Write the full orbital diagram for each element. a. S b. Ca...

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Key Concepts

Hund's Rule

Hund's rule indicates that electrons will fill degenerate orbitals (orbitals of the same energy) singly with parallel spins before pairing up. This minimizes electron-electron repulsion and is crucial for predicting the most stable electron arrangement in an atom.

Pauli Exclusion Principle

The Pauli exclusion principle asserts that no two electrons in an atom can have the same set of quantum numbers, which means each orbital can hold a maximum of two electrons with opposite spins. This rule is essential for constructing accurate orbital diagrams.

Aufbau Principle

The Aufbau principle states that electrons occupy the lowest energy orbitals available first before filling higher energy orbitals. This principle guides the order in which orbitals are populated in both electron configurations and orbital diagrams.

Orbital Diagram

An orbital diagram is a visual representation of the electron configuration in an atom. It depicts orbitals as boxes or lines and electrons as arrows, showing their distribution among the various energy levels and subshells.

Electron Configuration

Electron configuration is the arrangement of electrons in an atom's orbitals. It follows specific rules to determine which orbitals are occupied by electrons and reflects the energy levels and sublevels available in an atom.

Transcript

00:01 So now we'll work on problem 44.

00:06 This problem where has to write the orbital diagram for each element.

00:14 We're given sulfur, calcium, neon, and helium.

00:20 Start with sulfur.

00:26 So for sulfur, the orbital diagram is going to be similar to the electronic configuration, except we're going to write out the electron for each orbital and represent it as an up or down arrow.

00:37 So we have two electrons in the 1s.

00:43 In the 2s, we also have two electrons.

00:47 Then we have 2p, where we have 6 electrons.

00:52 So we want to write three pairs of electrons.

00:59 And then the 3s, we have two electrons.

01:08 Now here's where the orbital diagrams can get a little more tricky.

01:15 And we have to remember huns rule.

01:17 So in the 3p orbital, we have four electrons for sulfur because we can see that it's in that position on the periodic table right below oxygen.

01:30 So the question is, how do we fill in the electrons? so hun's rule tells us that we fill in all orbitals singly first.

01:40 So we first put in three parallel spins and then we put in the fourth electron.

01:48 So if we were to write something like this, for four electrons, that would be incorrect...

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