Name: transition metals in the periodic table
Uploaded: 2020-09-24T15:06:53.000Z
Duration: 2 min 58 s
Channel: JoVE

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-2

Properties of Transition Metals

Os metais de transição são um grupo de elementos localizados no bloco d. São colocados entre os principais elementos do grupo e têm características únicas, tais como como condutividade elétrica, cores, dureza, pontos de fusão alta e magnetismo. Muitas destas características são atribuídas ao preenchimento das orbitais d.Movendo-se através do período, os elétrons são adicionados seguindo o princípio de Aufbau. No entanto, o orbital s mais exterior é preenchido primeiro, antes do elétron entrar na subcapa d, com algumas exceções. O crómio e o cobre têm uma orbital s meia cheia porque é energeticamente mais favorecida por ter uma subcapa d meia cheia ou cheia.O tamanho atómico dos metais de transição diminui ligeiramente ao longo de um período. Á medida que os elétrons entram na subcapa d, o número de elétrons de valência na orbital s mais exterior mantém-se estável, levando a uma carga nuclear constante. Ao fundo da coluna, a tendência aumenta a partir do quarto até ao quinto período, mas não abaixo.O 6º período contém 14 elementos adicionais da série Lantanídea, onde os elétrons entram na subcapa f antes de entrar na subcapa d. Os elétrons localizados nas orbitais f não protegem suficientemente os elétrons de valência na orbital s mais exterior, resultando num aumento da carga nuclear efetiva. Assim, os elétrons de valência são mais fortemente atraídos, levando a rádios atómicos mais pequenos do que o esperado.Isto é conhecido como a Contração de Lantanídea. Da mesma forma, a eletronegatividade dos elementos de transição é influenciada pelo seu tamanho atómico e carga nuclear. Movendo-se através de um período, ele aumenta apenas ligeiramente.Ao fundo da coluna, a eletronegatividade aumenta a partir do quarto até ao quinto período mas permanece constante no sexto período. Isto deve-se a uma diminuição do tamanho atómico e um aumento da carga nuclear. A energia de ionização de metais de transição aumenta ligeiramente ao longo de um período.Curiosamente, ao fundo da coluna, é mais elevado no 6º período do que nos 4º e 5º períodos. Aqui, os elétrons de valência são mantidos mais apertados à medida que a carga nuclear aumenta com um aumento insignificante do tamanho atómico. Finalmente, os metais de transição podem ter uma gama de estados estáveis de oxidação perdendo os elétrons orbitais s mais externos antes dos elétrons orbitais d não emparelhados.As orbitais d parcialmente cheias permitem estados de oxidação que variam entre 7 a 1, cores características, e propriedades magnéticas.

