Name: electron sea model in metals
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 2 min 32 s
Channel: JoVE

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.2.1

Bonding in Metals

Une liaison métallique est une liaison entre deux atomes métalliques. Par rapport aux non-métaux, les métaux ont de faibles énergies d'ionisation, ce qui leur permet de perdre facilement des électrons de valence. Cela donne à la liaison métallique des propriétés distinctes contrairement aux liaisons ioniques et covalentes.Les liaisons métalliques et la plupart de leurs propriétés peuvent être expliquées en utilisant le modèle mer électronique simple. Considérez le potassium métallique. En raison de la faible énergie d'ionisation, chaque atome de potassium peut facilement perdre son électron de valence pour devenir un cation.Ces cations de potassium sont maintenus ensemble dans l'emballage étroit en raison de leur attraction à la mer chargée négativement des électrons. Ces électrons ne sont pas confinés à un seul ion, mais sont répartis uniformément et relativement libres de se déplacer à l'intérieur du métal. Le modèle electron mer tient compte de plusieurs caractéristiques importantes des métaux.Par exemple, lorsqu'une différence de tension est appliquée à un fil métallique, comme un fil de cuivre, les électrons chargés négativement se déplacent librement vers l'extrémité positive du fil, générant un courant électrique. C'est pourquoi la plupart des métaux sont d'excellents conducteurs d'électricité. En revanche, les composés ioniques sont des non-conducteurs d'électricité sous leur forme solide, mais peuvent conduire l'électricité lorsqu'ils sont dissous dans l'eau.C'est parce que, dans une liaison ionique cristalline, les électrons sont transférés du métal au non-métal, mais restent localisés à un ion. Cependant, lorsqu'ils sont dissous dans l'eau, les cations et les anions se dissocient et peuvent se déplacer lorsqu'ils sont soumis à une différence de potentiel créant un courant électrique. Les métaux sont également d'excellents conducteurs thermiques.Selon le modèle electron mer, lorsque la chaleur est appliquée à une extrémité du métal, les électrons se déplacent librement et dispersent rapidement la chaleur dans tout le métal. Les métaux peuvent facilement être pilés en feuilles en raison de leur malléabilité ou en fils en raison de la propriété de ductilité. Comme il n'y a pas de liaisons localisées dans les métaux, les atomes de métal peuvent glisser l'un au-delà de l'autre, ce qui permet une déformation facile.Les électrons s'écoulent ensuite dans la nouvelle forme pour s'adapter à la déformation.

liaisons des métaux

Les liaisons métalliques se forment entre deux atomes de métaux. Paul Drüde a conçu un modèle simplifié pour décrire la liaison métallique, appelé le “ modèle de la mer d’électrons ”.  
 
 <h4>Modèle de la mer d'électrons </h4>
 
 La plupart des atomes de métaux ne possèdent pas assez d'électrons de valence pour permettre une liaison ionique ou covalente. Cependant, les électrons de valence dans les atomes de métaux sont maintenus de façon lâche, en raison de leur faible électronégativité ou attraction avec le noyau. L'énergie d'ionisation des atomes de métaux (l'énergie nécessaire pour enlever un électron de l'atome) est faible, ce qui facilite l'arrachement facile des électrons de valence de l'atome parent. L'atome forme un ion métallique chargé positivement, tandis que les électrons externes libres existent sous la forme de nuages d'électrons délocalisés chargés négativement. Ces électrons peuvent être mis en commun avec plusieurs cations métalliques voisins grâce à une force intense d'attraction entre ces espèces chargées négativement et positivement. Une telle force d'attraction entre les électrons chargés négativement et les cations métalliques est appelée liaison métallique, maintenant les atomes ensemble. Ce modèle de la mer d'électrons tient compte de la plupart des propriétés physiques des métaux, comme la conductance à la chaleur et à l'électricité, les points de fusion et d'ébullition élevés, la malléabilité et la ductilité. 
 
