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

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.2.1

Bonding in Metals

Eine Metallbindung ist eine Bindung zwischen zwei Metallatomen. Im Vergleich zu Nichtmetallen haben Metalle niedrige Ionisierungsenergien, wodurch sie leicht Valenzelektronen verlieren können. Dies verleiht der Metallbindung im Gegensatz zu ionischen und kovalenten Bindungen unterschiedliche Eigenschaften.Metallische Bindungen und die meisten ihrer Eigenschaften können mit Hilfe des Elektronen-wolkenmodells erklärt werden. Betrachten Sie das Metall Kalium. Aufgrund der niedrigen Ionisierungsenergie kann jedes Kaliumatom leicht sein Valenzelektron verlieren und zu einem Kation werden.Diese Kalium-Kationen werden in einem engem Gitter zusammengehalten, da sie vom negativ geladenen Elektronen angezogen werden. Diese Elektronen sind nicht auf ein einzelnes Ion beschränkt, sondern sind gleichmäßig verteilt und können sich im Metall relativ frei bewegen. Das Modell der Elektronenwolke berücksichtigt mehrere wichtige Eigenschaften von Metallen.Wenn beispielsweise eine Spannungsdifferenz an einen Metalldraht, wie Kupferdraht, angelegt wird, bewegen sich die negativ geladenen Elektronen frei zum positiven Ende des Drahtes hin und erzeugen einen elektrischen Strom. Aus diesem Grund sind die meisten Metalle ausgezeichnete elektrische Leiter. Im Gegensatz dazu sind ionische Verbindungen in ihrer festen Form nicht elektrisch leitend, können aber Elektrizität leiten, wenn sie in Wasser gelöst sind.Das liegt daran, dass bei einer festen Ionenverbindung Elektronen vom Metall auf das Nichtmetall übertragen werden, aber auf ein Ion beschränkt bleiben. Wenn sie jedoch in Wasser gelöst werden, dissoziieren die Kationen und Anionen und können sich bewegen, wenn sie einer Potentialdifferenz ausgesetzt werden, wodurch ein elektrischer Strom erzeugt wird. Metalle sind auch ausgezeichnete Wärmeleiter.Nach dem Elektronenwolken-Modell, wenn an einem Ende des Metalls Wärme angelegt wird, bewegen sich die Elektronen frei und verteilen die Wärme schnell im Metall. Metalle können aufgrund ihrer Verformbarkeit leicht zu Blechen oder aufgrund ihrer Duktilitätseigenschaft zu Drähten verarbeitet werden. Da es in Metallen keine festen Bindungen gibt, können die Metallatome aneinander vorbeigleiten und sich leicht verformen.Elektronen fließen dann in die neue Form, um sich der Verformung anzupassen.

