To completely describe an electron in an atom, four quantum numbers are needed: energy (n), angular momentum (ℓ), magnetic moment (mℓ), and spin (ms).

Since you are dealing with a 3p-orbital, your principal and angular momentum quantum numbers will be n=3 and l=1 .

3s, n = 3 , 1 = 0, m = 0, s = +1⁄2 for first electron. n = 3 , 1 = 0 , m = 0 , s = -1⁄2 for second electron.

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Table of Allowed Quantum Numbers

Question: What Are The Four Quantum Numbers For Each Of The Two Electrons In A 4s Orbital? For The Second Electron: N=4, L=0, Ml=0, Ms=+1/2 N=3, L=1, Ml=0, Ms=-1/2 N=1, L=0, Ml=0, Ms=-1/2 N=4, L=3, Ml=3, Ms=+1/2.

Orbitals & Quantum Numbers:

After filling the 4d-orbital, an electron will enter in 5p orbital. As the value of (n+l) for 4d orbital is same as that of 5p orbital, 4d orbital is filled before 5p orbital as 4d orbital has lower value of n than 5 p orbital.

5p orbitals

When the 4d is filled the 5s is also filled. This leaves the 5p to be filled next.

Therefore, order of filling of orbitals is correct 4s, 3d, 5s, 4d. Hence, the correct answer is option B. Note: Aufbau principle is used in determining electronic configuration of atoms. This principle states that electrons should be filled in lower energy orbitals first and then filled in the higher energy orbitals.

The shape of the 4s orbital. That on the left is sliced in half to show the two spherical nodes of the 4s orbital. The shape on the right shows the nodal structure of the 4s-orbital. While still spherical, the higher s-orbitals (5s, 6s, and 7s) are more complex since they have more spherical nodes.

The 4s electrons are lost first followed by one of the 3d electrons. The electrons lost first will come from the highest energy level, furthest from the influence of the nucleus. So the 4s orbital must have a higher energy than the 3d orbitals.

The number of nodes is related to the principal quantum number, n. In general, the np orbital have (n – 2) radial nodes. Therefore, the 4p-orbital has (4 – 2) = 2 radial nodes, as shown in the above plot. Radial nodes become evident in the higher p-orbitals ( 5p, 6p, and 7p) while lower p-orbitals (2p, 3p) show fewer.

A node is a point where the probability of finding the electron is zero. They can be angular or radial. Whereas orbital is a region of space around nucleus of atom where probability of finding an electron is most likely.

3 radial nodes

1 radial node

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One radial node

two radial nodes

For a given orbital, there are two types of nodes i.e. 1) Angular nodes (also known as nodal planes) 2) Radial nodes (also known as nodal regions)….

Answer: Number of radial nodes = n – l – 1. So, 4p orbital has 2 radial nodes and 1 angular node. Number of radial nodes = n – l – 1 = 5 – 2 – 1 = 2 radial nodes.

The orbital with 4 total nodes.

Radial and Angular Nodes The total number of nodes present in this orbital is equal to n-1. In this case, 3-1=2, so there are 2 total nodes.

There arefour nodes total (5-1=4) and there aretwo angular nodes (d orbital has a quantum number ℓ=2) on the xz and zy planes.