Name: coordination complexes and chelation
Uploaded: 2020-09-24T15:06:53.000Z
Duration: 2 min 51 s
Channel: JoVE

K12 Standards

new-york-state-science-learning-standards

New York State Science Learning Standards

High School

Physical Science

HS. Structure and Properties of Matter

HS-PS2-6.

Metal-Ligand Bonds

I composti di coordinazione sono specie neutre costituite da un complesso neutro, o da ioni complessi caricati, e da controioni con carica opposta. Lo ione complesso è uno ione metallico centrale legato a molecole o ioni noti come ligandi. I ligandi sono composti con una o più coppie di elettroni.

Agiscono come basi di Lewis donando una coppia di elettroni allo ione metallico, che agisce come un acido di Lewis, per formare un legame covalente coordinato. Insieme, costituiscono una sfera di coordinamento. Nel 1893, Alfred Werner propose una teoria della coordinazione per spiegare perché specifiche molecole stabili reagissero e violassero la teoria della valenza per formare composti di coordinazione.

Studiando vari complessi cobalto-ammoniaca, Werner ipotizzò che l'atomo di metallo centrale esibisse due tipi di interazioni di valenza. La valenza primaria è il numero di ossidazione del metallo centrale, mentre la valenza secondaria è il numero di ligandi legati a esso, definito anche numero di coordinazione. Pertanto, se il numero di ligandi limitati diminuisce, i controioni possono legarsi direttamente allo ione metallico, mantenendo la valenza secondaria.

La teoria della coordinazione di Werner è usata oggi per scrivere formule chimiche di composti di coordinazione. Iniziate con il simbolo dello ione metallico, quindi elencate tutti i ligandi in ordine alfabetico. Mettete le parentesi quadre intorno allo ione complesso ed elencate i controioni per ultimi.

Usate pedici numerici per indicare il numero di ligandi e controioni coinvolti. Per una nomenclatura sistematica dei composti di coordinazione, innanzitutto, date un nome agli ioni complessi. Iniziate elencando i ligandi in ordine alfabetico.

Un ligando anionico termina con la lettera o, mentre un ligando neutro è indicato dal suo nome molecolare con poche eccezioni come acqua e ammina. Usate prefissi greci come di-tri-o tetra-per indicare il numero di ligandi. Se un prefisso è già presente nel nome del ligando, alternare i prefissi a bis-tri-o tetrakis-con il nome del ligando tra parentesi.

Quindi nominate il nome del metallo e il suo stato di ossidazione utilizzando numeri romani tra parentesi. Nel caso di un complesso anionico, il nome del metallo ha il suffisso ate. Infine, il composto di coordinazione è nominato aggiungendo prima il nome del catione, seguito dall'anione.

Pertanto, i due composti di coordinazione sono chiamati amminaclorobis(etilendiammina)cobalto(III)bromuro e diaquatetraclorocobaltato di ammonio(III)d parzialmente riempiti consentono stati di ossidazione compresi fra 7 e 1, colori caratteristici e proprietà magnetiche.

legami metallo-legante

L'emoglobina nel sangue, la clorofilla nelle piante verdi, la vitamina B-12 e il catalizzatore utilizzato nella produzione del polietilene contengono tutti composti di coordinazione. È probabile che gli ioni dei metalli, in particolare dei metalli di transizione, formino complessi.

In questi complessi, i metalli di transizione formano legami covalenti coordinati, una sorta di interazione acido-base di Lewis in cui entrambi gli elettroni nel legame vengono forniti da un donatore (base di Lewis) a un accettore di elettroni (acido di Lewis). L'acido di Lewis nei complessi di coordinazione, spesso chiamato ione metallico centrale (o atomo), è il metallo di transizione o metallo di transizione interna. I donatori di basi di Lewis, chiamati ligandi, possono essere un'ampia varietà di sostanze chimiche- atomi, molecole o ioni. L'unico requisito è che abbiano una o più coppie di elettroni, che possono essere donate al metallo centrale. Molto spesso, ciò coinvolge un atomo donatore con una coppia solitaria di elettroni che può formare un legame coordinato con il metallo. La sfera di coordinazione è costituita dallo ione o atomo metallico centrale più i suoi ligandi attaccati. Le parentesi in una formula racchiudono la sfera di coordinazione; le specie fuori parentesi non rientrano nella sfera di coordinamento.

