Name: predicting ion charges on the periodic table
Uploaded: 2020-09-03T13:38:25.000Z
Duration: 3 min 27 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

Physical Science

Matter and its Interactions

PS.PSc.1.5

Ions and Ionic Charges

Los átomos son partículas neutras con la misma cantidad de protones y electrones. Un elemento se define por el número de protones, el cual no cambia;sin embargo, muchos átomos pueden ganar o perder uno o más electrones para convertirse en una partícula cargada. Cuando un átomo o una molécula gana o pierde electrones, se le llama ion.Dado que los electrones tienen mucha menos masa que los protones, no contribuyen de forma significativa a la masa atómica. Por consiguiente, la masa atómica de un ion es básicamente la misma que la masa atómica del átomo neutro. Cuando los átomos o moléculas pierden electrones, se les llama cationes.Los cationes poseen una carga positiva porque tienen más protones, cuya carga es positiva, que electrones, cuya carga es negativa. A los cationes se les coloca el mismo nombre del elemento precedido de la palabra catión"Un átomo de calcio tiene 20 protones y 20 electrones. Pierde dos electrones para convertirse en un catión calcio con 20 protones y 18 electrones.Como ahora tiene dos cargas positivas más en comparación con las cargas negativas, posee una carga total de 2. El símbolo químico de un ion se escribe como el símbolo químico del átomo con la carga señalada en el superíndice derecho. El símbolo químico de un catión calcio, por lo tanto, se escribe Ca2+Cuando los átomos o moléculas ganan electrones, se les llama aniones.Los aniones tienen carga negativa porque poseen más electrones que protones. Para nombrar a los aniones, se le añade el sufijo uro"al nombre del elemento. Un átomo de flúor tiene 9 protones y 9 electrones.El flúor gana un electrón para convertirse en un fluoruro con 9 protones y 10 electrones. Dado que ahora posee una carga negativa más en comparación con las cargas positivas, tiene una carga total de 1. El símbolo químico del fluoruro se representa como F-Por lo general, el uno se omite en los iones que tienen carga 1 o carga 1.Los átomos pierden o ganan números específicos de electrones cuando forman un ion. Muchas de las cargas de los iones formados por los elementos representativos se pueden predecir usando la tabla periódica. Los metales, que están del lado izquierdo de la tabla periódica, pierden electrones.Los metales alcalinos del grupo 1 pierden un electrón y tienen una carga 1 cuando se transforman en un ion. Los metales alcalinotérreos del grupo 2 pierden dos electrones y tienen una carga 2. Los no metales, que están del lado derecho de la tabla periódica, ganan electrones.Los halógenos del grupo 17 ganan un electrón y tienen una carga 1. Los elementos del grupo 16 ganan dos electrones y tienen una carga 2. Muchos metales de transición pueden formar cationes con distintas cargas.Los gases nobles del grupo 18, por lo general, no forman iones.

<ol>
	<li>Jensen, William B. "La escritura adecuada de las cargas iónicas". Revista de Educación Química 89, no. 8 (2012): 1084-1085.</li>
	<li>Schmid, Roland. "La configuración del gas noble: no la fuerza motriz, sino la regla del juego en química". Revista de educación química 80, no. 8 (2003): 931.</li>
	<li>Gillespie, Ronald J. "Densidades de electrones, cargas atómicas y enlaces iónicos, covalentes y polares". Revista de Educación Química 78, no. 12 (2001): 1688. 
	 </li>
</ol>

iones y cargas iónicas

En las reacciones químicas ordinarias, el núcleo — que contiene los protones y neutrones de cada átomo y, por lo tanto, identifica al elemento — permanece inalterado. Los electrones, sin embargo, pueden ser agregados a los átomos por transferencia de otros átomos, perdidos por transferencia a otros átomos, o compartidos con otros átomos. La transferencia y el intercambio de electrones entre átomos rigen la química de los elementos. Durante la formación de algunos compuestos, los átomos ganan o pierden electrones para formar partículas cargadas eléctricamente llamadas iones.
 
 Cuando un átomo pierde electrones, forma un ión positivo llamado catión. Los cationes tienen más protones que electrones. Asimismo, cuando un átomo gana electrones, forma un ión negativo llamado anión. Los aniones tienen más electrones que los protones.
 
