Using Fig. 7.28, list the elements (ignore the lanthanides...

Name: Problem 116, Chapter 7: Chemistry
Uploaded: 2019-08-20T05:57:43-08:00
Duration: 3 min 4 s
Channel: James Irizarry
Description: Using Fig. 7.28, list the elements (ignore the lanthanides and actinides) that have ground-state electron configurations that differ from those we would expect from their positions in the periodic table.

Using Fig. 7.28, list the elements (ignore the lanthanides and actinides) that have ground-state electron configurations that differ from those we would expect from their positions in the periodic table.

Key Concepts

Electron Configuration

The electron configuration of an element describes the distribution of its electrons among the various orbitals defined by quantum mechanics. This configuration determines many of the element's chemical and physical properties and is represented using a notation that shows electrons arranged in energy levels and sublevels.

Aufbau Principle

The Aufbau principle is a guideline for filling atomic orbitals with electrons, stating that electrons occupy the lowest energy orbitals available before moving to higher ones. This rule generally helps predict the order in which orbitals are filled but does not account for all exceptions.

Exceptions to the Aufbau Principle

Some elements deviate from the electron configurations predicted by the Aufbau principle. These exceptions occur because certain electron arrangements, such as half-filled or fully-filled subshells, provide extra stabilization, leading to configurations that differ from the straightforward rule-based prediction.

Orbital Energy and Subshell Stability

The relative energy levels of atomic orbitals and the additional stability provided by specific subshell configurations (like half-filled or fully-filled subshells) play a crucial role in determining the actual electron configuration. Understanding these energy differences is key to explaining why some elements exhibit configurations that appear anomalous based on their positions in the periodic table.

Transcript

00:01 All right, guys, you're doing problem one, two of chapter seven.

00:03 So we're going to use figures, the figure is 7 .29, which we have here.

00:07 They want us to show the elements that have gratzi electron configurations that would differ from those we expect based on their position on the pric table.

00:16 So the s block and the p block, those don't have any deviations based on what we expect on the period of table.

00:24 We're going to find those deviations in the p block.

00:27 We can also find them in the f block, but they told us to ignore the lamponides and the actinides.

00:32 So let's see.

00:34 We have, so with here, we have 4s2, 3d1, and then we should keep adding the electrons.

00:41 So we have d2, d3, d5.

00:45 So one of our exceptions is chromium.

00:47 We add electrons to d orbital, but then the electron from 4s drops down.

00:52 All right, so then we add in our electron to our s, 4s orbital, 4s2, then we keep adding electrons to our d overall.

00:59 The 6, the 7, d, 8, the 10, chrome copper is also another exception.

01:06 We add an electron the orbital, but then that electron also will us, but then for us, electron will drop down to the d oracle.

01:16 All right.

01:16 Next one, 5s2, 4d1, 4d2, 44...

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