propriedades dos metais de transição

Os metais de transição são definidos como os elementos que têm orbitais d parcialmente preenchidas. Como mostra a Figura 1, os elementos do bloco d nos grupos 3–12 são elementos de transição. Os elementos do bloco f, também chamados metais de transição interna (os lantanídeos e actinídeos), também atendem a esse critério, pois a orbital d é parcialmente preenchida antes das orbitais f.
<img alt="Image1" src="/files/ftp_upload/11454/11454_Image_1.png" style="text-align: center; height: 500px;" />
Figura 1: Tabela Periódica. Os metais de transição estão localizados nos grupos 3–11 da tabela periódica. Os metais de transição interna estão nas duas linhas abaixo do corpo da tabela.
Os elementos do bloco d estão divididos na primeira série de transição (os elementos de Sc a Cu), na segunda série de transição (os elementos de Y a Ag), e na terceira série de transição (o elemento La e os elementos de Hf a Au). O actínio, Ac, é o primeiro membro da quarta série de transição, que também inclui de Rf a Rg.
Os elementos do bloco f são os elementos de Ce a Lu, que constituem a série dos lantanídeos (ou série lantanóide), e os elementos de Th a Lr, que constituem a série dos actinídeos (ou série actinóide). Como o lantânio se comporta muito como os elementos lantanídeos, ele é considerado um elemento lantanídeo, mesmo que a sua configuração eletrónica faça dele o primeiro membro da terceira série de transição. Da mesma forma, o comportamento do actínio significa que ele faz parte da série dos actinídeos, embora a sua configuração eletrónica faça dele o primeiro membro da quarta série de transição.
Os elementos de transição têm muitas propriedades em comum com outros metais. São quase todos sólidos duros, com alto ponto de fusão, que conduzem bem o calor e a eletricidade. Eles formam imediatamente ligas e perdem eletrões para formar catiões estáveis. Além disso, os metais de transição formam uma grande variedade de compostos de coordenação estáveis, nos quais o átomo ou o ião de metal central age como um ácido de Lewis e aceita um ou mais pares de eletrões. Muitas moléculas e iões diferentes podem doar pares solitários ao centro do metal, servindo como bases de Lewis.
Propriedades dos Elementos de Transição
Os metais de transição demonstram uma vasta gama de comportamentos químicos. Alguns metais de transição são agentes de redução fortes, enquanto que outros têm reatividade muito baixa. Por exemplo, os lantanídeos formam todos catiões aquosos 3+ estáveis. A força motriz para tais oxidações é semelhante à dos metais alcalinoterrosos, como Be ou Mg, formando Be2+ e Mg2+. Por outro lado, materiais como platina e ouro têm potenciais de redução muito mais elevados. A sua capacidade de resistir à oxidação torna-os materiais úteis para construir circuitos e jóias.
Iões dos elementos mais leves do bloco d, como Cr3+, Fe3+, e Co2+, formam iões hidratados coloridos que são estáveis em água. No entanto, iões no período imediatamente abaixo destes (Mo3+, Ru3+, e Ir2+) são instáveis e reagem prontamente com o oxigénio do ar. A maioria dos iões simples e estáveis em água formados pelos elementos mais pesados do bloco d são oxianiões como MoO42− e  ReO4−.
Ruténio, ósmio, ródio, irídio, paládio, e platina são os metais da platina. Com dificuldade, formam catiões simples que são estáveis em água e, ao contrário dos elementos anteriores da segunda e terceira série de transição, não formam oxianiões estáveis.
Tanto os elementos do bloco d como do bloco f reagem com não-metais para formar compostos binários; o aquecimento é frequentemente necessário. Estes elementos reagem com halogénios para formar uma variedade de haletos que variam em estado de oxidação de +1 a +6. Com aquecimento, o oxigénio reage com todos os elementos de transição, excepto paládio, platina, prata, e ouro. Os óxidos destes últimos metais podem ser formados utilizando outros reagentes, mas decompõem-se após o aquecimento. Os elementos do bloco f, os elementos do grupo 3, e os elementos da primeira série de transição, com excepção do cobre, reagem com soluções aquosas de ácidos, formando hidrogénio gasoso e soluções dos respectivos sais.
Os metais de transição podem formar compostos com uma vasta gama de estados de oxidação. Alguns dos estados de oxidação observados dos elementos da primeira série de transição são mostrados na Tabela 1. Indo da esquerda para a direita ao longo da primeira série de transição, o número de estados de oxidação comuns aumenta inicialmente para um máximo em direção ao meio da tabela e, em seguida, diminui. Os valores da tabela são valores típicos; existem outros valores conhecidos, e é possível sintetizar novas adições. Por exemplo, em 2014, os investigadores foram bem-sucedidos na síntese de um novo estado de oxidação do irídio (+9).
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<td style="color: black; border: 1px solid black; text-align: center;">21 Sc</td>
<td style="color: black; border: 1px solid black; text-align: center;">22 Ti</td>
<td style="color: black; border: 1px solid black; text-align: center;">23 V</td>
<td style="color: black; border: 1px solid black; text-align: center;">24 Cr</td>
<td style="color: black; border: 1px solid black; text-align: center;">25 Mn</td>
<td style="color: black; border: 1px solid black; text-align: center;">26 Fe</td>
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<td style="color: black; border: 1px solid black; text-align: center;">29 Cu</td>
<td style="color: black; border: 1px solid black; text-align: center;">30 Zn</td>
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Tabela 1. Os metais de transição da primeira série de transição podem formar compostos com diferentes estados de oxidação.
Para os elementos de escândio a manganês (a primeira metade da primeira série de transição), o estado de oxidação mais alto corresponde à perda de todos os eletrões, tanto nas orbitais s como d das suas camadas de valência. O ião de titânio(IV), por exemplo, é formado quando o átomo de titânio perde os seus dois eletrões 3d e dois 4s. Estes estados de oxidação mais elevados são as formas mais estáveis de escândio, titânio e vanádio. No entanto, não é possível continuar a remover todos os eletrões de valência dos metais, à medida que continuamos a percorrer a série. O ferro é conhecido por formar estados de oxidação de +2 a +6, sendo o ferro(II) e o ferro(III) os mais comuns. A maioria dos elementos da primeira série de transição formam iões com uma carga de 2+ ou 3+ que são estáveis em água, embora os dos membros anteriores da série possam ser facilmente oxidados pelo ar.
Os elementos da segunda e terceira série de transição são geralmente mais estáveis em estados de oxidação mais elevados do que os elementos da primeira série. No geral, o raio atómico aumenta ao descer um grupo, o que leva a que os iões da segunda e terceira série sejam maiores do que os da primeira série. A remoção de eletrões de orbitais que se encontram mais longe do núcleo é mais fácil do que a remoção de eletrões perto do núcleo. Por exemplo, o molibdénio e o tungsténio, membros do grupo 6, estão limitados principalmente a um estado de oxidação de +6 em solução aquosa. O crómio, o membro mais leve do grupo, forma iões Cr3+ estáveis em água e, na ausência de ar, iões Cr2+ menos estáveis. O sulfureto com o estado de oxidação mais elevado para o cromo é Cr2S3, que contém o ião Cr3+. Molibdénio e tungsténio formam sulfuretos em que os metais exibem estados de oxidação de +4 e +6.
A variedade de propriedades exibidas pelos metais de transição deve-se às suas camadas de valência complexas. Ao contrário da maioria dos metais do grupo principal onde um estado de oxidação é normalmente observado, a estrutura da camada de valência dos metais de transição significa que eles ocorrem geralmente em vários estados de oxidação estáveis diferentes. Além disso, as transições de eletrões nestes elementos podem corresponder à absorção de fotões no espectro eletromagnético visível, levando a compostos coloridos. Por causa desses comportamentos, os metais de transição exibem uma química rica e fascinante.
Este texto é adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/19-1-occurrence-preparation-and-properties-of-transition-metals-and-their-compounds">Openstax, Chemistry 2e, Chapter 19.1 Occurrence, Preparation, and Properties of Transition Metals and Their Compounds.</a>