 La tabla periódica ayuda a predecir si un átomo formará un anión o un catión, y también la carga del ión resultante. Moviéndose de la izquierda a la derecha en la tabla periódica, los átomos de metales del grupo principal pierden suficientes electrones para quedarse con el mismo número de electrones que un átomo del gas noble precedente. Forman cationes con una carga igual al número de grupo. Para ilustrar esto, un átomo de un metal alcalino (Grupo 1) pierde un electrón y forma un catión con una carga de 1+; un metal alcalinotérreo (Grupo 2) pierde dos electrones y forma un catión con una carga de 2+, y así sucesivamente. Por ejemplo, un átomo de calcio neutro, con 20 protones y 20 electrones, pierde fácilmente dos electrones. Esto resulta en un catión con 20 protones, 18 electrones y una carga de 2+. Tiene el mismo número de electrones que los átomos del gas noble precedente, argón, y es simbolizado Ca2+. El nombre de un ión metálico es el mismo que el nombre del átomo metálico del que se forma, por lo que Ca2+ se denomina ión de calcio.
 
 Moviéndose desde el extremo derecho a la izquierda en la tabla periódica,  los átomos de elementos no metálicos generalmente ganan suficientes electrones para darles el mismo número de electrones que un átomo del siguiente gas noble en la tabla periódica. Forman aniones con una carga negativa igual al número de grupos que se han desplazado a la izquierda de los gases nobles. Por ejemplo, los átomos de los elementos del grupo 17 (un grupo a la izquierda de los gases nobles) ganan un electrón y forman aniones con una carga de 1−; los átomos de los elementos del grupo 16 (dos grupos a la izquierda) ganan dos electrones y forman iones con una carga de 2−, y así sucesivamente. Por ejemplo, el átomo de bromo neutro, con 35 protones y 35 electrones, puede ganar un electrón para proporcionarle 36 electrones. Esto resulta en un anión con 35 protones, 36 electrones y una carga de 1−. Tiene el mismo número de electrones que los átomos del siguiente gas noble, el criptón, y es simbolizado por Br−.
 
 La tendencia entre la carga del ion y la posición del grupo en la tabla periódica puede ser utilizada como guía en muchos casos. Sin embargo, su valor predictivo disminuye al desplazarse hacia el centro de la tabla periódica. Los metales de transición y algunos otros metales a menudo presentan cargas variables que no son predecibles por su ubicación en la tabla. Por ejemplo, el cobre puede formar iones con una carga de 1+ o 2+, y el hierro puede formar iones con una carga de 2+ o 3+.
 
 Este texto es adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/2-6-molecular-and-ionic-compounds">Openstax, Química 2e, Sección 2.6: Compuestos Moleculares e Iónicos</a>.

Iones y Cargas Iónicas

En las reacciones químicas ordinarias, el núcleo, que contiene los protones y neutrones de cada átomo y, por lo tanto, identifica el elemento, permanece ...

Education

Educación

JoVE Core

Chemistry

Química

Atoms and Elements

Átomos y elementos

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

predicting ion charges on the periodic table

Ion charges can often be predicted from an element’s position on the periodic table. In chemical reactions, the nucleus stays unchanged, but electrons may be transferred, lost, or shared. When atoms gain or lose electrons during compound formation, they become ions, which are electrically charged particles.

A positive ion is called a cation. A cation has more protons than electrons because it lost electrons. A negative ion is called an anion. An anion has more electrons than protons because it gained electrons.

The periodic table gives useful clues about ion charge. Main-group metals on the far left usually lose electrons until they have the same number of electrons as the preceding noble gas. Their cation charge often matches the group number. For example, a Group 1 alkali metal forms a 1+ cation, and a Group 2 alkaline earth metal forms a 2+ cation.

Calcium shows this pattern clearly. A neutral calcium atom has 20 protons and 20 electrons. It can lose two electrons to form Ca2+, which has 20 protons, 18 electrons, and a 2+ charge. This ion has the same number of electrons as argon. The name of the metal ion is the same as the metal atom, so Ca2+ is called a calcium ion.

Nonmetals on the far right usually gain electrons to reach the electron count of the next noble gas. Their anion charge often matches how many groups they are away from the noble gases. Group 17 elements usually gain one electron to form 1− anions, and Group 16 elements usually gain two electrons to form 2− anions.

Bromine is one example. A neutral bromine atom has 35 protons and 35 electrons. It can gain one electron to form Br− with 35 protons, 36 electrons, and a 1− charge. This ion has the same number of electrons as krypton. The trend between group position and ion charge helps in many cases, but it becomes less reliable near the center of the periodic table. Transition metals and some other metals often have variable charges. Copper can form 1+ or 2+ ions, and iron can form 2+ or 3+ ions.