I ligandi sono monodentati, dal greco “con un dente”, quando si collegano al metallo centrale attraverso un solo atomo. Qui il numero di ligandi e il numero di coordinazione sono uguali. I ligandi con un atomo donatore, come NH_3, Cl^− e H_2O, sono ligandi monodentati. Molti altri ligandi si coordinano al metallo in modi più complessi.

I ligandi bidentati sono quelli in cui due atomi si coordinano al centro metallico. Ad esempio, l'etilendiammina (en, H_2NCH_2CH_2NH_2) contiene due atomi di azoto, ciascuno dei quali ha una coppia solitaria e può fungere da base di Lewis (Figura 1a). Entrambi gli atomi possono coordinarsi ad un singolo centro metallico. Nel complesso [Co(en)_3]^3+, ci sono tre ligandi bidentati e il numero di coordinazione dello ione cobalto(III) è sei (Figura 1b). I numeri di coordinazione più comuni sono due, quattro e sei, ma sono noti esempi di tutti i numeri di coordinazione da 1 a 15.

<img alt="Image1" src="/files/ftp_upload/11456/11456_Image_1.svg" style="text-align: center; height: 200px;" />

Figure 1. (a) l'etilendiammina (en) contiene due atomi di azoto, con una coppia solitaria ciascuno, che possono coordinarsi con uno ione metallico. (b) Tre ligandi bidentati si coordinano con un singolo ione cobalto.

Qualsiasi ligando che si lega a uno ione metallico centrale tramite più di un atomo donatore è un ligando polidentato (o “molti denti”) perché può mordere il centro metallico con più di un legame. Per descrivere questo tipo di interazione viene utilizzato anche il termine chelato, dal greco “artiglio”. Molti ligandi polidentati sono ligandi chelanti e un complesso costituito da uno o più di questi ligandi e un metallo centrale è un chelato. Un ligando chelante è anche noto come agente chelante. Un ligando chelante trattiene lo ione metallico proprio come la chela di un granchio trattiene una biglia. I ligandi polidentati sono talvolta identificati con prefissi che indicano il numero di atomi donatori nel ligando. Il complesso eme nell'emoglobina è un altro esempio importante (Figura 2). Contiene un ligando polidentato con quattro atomi donatori che si coordinano con il ferro.

<img alt="Image2" src="/files/ftp_upload/11456/11456_Image2.svg" style="text-align: center; height: 200px;" />

Figure 2: Il singolo ligando eme contiene quattro atomi di azoto che si coordinano con il ferro nell'emoglobina per formare un chelato.

Questo testo è adattato da <a href="https://openstax.org/books/chemistry-2e/pages/19-2-coordination-chemistry-of-transition-metals">Openstax, Chemistry 2e, Chapter 19.2 Coordination Chemistry of Transition Metals</a>.

Legami metallo-legante

L'emoglobina nel sangue, la clorofilla nelle piante verdi, la vitamina B-12 e il catalizzatore utilizzato nella produzione del polietilene contengono ...

Education

Didattica

JoVE Core

Chemistry

Chimica

Transition Metals and Coordination Complexes

Metalli di transizione e complessi di coordinazione

transition-metals-and-coordination-complexes

KEY TERMS AND CONCEPTS

TERMINI E CONCETTI CHIAVE

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 it has one or more electron pairs to share with the metal. The central metal ion or atom, along with its attached ligands, makes up the coordination sphere. Brackets in a formula show the coordination sphere, and anything outside the brackets is not part of it.

Ligands can bind in different ways. Monodentate ligands connect through only one atom, so the number of ligands equals the coordination number. Common examples are NH3, Cl−, and H2O. Bidentate ligands bind through two atoms. Ethylenediamine, or en, has two nitrogen atoms with lone pairs that can both bond to one metal center. In the complex [Co(en)3]3+, three bidentate ligands give cobalt(III) a coordination number of six.

Ligands that attach through more than one donor atom are called polydentate ligands. The word chelate comes from a Greek word meaning “claw,” and it describes how these ligands hold a metal ion. A complex with one or more chelating ligands is called a chelate, and a chelating ligand is also called a chelating agent. These ligands can be identified with prefixes that show the number of donor atoms they use.