Propriedades dos Metais de Transição

Os metais de transição são definidos como aqueles elementos que preencheram parcialmente os orbitais d. Conforme mostrado na Figura 1, os elementos do bloco d nos grupos 3–12 são ...

Education

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Química

Transition Metals and Coordination Complexes

Metais de Transição e Complexos de Coordenação

transition-metals-and-coordination-complexes

KEY TERMS AND CONCEPTS

TERMOS-CHAVE E CONCEITOS

transition metals in the periodic table

Transition metals are the d-block elements and the inner transition metals in the f-block. They are defined by partially filled d orbitals. In the periodic table, the transition elements are in groups 3 through 11, and the inner transition metals appear in the two rows below the main body of the table.

The d-block is often grouped into transition series. The first transition series runs from Sc through Cu. The second series runs from Y through Ag. The third series includes La and Hf through Au, and the fourth series begins with Ac and continues through Rg. The f-block includes Ce through Lu, which make up the lanthanide series, and Th through Lr, which make up the actinide series. Lanthanum and actinium behave like the lanthanides and actinides, so they are included with those series even though their electron configurations place them at the start of the third and fourth transition series.

Transition metals share several common metal properties. Most are hard, high-melting solids that conduct heat and electricity well. They also form alloys easily and lose electrons to make stable cations. Another major feature is their ability to form stable coordination compounds, where the metal atom or ion acts as a Lewis acid and accepts electron pairs from Lewis bases such as molecules or ions with lone pairs.