Predicting Ion Charges on the Periodic Table

predicting-ion-charges-on-the-periodic-table

the atomic theory of matter

Dalton’s Laws and Early Atomic Ideas

Dalton’s atomic theory explains matter with atoms, elements, and compounds. It also shows how chemical changes follow simple laws. This idea gave chemistry a microscopic model for what can be seen in the lab. The earliest recorded ideas about matter came from ancient Greek philosophers. Leucippus and Democritus said all matter was made of tiny, finite particles called atomos, meaning “indivisible.” Aristotle and others later argued that matter was made from four elements: fire, earth, air, and...

subatomic particles

Atomic Structure: Protons, Neutrons, and Electrons

Atomic structure is built from three subatomic particles: protons, neutrons, and electrons. Atoms make up all matter, and these particles explain an atom’s mass and charge. The electron was first identified at the end of the 19th century by J.J. Thomson. He used a cathode ray tube, a sealed glass tube with almost all the air removed and two metal electrodes. When high voltage was applied, a visible beam called a cathode ray formed. The beam bent toward positive charge and away from negative...

elements: chemical symbols and isotopes

Reading Element Symbols and Isotope Notation

Chemical symbols and isotope notation help identify elements and their atoms. A chemical symbol is an abbreviation for an element or a single atom of that element. Mercury, for example, is written as Hg. The same symbol can point to one atom in the microscopic domain or to many atoms of the element in a container or sample. Many symbols come from the element’s common English name. Others come from Latin, Greek, or German names. Aluminum uses Al, while iron uses Fe from the Latin word Ferrum.

ions and ionic charges

Ion charges can often be predicted from an element’s position on the periodic table. In chemical reactions, the nucleus stays unchanged, but electrons may be transferred, lost, or shared. When atoms gain or lose electrons during compound formation, they become ions, which are electrically charged particles. A positive ion is called a cation. A cation has more protons than electrons because it lost electrons. A negative ion is called an anion. An anion has more electrons than protons because it...

the periodic table

Periodic Table Patterns and Element Groups

The periodic table organizes elements by repeating patterns in their properties. Chemists first noticed that some elements behaved alike, so they grouped them by chemical behavior. Lithium, sodium, and potassium are one example. They are shiny and conduct heat and electricity well. Calcium, strontium, and barium form another group with similar physical and chemical properties. Yet these two groups are not the same. The lithium group is much more reactive, and its elements form oxygen compounds...

atomic mass

Average Atomic Mass and Isotopes

Average atomic mass explains why many elements on the periodic table have decimal values. Atoms are extremely small, so scientists use the atomic mass unit, or amu, to measure them. A carbon atom weighs less than 2 × 10−23 g, and the amu is defined from carbon-12. One amu is exactly 1/12 the mass of one carbon-12 atom, which is 1.6605 × 10−24 g. The dalton (Da) and the unified atomic mass unit (u) mean the same thing as the amu. For a single atom, atomic mass is usually close to its mass...

molar mass

Mole, Mass, and Avogadro’s Number

The mole links mass and the number of particles in a substance. It gives chemists a standard way to count atoms and molecules in samples that are far too small to see. It also helps show why substances with the same kinds of atoms can still have very different properties, like water, H2O, and hydrogen peroxide, H2O2. The mole is an amount unit, like a pair or a dozen. One mole contains 6.02214076 × 10^23 discrete entities, such as atoms or molecules. This number is usually rounded to 6.022 ×...

key terms and concepts

Learn how the periodic table helps predict cation and anion charges, with examples like calcium, bromine, copper, and iron for grades 9–12.

Predicting Ion Charges on the Periodic Table | JoVE K12

chemistry

JoVE Core Química da vida a los conceptos de química general mediante lecciones de vídeo basadas en animaciones, concisas y fáciles de entender. Además, en los vídeos de científicos en acción, se muestran experimentos de investigación clásicos y originales realizados en laboratorios de todo el mundo.

Louisiana Student Standards for Science

High School

Matter And Its Interactions

HS-PS1-1

motion-and-stability-forces-and-interactions

Motion And Stability: Forces And Interactions

HS-PS2-6

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Atoms

Tennessee Academic Standards

Matter and Its Interactions

CHEM1.PS1.13

Virginia  Standards of Learning

HIgh School

CH.2

CH.2.a

PS.4

PS.4.a

Arizona Science Standards

HS+C.P1

HS+C.P1U1.1

HS.P1

HS.P1U1.2

Alabama Course of Study Science

9-12.C.1.1.a

9-12.C.1.1.b

9-12.PS.3.4

9-12.PS.3.4.d

Florida Department of Education

SC.912.P.8

SC.912.P.8.4

Texas Essential Knowledge and Skills

Chemistry and Physics

IPC.7

IPC.7.A

Georgia Standards of Excellence

SPS1.

Properties of Atoms, Ions, and Isotopes

Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
According to its composition, the matter can be classified into two broad categories &mdash; pure substances and ...

