Name: ionic compounds and crystal lattices
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 2 min 48 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.3.1

Ionic Bonding and Electron Transfer

Los enlaces iónicos se forman mediante la transferencia de electrones de metales a no metales. En comparación con los enlaces covalentes donde se comparten los electrones, en los enlaces iónicos los metales tienden a perder electrones y los no metales tienden a aceptar electrones, pero por qué? La configuración electrónica más estable de un átomo es con un octeto completo.Lograr este estado junto con la reducción de las energías potenciales es una fuerza impulsora importante para la formación de enlaces. Pero, cómo predecir cuándo los electrones se transferirán y no se compartirán? Para ello, examina las energías de ionización y las afinidades electrónicas de los átomos.En la tabla periódica, los metales del bloque s tienen bajas energías de ionización. Esto facilita la pérdida más fácil de electrones para alcanzar un octeto mientras se forman cationes al mismo tiempo. Por el contrario, los no metales del bloque p, excepto los gases nobles, tienen altas afinidades electrónicas y aceptan fácilmente electrones para formar aniones.Los cationes y aniones con carga opuesta experimentan fuertes interacciones electrostáticas, atrayéndose entre sí para formar enlaces iónicos. Los compuestos iónicos a menudo forman estructuras cristalinas duras y bien definidas con altos puntos de fusión, debido a la fuerte atracción electrostática entre iones. Consideremod el fluoruro de litio, un compuesto iónico hecho de litio y flúor.Cuando el litio pierde un electrón para convertirse en un catión de litio con un dúo, el flúor absorbe el electrón para formar el anión con un octeto. Según la ley de Coulomb, estas dos partículas cargadas se atraen entre sí para formar fluoruro de litio, un compuesto neutro. El modelo de Lewis se puede utilizar para describir y predecir la fórmula química de compuestos iónicos.El símbolo de Lewis muestra las cargas en la esquina superior derecha y representa los aniones y cationes con el símbolo escrito entre paréntesis. Considere el cloruro de estroncio, una sal de uso común para obtener un color rojo brillante en los fuegos artificiales. El símbolo de Lewis para el estroncio tiene un dos y el cloro tiene un electrón desapareado.El estroncio debe perder dos electrones, mientras que el cloro debe ganar un electrón para alcanzar un octeto. Por lo tanto, un catión de estroncio se une a dos aniones de cloruro, en una proporción de uno a dos

enlace iónico y transferencia de electrones

Los iones son átomos o moléculas que llevan una carga eléctrica. Un catión (un ion positivo) se forma cuando un átomo neutro pierde uno o más electrones de su capa de valencia, y un anión (un ion negativo) se forma cuando un átomo neutro gana uno o más electrones en su capa de valencia. Los compuestos conformados por iones se llaman compuestos iónicos (o sales), y sus iones constituyentes se mantienen juntos por enlaces iónicos: Fuerzas electrostáticas de atracción entre cationes y aniones con cargas opuestas. 
 
 <h4>Propiedades de los compuestos iónicos</h4>
 
 Las propiedades de los compuestos iónicos arrojan algo de luz sobre la naturaleza de los enlaces iónicos.
 
 <ul>
 <li>Los sólidos iónicos presentan una estructura cristalina y tienden a ser rígidos y quebradizos; también tienden a tener altos puntos de fusión y ebullición, lo que sugiere que los enlaces iónicos son muy fuertes. </li>
 <li>Los sólidos iónicos también son malos conductores de la electricidad por la misma razón: La fuerza de los enlaces iónicos impide que los iones se muevan libremente en estado sólido. </li>
 <li>Sin embargo, la mayoría de los sólidos iónicos se disuelven fácilmente en agua. Una vez disueltos o fundidos, los compuestos iónicos son excelentes conductores de la electricidad y el calor, ya que los iones pueden moverse libremente.</li>
 </ul>
 
 <h4>Formación de los compuestos iónicos</h4>
 
 Muchos elementos metálicos tienen potenciales de ionización relativamente bajos y pierden electrones fácilmente. Estos elementos se encuentran a la izquierda en un período o cerca de la parte inferior de un grupo en la tabla periódica. Los átomos no metálicos tienen afinidades electrónicas relativamente altas y, por lo tanto, ganan fácilmente electrones perdidos por los átomos metálicos, llenando así sus capas de valencia. Los elementos no metálicos se encuentran en la esquina superior derecha de la tabla periódica.
 
