Name: ionization energy trends in the periodic table
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 3 min 12 s
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K12 Standards

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NC K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.2.2

Ionization Energy

El comportamiento químico de los átomos y los iones. se ve muy afectado por lo fácil o difícil que es eliminar sus electrones, especialmente los electrones más externos que participan en la formación del enlace químico. La energía necesaria para eliminar un electrón de un átomo gaseoso en su estado base se llama la primera energía de ionización y se expresa en kilojulios por mol.La energía necesaria para eliminar el electrón siguiente se denomina segunda energía de ionización, y así sucesivamente. Al descender por una columna, las energías de ionización disminuyen. Recuerde que el número del quantum principal más elevado de los electrones de una valencia aumenta en la columna conduciendo tamaños atómicos más grandes.Así, cuanto más lejos están los electrones más externos, más fáciles son de eliminar. Para los elementos del grupo principal, la energía de ionización aumenta a lo largo del período. La razón radica en el número atómico creciente, donde los electrones de valencia experimentan una carga nuclear efectiva más alta.dificultando la eliminación de los electrones más externos. Esto explica por qué el cloro tiene una mayor energía de ionización que el sodio, por ejemplo. Generalmente, la energía de ionización es mínima para un metal alcalino.y se eleva a un pico con cada gas noble. Los metales de transición muestran un pequeño aumento en la energía de ionización a lo largo del período, y los elementos del bloque f muestran un cambio aún menor. Pero hay algunas excepciones a considerar.El boro tiene una energía de ionización menor que el berilio, aunque está más a la derecha en la tabla periódica. El berilio tiene electrones 2s de menor energía, mientras que el boro tiene un electrón con una energía 2p más alta que hace que su eliminación sea energéticamente más favorable. Otra excepción es el oxígeno, que tiene menor energía de primera ionización que el nitrógeno.Comparado al nitrógeno, el oxígeno tiene cuatro electrones p, y al eliminar un electrón se elimina la repulsión electrón-electrón. Por lo tanto, se requiere menos energía para la ionización. Estas excepciones también se observan en períodos sucesivos.La eliminación de electrones de los cationes es más difícil que de los átomos neutros. Generalmente, las energías sucesivas de ionización aumentan para los elementos. Considere el potasio.La segunda energía de ionización es significativamente mayor, ya que implica la eliminación de un electrón central de un ion con una configuración de gas noble. Del mismo modo, para el calcio, se observa un alto aumento de la segunda a la tercera energía de ionización puesto que un electrón del núcleo se elimina de un catión con una configuración de gas noble.

energía de ionización

La cantidad de energía requerida para quitar el electrón más débilmente unido de un átomo gaseoso en su estado fundamental se llama primera energía de ionización (EI1). La primera energía de ionización para un elemento, X, es la energía necesaria para formar un catión con una carga de 1+:
 
 <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/1049/1049_Equations-01.png" style="height: 40px;" />
 
 La energía requerida para remover el segundo electrón más suelto se llama segunda energía de ionización (EI2).
 
 <img alt="Eq2" src="https://www.jovecore.com/CDNSource/lessons/1049/1049_Equations-02.png" style="height: 40px;" />
 
 La energía necesaria para remover el tercer electrón es la tercera energía de ionización, y así sucesivamente. La energía siempre es necesaria para remover electrones de átomos o iones, por lo que los procesos de ionización son endotérmicos y los valores de EI siempre son positivos. Para los átomos más grandes, el electrón más suelto se localiza más lejos del núcleo y por tanto es más fácil de remover. Así, a medida que aumenta el tamaño (radio atómico), la energía de ionización debe disminuir. 
 
 Dentro de un período, la EI1 generalmente aumenta con el aumento de Z. Hacia abajo en un grupo, el valr de EI1 generalmente disminuye con el aumento de Z. Sin embargo, hay algunas desviaciones sistemáticas de esta tendencia. Observe que la energía de ionización del boro (número atómico 5) es menor que la del berilio (número atómico 4) aunque la carga nuclear del boro sea mayor por un protón. Esto se puede explicar porque la energía de las subcapas aumenta a medida que l aumenta, debido a la penetración y el apantallamiento. Dentro de cualquier capa, los electrones s tienen menor energía que los electrones p. Esto significa que un electrón s es más difícil de remover de un átomo que un electrón p en la misma capa. El electrón removido durante la ionización del berilio ([He]2ss2) es un electrón s, mientras que el electrón removido durante la ionización del boro ([He]2s22p1) es un electrón p; esto resulta en una primera energía de ionización más baja para el boro, aunque su carga nuclear sea mayor en un protón. Por lo tanto, vemos una pequeña desviación de la tendencia prevista que ocurre cada vez que comienza una nueva subcapa.
 