bindung in metallen

Zwischen zwei Metallatomen entstehen metallische Bindungen. Ein vereinfachtes Modell zur Beschreibung metallischer Bindungen wurde von Paul Drüde mit dem Namen „Electron Sea Model“ entwickelt. <h4>Elektronenmeermodell</h4> Die meisten Metallatome verfügen nicht über genügend Valenzelektronen, um eine ionische oder kovalente Bindung einzugehen. Allerdings werden die Valenzelektronen in Metallatomen aufgrund ihrer geringen Elektronegativität oder Anziehung zum Kern lose gehalten. Die Ionisierungsenergie von Metallatomen (Energie, die erforderlich ist, um ein Elektron aus dem Atom zu entfernen) ist niedrig, was die einfache Entfernung von Valenzelektronen aus dem Mutteratom erleichtert. Das Atom bildet ein positiv geladenes Metallion, während die freien Außenelektronen als negativ geladene delokalisierte Elektronenwolken vorliegen. Diese Elektronen können durch eine starke Anziehungskraft zwischen diesen negativ und positiv geladenen Spezies von mehreren benachbarten Metallkationen gemeinsam genutzt werden. Eine solche Anziehungskraft zwischen den negativ geladenen Elektronen und Metallkationen nennt man Metallbindungen und hält die Atome zusammen. Dieses Elektronenmeermodell berücksichtigt die meisten physikalischen Eigenschaften von Metallen, wie etwa die Wärme- und Elektrizitätsleitfähigkeit, hohe Schmelz- und Siedepunkte, Formbarkeit und Duktilität. <h4>Metallische Feststoffe</h4> Das Elektronenmeermodell berücksichtigt mehrere metallische Eigenschaften, darunter hohe thermische und elektrische Leitfähigkeit, metallischen Glanz, Duktilität und Formbarkeit. Die delokalisierten Elektronen können sowohl Strom als auch Wärme mit geringem Widerstand von einem Ende des Metalls zum anderen leiten. Die metallische Bindung besteht nicht zwischen zwei bestimmten Metallatomen, sondern zwischen Metallionen und vielen delokalisierten Elektronen, wodurch sich Metalle unter Druck und Hitze verformen können, ohne zu zersplittern oder zu brechen. Verschiedene Metalle wie Eisen, Quecksilber oder Kupfer unterscheiden sich in ihren physikalischen Eigenschaften, was auf die unterschiedliche metallische Bindungsstärke zwischen den Metallen zurückzuführen ist. Metallische Feststoffe wie Kristalle aus Kupfer, Aluminium und Eisen werden durch Metallatome gebildet: Sie alle weisen eine hohe thermische und elektrische Leitfähigkeit, metallischen Glanz und Formbarkeit auf. Viele sind sehr hart und ziemlich stark. Aufgrund ihrer Formbarkeit (der Fähigkeit, sich unter Druck oder Hämmern zu verformen) zersplittern sie nicht und sind daher nützliche Baumaterialien. Die Schmelzpunkte der Metalle variieren stark. Quecksilber ist bei Raumtemperatur flüssig und die Alkalimetalle schmelzen unterhalb von 200 °C. Einige Post-Übergangsmetalle haben auch niedrige Schmelzpunkte, während die Übergangsmetalle bei Temperaturen über 1000 °C schmelzen. Diese Unterschiede spiegeln Unterschiede in der Stärke der metallischen Bindung zwischen den Metallen wider. Dieser Text wurde adaptiert von <a href="https://openstax.org/books/chemistry-2e/pages/10-5-the-solid-state-of-matter">Openstax, Chemistry 2e, Section 10.5: The Solid State of Matter.</a>

Bindung in Metallen

Metallische Bindungen werden zwischen zwei Metallatomen gebildet. Ein vereinfachtes Modell zur Beschreibung metallischer Verklebungen wurde von Paul Drüde entwickelt, das als ...

Education

Lehre

JoVE Core

Chemistry

Chemie

Eins

Chemical Bonding: Basic Concepts

Chemische Bindungen: Grundkonzepte

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

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

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

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

chemistry

JoVE Core Chemie erweckt allgemeine Konzepte der Chemie durch kompakte und leicht verständliche animierte Videolektionen zum Leben. Außerdem zeigen wir in den Videos Wissenschaftler in Aktion bei klassischen und neuartigen Forschungsexperimenten, wie sie heutzutage in Laboren weltweit durchgeführt wurden.

Pennsylvania State Academic Standards

Structure and Properties of Matter

3.2.9-12.B

3.2.9-12.N

ohios-learning-standards-and-model-curriculum

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)

Virginia  Standards of Learning

HIgh School

CH.3

CH.3.d

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

motion-and-stability-forces-and-interactions

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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New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-3.

HS. Chemical Reactions

HS-PS1-2.

HS-PS1-4.

HS-PS1-12.

Georgia Standards of Excellence

SC2.

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 ...

phase-transitions-vaporization-and-condensation

Phase Transitions: Vaporization and Condensation

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

Vapor Pressure

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

Clausius-Clapeyron Equation

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

Phase Transitions: Melting and Freezing

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

phase-transitions-sublimation-and-deposition

Phase Transitions: Sublimation and Deposition

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

Heating and Cooling Curves

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

Phase Diagrams

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

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

PS.PSc.1.2

physical-and-chemical-properties-of-matter

Physical and Chemical Properties of Matter

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

Physical Properties of Matter

A physical property is ...

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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 ...

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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