 Como todas las sustancias deben ser eléctricamente neutras, el número total de cargas positivas en los cationes de un compuesto iónico debe ser igual al número total de cargas negativas en sus aniones. La fórmula de un compuesto iónico representa la relación más simple del número de iones necesario para dar números idénticos de cargas positivas y negativas. 
 
 <h4>Los compuestos iónicos forman estructuras de 3 dimensiones dispuestas regularmente</h4>
 
 Es importante notar, sin embargo, que la fórmula para un compuesto iónico no representa la disposición física de sus iones. Es incorrecto referirse a la “molécula” de cloruro de sodio (NaCl) porque no hay un único enlace iónico, per se, entre cualquier par específico de iones de sodio y cloruro. Las fuerzas de atracción entre los iones son isotrópicas — iguales en todas las direcciones — lo que significa que cualquier ión en particular es igualmente atraído a todos los iones cercanos de carga opuesta. Esto resulta en que los iones se acomodan en una estructura de entramado tridimensional estrechamente unida. El cloruro de sodio, por ejemplo, consiste en una disposición regular de números iguales de cationes Na+ y aniones Cl–. La fuerte atracción electrostática entre los iones Na+ y Cl– los mantiene unidos firmemente en NaCl sólido. Se requieren 769 kJ de energía para disociar un mol de NaCl sólido en iones gaseosos Na+ y Cl– separados. 
 
 <h4>Estructuras electrónicas de los cationes</h4>
 
 Al formar un catión, un átomo del elemento del grupo principal tiende a perder todos sus electrones de valencia, asumiendo así la estructura electrónica del gas noble que lo precede en la tabla periódica. 
 
 <ul>
 <li>Para los grupos 1 (los metales alcalinos) y 2 (los metales alcalinotérreos), el número de grupo es igual al número de electrones de la capa de valencia y, en consecuencia, a las cargas de los cationes formados a partir de átomos de estos elementos cuando todos los electrones de la capa de valencia son removidos. </li>
 <li>Por ejemplo, el calcio es un elemento del grupo 2 cuyos átomos neutros tienen 20 electrones y una configuración electrónica en estado fundamental de 1s22s22p63s23p64s2. Cuando un átomo de Ca pierde ambos electrones de valencia, el resultado es un catión con 18 electrones, una carga de 2+ y una configuración electrónica de 1s22s22p63s23p6. El ion Ca2+ es, por lo tanto, isoelectrónico con el gas noble Ar.</li>
 <li>Para los grupos 13–17, los números de grupo exceden el número de electrones de valencia por 10 (teniendo en cuenta la posibilidad de subcapas d llenas en átomos de elementos en el cuarto período y mayores). Así, la carga de un catión formado por la pérdida de todos los electrones de valencia es igual al número de grupo menos 10. Por ejemplo, el aluminio (en el grupo 13) forma iones 3+ (Al3+).</li>
 </ul>
 
 <h4>Excepciones</h4>
 
 <ul>
 <li>Las excepciones al comportamiento esperado implican elementos hacia la parte inferior de los grupos. </li>
 <li>Además de los iones esperados Tl3+, Sn4+, Pb4+ y Bi5+, una pérdida parcial de los electrones de la capa de valencia de estos átomos también puede conducir a la formación de iones Tl+, Sn2+, Pb2+ y Bi3+. La formación de estos cationes 1+, 2+ y 3+ se atribuye al efecto de par inerte, que refleja la energía relativamente baja del par de electrones de valencia s para los átomos de los elementos pesados de los grupos 13, 14 y 15. </li>
 <li>El mercurio (grupo 12) también muestra un comportamiento inesperado: Forma un ion diatómico, Hg22+ (un ion formado a partir de dos átomos de mercurio, con un enlace Hg-Hg), además del ion monatómico esperado Hg2+ (formado a partir de un solo átomo de mercurio).</li>
 <li>Los elementos metálicos de transición y transición interna se comportan de forma diferente que los elementos del grupo principal. La mayoría de los cationes de metales de transición tienen cargas 3+ o 2+ que resultan de la pérdida de su electrón s más externo(s) primero, seguido a veces por la pérdida de uno o dos electrones d de la capa inmediatamente adyacente.</li>
 <li>Aunque los d orbitales de los elementos de transición son, según el principio de aufbau — los últimos que se llenan al formar las configuraciones electrónicas — los electrones más externos son los primeros que se pierden cuando estos átomos se ionizan. Cuando los metales de transición interna forman iones, suelen tener una carga de 3+, que resulta de la pérdida de sus electrones más externos y de un electrón d o f.</li>
 </ul>
 
