Name: periodic table patterns and element groups
Uploaded: 2020-09-03T13:38:25.000Z
Duration: 3 min 25 s
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K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.2.1

The Periodic Table

La tabla periódica de los elementos es una referencia importante en la química para organizar los elementos. La tabla consta de siete filas o periodos, enumeradas de arriba abajo, y dieciocho columnas llamadas grupos o familias. Estos grupos se pueden enumerar de dos formas distintas.El sistema moderno de numeración recomendado por la Unión Internacional de Química Pura y Aplicada, o IUPAC, enumera los grupos del 1 al 18;y el Servicio de Resúmenes Químicos utiliza números romanos y letras para designar dichos grupos. En este último, los elementos representativos se designan con la letra A y los elementos de transición se designan con la letra B.Los elementos en una tabla periódica se ordenan de izquierda a derecha, de arriba abajo y siguiendo el orden ascendente de los números atómicos. Aquellos elementos con propiedades parecidas se incluyen dentro del mismo grupo.Algunos de los grupos tienen nombres comunes. Los elementos del grupo 1, a excepción del hidrógeno, se conocen como metales alcalinos, y los elementos del grupo 2 como metales alcalinotérreos. Todos estos metales son bastante reactivos y se hallan en la naturaleza combinados con otros elementos.Los elementos no metálicos y altamente reactivos del grupo 17 se conocen como halógenos. Los elementos no metálicos y no reactivos del grupo 18 se conocen como gases nobles o inertes. Los elementos se pueden dividir en tres grandes clases:metales, no metales y metaloides.Los metales se agrupan hacia la izquierda y el centro de la tabla periódica y representan la gran mayoría de los elementos. Son buenos conductores de electricidad y calor. Todos son sólidos a temperatura ambiente, a excepción del mercurio, que es líquido.Los metales son brillantes y se pueden aplanar como láminas y alargar como cables. Los metales, al igual que el potasio, tienden a perder electrones para formar cationes, iones con carga positiva, cuando reaccionan con otros elementos. Los no metales se agrupan del lado derecho de la tabla periódica y, por lo general, son malos conductores de calor y electricidad.A temperatura ambiente, algunos son sólidos y otros líquidos y gaseosos. Los no metales tienden a ganar electrones y formar aniones, que son iones de carga negativa, cuando reaccionan con otros elementos. Los metaloides son elementos que se hallan a lo largo de la división entre los metales y los no metales.Son la clase más pequeña de elementos y presentan propiedades combinadas. Todos los metaloides existen en estado sólido a temperatura ambiente. Algunos de ellos, como el silicio y el germanio, por ejemplo, actúan como semiconductores, es decir, que, a diferencia de los metales, su conductividad eléctrica mejora a medida que aumenta la temperatura.A temperatura ambiente, todos los metaloides existen en estado sólido. Los elementos de la tabla periódica a menudo se dividen también en tres categorías según su ubicación:elementos representativos, elementos de transición y elementos de transición interna, siendo estos últimos también conocidos como lantanoides y actinoides, nombres que toman a partir del primer elemento de sus respectivas filas.

la tabla periódica

A medida que los primeros químicos descubrieron más elementos, se dieron cuenta de que varios elementos podrían agruparse por sus comportamientos químicos similares. Uno de estos grupos incluye el litio (Li), el sodio (Na) y el potasio (K). Todos estos elementos son brillantes, conducen bien el calor y la electricidad, y tienen propiedades químicas similares. Una segunda agrupación incluye el calcio (Ca), el estroncio (Sr) y el bario (Ba), que también son brillantes, buenos conductores de calor y electricidad, y tienen propiedades químicas en común. Sin embargo, las propiedades específicas de estas dos agrupaciones son notablemente diferentes entre sí. Por ejemplo, Li, Na y K son mucho más reactivos que Ca, Sr y Ba. Además, Li, Na y K forman compuestos con oxígeno en una proporción de dos de sus átomos por un átomo de oxígeno, mientras que Ca, Sr y Ba forman compuestos con uno de sus átomos por un átomo de oxígeno. El flúor (F), el cloro (Cl), el bromo (Br) y el yodo (I) también presentan propiedades similares entre sí, pero estas propiedades son drásticamente diferentes de las de cualquiera de los elementos anteriores.
 
 Dimitri Mendeleev en Rusia (1869) y Lothar Meyer en Alemania (1870) reconocieron independientemente una relación periódica entre las propiedades de los elementos conocidos en ese momento. Ambos publicaron tablas con los elementos dispuestos según el aumento de la masa atómica. Sin embargo, Mendeleev fue un paso más allá que Meyer; usó su tabla para predecir la existencia de elementos que tendrían propiedades similares al aluminio y al silicio, pero que aún no eran conocidos. Los descubrimientos del galio (1875) y el germanio (1886) proporcionaron un respaldo significativo al trabajo de Mendeleev. Aunque Mendeleev y Meyer tuvieron una larga disputa sobre la prioridad, las contribuciones de Mendeleev al desarrollo de la tabla periódica son ahora más ampliamente reconocidas.
 
