Name: chemical bonds: types and strength
Uploaded: 2023-04-30T18:28:31.000Z
Duration: 2 min 40 s
Channel: JoVE

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Chemistry

Matter And Its Interactions

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Chemical Bonds

Wenn sich Atome einander annähern, stoßen sich ihre Kerne ab, ebenso wie die Elektronen. Gleichzeitig werden die Elektronen jedes Atoms vom Kern des anderen angezogen und so angeordnet, dass die Anziehungskräfte zwischen den Atomen maximiert und die Abstoßungskräfte minimiert werden.
Ergibt sich daraus eine Nettoanziehungskraft, wird die potentielle Energie des Systems gesenkt. Diese Wechselwirkung wird als chemische Bindung bezeichnet.
Allerdings kann nicht jede Kombination von Atomen stabile chemische Bindungen eingehen. Das chemische Verhalten eines Atoms wird in erster Linie dadurch bestimmt, welche Bindungen sie bilden und um welche Art von Bindungen es sich handelt. Das Verständnis der Bindung zwischen Atomen, aus denen eine Verbindung besteht, hilft, ihr molekulares Verhalten zu verstehen und vorherzusagen.
Die Bindungsenergie ist die Energie, die erforderlich ist, um eine Bindung in einem Mol einer gasförmigen Verbindung zu brechen. Das hängt von der Art der gebundenen Atome und der Anzahl der beteiligten Elektronen ab. Die Haftfestigkeit nimmt mit der Bindungsenergie zu.
Die Art der gebundenen Atome und die Anzahl der beteiligten Elektronen beeinflussen auch die Bindungslänge, die den durchschnittlichen Abstand zwischen den Kernen zweier gebundener Atome darstellt und umgekehrt proportional zur Bindungsvielfalt und Bindungsstärke ist.
Die häufigsten Bindungswechselwirkungen fallen in ein Spektrum, das von ionischen Bindungen, die elektrostatische Anziehungskräfte zwischen entgegengesetzt geladenen Ionen beinhalten, bis hin zu kovalenten Bindungen, die Valenzelektronen zwischen Atomen teilen, reicht.
Ionenbindungen sind die primäre Wechselwirkung in ionischen Verbindungen. Die Bestandteile Kationen und Anionen werden durch elektrostatische Anziehungskräfte zusammengehalten. Oft geht der Ionenbildung der Transfer von Valenzelektronen zwischen beteiligten Atomen voraus.
Das Atom, das Elektronen verliert, wird zum Kationen, während das Atom, das Elektronen aufnimmt, zum Anion wird. Durch den Elektronentransfer erhält jedes Ion in der Regel die nächstgelegene Edelgaskonfiguration, d. h. die Konfiguration, die mit der geringsten Änderung der Elektronenanzahl erreicht wird, wodurch die Ionen energetisch stabiler werden.
Bei der kovalenten Bindung interagieren die gemeinsamen Elektronen mit den Kernen der Bindungsatome und senken die potentielle Energie. Doppel- und Dreifachbindungen teilen sich zwei bzw. drei Elektronenpaare zwischen Atomen. Da dadurch die Anzahl der Elektronen zunimmt, die zusätzlichen Anziehungskräften aus dem anderen Kern ausgesetzt sind, nimmt die Bindungsstärke mit der Bindungsvielfalt zu.

chemische bindungen

Atome nehmen an der Bildung chemischer Bindungen teil, um eine vollständige Valenzschalen-Elektronenkonfiguration zu erhalten, die der des Edelgases ähnelt, das ihm in der Ordnungszahl am nächsten ist. Zu den wichtigen Arten chemischer Bindungen zählen ionische, kovalente und metallische Bindungen. Bindungsenergie und Bindungslänge bestimmen die Stärke einer chemischen Bindung.

Arten chemischer Bindungen

Eine Ionenbindung entsteht aufgrund der elektrostatischen Anziehung zwischen Kationen und Anionen. Oft entstehen die Ionen durch die Übertragung von Elektronen von einem beteiligten Atom auf das andere. Allerdings haben diese Bindungen keine definierte Richtung, da die elektrostatische Anziehungskraft gleichmäßig im dreidimensionalen Raum verteilt ist.

Eine kovalente Bindung ist eine chemische Bindung, die durch die gemeinsame Nutzung von Elektronenpaaren zwischen benachbarten Atomen entsteht. Das gemeinsame Elektronenpaar wird Bindungspaar genannt. Kovalente Bindungen sind richtungsabhängig.