 Otra desviación ocurre cuando los orbitales se llenan más de la mitad. La primera energía de ionización para el oxígeno es ligeramente inferior a la del nitrógeno, a pesar de la tendencia de los valores de EI1 a aumentar a lo largo de un período. Para el oxígeno, la remoción de un electrón eliminará la repulsión electrón-electrón causada por el apareamiento de los electrones en el orbital 2p y dará lugar a un orbital medio-lleno (que es energéticamente favorable). Cambios análogos ocurren en períodos sucesivos.
 
 Quitar un electrón de un catión es más difícil que quitar un electrón de un átomo neutro debido a la mayor atracción electrostática al catión. De la misma manera, eliminar un electrón de un catión con una carga positiva más alta es más difícil que eliminar un electrón de un ión con una carga más baja. Así, las energías de ionización sucesivas para un elemento siempre aumentan. Como se ve en la Tabla 1, hay un gran aumento en las energías de ionización para cada elemento. Este salto corresponde a la remoción de los electrones centrales, que son más difíciles de remover que los electrones de valencia. Por ejemplo, tanto Sc como Ga tienen tres electrones de valencia, por lo que el rápido aumento de la energía de ionización ocurre después de la tercera ionización.
 
 Tabla 1: Energías de ionización sucesivas para elementos seleccionados (kJ/mol)
 
 <table style="margin-left: auto; margin-right: auto;">
 <tbody style="border: 1px solid black;">
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Elemento</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">EI1</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">EI2</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">EI3</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">EI4</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">EI5</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">EI6</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">EI7</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">K</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">418,8</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">3051,8</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">4419,6</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">5876,9</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">7975,5</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">9590,6</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">11343</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Ca</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">589,8</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">1145,4</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">4912,4</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">6490,6</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">8153,0</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">10495,7</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">12272,9</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Sc</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">633,1</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">1235,0</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">2388,7</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">7090,6</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">8842,9</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">10679,0</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">13315,0</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Ga</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">578,8</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">1979,4</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">2964,6</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">6180</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">8298,7</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">10873,9</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">13594,8</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Ge</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">762,2</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">1537,5</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">3302,1</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">4410,6</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">9021,4</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">No disponible</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">No disponible</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">As</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">944,5</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">1793,6</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">2735,5</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">4836,8</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">6042,9</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">12311,5</td>
 <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">No disponible</td>
 </tr>
 </tbody>
 </table>
 
 Este texto es adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/6-5-periodic-variations-in-element-properties">OpenStax Química 2e, Sección 6.5: Variaciones Periódicas en las Propiedades de los Elementos.</a>

Energía de Ionización

La cantidad de energía requerida para eliminar el electrón más débilmente unido de un átomo gaseoso en su estado fundamental se denomina su primera energía de ionización ...

Education

Educación

JoVE Core

Química

Periodic Properties of the Elements

Propiedades periódicas de los elementos

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

ionization energy trends in the periodic table

Ionization energy is the energy needed to remove an electron from a gaseous atom or ion in its ground state. The first ionization energy, or IE1, removes the most loosely bound electron and forms a 1+ cation. The second ionization energy, IE2, removes the next electron, and each later ionization energy removes another electron from the atom or ion.

Ionization always requires energy, so these processes are endothermic. That means ionization energy values are always positive. In general, larger atoms have lower ionization energy because their outermost electrons are farther from the nucleus and easier to remove.

Across a period, first ionization energy generally increases as atomic number increases. Down a group, first ionization energy generally decreases as atomic number increases. The trend is useful, but there are some clear exceptions.

One exception appears when a new subshell begins. Boron has a lower first ionization energy than beryllium, even though boron has one more proton. This happens because s electrons are lower in energy than p electrons in the same shell, so the s electron in beryllium is harder to remove than the p electron in boron. The effect comes from penetration and shielding.

Another exception appears when a p subshell becomes more than half filled. Oxygen has a slightly lower first ionization energy than nitrogen. Removing one electron from oxygen reduces electron-electron repulsion in the 2p orbital and gives a more stable half-filled orbital.

Successive ionization energies always increase. It is harder to remove an electron from a cation than from a neutral atom because the positive charge pulls more strongly on the remaining electrons. It is even harder to remove an electron from a cation with a higher positive charge.

