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

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-1

Chemical Bonds

Cuando los átomos se acercan, sus núcleos se repelen, al igual que los electrones. Al mismo tiempo, los electrones de cada átomo son atraídos por el núcleo del otro y se organizan de tal manera que maximizan las fuerzas de atracción entre los átomos y minimizan las fuerzas repulsivas.
Si esto da como resultado una fuerza de atracción neta, la energía potencial del sistema se reduce. Esta interacción se denomina enlace químico.
Sin embargo, no todas las combinaciones de átomos pueden formar enlaces químicos estables. El comportamiento químico de un átomo está determinado principalmente por qué forma enlaces y qué tipo de enlaces son. Comprender el enlace entre los átomos que forman un compuesto ayuda a comprender y predecir su comportamiento molecular.
La energía de enlace es la energía necesaria para romper un enlace en un mol de un compuesto gaseoso. Depende del tipo de átomos enlazados y del número de electrones involucrados. La fuerza del enlace aumenta con la energía del enlace.
El tipo de átomos enlazados y el número de electrones involucrados también influyen en la longitud del enlace, que es la distancia media entre los núcleos de dos átomos enlazados y es inversamente proporcional a la multiplicidad del enlace y la fuerza del enlace.
Las interacciones de enlace más comunes se encuentran en un espectro que va desde enlaces iónicos, que involucran atracciones electrostáticas entre iones con carga opuesta, hasta enlaces covalentes, que comparten electrones de valencia entre átomos.
El enlace iónico es la interacción principal que se encuentra en los compuestos iónicos. Los cationes y aniones constituyentes se mantienen unidos por fuerzas electrostáticas de atracción. A menudo, la formación de iones está precedida por la transferencia de electrones de valencia entre los átomos participantes.
El átomo que pierde electrones se convierte en el catión, mientras que el átomo que acepta electrones se convierte en el anión. La transferencia de electrones generalmente le da a cada ion la configuración de gas noble más cercana, que es la configuración alcanzada con el cambio más mínimo en el número de electrones, lo que hace que los iones sean energéticamente más estables.
En el enlace covalente, los electrones compartidos interactúan con los núcleos de los átomos de enlace y disminuyen la energía potencial. Los enlaces dobles y triples comparten dos y tres pares de electrones entre átomos, respectivamente. A medida que esto aumenta el número de electrones sujetos a fuerzas de atracción adicionales del otro núcleo, la fuerza del enlace aumenta con la multiplicidad de enlaces.

enlaces químicos

Los átomos participan en la formación de un enlace químico para adquirir una configuración electrónica completa de la capa de valencia similar a la del gas noble más cercano a él en número atómico. Los enlaces iónicos, covalentes y metálicos son algunos de los tipos importantes de enlaces químicos. La energía y la longitud del enlace determinan la fuerza de un enlace químico.


 Tipos de enlaces químicos


 Un enlace iónico se forma debido a la atracción electrostática entre cationes y aniones. A menudo, los iones se forman mediante la transferencia de electrones de un átomo participante a otro. Sin embargo, estos enlaces no tienen una direccionalidad definida, porque la fuerza de atracción electrostática se distribuye uniformemente por todo el espacio tridimensional.


 Un enlace covalente es un enlace químico formado por el intercambio de pares de electrones entre átomos adyacentes. El par de electrones compartido se llama par de enlace. Los enlaces covalentes son de naturaleza direccional.


 Un enlace metálico se forma entre dos átomos de metal. La unión metálica se describe mediante el “modelo del mar de electrones”. Basado en las bajas energías de ionización de los metales, el modelo establece que los átomos metálicos pierden fácilmente sus electrones de valencia y se convierten en cationes. Estos electrones de valencia crean un conjunto de electrones deslocalizados que rodean los cationes en todo el metal.


 Energías de enlace y longitud de enlace


 La fuerza de un enlace covalente se mide por la energía necesaria para romperlo, es decir, la energía necesaria para separar los átomos unidos. Separar cualquier par de átomos unidos requiere energía. Cuanto más fuerte es un vínculo, mayor es la energía necesaria para romperlo.


 La energía necesaria para romper un enlace covalente específico en un mol de moléculas gaseosas se llama energía de enlace o energía de disociación del enlace. La energía de enlace de una molécula diatómica se define como el cambio de entalpía estándar de la reacción endotérmica. Las moléculas con tres o más átomos tienen dos o más enlaces. La suma de todas las energías de enlace en dicha molécula es igual al cambio de entalpía estándar de la reacción endotérmica que rompe todos los enlaces de la molécula.


 La fuerza de un enlace entre dos átomos aumenta a medida que aumenta el número de pares de electrones en el enlace. Generalmente, cuanto mayor es el número de enlaces entre dos átomos, más corta es la longitud del enlace y mayor es la fuerza del enlace. Por tanto, los triples enlaces son más fuertes y más cortos que los dobles enlaces entre los mismos dos átomos. Por tanto, los dobles enlaces son más fuertes y más cortos que los enlaces simples entre los mismos dos átomos. Cuando un átomo se une a varios átomos de un grupo, la fuerza del enlace generalmente disminuye a medida que avanzamos en el grupo.

Enlaces químicos


Los átomos participan en la formación de un enlace químico para adquirir una configuración electrónica completa de capa de valencia similar a la del gas noble más cercano.

Education

Educación

JoVE Core

Organic Chemistry

Química Orgánica

Unit 1

Unidad 1

Covalent Bonding and Structure

Enlace covalente y estructura

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

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.

Chemical Bonds: Types and Strength

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chemical bonds

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...

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intermolecular forces and physical properties

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overview of advanced functional groups

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key terms and concepts

Explore ionic, covalent, and metallic bonds, plus bond energy and bond length. Learn how bond type affects strength in high school chemistry.

Chemical Bonds: Types and Strength | JoVE K12

organic chemistry

JoVE Core Química Orgánica explica los conceptos básicos de la estereoquímica, las reacciones y sus mecanismos mediante lecciones de vídeo animadas, concisas y fáciles de entender. Además, los vídeos de científicos en acción muestran la aplicación de esos conceptos en experimentos de investigación clásicos y originales, desarrollados actualmente en laboratorios de todo el mundo.

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9-12

Physical Geology

Minerals

Chemical bonding (ionic, covalent, metallic)

Tennessee Academic Standards

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CHEM1.PS2.1

Virginia  Standards of Learning

HIgh School

Physics

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PH.9.e

Minnesota Academic Standards in Science

1.1.1 9L.4.2.1.1

3.1.1 9C.2.2.1.2

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HS-PS1-4

Chemical Bonds: Types and Strength

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