These elements show a wide range of chemical behavior. Some transition metals are strong reducing agents, while others are much less reactive. The lanthanides, for example, form stable 3+ aqueous cations, and this oxidation is similar in driving force to the formation of Be2+ and Mg2+ by alkaline earth metals. At the other extreme, platinum and gold have high reduction potentials, so they resist oxidation and are useful in circuits and jewelry.

Ion stability also changes across the d-block. Lighter ions such as Cr3+, Fe3+, and Co2+ often form colorful hydrated ions that remain stable in water. The next heavier ions, such as Mo3+, Ru3+, and Ir2+, are unstable and react quickly with oxygen in air. For the heavier d-block elements, many of the water-stable simple ions are oxyanions, such as MoO4 2− and ReO4−. Ruthenium, osmium, rhodium, iridium, palladium, and platinum are called the platinum metals. They form simple cations only with difficulty, and they do not form stable oxyanions like the earlier elements in the second and third transition series.

Transition metals and inner transition metals also react with nonmetals to form binary compounds, and heating is often needed. They react with halogens to make halides in oxidation states from +1 to +6. When heated, oxygen reacts with all transition elements except palladium, platinum, silver, and gold. The oxides of those metals can be made by other reactions, but they break down when heated. The f-block elements, group 3 elements, and the first transition series except copper react with aqueous acids to form hydrogen gas and the matching salts.

A key reason transition metals are so versatile is that they can form compounds in many oxidation states. In the first transition series, scandium through manganese show a rise in the number of common oxidation states, with a maximum near the middle of the series, and then the number falls again. For scandium through manganese, the highest oxidation state usually comes from removing all valence s and d electrons. Titanium(IV), for example, forms when titanium loses its two 3d and two 4s electrons. Iron can form oxidation states from +2 to +6, but +2 and +3 are the most common. Most first-series transition metals form 2+ or 3+ ions that are stable in water, although the early members are easily oxidized by air.

The second and third transition series are usually more stable in higher oxidation states than the first series. Their larger atomic radius makes electron removal easier because the electrons are farther from the nucleus. For example, molybdenum and tungsten, both group 6 elements, are mostly limited to +6 in aqueous solution. Chromium, the lightest member of the group, forms stable Cr3+ ions in water and less stable Cr2+ ions when air is absent. The highest chromium sulfide is Cr2S3, which contains Cr3+, while molybdenum and tungsten form sulfides with +4 and +6 oxidation states.

The many properties of transition metals come from their complex valence shells. Unlike most main group metals, which usually show one oxidation state, transition metals often appear in several stable oxidation states. Their electron transitions can also absorb visible light, which gives many of their compounds color. These features make transition metal chemistry especially varied and important.

Transition Metals in the Periodic Table

properties of transition metals

Transition metals are the d-block elements and the inner transition metals in the f-block. They are defined by partially filled d orbitals. In the periodic table, the transition elements are in groups 3 through 11, and the inner transition metals appear in the two rows below the main body of the table. The d-block is often grouped into transition series. The first transition series runs from Sc through Cu. The second series runs from Y through Ag. The third series includes La and Hf through...

coordination compounds and nomenclature

How Transition Metal Complexes Are Named

Transition metal complexes are named by following rules for ligands, metal ions, and oxidation state. These compounds form when a central metal ion or atom, often a transition metal or inner transition metal, accepts electron pairs from ligands. A ligand is a Lewis base that can be an atom, molecule, or ion with one or more lone pairs to donate. In these complexes, the bond is a coordinate covalent bond. That means both electrons in the bond come from the donor, such as ammonia, and are...

metal-ligand bonds

Coordination Complexes and Chelation

Coordination complexes form when a metal ion bonds to ligands. These compounds appear in familiar examples such as hemoglobin in blood, chlorophyll in green plants, vitamin B-12, and the catalyst used to make polyethylene. Transition metal ions are especially likely to form these complexes. In a coordination complex, the metal acts as a Lewis acid. The ligand acts as a Lewis base and donates both electrons in the coordinate covalent bond. A ligand can be an atom, molecule, or ion, as long as...