 <h4>Estructuras electrónicas de los aniones</h4>
 
 La mayoría de los aniones monatómicos se forman cuando un átomo neutro no metálico gana suficientes electrones para llenar completamente sus orbitales externos s y p, alcanzando así la configuración electrónica del siguiente gas noble. Por lo tanto, es simple determinar la carga en tal ión negativo: La carga es igual al número de electrones que deben ser ganados para llenar los orbitales s y p del átomo padre. El oxígeno, por ejemplo, tiene la configuración electrónica 1s22s22p4, mientras que el anión de oxígeno tiene la configuración electrónica del gas noble neón (Ne), 1s22s22p6. Los dos electrones adicionales necesarios para llenar los orbitales de valencia le dan al ion óxido la carga de 2– (O2–).
 
 Este texto es adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/7-1-ionic-bonding">Openstax, Química 2e, Sección 7.3: Enlace Iónico.</a>

Enlace Iónico y Transferencia de Electrones

Los iones son átomos o moléculas que llevan una carga eléctrica. Un catión (un ion positivo) se forma cuando un átomo neutro pierde uno o más electrones de su valencia.

Education

Educación

JoVE Core

Química

Chemical Bonding: Basic Concepts

Enlace químico: conceptos básicos

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

ionic compounds and crystal lattices

Ionic compounds form when positive and negative ions attract each other. A cation is a positive ion, and it forms when an atom loses one or more valence electrons. An anion is a negative ion, and it forms when an atom gains one or more valence electrons. Compounds made of these ions are called ionic compounds, or salts, and the force between them is an ionic bond.

The properties of ionic solids help show how strong this attraction is. They usually form rigid, brittle crystals and have high melting and boiling points. They are also poor conductors of electricity in the solid state because the ions cannot move freely. Most ionic solids dissolve readily in water. When an ionic compound is melted or dissolved, it conducts electricity and heat well because the ions can move about freely.

Ionic compounds form most easily when metals lose electrons and nonmetals gain them. Many metals have low ionization potentials, so they lose electrons easily. These elements are found on the left side of the periodic table or near the bottom of a group. Nonmetals have high electron affinities, so they readily gain the electrons lost by metals. They are found in the upper-right corner of the periodic table.

Ionic compounds must remain electrically neutral. That means the total positive charge from the cations must equal the total negative charge from the anions. The formula of an ionic compound gives the simplest ratio of ions needed to balance charge. The formula does not show the physical layout of the ions. In solid sodium chloride, for example, the ions form a tightly bound three-dimensional lattice. The attraction between Na+ and Cl- ions is strong, and it takes 769 kJ of energy to separate one mole of solid NaCl into gaseous ions.

Main-group cations often form by losing all valence electrons and taking on the electron structure of the noble gas before them. For groups 1 and 2, the group number matches the number of valence electrons and also the charge of the ion formed. Calcium is a group 2 element. A neutral calcium atom has 20 electrons, and Ca2+ has 18 electrons with the same electron configuration as argon. For groups 13 through 17, the cation charge equals the group number minus 10. Aluminum, in group 13, forms Al3+.

Some heavy main-group elements do not follow the expected pattern exactly. Thallium, tin, lead, and bismuth can also form lower-charge ions such as Tl+, Sn2+, Pb2+, and Bi3+. This is explained by the inert pair effect, which reflects the relatively low energy of the valence s-electron pair in these heavy atoms. Mercury is another exception. It can form the diatomic ion Hg2^2+, which contains a Hg-Hg bond, as well as the monatomic ion Hg2+.