 <h4>Solides métalliques </h4>
 
 Le modèle de la mer d'électrons tient compte de plusieurs propriétés métalliques, dont la conductivité thermique et électrique élevée, l'éclat métallique, la ductilité et la malléabilité. Les électrons délocalisés peuvent conduire à la fois l'électricité et la chaleur d'une extrémité du métal à l'autre avec une résistance faible. La liaison métallique ne se trouve pas entre deux atomes de métaux précis, mais entre les ions métalliques et de nombreux électrons délocalisés, ce qui permet aux métaux de se déformer sous la pression et à la chaleur sans se briser ni casser. Différents métaux, comme le fer, le mercure ou le cuivre, présentent des propriétés physiques différentes, reflétant la différence de la  force des liaisons métalliques qui existe entre les métaux. 
 
 Les solides métalliques tels que les cristaux de cuivre, d'aluminium et de fer sont formés par les atomes des métaux : tous présentent une conductivité thermique et électrique élevée, un éclat métallique et une malléabilité. Beaucoup sont très durs et assez solides. En raison de leur malléabilité (la capacité de se déformer sous la pression ou le martelage), ils ne se brisent pas et, par conséquent, font des matériaux de construction utiles. Les points de fusion des métaux varient considérablement. Le mercure est un liquide à température ambiante et les métaux alcalins fondent en dessous de 200 °C. Plusieurs métaux de post-transition ont également des points de fusion bas, alors que les métaux de transition fondent à des températures supérieures à 1000 °C. Ces différences reflètent les différences de la force de la liaison métallique qui existent entre les métaux. 
 
 Ce texte est adapté de <a href="https://openstax.org/books/chemistry-2e/pages/10-5-the-solid-state-of-matter">Openstax, Chimie 2e, Section 10.5 : L'état solide de la matière.</a>

Liaisons des métaux

Des liaisons métalliques se forment entre deux atomes métalliques. Un modèle simplifié pour décrire le collage métallique a été développé par Paul Drüde, appelé le ...

Education

Enseignement

JoVE Core

Chemistry

Chimie

Chemical Bonding: Basic Concepts

Liaisons chimiques : concepts de base

KEY TERMS AND CONCEPTS

TERMES ET CONCEPTS CLÉS

electron sea model in metals

Electron sea model explains how metallic bonding holds metals together. In this model, most metal atoms do not have enough valence electrons to form ionic or covalent bonds in the usual way. Their valence electrons are held loosely because metals have low electronegativity, and their ionization energy is low, so electrons are removed easily.

When a metal atom loses these outer electrons, it becomes a positively charged metal ion. The freed electrons form a delocalized electron cloud around many neighboring metal cations. Metallic bonds are the attractive forces between the negative electrons and the positive ions. These bonds do not link just two atoms. They connect metal ions to many shared electrons throughout the solid.

This electron sea model helps explain the main properties of metallic solids. Delocalized electrons carry heat and electricity with low resistance, so metals are good conductors. Metals also have metallic luster, high melting and boiling points, ductility, and malleability. Because the bonding is spread through the structure, metals can deform under pressure or heat without shattering or breaking.

Different metals can have different physical properties because their metallic bond strength is not the same. Examples of metallic solids include copper, aluminum, and iron crystals, and all show high thermal and electrical conductivity, luster, and malleability. Many metals are very hard and strong, which makes them useful as construction materials. Their melting points also vary widely. Mercury is liquid at room temperature, alkali metals melt below 200 °C, several post-transition metals melt at low temperatures, and transition metals often melt above 1000 °C. These differences reflect changes in metallic bonding strength.

