Write the expected ground-state electron configuration for the following: a. the element with on

Write the expected ground-state electron configuration for...

Key Concepts

Electron Configuration Notation

This concept involves the use of a standardized shorthand method to represent the arrangement of an atom’s electrons into various orbitals. Typically, it uses the electron configuration of a noble gas to summarize the inner electrons, followed by the explicit filling of the outer orbitals (s, p, d, f) to show the valence configuration.

Aufbau Principle

The Aufbau principle dictates that electrons fill orbitals starting from the lowest energy level and move upward to higher energy levels. This rule establishes the order in which the subshells are occupied as the atomic number increases, providing the framework for predicting the ground-state electron configuration of elements.

Hund’s Rule

Hund’s rule states that when electrons occupy degenerate orbitals (orbitals with the same energy), they will fill them singly with parallel spins before any pairing occurs. This principle is key to determining the number of unpaired electrons in an atom, which directly influences magnetic properties and bonding behavior.

Periodic Table Groupings and Blocks

Understanding the arrangement of elements into blocks (s, p, d, f) on the periodic table is crucial because it correlates with the electron configurations. The division into these blocks helps predict the orbital type being filled (for instance, p-block elements versus d-block or f-block elements) and is essential in understanding trends across the periodic table.

Electron Orbital Capacities

This concept refers to knowing the maximum number of electrons that each type of orbital can hold—2 in s, 6 in p, 10 in d, and 14 in f. This information is fundamental when determining how electrons populate the available orbitals in the ground state, especially in situations involving elements with variable numbers of unpaired electrons or extended electron configurations.

Transcript

00:01 In answering these questions, it's important to remember that the periodic table represents the arrangement of electrons or the electron configuration in for any given atom.

00:11 Each section corresponds to a different sub -level.

00:16 And so the first part here, the first two rows are referred to as the s block.

00:22 The rows over here are the p block.

00:25 These are the d block.

00:27 Down here is the f block.

00:30 And each row is a different energy level.

00:39 Remembering that the ds are one behind, so even though this is the fourth row, these are three ds.

00:48 And the fs are two behind.

00:50 So even though these fall, number 58 should fall in the sixth row, these are the 4f, and these are the 5f.

00:59 So if you can identify the element that you're looking for the electron configuration, you can use the periodic chart to find the valence electrons.

01:09 So for example, in our first problem a, it asks to find the element who has one unpaired electron in the 5p orbital that covalently bonds with fluorine.

01:24 So 5p, we look at our rows 5, would be this section here.

01:29 And we have two options for having one electron unpaired in the p orbital.

01:39 Could have one, or we could have a total of five electrons, which also has only one unpaired electron.

01:54 So if we're looking at an element that has one p electron in the 5 p orbital, it would be i .n.

02:01 If we're looking at one that has five, it would be two, three, four, five i.

02:07 So we have to choose between those two.

02:09 Because it covalently bonds with fluorine, we're looking for the non -metal, which is iodine.

02:15 So the correct answer to a is iodine.

02:19 And the electron configuration for iodine, i'm going to use our noble gas configuration.

02:24 So we write in brackets the preceding noble gas, which is krypton, which brings us here to 5s2, then to the 4d.

02:43 And we go all the way across, so 4d10, and then 5p, 1, 2, 3, 4, 4, 5...

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