positive integer and primarily determines the size and energy of the orbital.

Transcript

00:01 In this problem, we're given some quantum numbers and we're asked to specify the orbital if the orbital is even possible.

00:09 So we're given the numbers, we're given the values for the first three columns, and then we're asked to specify the orbital.

00:16 We are told that we don't have to worry about whether it's an xyz and a p, just the general orbital.

00:23 For our first scenario, we're given principal quantum number of one and l is two, or excuse me, l is one.

00:31 And this is a minus one.

00:34 So this is an example, and that's a 2p.

00:38 Because this tells us we're in 2, this tells us we're in p, and we can have a negative 1 because there are three orbitals in the sub -level.

00:52 Next, we are given 1 in 0, and 0.

01:00 And this, of course, is the 1 -s sub -level.

01:08 Okay, next, we are given.

01:11 Let's start with here.

01:13 A 3 and a negative 3, which we can't have.

01:19 I can already see it's not allowed.

01:21 And a 2.

01:23 You can't have a negative l.

01:35 And even if it was positive, it would be in a different in a sub -shell that doesn't exist there.

01:42 For the next one, we have another 3.

01:44 And now i have a 2, which means it's a d sub -level, and a negative 2, which can exist...

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