<section>
<h2>The Energy of Electrons</h2>
<p>The electrons of an atom all have the same charge and the same mass, but each electron has a different amount of <em>energy</em>. Electrons that have the <em>lowest</em> energy are found closest to the nucleus (where the attractive force of the positively charged nucleus is the greatest) and the electrons that have <em>higher</em> energy (and are able to overcome the attractive force of the nucleus) are found further away.</p>
<h2>Electron Arrangement</h2>
<p>We will start with a very simple view of the arrangement or configuration of electrons around an atom. This view simply states that electrons are arranged in energy levels (or shells) around the nucleus of an atom. These energy levels are numbered 1, 2, 3, etc. Electrons that are in the first energy level (energy level 1) are closest to the nucleus and will have the lowest energy. Electrons further away from the nucleus will have a higher energy.</p>
<p>In the following examples, the energy levels are shown as concentric circles around the central nucleus. The important thing to know for these diagrams is that the first energy level can hold 2 electrons, the second energy level can hold 8 electrons and the third energy level can hold 8 electrons.</p>
<h3><strong>1. Lithium</strong></h3>

Lithium (\(\text{Li}\)) has an atomic number of 3, meaning that in a neutral atom, the number of electrons will also be 3. The first two electrons are found in the first energy level, while the third electron is found in the second energy level (see figure below<span style="font-size: 16px;">)</span>
<div class="wp-caption alignnone" style="width: 506px"><img alt="6697d1d8f904b1cdbb6bc95830848495.png" height="211" src="https://data.ulearngo.com/assets/4d0931be-61c3-486e-b85f-2353d23d60d5" width="506"/><p class="wp-caption-text">Electron arrangement of a lithium atom.</p></div>
<h3>2. Fluorine</h3>

Fluorine (\(\text{F}\)) has an atomic number of 9, meaning that a neutral atom also has 9 electrons. The first 2 electrons are found in the first energy level, while the other 7 are found in the second energy level (see figure below).
<div class="wp-caption alignnone" style="width: 181px"><img alt="771f30e5a24ff910b47988729853f115.png" height="181" src="https://data.ulearngo.com/assets/0578eab8-89e2-4bd8-b2fb-030f8c896348" width="181"/><p class="wp-caption-text">Electron arrangement of a fluorine atom.</p></div>
<h3>3. Neon</h3>

Neon (\(\text{Ne}\)) has an atomic number of 10, meaning that a neutral atom also has 10 electrons. The first 2 electrons are found in the first energy level and the last 8 are found in the second energy level. (see figure below<span style="font-size: 16px;">)</span>
<div class="wp-caption alignnone" style="width: 181px"><img alt="1445808cc4d240b7d63bf051525ef43f.png" height="181" src="https://data.ulearngo.com/assets/46c92978-151a-499a-8b4b-e13708bd73d8" width="181"/><p class="wp-caption-text">Electron arrangement of a neon atom.</p></div>
<p>But the situation is slightly more complicated than this. Within each energy level, the electrons move in <strong>orbitals</strong>. An orbital defines the spaces or regions where electrons move.</p>
<div class="ns-school-emp">
<h3>Definition: Atomic Orbital</h3>
<div class="ns-school-defn">
<p>An atomic orbital is the region in which an electron may be found around a single atom.</p>
</div>
</div>
<p>The first energy level contains only one s orbital, the second energy level contains one s orbital and three <a data-lesson="hybrid-atomic-orbitals" data-subject="chemistry" data-tutorial="covalent-bonding-continued" href="https://app.ulearngo.com/chemistry/covalent-bonding-continued/hybrid-atomic-orbitals">p orbitals</a> and the third energy level contains one s orbital and three p orbitals (as well as five d orbitals). Within each energy level, the s orbital is at a lower energy than the p orbitals. This arrangement is shown in the figure below.</p>
<div class="wp-caption alignnone" style="width: 701px"><img alt="0d951834f0bd1821708984b45d56eb43.png" height="736" src="https://data.ulearngo.com/assets/79406ecf-61e6-4a92-8e77-2d637f7004e0" width="701"/><p class="wp-caption-text">The positions of the first ten orbitals of an atom on an energy diagram.</p></div>
<div class="ns-school-defn2">
<h3>Fact:</h3>
<p>Each block in the figure above is able to hold two electrons. This means that the s orbital can hold two electrons, while the p orbital can hold a total of six electrons, two in each of the three blocks.</p>
</div>
<p>This diagram also helps us when we are working out the electron configuration of an element. The electron configuration of an <a data-lesson="elements" data-subject="chemistry" data-tutorial="classification-of-matter" href="https://app.ulearngo.com/chemistry/classification-of-matter/elements">element</a> is the arrangement of the electrons in the shells and subshells. There are a few guidelines for working out the electron configuration. These are:</p>
<ul>
<li>
<p>Each orbital can only hold <strong>two electrons</strong>. Electrons that occur together in an orbital are called an <strong>electron pair</strong>.</p>
</li>
<li>
<p>An electron will always try to enter an orbital with the lowest possible energy.</p>
</li>
<li>
<p>An electron will occupy an orbital on its own, rather than share an orbital with another electron. An electron would also rather occupy a lower energy orbital <em>with</em> another electron, before occupying a higher energy orbital. In other words, within one energy level, electrons will fill an s orbital before starting to fill p orbitals.</p>
</li>
<li>
<p>The s subshell can hold 2 electrons</p>
</li>
<li>
<p>The p subshell can hold 6 electrons</p>
</li>
</ul>
<p>The way that the electrons are arranged in an atom is called its <strong>electron configuration</strong>.</p>
<div class="ns-school-defn2">
<h3>Tip:</h3>
<p>When there are two electrons in an orbital, the electrons are called an <strong>electron pair</strong>. If the orbital only has one electron, this electron is said to be an <strong>unpaired electron</strong>. Electron pairs are shown with arrows pointing in opposite directions.</p>
</div>
<div class="ns-school-emp">
<h3>Definition: Electron Configuration</h3>
<div class="ns-school-defn">
<p>Electron configuration is the arrangement of electrons in an atom, molecule or other <a data-lesson="physical-chemical-properties" data-subject="chemistry" data-tutorial="chemistry-essential-ideas" href="https://app.ulearngo.com/chemistry/chemistry-essential-ideas/physical-chemical-properties">physical</a> structure.</p>
</div>
</div>
</section>
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Electronic Configuration

Chemistry generally explores the substances of which matter is composed, the investigation of their properties and reactions, and the use of such reactions to form new substances. 

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Explore the essential ideas in chemistry, including the scientific method, laboratory skills and safety, states of matter, measurement uncertainty, models of the atom, electronic configurations, and more.


Electronic Configuration

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