Electron Sea Model in Metals

types of chemical bonds

Chemical Bonding and Bond Properties

Chemical bonding explains how atoms and ions join to form molecules and compounds. American chemist Gilbert N. Lewis pioneered chemical bonding theory with the Lewis model. This model helps explain why bonds form, why some are stronger than others, and why compounds have fixed formulas like H2O instead of H4O. Ionic bonding involves ions, which are atoms or molecules with an electrical charge. A cation is a positive ion formed when a neutral atom loses one or more electrons from its valence...

the born-haber cycle

Predicting Ionic Stability with Lattice Energy

Lattice energy helps explain why ionic compounds are stable. It measures the strength of attraction between positive and negative ions in a crystal. In one common definition, lattice energy is the energy required to separate one mole of an ionic solid into gaseous ions, so it has a positive value. Another definition uses the opposite sign and describes the energy released when gaseous ions form a lattice. When checking data, it is important to confirm which convention is being used. In either...

lewis symbols and the octet rule

Valence Electrons, Lewis Symbols, and Bonding

Chemical bonds form when atoms or ions interact in ways that lower the potential energy of a molecule. Gilbert N. Lewis created a simple model to show bond formation using valence electrons, the electrons in the outer shell. In this model, electrons are shared or transferred to help atoms reach a stable electron configuration. The Lewis model helps describe two common bond types. An ionic bond forms when electrons move from a metal to a nonmetal. A covalent bond forms when two nonmetals share...

electronegativity

Electronegativity and Polar Bonds

Electronegativity helps explain why some covalent bonds are nonpolar and others are polar covalent. It is a measure of how strongly an atom attracts shared electrons toward itself. That pull controls how electron density is distributed in a bond. Linus Pauling proposed the first electronegativity values by studying bond energies in heteronuclear molecules such as hydrogen fluoride. He expected the bond energy of HF to be about the average of the bond energies of H2 and F2, or 296 kJ/mol. The...

ionic bonding and electron transfer

Ionic Compounds and Crystal Lattices

Ionic compounds form when positive and negative ions attract each other. A cation is a positive ion, and it forms when an atom loses one or more valence electrons. An anion is a negative ion, and it forms when an atom gains one or more valence electrons. Compounds made of these ions are called ionic compounds, or salts, and the force between them is an ionic bond. The properties of ionic solids help show how strong this attraction is. They usually form rigid, brittle crystals and have high...

trends in lattice energy: ion size and charge

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

Lattice Energy Patterns in Ionic Solids

Lattice energy shows how strongly ions hold an ionic solid together. It is the energy required to separate one mole of a solid into its gaseous ions. For sodium chloride, this process requires 769 kJ per mole. The opposite convention may also be used, where lattice energy is the energy released when gaseous ions form the solid. In either case, a larger magnitude means a more stable ionic compound. For ionic crystals, lattice energy follows a pattern based on charge and ion size. The...

covalent bonding and lewis structures

Shared Electrons in Covalent Molecules

Covalent molecules form when atoms share electrons instead of transferring them. This bonding usually happens between nonmetal atoms with similar tendencies to attract electrons. Because the atoms pull on the electrons in a shared way, the bond is held together by mutual attraction. Covalent compounds often have physical properties that differ from ionic compounds. The attraction between neutral molecules is weaker than the attraction between charged ions. As a result, many covalent compounds...

bond polarity, dipole moment, and percent ionic character

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How Bond Polarity Shapes Molecular Dipoles

Bond polarity depends on electronegativity, the ability of an atom to attract shared electrons. The absolute value of the electronegativity difference, or ΔEN, gives a rough guide to bond type. When the difference is very small or zero, the bond is covalent and nonpolar. When it is larger, the bond may be polar covalent or ionic. Examples show how this works in real compounds. H–H has a ΔEN of 0, so it is nonpolar. H–Cl has a ΔEN of 0.9, so it is polar covalent. Na–Cl has a ΔEN of 2.1, so it...