The heme complex in hemoglobin is another key example. Heme is a single polydentate ligand with four donor atoms, and all four coordinate to iron. Coordination numbers in complexes are often 2, 4, or 6, but examples from 1 to 15 are known. These bonding patterns help explain the structure of many important metal-containing compounds.

Coordination Complexes and Chelation

properties of transition metals

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...

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 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

Explore coordination complexes, ligand types, coordination numbers, and chelation using examples like hemoglobin, chlorophyll, and heme for high school chemistry.

Coordination Complexes and Chelation | JoVE K12

chemistry

JoVE Core: Chimica illustra concetti chiave di chimica attraverso video animazioni concise e di immediata comprensione. Inoltre, i video della sezione "scienziati in azione" mostrano procedure metodologiche realizzate da ricercatori provenienti dai migliori laboratori internazionali.

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 ...

Electron Orbital Model

Orbitals are the areas outside of the atomic nucleus where electrons are most likely to reside. They are characterized by different energy levels, shapes, ...

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 ...

Coordination Chemistry Complexes

Source: Laboratory of Dr. Neal Abrams &#8212; SUNY College of Environmental Science and Forestry
Transition metals are found everywhere from vitamin ...

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 of atoms.

HS-PS1-1.

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 ...

Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

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 ...

The Born-Haber Cycle

Lattice Energy&#xA0;

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

trends-in-lattice-energy-ion-size-and-charge

Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

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 ...

Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity.&#xA0;

Electronegativity values of ...

bond-polarity-dipole-moment-and-percent-ionic-character

Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

The absolute value of the difference in electronegativity (&Delta;EN) of two bonded atoms provides a rough measure of the polarity to be ...

lewis-structures-of-molecular-compounds-and-polyatomic-ions

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 ...

Resonance

The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

Formal Charges

In some cases, there are seemingly more than one valid Lewis structures for molecules and polyatomic ions. The concept of formal charges can be used to ...

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:


	...

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 ...

VSEPR Theory and the Basic Shapes

Overview of VSEPR Theory

Valence shell electron-pair repulsion theory (VSEPR theory) enables us to predict the molecular structure, including approximate ...

vsepr-theory-and-the-effect-of-lone-pairs

VSEPR Theory and the Effect of Lone Pairs

Effect of Lone Pairs of Electrons&nbsp;on Molecule Geometry

It is important to note that electron-pair geometry around a central atom is not the same ...

Predicting Molecular Geometry

VSEPR Theory for Determination of Electron Pair Geometries

The following procedure uses VSEPR theory to determine the electron pair geometries and the ...

Molecular Shape and Polarity

Dipole Moment of a Molecule

Polar covalent bonds connect two atoms with differing electronegativities, leaving one atom with a partial positive charge ...

Valence Bond Theory

Overview of Valence Bond Theory

Valence bond theory describes a covalent bond as the overlap of half-filled atomic orbitals (each containing a single ...

Hybridization of Atomic Orbitals I

The mathematical expression known as the wave function, &#x3C8;, contains information about each orbital and the wavelike properties of electrons in an ...

Hybridization of Atomic Orbitals II

sp3d and sp3d&nbsp;2 Hybridization

To describe the five bonding orbitals in a trigonal bipyramidal arrangement, we must use five of the valence shell ...

Molecular Orbital Theory I

Overview of Molecular Orbital Theory

Molecular orbital theory describes the distribution of electrons in molecules in the same way as the distribution of ...

Molecular Orbital Theory II

Molecular Orbital Energy Diagrams

The relative energy levels of atomic and molecular orbitals are typically shown in a molecular orbital diagram. For a ...

Molecular Orbital (MO) Theory

Source: Tamara M. Powers, Department of Chemistry, Texas A&#38;M University
This protocol serves as a guide in the synthesis of two metal complexes ...

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 ...

Molecular and Ionic 
Solids

Crystalline solids are divided into four types: molecular, ionic, metallic, and covalent network based on the type of constituent units and their ...

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, ...

Plan and conduct an investigation to gather evidence to compare the structure of substances at the bulk scale to infer the strength of electrical forces between particles.

HS-PS1-3.

Radioactivity and Nuclear Equations

Nuclear chemistry is the study of reactions that involve changes in nuclear structure. The nucleus of an atom is composed of protons and, except for ...

Types of Radioactivity

The most common types of radioactivity are &#945; decay, &#946; decay, &#947; decay, neutron emission, and electron capture.
Alpha (&#945;) decay is the ...