coordination number and geometry

Transition Metal Shapes from Coordination Number

Transition metal complexes are often identified by their coordination number and the shape around the metal ion. The coordination number is the number of donor atoms bonded to the central metal. In many complexes, the most common shapes are octahedral, tetrahedral, and square planar. Coordination number and molecular geometry are linked in a clear pattern. A coordination number of 2 gives a linear shape, as in [Ag(NH3)2]+. A coordination number of 3 gives a trigonal planar shape, as in...

structural isomerism

Linkage and Ionization Isomers

Isomers are different chemical species that share the same chemical formula. In coordination compounds, structural isomerism includes linkage isomers and coordination-sphere isomers. These two forms show how the same atoms can be arranged in different ways around a metal center. Linkage isomers form when a ligand can attach to a transition metal through two different atoms. The cyanide ligand, CN−, can bind through carbon or nitrogen. The thiocyanate ligand, SCN−, can bind through sulfur or...

stereoisomerism

Isomer Shapes in Coordination Complexes

Isomer shapes in coordination complexes can change a compound’s properties even when the chemical formula stays the same. Isomers are different chemical species with the same formula. In transition metal complexes, the atoms stay connected through the same types of bonds, but their arrangement in space can differ. One common form is geometric isomerism. In these complexes, ligands (the ions or molecules attached to the metal) can sit in cis or trans positions. The octahedral [Co(NH3)4Cl2]+ ion...

valence bond theory

Metal Ligand Bonds in Coordination Complexes

Coordination complexes form metal-ligand bonds through valence bond theory. In this model, Linus Pauling explained bonding with hybridization and overlap of atomic orbitals. The central metal atom or ion acts as a Lewis acid. It uses empty orbitals of suitable energy to accept electron pairs from ligands, which act as Lewis bases. These coordinate covalent bonds help explain the color, geometry, and magnetic behavior seen in coordination compounds. The type of hybridization helps determine the...

crystal field theory - octahedral complexes

crystal-field-theory-octahedral-complexes

Octahedral d-Orbital Splitting in Crystal Fields

Crystal field theory explains how ligands affect the d orbitals in transition metal complexes. This electrostatic model helps predict the colors, magnetic behavior, and some structures of coordination compounds. It focuses on the nonbonding electrons on the central metal ion, not on the metal-ligand bonds. In crystal field theory, the metal ion and ligands are treated as very small point charges. Because electrons are negative, electrons donated by the ligands repel the electrons in the...

crystal field theory - tetrahedral and square planar complexes

crystal-field-theory-tetrahedral-and-square-planar-complexes

Crystal Field Splitting in Non-Octahedral Shapes

Crystal field theory also explains d orbital splitting in tetrahedral and square planar complexes. These shapes do not follow the same pattern as an octahedral complex, so the d orbitals respond to ligand placement in different ways. In tetrahedral complexes, the four ligands sit between the axes. None of the d orbitals points directly at the ligands, but the d x2−y2 and d z2 orbitals lie along the Cartesian axes and overlap less with the ligands than the d xy, d xz, and d yz orbitals. The d...

colors and magnetism

Color and Spin in Coordination Complexes

Color in coordination complexes comes from how metal electrons absorb light. When atoms or molecules absorb light at the right frequency, electrons move to higher-energy orbitals. For many main-group atoms and molecules, the absorbed light is ultraviolet and cannot be seen. In coordination compounds, the energy gap between d orbitals often matches visible light, so the compound can absorb and emit colors that the human eye detects. Small changes in orbital energy can cause large shifts in the...

key terms and concepts

Learn where transition metals and inner transition metals are found, why they form many oxidation states, and how their ions, compounds, and colors differ.