lewis structures of molecular compounds and polyatomic ions

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

Drawing Lewis Structures with Valence Electron Counts

Drawing Lewis structures starts with counting valence electrons and building the atom arrangement step by step. Valence electrons are the outer-shell electrons that help show how atoms bond. For ions, a positive charge means one electron is removed for each plus sign, and a negative charge means one electron is added for each minus sign. The next step is to sketch the skeleton structure. The least electronegative atom usually goes in the center, while hydrogen is almost never central. Fluorine...

resonance

Resonance Forms in Lewis Structures

Resonance forms in Lewis structures help explain molecules and ions that cannot be shown correctly with just one drawing. In nitrite ion, NO2−, the Lewis structure can be drawn in two ways. The N-O and N=O bonds switch positions in the two drawings, but the atoms stay in the same arrangement. If nitrite really had one single bond and one double bond, the two bond lengths should be different. A double bond is shorter and stronger than a single bond between the same atoms. Experiments show that...

formal charges

Lewis Structures with Formal Charge

Lewis structures can sometimes show more than one reasonable arrangement for a molecule or polyatomic ion. Formal charge helps chemists choose the best Lewis structure when that happens. It is a useful way to compare possible structures in chemistry. Formal charge is the hypothetical charge an atom would have if bonding electrons were shared evenly between the atoms. It can also be found by starting with the valence electrons of the neutral atom, subtracting the nonbonding electrons, and then...

exceptions to the octet rule

Octet Rule Exceptions in Lewis Structures

Some covalent molecules do not follow the octet rule in their Lewis structures. Their central atoms can fall into three groups: odd-electron molecules, electron-deficient molecules, and hypervalent molecules. These cases show why a Lewis structure may not always give every atom eight valence electrons. Odd-electron molecules have an odd number of valence electrons, so one electron remains unpaired. Molecules with an odd number of electrons are called radicals. Nitric oxide, NO, is one example,...

bond energies and bond lengths

How Bond Energy Predicts Reaction Heat

Bond energy helps explain why molecules stay together and how much heat a reaction may release or absorb. A covalent bond is stronger when more energy is needed to separate the atoms. The energy needed to break one specific covalent bond in one mole of gaseous molecules is called bond energy, or bond dissociation energy. For a diatomic molecule, bond energy is the standard enthalpy change for an endothermic reaction that breaks that bond. The H-H bond is a common example. Its bond energy is...

bonding in metals

Electron sea model explains how metallic bonding holds metals together. In this model, most metal atoms do not have enough valence electrons to form ionic or covalent bonds in the usual way. Their valence electrons are held loosely because metals have low electronegativity, and their ionization energy is low, so electrons are removed easily. When a metal atom loses these outer electrons, it becomes a positively charged metal ion. The freed electrons form a delocalized electron cloud around...

key terms and concepts

Learn how the electron sea model explains metallic bonding, conductivity, malleability, luster, and why metals like mercury, copper, and iron differ.

Electron Sea Model in Metals | JoVE K12

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Pennsylvania State Academic Standards

Structure and Properties of Matter

3.2.9-12.B

3.2.9-12.N

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Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Bonding and compounds

Structure And Properties Of Matter

Chemical bonding

Physical Geology

Minerals

Chemical bonding (ionic, covalent, metallic)

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CH.3

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Physics

PH.9

PH.9.e

Arizona Science Standards

High School

HS.P1

HS.P1U1.2

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New Jersey Student Learning Standards for Science

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Motion and Stability: Forces and Interactions

HS-PS2-6

Alabama Course of Study Science

9-12.C.2.2.c

Next Generation Science Standards

Matter and Its Interactions

HS-PS1-4

Florida Department of Education

SC.912.P.8

SC.912.P.8.6

Texas Essential Knowledge and Skills

Chemistry and Physics

IPC.7

IPC.7.A

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Georgia Standards of Excellence

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Molecular Structures in Material Design

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 ...

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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 ...

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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

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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 ...

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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

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

PS.PSc.1.5

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 ...

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

Understand types, properties, and structure of matter.

Electron Sea Model in Metals

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