Eine metallische Bindung wird zwischen zwei Metallatomen gebildet. Metallische Bindungen werden durch das „Electron Sea Model“ beschrieben. Aufgrund der niedrigen Ionisierungsenergien von Metallen besagt das Modell, dass Metallatome ihre Valenzelektronen leicht verlieren und zu Kationen werden. Diese Valenzelektronen erzeugen einen Pool delokalisierter Elektronen, der die Kationen im gesamten Metall umgibt.

Bindungsenergien und Bindungslänge

Die Stärke einer kovalenten Bindung wird durch die Energie gemessen, die benötigt wird, um sie aufzubrechen – das heißt, die Energie, die notwendig ist, um die gebundenen Atome zu trennen. Die Trennung eines Paares gebundener Atome erfordert Energie. Je stärker eine Bindung ist, desto größer ist die Energie, die benötigt wird, um sie aufzubrechen.

Die Energie, die erforderlich ist, um eine bestimmte kovalente Bindung in einem Mol gasförmiger Moleküle aufzubrechen, wird Bindungsenergie oder Bindungsdissoziationsenergie genannt. Die Bindungsenergie für ein zweiatomiges Molekül ist definiert als die Standard-Enthalpieänderung für die endotherme Reaktion. Moleküle mit drei oder mehr Atomen haben zwei oder mehr Bindungen. Die Summe aller Bindungsenergien in einem solchen Molekül entspricht der Standard-Enthalpieänderung für die endotherme Reaktion, die alle Bindungen im Molekül aufbricht.

Die Stärke einer Bindung zwischen zwei Atomen nimmt mit zunehmender Anzahl der Elektronenpaare in der Bindung zu. Im Allgemeinen gilt: Je größer die Anzahl der Bindungen zwischen zwei Atomen, desto kürzer ist die Bindungslänge und desto größer ist die Bindungsstärke. Somit sind Dreifachbindungen stärker und kürzer als Doppelbindungen zwischen denselben beiden Atomen; Ebenso sind Doppelbindungen stärker und kürzer als Einfachbindungen zwischen denselben beiden Atomen. Wenn sich ein Atom an verschiedene Atome in einer Gruppe bindet, nimmt die Bindungsstärke in der Regel ab, je weiter man sich in der Gruppe nach unten bewegt.

Dieser Text wurde angepasst von <a href="https://openstax.org/books/chemistry-2e/pages/7-1-ionic-bonding">Openstax, Chemistry 2e, Sektion 7.1: Ionic Bonding</a>, <a href="https://openstax.org/books/chemistry-2e/pages/7-2-covalent-bonding">Openstax, Abschnitt 7.2: Covalent Bonding</a>, <a href="https://openstax.org/books/chemistry-2e/pages/10-5-the-solid-state-of-matter">Section 10.5: The Solid State of Matter</a>, and Abschnitt<a href="https://openstax.org/books/chemistry-2e/pages/7-5-strengths-of-ionic-and-covalent-bonds"> 7.5. Bond Strength: Covalent Bonds</a>.

Chemische Bindungen


Atome nehmen an einer chemischen Bindungsbildung teil, um eine vollständige Valenz-Schale-Elektronenkonfiguration zu erhalten, die der des Edelgases ähnelt, das dem ...

Education

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Organic Chemistry

Organische Chemie

Unit 1

Einheit 1

Covalent Bonding and Structure

Kovalente Bindung und Struktur

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

chemical bonds: types and strength

Chemical bonds help atoms reach a full valence shell like the nearest noble gas. The main bond types are ionic, covalent, and metallic. Bond energy and bond length also help explain how strong a bond is.

An ionic bond forms from electrostatic attraction between cations and anions. In many cases, one atom transfers electrons to another atom, and the ions form from that transfer. Ionic bonds have no defined direction because the attraction spreads evenly through three-dimensional space.

A covalent bond forms when adjacent atoms share electron pairs. The shared pair is called the bonding pair. Covalent bonds are directional, so the atoms are linked in a specific orientation.

A metallic bond forms between two metal atoms. The electron sea model describes this type of bonding. In this model, metal atoms lose valence electrons easily and become cations, while the delocalized electrons form a pool around the cations across the metal.

The strength of a covalent bond is measured by the energy needed to break it and separate the bonded atoms. Stronger bonds require more energy. For one mole of gaseous molecules, this value is called bond energy, or bond dissociation energy. For a diatomic molecule, it is the standard enthalpy change for the endothermic reaction that breaks the bond.

Molecules with three or more atoms have more than one bond. In those cases, the total bond energy is the sum of all bond energies needed to break every bond in the molecule. Bond strength also increases as the number of electron pairs in the bond increases. Triple bonds are stronger and shorter than double bonds between the same atoms, and double bonds are stronger and shorter than single bonds. When one atom bonds to different atoms in a group, bond strength usually decreases as you move down the group.

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Chemical Bonds: Types and Strength

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