The large jump in successive ionization energies shows when core electrons begin to be removed. Core electrons are harder to remove than valence electrons. For example, scandium and gallium both have three valence electrons, so the sharp rise in ionization energy comes after the third ionization. The table of values for K, Ca, Sc, Ga, Ge, and As shows this pattern clearly.

Ionization Energy Trends in the Periodic Table

periodic classification of the elements

How Valence Electrons Shape the Periodic Table

The periodic table organizes elements by increasing atomic number, and it also shows why elements in the same group behave alike. As the electron configurations are placed into the table, a repeating pattern appears in the outer shells of atoms. These outer electrons are called valence electrons, and they play the biggest role in chemical reactions. They are the highest-energy electrons in an atom, so they are easier to lose or share than core electrons. Valence electrons also help determine...

ionization energy

Ionization energy is the energy needed to remove an electron from a gaseous atom or ion in its ground state. The first ionization energy, or IE1, removes the most loosely bound electron and forms a 1+ cation. The second ionization energy, IE2, removes the next electron, and each later ionization energy removes another electron from the atom or ion. Ionization always requires energy, so these processes are endothermic. That means ionization energy values are always positive. In general, larger...

atomic radii and effective nuclear charge

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Periodic Trends in Atomic Size

Periodic trends in atomic size help explain why atoms get larger or smaller across the periodic table. Elements in the same group show similar chemical behavior because they have the same number and arrangement of valence electrons. Across a period, each new element adds one proton to the nucleus and one electron to the valence shell. Down a group, the number of valence electrons stays the same, but the principal quantum number increases by one. Atomic radius is not easy to define with perfect...

ionic radii

How Ionic Charge Changes Ion Size

Ionic radius describes the size of an ion. It changes when an atom gains or loses electrons. Cations are positive ions with fewer electrons than the parent atom, and they are smaller than the atoms they come from. Aluminum shows this pattern clearly. A neutral aluminum atom has a covalent radius of 118 pm, while Al3+ has an ionic radius of 68 pm. When electrons are removed from the outer valence shell, the remaining core electrons feel a stronger effective nuclear charge, or Zeff. That pull...

electron affinity

Electron Affinity Trends on the Periodic Table

Electron affinity is the energy change that happens when a gaseous atom gains an electron and becomes a negative ion, or anion. For many elements, this process releases energy, so the electron affinity value is negative. For some elements, energy must be added instead, so the value is positive. Electron affinity also applies when more than one electron is added. The second electron affinity is the energy change for adding an electron to an anion to make a 2− ion. Later electron affinities...

alkali metals

Alkali Metals: Reactivity Trends

Alkali metals are Group 1 elements with one valence electron. They are soft, shiny metallic solids that are malleable, ductile, and good conductors of heat and electricity. Their melting points are unusually low for metals and drop as you move down the group. Density generally increases down the group, except for potassium. The trend in atomic size helps explain their behavior. Moving from lithium to cesium, each element has a higher principal quantum number, so the outer electron is farther...

halogens

Halogens: Trends and Reactions

Halogens are Group 17 nonmetals that show clear trends in structure and reactivity. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid. Astatine is highly unstable and radioactive, so most of its properties are still unknown because it has a very short half-life. Tennessine is a synthetic element that is also predicted to belong to this group. These elements do not usually exist as single atoms. Instead, they form diatomic molecules, which means...

noble gases

Noble Gases: Sources, Uses, and Reactions

Noble gases are the group 18 elements helium, neon, argon, krypton, xenon, and radon. They were called “noble” because they were once thought to be nonreactive. That idea changed in 1962, when Dr. Neil Bartlett at the University of British Columbia showed that this assumption was not fully correct. These gases occur in very small amounts in the atmosphere. Some natural gas contains 1–2% helium by mass. Helium is separated from natural gas by removing the condensable components, which leaves...

key terms and concepts

Explore first and successive ionization energy, periodic trends, and key exceptions such as boron, oxygen, and the jump to core electrons.

Ionization Energy Trends in the Periodic Table | JoVE K12

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Periodic Table Trends: Atomic Radii, Ionization, and Electronegativity

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Scientific Laws

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Electron Configuration of Multielectron Atoms

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The Periodic Table

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The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

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This process can be either ...

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Electronegativity values of ...

Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

PS.Chm.3.1

Analyze the structure of atoms and isotopes.

Ionization Energy Trends in the Periodic Table

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