Transition Metals in the Periodic Table | JoVE K12

chemistry

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9-12

Physical Geology

Minerals

properties-minerals-hardness-luster-cleavage-streak-crystal-shape

Properties of minerals (hardness, luster, cleavage, streak, crystal shape, fluorescence, flammability, density/specific gravity, malleability)

Minnesota Academic Standards in Science

3.1.1 9C.3.1.1.1

Alabama Course of Study Science

Earth and Space Science

Earth's Systems

9-12.ESS.2.6

Environmental Science

Earth and Human Activity

9-12.EVS.4.7

south-carolina-college-and-career-ready-science-standards

South Carolina College and Career Ready Science Standards

Matter and Its Interactions

C-PS1-2

new-york-state-science-learning-standards

New York State Science Learning Standards

Physical Science

HS. Structure and Properties of Matter

HS-PS2-6.

Georgia Standards of Excellence

SC1.

electron-configuration-and-chemical-properties

Electron Configuration and Chemical Properties

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 ...

the-periodic-table-and-organismal-elements

The Periodic Table And Organismal Elements

Atomic Structure

The Greek philosopher Democritus proposed that everything on Earth is made up of tiny particles called atomos, Greek for &#34;indivisible,&#34; from which ...

Electron Configurations

Electron configurations and orbital diagrams can be determined by applying the Aufbau principle (each added electron occupies the subshell of lowest ...

Electronic Structure of Atoms


An atom comprises protons and neutrons, which are contained inside the dense, central&#160;core called the nucleus, with electrons present around the ...

electron-configuration-of-multielectron-atoms

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 ...

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 ...

The Aufbau Principle and Hund's Rule

To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and ...

Coulomb's Law

Experiments with electric charges have shown that if two objects each have an electric charge, they exert an electric force on each other. The magnitude ...

Electric Charges

From lightning during thunderstorms to electronic devices, the phenomenon of electromagnetism is all around us. The electromagnetic force is one of the ...

sources-and-properties-of-electric-charge

Sources and Properties of Electric Charge

All objects we see around us consist of atoms, which combine to form molecules. The lightest element in the universe is hydrogen, and a hydrogen atom ...

Types of Forces

In most situations, forces can be grouped into two categories: contact forces and field forces.&#160; Contact forces occur as a result of direct physical ...

Electric Fields

Source: Yong P. Chen, PhD, Department of Physics &#38; Astronomy, College of Science, Purdue University, West Lafayette, IN
An electric field is generated ...

Intermolecular Forces

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

Van der Waals Interactions

Atoms and molecules interact with each other through intermolecular forces. These electrostatic forces arise from attractive or repulsive interactions ...

Chemical Bonds


Atoms participate in a chemical bond formation&#160;to acquire a completed valence-shell electron configuration similar to that of the noble gas nearest ...

Electron Behavior

Electrons are negatively charged subatomic particles attracted to and orbit around the positively-charged nucleus of an atom. They reside in spaces ...

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 ...

Ions and Ionic Charges

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

Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level and the composition of the nucleus of atoms.  Clarification Statement: Chemistry: Examples of properties that could be predicted from patterns could include reactivity of metals, types of bonds formed, numbers of bonds formed, atomic radius, atomic mass, or reactions with oxygen. Emphasis is on main group elements and qualitative understanding of the relative trends of ionization energy and electronegativity.

HS-PS1-1

Transition metals are defined as those elements that have partially filled d orbitals. As shown in Figure 1, the d-block elements in groups 3&#8211;12 are ...

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 ...

Chemical Reactions

A chemical reaction is a process by which the bonds in the atoms of substances are rearranged to generate new substances. Matter cannot be created or ...

Chemical Equations

Chemical equations represent the identities and relative quantities of substances involved in a chemical reaction. The substances undergoing reaction are ...

Introduction to Chemical Reactions

All chemical reactions begin with a reactant, the general term for one or more substances entering the reaction. Sodium and chloride ions, for example, ...

Temperature Dependence on Reaction Rate

The Collision Theory
Atoms, molecules, or ions must collide before they can react with each other. Atoms must be close together to form chemical bonds. ...

stoichiometry-product-yield-and-limiting-reactants

Stoichiometry, Product Yield, and Limiting Reactants

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Preparation of 25% v/v Ethylenediamine in Deionized WaterExpand
	Here, we show the laboratory ...

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 ...

