Give the electron configurations of (a) S,(𝐛) K,(𝐜) Ti, and (𝐝) S n .

Name: Problem 105, Chapter 8: Chemistry The Molecular Nature of Matter
Uploaded: 2021-12-22T19:21:02-08:00
Duration: 3 min 56 s
Channel: Crystal Wang
Description: Give the electron configurations of (a) S,(𝐛) K,(𝐜) Ti, and (𝐝) S n .

Give the electron configurations of (a) S,(𝐛) K,(𝐜) Ti, and...

Key Concepts

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 result, each orbital can hold a maximum of two electrons with opposite spins, limiting the occupancy of each energy state.

Electron Configuration

Electron configuration is the method of describing the distribution of electrons among the orbitals of an atom. It indicates how electrons are arranged in various energy levels (shells) and subshells (s, p, d, f), which is crucial for understanding an element's chemical behavior and properties.

Aufbau Principle

The Aufbau principle states that electrons occupy orbitals of the lowest available energy before filling higher energy ones. This principle helps determine the sequence in which atomic orbitals are filled, starting from the 1s orbital and progressing to higher orbitals.

Noble Gas Notation

Noble gas notation is a shorthand method for writing electron configurations by using the electron configuration of the nearest preceding noble gas as a reference. This simplifies the representation by compactly summarizing core electrons while focusing on the valence electrons.

Hund's Rule

Hund's Rule specifies that for orbitals of equal energy (degenerate orbitals), electrons are placed in separate orbitals with parallel spins as long as possible before any pairing occurs. This minimizes electron repulsion and stabilizes the electron configuration.

Transcript

00:01 In this question, we were asked to give the electron configurations of sulfur, potassium, titanium, and tin.

00:08 So let's first locate the element on the periodic table.

00:14 So here, the first one is sulfur.

00:17 The sulfur is right here.

00:19 So you see that this is not a transition metal, so we don't have to worry about any exceptions to the rules.

00:25 So we are going to first start with the.

00:33 Level gas configuration, or if you want, you can write out the entire configuration.

00:38 You would have to write out everything before this, which would be 1s2, 2s2, and 2p6, or you can just write neon in brackets, which would imply that every electron before sodium is already filled in.

00:55 So we can do that, and then afterwards we are going to go to the next period, which is going to be period 3.

01:04 This is the s block, so we have to fill in these two electrons.

01:08 So it's 3s2, and then we're going to count into the 3p block.

01:12 So it's 1, 2, 3, 4, so that's 3p4.

01:16 So then we end up with this as the electron configuration for sulfur.

01:22 If you were to write out the entire electron configuration, everything before the sodium would be filled in, so 1s2, 2s2, 2p6.

01:35 So now let's do the next one.

01:37 That would be potassium...