 Para el siglo XX, se hizo evidente que la relación periódica implicaba números atómicos más que masas atómicas. La declaración moderna de esta relación, la ley periódica, establece lo siguiente: las propiedades de los elementos son funciones periódicas de sus números atómicos. Una tabla periódica moderna organiza los elementos en orden creciente de sus números atómicos y agrupa átomos con propiedades similares en la misma columna vertical. Cada cuadro representa un elemento y contiene su número atómico, símbolo, masa atómica media y (a veces) su nombre. 
 
 Los elementos se organizan en siete filas horizontales, denominadas períodos o series y 18 columnas verticales, denominadas grupos. Los grupos se etiquetan en la parte superior de cada columna. Para que la tabla quepa en una sola página, partes de dos de las filas, un total de 14 columnas, se escriben normalmente debajo del cuerpo principal de la tabla.
 
 Muchos elementos difieren significativamente en sus propiedades químicas y físicas, pero algunos elementos son similares en su comportamiento. Por ejemplo, muchos elementos parecen brillantes, son maleables y dúctiles, y conducen bien el calor y la electricidad. Otros elementos no son brillantes, maleables o dúctiles, y son malos conductores de calor y electricidad. Los elementos se pueden clasificar en grandes clases con propiedades comunes: metales (elementos brillantes, maleables, buenos conductores de calor y electricidad — amarillo sombreado); no metales (elementos que parecen apagados, malos conductores de calor y electricidad — rojo sombreado); y los metaloides (elementos que conducen el calor y la electricidad moderadamente bien, y poseen algunas propiedades de metales y algunas propiedades de los no metales — púrpura sombreado).
 
 <img alt="Figure1" src="https://www.jovecore.com/CDNSource/lessons/806/806_Image_1_white.png" style="width: 700px;" />
 
 Los elementos también se pueden clasificar en los elementos del grupo principal (o elementos representativos) en las columnas etiquetadas 1, 2 y 13–18; los metales de transición en las columnas etiquetadas 3–12; y los metales de transición internos en las dos filas en la parte inferior de la tabla. Los elementos de la fila superior en la parte inferior de la tabla son lantanos y los elementos de la fila inferior son actínidos. Los elementos pueden subdividirse aún más por propiedades más específicas, como la composición de los compuestos que forman. Por ejemplo, los elementos del grupo 1 (la primera columna) forman compuestos que consisten en un átomo del elemento y un átomo de hidrógeno. Estos elementos (excepto el hidrógeno) se conocen como metales alcalinos y todos tienen propiedades químicas similares. Los elementos del grupo 2 (la segunda columna) forman compuestos que consisten en un átomo del elemento y dos átomos de hidrógeno: Estos son llamados metales alcalinotérreos, con propiedades similares entre los miembros de ese grupo. 
 
 Otros grupos con nombres específicos son los pnictógenos (grupo 15), los calcógenos (grupo 16), los halógenos (grupo 17) y los gases nobles (grupo 18, también conocidos como gases inertes). Los grupos también pueden ser denominados por el primer elemento del grupo: Por ejemplo, los calcógenos pueden ser llamados el grupo del oxígeno o la familia del oxígeno. El hidrógeno es un elemento único, no metálico, con propiedades similares a los elementos del grupo 1 y del grupo 17. Por esa razón, el hidrógeno puede mostrarse en la parte superior de ambos grupos o solo.
 
 El elemento 43 (tecnecio), el elemento 61 (prometio) y la mayoría de los elementos con número atómico 84 (polonio) y superior tienen su masa atómica entre corchetes. Esto se hace para elementos que consisten enteramente en isótopos radiactivos inestables (la radiactividad se trata con más detalle en el capítulo de química nuclear). No se puede determinar un peso atómico promedio para estos elementos porque sus radioisótopos pueden variar significativamente en abundancia relativa, dependiendo de la fuente, o puede que ni siquiera existan en la naturaleza. El número entre corchetes es el número de masa atómica, que es una masa atómica aproximada del isótopo más estable de ese elemento.
 
 Texto adaptado de<a href="https://openstax.org/books/chemistry-2e/pages/2-5-the-periodic-table"> Openstax, Química 2e, Sección 2.5: La Tabla Periódica.</a>

La Tabla Periódica

A medida que los primeros químicos descubrieron más elementos, se dieron cuenta de que varios elementos podían agruparse por sus comportamientos químicos similares. Uno de esos grupos ...

Education

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Atoms and Elements

Átomos y elementos

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

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 in a 2-to-1 atom ratio. The calcium group is less reactive, and its elements form oxygen compounds in a 1-to-1 atom ratio. Fluorine, chlorine, bromine, and iodine also share similar properties, but those properties are very different from the metal groups above.