Transition metals and inner transition metals form ions in a different way. Most transition metal cations have 2+ or 3+ charges. These usually come from losing the outermost s electron or electrons first, and sometimes one or two d electrons after that. Even though d orbitals fill later according to the Aufbau principle, the outermost s electrons are lost first when transition metals ionize. Inner transition metals usually form 3+ ions by losing their outermost s electrons and one d or f electron.

Most monatomic anions form when a nonmetal atom gains enough electrons to fill its outer s and p orbitals. The charge on the ion equals the number of electrons needed to reach the next noble-gas electron configuration. Oxygen is a clear example. A neutral oxygen atom has the configuration 1s2 2s2 2p4. The oxide ion, O2-, has the neon configuration, 1s2 2s2 2p6, after gaining two electrons.

Ionic Compounds and Crystal Lattices

types of chemical bonds

Chemical Bonding and Bond Properties

Chemical bonding explains how atoms and ions join to form molecules and compounds. American chemist Gilbert N. Lewis pioneered chemical bonding theory with the Lewis model. This model helps explain why bonds form, why some are stronger than others, and why compounds have fixed formulas like H2O instead of H4O. Ionic bonding involves ions, which are atoms or molecules with an electrical charge. A cation is a positive ion formed when a neutral atom loses one or more electrons from its valence...

the born-haber cycle

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Chemical bonds form when atoms or ions interact in ways that lower the potential energy of a molecule. Gilbert N. Lewis created a simple model to show bond formation using valence electrons, the electrons in the outer shell. In this model, electrons are shared or transferred to help atoms reach a stable electron configuration. The Lewis model helps describe two common bond types. An ionic bond forms when electrons move from a metal to a nonmetal. A covalent bond forms when two nonmetals share...

electronegativity

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ionic bonding and electron transfer

Ionic compounds form when positive and negative ions attract each other. A cation is a positive ion, and it forms when an atom loses one or more valence electrons. An anion is a negative ion, and it forms when an atom gains one or more valence electrons. Compounds made of these ions are called ionic compounds, or salts, and the force between them is an ionic bond. The properties of ionic solids help show how strong this attraction is. They usually form rigid, brittle crystals and have high...

trends in lattice energy: ion size and charge

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Lattice energy shows how strongly ions hold an ionic solid together. It is the energy required to separate one mole of a solid into its gaseous ions. For sodium chloride, this process requires 769 kJ per mole. The opposite convention may also be used, where lattice energy is the energy released when gaseous ions form the solid. In either case, a larger magnitude means a more stable ionic compound. For ionic crystals, lattice energy follows a pattern based on charge and ion size. The...

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resonance

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key terms and concepts

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Ionic Compounds and Crystal Lattices | JoVE K12

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Physical Science

PS.PSc.2.1

Pennsylvania State Academic Standards

Structure and Properties of Matter

3.2.9-12.B

3.2.9-12.N

Louisiana Student Standards for Science

High School

Matter And Its Interactions

HS-PS1-3

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Bonding and compounds

Structure And Properties Of Matter

Chemical bonding

Physical Geology

Minerals

Chemical bonding (ionic, covalent, metallic)

Tennessee Academic Standards

Matter and Its Interactions

CHEM1.PS1.13

CHEM1.PS1.14

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Motion and Stability: Forces and Interactions

CHEM1.PS2.1

Virginia  Standards of Learning

HIgh School

CH.3

CH.3.d

PS.3

PS.3.c

Physics

PH.9

PH.9.e

Minnesota Academic Standards in Science

1.2.1 9L.4.2.2.1

Arizona Science Standards

HS.P1

HS.P1U1.2

new-jersey-student-learning-standards-for-science

New Jersey Student Learning Standards for Science

HS-PS1-2

Alabama Course of Study Science

9-12.C.2.2.b

Florida Department of Education

SC.912.P.8

SC.912.P.8.6

Texas Essential Knowledge and Skills

Chemistry and Physics

IPC.7

IPC.7.A

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-3.

HS. Chemical Reactions

HS-PS1-2.

Georgia Standards of Excellence

SPS2.

Chemical Bonds

SC2.

bonding-types-from-nonpolar-covalent-to-ionic

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PS.Chm.1.3

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