Elements: Chemical Symbols and Isotopes

A chemical symbol is an abbreviation used to indicate an element or an atom of an element. For example, the symbol for mercury is Hg. The same symbol is ...

Molecules and Compounds

Atoms and Molecules

Everything in the universe is made up of matter, and matter is composed of a combination of elements. An atom is the smallest unit of ...

Solution Formation

There is no one solvent that can dissolve every type of solute. Some substances that readily dissolve in a certain solvent might be insoluble in a ...

Colloids

Children at play often make suspensions such as mixtures of mud and water, flour and water, or a suspension of solid pigments in water known as tempera ...

Construct an explanation to classify matter as a pure substance or mixture; homogeneous or heterogeneous; element or compound; solution, colloid or suspension.

PS.PSc.1.1

Phase Transitions

Whether solid, liquid, or gas, a substance&#39;s state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the ...

phase-transitions-vaporization-and-condensation

Phase Transitions: Vaporization and Condensation

The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize ...

Vapor Pressure

When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules move randomly about, they will occasionally ...

Clausius-Clapeyron Equation

The equilibrium between a liquid and its vapor depends on the temperature of the system; a rise in temperature causes a corresponding rise in the vapor ...

Phase Transitions: Melting and Freezing

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy ...

phase-transitions-sublimation-and-deposition

Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and ...

Heating and Cooling Curves

When a substance&#8212;isolated from its environment&#8212;is subjected to heat changes, corresponding changes in temperature and phase of the substance ...

Phase Diagrams

A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. ...

Use models to compare the phases of matter and the physical changes they undergo.

PS.PSc.1.2

physical-and-chemical-properties-of-matter

Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

molecular-comparison-of-gases-liquids-and-solids

Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

comparing-intermolecular-forces-melting-point-boiling-point

Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

Carry out investigations to compare physical and chemical properties of matter.

PS.PSc.1.3

The Atomic Theory of Matter

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

Subatomic Particles

Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

The Bohr Model

Following the work of Ernest Rutherford and his colleagues in the early twentieth century, the picture of atoms consisting of tiny dense nuclei surrounded ...

Emission Spectra

When solids, liquids, or condensed gases are heated sufficiently, they radiate some of the excess energy as light. Photons produced in this manner have a ...

The de Broglie Wavelength

In the macroscopic world, objects that are large enough to be seen by the naked eye follow the rules of classical physics. A billiard ball moving on a ...

The Uncertainty Principle

Werner Heisenberg considered the limits of how accurately one can measure properties of an electron or other microscopic particles. He determined that ...

Use models to interpret the data presented in Bohr diagrams and electron dot diagrams for neutral atoms of elements 1 through 18.

PS.PSc.1.4

In ordinary chemical reactions, the nucleus &mdash; which contains the protons and neutrons of each atom and thus identifies the element &mdash; remains ...

Use models to compare representations of atoms, ions, and isotopes.

The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

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 ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Alkali Metals

Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

Halogens

Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. ...

Noble Gases


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were ...

Use the Periodic Table as a model to predict the relative properties (metallic/nonmetallic character, ionic charge, and reactivity) and arrangement of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.PSc.1.6

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Dr&#xFC;de called the ...

Construct an explanation to classify the type of chemical bond that occurs (covalent, ionic, or metallic) in a given substance.

PS.PSc.2.1

Nomenclature of Alkanes

In the late 19th-century, the number of new chemical compounds discovered increased tremendously. Hence, the necessity arose to develop a naming system ...

Nomenclature of Alkenes

The IUPAC naming system for alkenes replaces -an- with -en- in the corresponding parent alkanes. Accordingly, a simple alkene replaces the -ane suffix of ...

Nomenclature of Alkynes

Alkynes are unsaturated hydrocarbons characterized by the presence of carbon-carbon triple bonds and have a general formula CnH2n-2. The nomenclature of ...

structure-and-nomenclature-of-alcohols-and-phenols

Structure and Nomenclature of Alcohols and Phenols

Overview 
Alcohols are one of the most important functional groups in organic chemistry. The name of alcohol comes from the hydrocarbon from which it is ...

Structure and Nomenclature of Ethers

Structure and Bonding
Ethers are organic compounds with an ether functional group which is characterized by an oxygen atom connected to two &#8212; ...

IUPAC Nomenclature of Aldehydes

Aldehydes are named based on the systematic nomenclature rules set by the IUPAC. For acyclic aldehydes, the longest carbon chain containing the aldehydic ...

Use models to apply International Union of Pure and Applied Chemistry (IUPAC) conventions to name and write formulas for simple compounds.

PS.PSc.2.2

Understand types, properties, and structure of matter.

Predicting Ion Charges on the Periodic Table

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