Draw representations of ground state electron configurations using the orbital notation (↑↓) for

step 1 Hi there. This will be question number 96. And for 96, we need to write the orbital notations fo

Draw representations of ground state electron configurations...

Key Concepts

Electron Configuration

Electron configuration refers to the assignment of electrons within an atom's various orbitals, indicating the energy levels and subshells that the electrons occupy. It provides a systematic way to represent the distribution of electrons in accordance with principles like the Aufbau principle and the Pauli Exclusion Principle.

Orbital Notation

Orbital notation is a method of depicting electron configurations using boxes or lines to represent orbitals along with arrows to denote electrons and their spin direction. This visual representation clarifies how electrons fill available orbitals and adheres to fundamental rules like Hund's rule and the Pauli Exclusion Principle.

Aufbau Principle

The Aufbau principle states that electrons occupy the lowest energy orbitals first before moving to higher energy ones. This principle guides the sequential filling of electron orbitals in an atom and is essential for constructing ground state electron configurations.

Hund's Rule

Hund's rule explains that when electrons fill degenerate orbitals (orbitals with the same energy), they do so by entering each orbital singly with parallel spins before any orbital gets a second electron. This minimizes repulsions and stabilizes the atom's electron configuration.

Pauli Exclusion Principle

The Pauli Exclusion Principle asserts that no two electrons in an atom can have the same set of four quantum numbers. As a consequence, an orbital can accommodate a maximum of two electrons, and they must have opposite spins. This principle is fundamental to understanding the limitations in electron occupancy of orbitals.

Transcript

00:02 Hi there.

00:03 This will be question number 96.

00:07 And for 96, we need to write the orbital notations for the ground state electron configurations for each of the elements.

00:16 So let's go ahead and get started.

00:17 Our first one is for phosphorus.

00:20 So the first thing we need to do is look on the periodic table to determine the atomic number, which is 15.

00:26 We need that because that tells us the number of protons, but more importantly for this question, since that's the number of protons, that is also the number of electrons.

00:36 So we need to do the orbital notation for 15 electrons.

00:42 So let's go ahead and get started.

00:43 We're going to fill the electrons in order from lowest energy upward as alf bile predicted.

00:50 So we'll start with the 1s.

00:52 There's only one 1s orbital.

00:55 So i'm going to put my two electrons of opposite spin into that orbital.

01:00 I'm drawing half arrows just to speed this up a little bit.

01:02 It as we go through here.

01:05 All right.

01:05 Next is 2s.

01:08 2s is again an s, so there's only one s orbital, so the next two electrons go there.

01:15 Next we come to 2p.

01:17 Anytime we have a p, there are three p orbitals of equal energy, and the electrons enter one into each of those before they double up.

01:28 So our next six electrons go like that.

01:31 So so far we have placed 10 electrons, we have five more.

01:36 So continuing on, next would be 3s, 3s holds two, and then 3p.

01:45 Again, it's a p orbital, so i need to draw the three p orbitals, and i only have three electrons remaining because we have 12 arrows here so far, so i only have three remaining.

01:56 So remember, one goes into each of the empty orbitals before they double up.

02:01 So our final configuration would look like this.

02:05 So this would be our final answer for phosphorus.

02:10 We're going to repeat this process for the next three elements, but we're going to have to continue on a little further for each of those because they have higher atomic numbers.

02:21 So let's go on to letter b.

02:23 Letter b is nickel, and nickel has 28 electrons because its atomic number is 28.

02:32 So i'm going a little more quickly this time.

02:35 The two electrons in the 1s, next two electrons in the 2s.

02:43 Then we come to the 2p, then the 3s, followed by the 3p.

03:08 All right, and then after the 3p, we don't go to the 3d next in order of energy.

03:14 The 4s has lower energy than the 3d.

03:18 So we fill up the 4s next.

03:20 Then we come to 3d.

03:22 And since it's a d, there are five orbitals of equal energy.

03:27 And we are getting close at this point.

03:30 We only need eight more electrons...