Write orbital diagrams for each ion and indicate whether the ion is diamagnetic or paramagnetic.

step 1 So now we'll work on problem 68 from chapter 8. In this problem, to draw orbital diagrams for fo

Write orbital diagrams for each ion and indicate whether the...

Key Concepts

Diamagnetism and Paramagnetism

Diamagnetism and paramagnetism describe the magnetic properties of substances based on the presence or absence of unpaired electrons. Diamagnetic substances have all electrons paired, resulting in weak magnetic repulsion, while paramagnetic substances have one or more unpaired electrons, leading to attraction in the presence of a magnetic field.

Ionic Electron Removal

This process involves removing electrons from an atom to form a positive ion (cation). The electron configuration of the resultant ion is determined by removing electrons from the highest energy orbitals first. Understanding this concept is essential for accurately drawing orbital diagrams for ions and predicting their chemical and physical properties.

Aufbau Principle, Hund’s Rule, and Pauli Exclusion Principle

These fundamental quantum mechanical rules govern the filling of electrons in atomic orbitals. The Aufbau Principle dictates that electrons occupy the lowest energy orbitals first, Hund’s Rule states that electrons fill degenerate orbitals singly before pairing, and the Pauli Exclusion Principle ensures that no two electrons in an atom can have the same set of quantum numbers. Together, these principles are crucial for determining the electron arrangement in both atoms and ions.

Electron Configuration

This concept refers to the arrangement of electrons in an atom or ion’s orbitals according to specific rules. It is fundamental to understanding the chemical properties of an element, including how electrons populate energy levels and subshells, and serves as the basis for constructing orbital diagrams.

Orbital Diagram

An orbital diagram is a visual representation of the electron configuration in specific orbitals using arrows to indicate the spin of electrons. It communicates not only the number of electrons but also their distribution among orbitals, which is critical in predicting the magnetic behavior and bonding characteristics of atoms and ions.

Transcript

00:01 So now we'll work on problem 68 from chapter 8.

00:08 In this problem, to draw orbital diagrams for four ions and indicate whether the ion is diamagnetic or paramagnetic.

00:20 So we can go ahead and start with the first problem, which is cadmium 2 plus.

00:28 So just to be clear, let's go ahead and write the electron configuration for cadmium.

00:36 So we have krypton 5s2, 4d10.

00:42 And then for cadmium 2 plus, we have krypton, and then the two electrons are going to be lost from the s orbitals.

00:52 So we have 4d10.

00:53 So this is the configuration.

00:56 So on the right, we can draw the orbital diagram.

01:02 We have krypton accounting for the core electrons.

01:06 And then in the valence electron, we're going to have the 4d.

01:09 With five pairs of electrons.

01:19 So they ask us if it's diamagnetic or paramagnetion.

01:23 So for something to be paramagnetic, it needs to have unpaired electrons.

01:27 Since this does not, we will call it diomagnetic.

01:35 So we don't necessarily have to write the electron configuration first, but just to be clear before that we write the diagram, it's useful.

01:44 So now we're going to do gold plus.

01:47 So first the electron configuration for gold is xenon 6s1, 4f14, 5d10, and gold plus will be xenon 4f14, since we're losing the electron from the s orbital 5d10...

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