Name: electron waves and standing orbits
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 32 s
Channel: JoVE

K12 Standards

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

NC K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.1.4

The de Broglie Wavelength

Wenn Elektronen Teilchen sind, dann wird wenn ein Elektronenstrahl durch zwei eng beieinander liegende Schlitze verläuft erwartet, dass zwei kleinere Elektronenstrahlen auftauchen und zwei helle Streifen mit Dunkelheit dazwischen erzeugen. Am Anfang erscheinen mit nur wenigen Elektronen lokalisierte Flecken zufällig auf dem Bildschirm. Dies deutet auf teilchenhaftes Verhalten hin.Da jedoch immer mehr Elektronen durch die Schlitze durchgehen, taucht ein Interferenzmuster das Markenzeichen des wellenartigen Verhaltens auf. Wie ist das möglich? Erinnern Sie sich, dass das Bohr-Modell postuliert, dass das Elektron ein Teilchen ist, welches den Kern umkreist.Der französische Physiker Louis de Broglie postuliert, dass das Elektron Welleneigenschaften aufweisen kann. Er postuliert, dass sich das Elektron wie eine kreisförmig stehende Welle mit einer Wellenlänge, Lambda, verhält. Der Umfang jeder Umlaufbahn enthält eine ganze Zahl der Wellenlängen.Bestimmte Punkte auf der Welle haben keine Amplitude dies sind Knoten. De Broglie postulierte die folgende Beziehung, in der die Wellenlänge des Elektrons von seiner Masse und Geschwindigkeit abhängt, wobei h die Planck'sche Konstante ist. Je größer die Geschwindigkeit des Elektrons ist, desto kürzer ist seine Wellenlänge.Die De Broglie-Hypothese bezieht sich auf alle Materien, und diese Wellen werden Materiewellen"genannt. Allerdings große, makroskopische Objekte, wie zum Beispiel ein Golfball, erscheinen nicht als Wellen. Wenn wir die de Broglie-Beziehung anwenden, und der winzige Wert der Planck'schen Konstante durch die Masse und Geschwindigkeit des Golfballs geteilt wird zeigt es eine extrem kleine Wellenlänge, die zu klein ist, um beobachtet zu werden.Jedoch für subatomare Teilchen mit extrem kleinen Massen wie Elektronen kann ihre Wellennatur nicht ignoriert werden. Wenn Röntgenstrahlen einen Kristall durchdringen, werden die Wellen gebeugt, und ein ausgeprägtes Interferenzmuster, die die Anordnung der Atome im Kristall zeigt, wird beobachtet. Dies ist die als Röntgendiffraktometrie bekannte Labortechnik.Wenn ein ähnliches Experiment wo das Passieren von Elektronen anstatt durch den Kristall, durch Röntgenstrahlen durchgeführt wird, wird ein ähnliches Verhalten beobachtet. Dies ist ein experimenteller Beweis dafür, dass Elektronen Teilchen sind, die ein wellenförmiges Verhalten zeigen.

