Play a game to memorize the order in which orbitals fill....

Play a game to memorize the order in which orbitals fill. Have each group member in turn state the name of the next orbital to fill and the maximum number of electrons it can hold (for example, "1s bers can help, consulting Figure 9.5 and the accompanying text summary if necessary. However, when a member gets stuck, the next player starts back at "1s two." Keep going until each group member can list all the orbitals in order up to "6s two."

Play a game to memorize the order in which orbitals fill. Have each group member in turn state the name of the next orbital to fill and the maximum number of electrons it can hold (for example, "1s
bers can help, consulting Figure 9.5 and the accompanying text summary if necessary. However, when a member gets stuck, the next player starts back at "1s two." Keep going until each group member can list all the orbitals in order up to "6s two."

Key Concepts

Atomic Orbitals

Atomic orbitals are regions around an atom’s nucleus where electrons are most likely to be found. Each orbital is characterized by its shape and energy, and they are defined by quantum numbers. Understanding orbitals is fundamental to grasping how electrons are distributed within an atom.

Electron Configuration

Electron configuration refers to the arrangement of electrons in the orbitals of an atom. It describes how electrons occupy various orbitals according to specific rules and helps explain the chemical behavior of elements. This configuration is determined by underlying quantum mechanical principles.

Aufbau Principle

The Aufbau Principle is a guideline for determining the sequence in which orbitals are filled by electrons. It states that electrons occupy the lowest energy orbitals available before moving to higher energy ones. This principle explains the observed order of orbital filling and is essential in predicting the electron configuration of atoms.

Maximum Electron Capacity

Each type of atomic orbital has a specific maximum number of electrons it can hold, dictated by quantum mechanics. For example, s orbitals can hold 2 electrons, p orbitals 6, d orbitals 10, and f orbitals 14. This concept is crucial for determining electron configuration limits and for understanding the periodic trends in the elements.

Orbital Notation

Orbital notation is a shorthand method of representing the electron configuration of atoms, using symbols and numbers to indicate the type of orbital and the number of electrons it contains. This notation helps in organizing and memorizing the order of orbital filling, essential for studying atomic structure and the periodic table.

Transcript

00:03 In this problem, we want to try to devise a game in which we memorize the order in which orbitals fill.

00:13 So the orbitals will fill according to the off -baw principle.

00:19 So the off -wop principle is basically showing us the order in which we're going to fill the spd -f orbitals.

00:30 So what we're going to do is we're going to take a look at the period of table.

00:40 Let's practice filling in the orbitals up until neon, which is the first noble gas we'll encounter after helium.

00:51 So let's start with hydrogen.

00:56 So for hydrogen, we see that this is group one.

00:59 It's going to be a 1 -s orbital because the s -orbital is, on the left of periodont table.

01:07 So we're going to say it's one s one because that is the first element that we encounter.

01:13 And each s orbital can hold two electrons.

01:17 So now let's move on to the next element.

01:21 So when filling in the electrons, we have to move one element to the right.

01:27 So we move one element to the right and we see we jump to helium.

01:31 So the next electron is going to be in the same orbital.

01:38 So for helium, the electron configuration is 1s2.

01:42 Then we're going to move to lithium.

01:46 So for lithium, you see that we are in the second row.

01:50 That means that we are now filling 2s because we are still on the left side of a period table.

01:57 So since we're filling in the 2s and we're on the first element for that, it's going to be 2s1.

02:03 So now let's move on to beryllium.

02:05 So so brulium is again also on the left of periodic table.

02:09 So therefore, we are going to fill in another electron into the s orbital.

02:17 Now let's move on to the next element.

02:19 You can see that the next one is boron.

02:21 So now we are on the right side of the periodic table.

02:26 So excluding helium, when we move to the right side of the periodic table, we have to fill in the p orbitals.

02:33 And they're going to be in the same energy level as the row number.

02:38 So the real number is two, so therefore we're in the two p orbitals...

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