Nuclear Stability

Protons and neutrons, collectively called nucleons, are packed together tightly in a nucleus. With a radius of about 10&#8722;15 meters, a nucleus is ...

Nuclear Binding Energy

The difference between the calculated and experimentally measured masses is known as the mass defect of the atom. In the case of helium-4, the mass defect ...

Radioactive Decay and Radiometric Dating

Radioactivity is a spontaneous disintegration of an unstable nuclide and is a random process, as all the nuclei in the sample do not decay simultaneously. ...

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

The process of converting very light nuclei into heavier nuclei is also accompanied by the conversion of mass into large amounts of energy, a process ...

Nuclear Transmutation

Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with ...

Biological Effects of Radiation

All radioactive nuclides emit high-energy particles or electromagnetic waves. When this radiation encounters living cells, it can cause heating, break ...

determining-rate-laws-and-the-order-of-reaction

Determining Rate Laws and the Order of Reaction

Source: Laboratory of Dr. Neal Abrams &#8212; SUNY College of Environmental Science and Forestry
All chemical reactions have a specific rate defining the ...

Develop models to illustrate the changes in the composition of the nucleus of the atom and the energy released during the processes of fission, fusion, and radioactive decay.

HS-PS1-8.

Properties of Transition Metals

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 ...

Coordination Compounds and Nomenclature

In most main group element compounds, the valence electrons of the isolated atoms combine to form chemical bonds that satisfy the octet rule. For ...

The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain ...

Coordination Number and Geometry

For transition metal complexes, the coordination number determines the geometry around the central metal ion. Table 1 compares coordination numbers to ...

physical-properties-of-minerals-i-crystals-and-cleavage

Physical Properties Of Minerals I: Crystals and Cleavage

Source: Laboratory of Alan Lester - University of Colorado Boulder
The physical properties of minerals comprise various measurable and discernible ...

physical-properties-of-minerals-ii-polymineralic-analysis

Physical Properties Of Minerals II: Polymineralic Analysis

Source: Laboratory of Alan Lester - University of Colorado Boulder
The physical properties of minerals include various measurable and discernible ...

Porosimetry of a Silica Alumina Powder

Source: Kerry M. Dooley and Michael G. Benton, Department of Chemical Engineering, Louisiana State University, Baton Rouge, LA
Surface area and pore size ...

Structures of Solids

Solids in which the atoms, ions, or molecules are arranged in a definite repeating pattern are known as crystalline solids. Metals and ionic compounds ...

Le Ch&#226;telier's Principle

Source: Laboratory of Dr. Lynne O&#39;Connell &#8212; Boston College
When the conditions of a system at equilibrium are altered, the system responds in ...

Communicate scientific and technical information about why the particulate-level structure is important in the functioning of designed materials.

definition-measurement-pressure-atmospheric-pressure-barometer

Definition and Measurement of Pressure: Atmospheric Pressure, Barometer, and Manometer

Gas pressure is caused by force exerted by gas molecules colliding with the surfaces of objects. Although the force of each collision is very small, any ...

gas-laws-boyle-s-gay-lussac-charles-avogadro-s-and-ideal-gas-law

Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law

Through experiments, scientists established the mathematical relationships between pairs of variables, such as pressure and temperature, pressure and ...

applications-of-the-ideal-gas-law-molar-mass-density-and-volume

Applications of the Ideal Gas Law: Molar Mass, Density, and Volume

The volume occupied by one mole of a substance is its molar volume. The ideal gas law, PV = nRT, &nbsp;suggests that the volume of a given quantity of gas ...

mixtures-of-gases-dalton-s-law-of-partial-pressures-and-mole-fractions

Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions

Unless individual gases chemically react with each other, the individual gases in a mixture of gases do not affect each other&rsquo;s pressure. Each gas ...

chemical-stoichiometry-gases-using-ideal-gas-law-to-determine

Chemical Stoichiometry and Gases: Using Ideal Gas Law to Determine Moles

Chemical stoichiometry describes the quantitative relationships between reactants and products in chemical reactions.

In addition to measuring quantities ...

Analyze data to support the claim that the combined gas law describes the relationships among volume, pressure, and temperature for a sample of an ideal gas.

HS-PS1-9.

Coordination Complexes and Chelation

Description

Transcript

Tags

More videos by Standards