Dynamic Equilibrium

A reversible chemical reaction represents a chemical process that proceeds in both forward (left to right) and reverse (right to left) directions. When ...

Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.  Clarification Statement: Chemistry: Examples of chemical reactions could include the reaction of sodium and chlorine, carbon and oxygen, or carbon and hydrogen. Reaction classification aids in the prediction of products (e.g. synthesis, decomposition, single displacement, double displacement, and acid-base).

Intermolecular vs Intramolecular Forces

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

comparison-between-electrical-and-gravitational-forces

Comparison Between Electrical And Gravitational Forces

There are four fundamental forces in nature: the gravitational force, the electromagnetic force, the strong nuclear force, and the weak nuclear force. To ...

intermolecular-forces-and-physical-properties

Intermolecular Forces and Physical Properties



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

electric-field-of-two-equal-and-opposite-charges

Electric Field of Two Equal and Opposite Charges

Atoms generally contain the same number of positively and negatively charged particles, protons, and electrons. Hence, they are electrically neutral. ...

Electric Field

Consider two point charges, each exerting Coulomb force on the other. It is possible to describe the Coulomb interaction via an intermediate step by ...

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 ...

Electric Dipoles and Dipole Moment

Consider two charges of equal magnitude but opposite signs. If they cannot be separated by an external electric field, the system is called a permanent ...

Plan and conduct an investigation to gather evidence to compare the structure of substances at the macroscale to infer the strength of electrical forces between particles.  Clarification Statement: Emphasis is on understanding the strengths of forces between particles, not on naming specific intermolecular forces (such as dipole-dipole). Examples of particles could include ions, atoms, molecules, and network solids (such as graphite). Examples of macro-properties of substances could include the melting point and boiling point, vapor pressure, and surface tension.

HS-PS1-3

bond-dissociation-energy-and-activation-energy

Bond Dissociation Energy and Activation Energy

Bond energy is the energy required to break a bond homolytically. These values are usually expressed in units of kcal/mol or kJ/mol and are referred to as ...

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

Coupled Reactions

Cellular processes such as building and breaking down complex molecules occur through stepwise chemical reactions. Some of these chemical reactions are ...

energy-diagrams-transition-states-and-intermediates

Energy Diagrams, Transition States, and Intermediates

Free-energy diagrams, or reaction coordinate diagrams, are graphs showing the energy changes that occur during a chemical reaction. The reaction ...

What is Metabolism?

Overview

Metabolism represents all of the chemical activity in a cell, including reactions that build molecules (anabolism) and those that break ...

types-of-chemical-reactions-anabolic-and-catabolic

Types of Chemical Reactions: Anabolic and Catabolic

The first law of thermodynamics holds that energy can neither be created nor destroyed&#8212;it can only change form. An organism&#39;s essential function ...

Non-equilibrium in the Cell

An important concept in studying metabolism and energy is that of chemical equilibrium. Most chemical reactions are reversible. They can proceed in both ...

Activation Energy

Activation energy is the minimum amount of energy necessary for a chemical reaction to move forward. The higher the activation energy, the slower the rate ...

Energy Transfer in Chemical Reactions

Chemical reactions require sufficient energy to cause the matter to collide with enough precision and force that old chemical bonds can be broken and new ...

factors-influencing-the-rate-of-chemical-reactions

Factors Influencing the Rate of Chemical Reactions

A variety of factors influence the rate of chemical reactions. For a chemical reaction to happen, atoms must collide with enough energy to overcome the ...

Predicting Reaction Outcomes

Kinetics describes the rate and path by which a reaction occurs. In contrast, thermodynamics deals with state functions and describes the properties, ...

States of Matter and Phase Changes

The internal energy of a substance&#8212;the total kinetic energy of all its molecules and the potential energy of their associated forces&#8212;depends ...

Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.  Clarification Statement: Emphasis is on the idea that a chemical reaction is a system that affects the energy change.  Examples of models could include molecular-level drawings and diagrams of reactions, graphs showing the relative energies of reactants and products, and representations showing energy is conserved.

HS-PS1-4

Transition Metals in the Periodic Table

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