Dimitri Mendeleev in Russia and Lothar Meyer in Germany both recognized this repeating pattern in the elements in the 1860s and 1870s. They arranged the known elements by increasing atomic mass. Mendeleev went further by predicting elements that had not yet been discovered. He expected elements with properties similar to aluminum and silicon. Later, gallium and germanium were discovered, and they supported his work. Mendeleev and Meyer later disputed who deserved priority, but Mendeleev is now more widely recognized for helping develop the periodic table.

By the twentieth century, scientists saw that the pattern depends on atomic number, not atomic mass. The periodic law says that the properties of the elements change in a repeating way as atomic number increases. A modern periodic table follows this rule. It places elements in order of increasing atomic number and groups elements with similar properties in the same vertical column.

Each box on the periodic table shows one element. It usually includes the atomic number, symbol, average atomic mass, and sometimes the name. The table has seven horizontal rows, called periods, and 18 vertical columns, called groups. The group labels appear at the top. To fit the table on one page, parts of two rows are often shown below the main table. These 14 columns belong to the lanthanides and actinides.

Elements can also be sorted by their physical properties. Metals are shiny, malleable, and ductile, and they conduct heat and electricity well. Nonmetals are usually dull and are poor conductors. Metalloids fall between these two groups. They conduct heat and electricity moderately well and have some properties of metals and some of nonmetals. The table also separates main-group elements in columns 1, 2, and 13 through 18, transition metals in columns 3 through 12, and inner transition metals in the two rows at the bottom.

Some groups have special names based on their chemistry. Group 1 elements, except hydrogen, are alkali metals. They form compounds with one atom of the element and one atom of hydrogen. Group 2 elements are alkaline earth metals, and they form compounds with one atom of the element and two atoms of hydrogen. Other named groups include the pnictogens, chalcogens, halogens, and noble gases. The chalcogens are also called the oxygen family. Hydrogen is unusual because it is a nonmetal with properties similar to both group 1 and group 17. It may appear at the top of either group or by itself.

Some elements have atomic masses shown in square brackets. This includes element 43, technetium, element 61, promethium, and most elements with atomic number 84 and higher, such as polonium. These elements are made entirely of unstable, radioactive isotopes. Because their isotopes can vary in abundance or may not occur naturally, an average atomic weight cannot be given. The bracketed value is the mass number of the most stable isotope, which is an approximate atomic mass.

Periodic Table Patterns and Element Groups

periodic-table-patterns-and-element-groups

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

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...

the periodic table

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 groups elements by repeating patterns, atomic number, and chemical behavior, including metals, nonmetals, groups, and special names.

Periodic Table Patterns and Element Groups | JoVE K12

chemistry

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Physical Science

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Pennsylvania State Academic Standards

Chemical Reactions

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Louisiana Student Standards for Science

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Matter And Its Interactions

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Ohio’s Learning Standards and Model Curriculum

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New Jersey Student Learning Standards for Science

Matter and Its Interactions

Alabama Course of Study Science

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New York State Science Learning Standards

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Periodic Table Trends

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Periodic Table Trends: Atomic Radii, Ionization, and Electronegativity

Scientific Laws and Theories

Scientific Laws

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The Scientific Method

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Classifying Matter by Composition

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Subatomic Particles

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Elements: Chemical Symbols and Isotopes

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PS.Chm.1.1

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Types of Radioactivity

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Nuclear Binding Energy

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Radioactive Decay and Radiometric Dating

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Nuclear Fission

Many heavier elements with smaller binding energies per nucleon can decompose into more stable elements that have intermediate mass numbers and larger ...

Nuclear Power

Controlled nuclear fission reactions are used to generate electricity. Any nuclear reactor that produces power via the fission of uranium or plutonium by ...

Nuclear Fusion

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Nuclear Transmutation

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Use models to compare nuclear reactions including alpha decay, beta decay and gamma decay; nuclear fusion and nuclear fission.

PS.Chm.1.2

Atomic Orbitals

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The Pauli Exclusion Principle

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The Energies of Atomic Orbitals

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The Aufbau Principle and Hund's Rule

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Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the ...

Use models to explain how electrons are distributed in atoms.

PS.Chm.1.3

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 ...

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

Atomic Mass

Atoms &mdash; and the protons, neutrons, and electrons that compose them &mdash; are extremely small. For example, a carbon atom weighs less than 2 ...

Molar Mass

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Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

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Atomic Radii and Effective Nuclear Charge

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Ionic Radii

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Ionization Energy

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Electron Affinity

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PS.Chm.2.2

Types of Chemical Bonds

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Lewis Symbols and the Octet Rule

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Ionic Bonding and Electron Transfer

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The Born-Haber Cycle

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Covalent Bonding and Lewis Structures

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Electronegativity

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Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

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Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

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.

Periodic Table Patterns and Element Groups

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