die de broglie-wellenlänge

In der makroskopischen Welt folgen Objekte, welche groß genug sind um noch mit bloßem Auge gesehen zu werden, den Regeln der klassischen Physik. Eine Billardkugel, die sich auf einem Tisch bewegt, verhält sich wie ein Teilchen; Es bewegt sich geradlinig weiter es sei denn, es kollidiert mit einer anderen Kugel oder es wirkt eine andere Kraft, beispielsweise Reibung auf ihn ein. Der Ball hat eine genau definierte Position und Geschwindigkeit oder einen genau definierten Impuls, p = mv, der durch die Masse m und die Geschwindigkeit v zu jedem gegebenen Zeitpunkt definiert wird. Dies ist das typische Verhalten eines klassischen Objekts. Wenn Wellen miteinander interagieren zeigen sie Interferenzmuster, die bei makroskopischen Teilchen wie die Billardkugel nicht beobachtet werden. In den 1920er Jahren wurde jedoch immer deutlicher, dass für sehr kleine Materiestücke andere Regeln gelten als für große Objekte. In der mikroskopischen Welt sind Wellen und Teilchen untrennbar miteinander verbunden. Einer der ersten Menschen, der auf das besondere Verhalten der mikroskopischen Welt aufmerksam machte war Louis de Broglie. Er stellte die Frage ob, wenn elektromagnetische Strahlung teilchenähnlichen Charakter haben kann, Elektronen und andere submikroskopische Teilchen wellenförmigen Charakter aufweisen können? De Broglie erweiterte den Welle-Teilchen-Dualismus des Lichts, den Einstein zur Lösung des Paradoxons des photoelektrischen Effekts verwendete, auf materielle Teilchen. Er sagte voraus, dass ein Teilchen mit Masse m und Geschwindigkeit v (d. h. mit linearem Impuls p) auch das Verhalten einer Welle mit einem Wellenlängenwert λ zeigen sollte, gegeben durch folgenden Ausdruck, in dem h das Plancksche Wirkungsquantum darstellt: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/979/979_Equations-01.png" style="height: 40px;"> Dies wird als De-Broglie-Wellenlänge bezeichnet. Während Bohr postuliert hatte, dass das Elektron ein Teilchen sei, das den Kern auf quantisierten Bahnen umkreise, argumentierte de Broglie, dass Bohrs Annahme der Quantisierung erklärt werden könne, wenn das Elektron stattdessen als kreisförmige stehende Welle betrachtet werde. Nur eine ganze Zahl von Wellenlängen könnte genau in die Umlaufbahn passen. Betrachtet man ein Elektron als Welle die um den Kern kreist, muss eine ganze Zahl von Wellenlängen in die Umlaufbahn passen, damit das Verhalten einer stehenden Welle möglich ist. Für eine kreisförmige Umlaufbahn mit dem Radius r beträgt der Umfang 2πr, und daher lautet die Bedingung von de Broglie: <img alt="Eq2" src="https://www.jove.com/files/core/CDNSource/lessons/979/979_Equations-02.png" style="height: 40px;"> wobei n = 1, 2, 3 usw. Kurz nachdem de Broglie die Wellennatur der Materie vorgeschlagen hatte, zeigten zwei Wissenschaftler der Bell Laboratories, C. J. Davisson und L. H. Germer, experimentell, dass Elektronen wellenartiges Verhalten zeigen könnten. Dies wurde demonstriert, indem ein Elektronenstrahl auf einen Nickelkristall gerichtet wurde. Der Abstand der Atome innerhalb des Gitters entsprach ungefähr den De-Broglie-Wellenlängen der darauf gerichteten Elektronen, und die Abstände der Atomschichten des Kristalls dienten als „Schlitze“, wie bereits in anderen Interferenzexperimenten verwendet. Nachdem nur wenige Elektronen den Schlitz passierten, wurde ein scheinbar teilchenartiges Verhalten beobachtet. Als jedoch immer mehr Elektronen aufgezeichnet werden konnten, entstand ein deutliches Interferenzmuster, welches als Anzeichen von wellenförmigen Verhaltens verstanden werden kann. Es scheint also, dass Elektronen zwar kleine lokalisierte Teilchen sind, ihre Bewegung jedoch nicht strikt den Bewegungsgleichungen der klassischen Mechanik folgt. Stattdessen wird ihre Bewegung durch eine Wellengleichung bestimmt. Somit ist der erstmals bei Photonen beobachtete Welle-Teilchen-Dualismus ein grundlegendes Verhalten das allen Quantenteilchen innewohnt. Dieser Text wurde angepasst von <a href="https://openstax.org/books/chemistry-2e/pages/6-3-development-of-quantum-theory">Openstax, Chemistry 2e, Section 6.3: Development of Quantum Theory</a>.

Die de Broglie-Wellenlänge

In der makroskopischen Welt folgen Objekte, die groß genug sind, um mit bloßem Auge gesehen zu werden, den Regeln der klassischen Physik. Eine Billardkugel, die sich auf einem ...

Education

Lehre

JoVE Core

Chemistry

Chemie

Eins

Electronic Structure of Atoms

Elektronische Struktur von Atomen

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

electron waves and standing orbits

Electron waves and standing orbits explain how tiny particles can behave like waves. Large objects in the macroscopic world, like a billiard ball on a table, follow classical physics. A ball keeps moving in a straight line unless it hits another ball or a force such as friction acts on it. It also has a well-defined position, velocity, and momentum, where momentum is mass times velocity.

Waves behave differently from macroscopic particles. When waves interact, they can form interference patterns. These patterns do not appear in the motion of a billiard ball. By the 1920s, scientists saw that very small pieces of matter do not always follow the same rules as large objects.

Louis de Broglie was one of the first to study this difference. He asked whether electrons and other submicroscopic particles could also show wavelike behavior if light can act like both a wave and a particle. He extended the wave-particle duality of light, which Einstein used to explain the photoelectric-effect paradox, to material particles. De Broglie predicted that a particle with mass m and velocity v, and therefore momentum p, should have a wavelength λ given by a formula that includes Planck’s constant h. This is called the de Broglie wavelength.

De Broglie also offered a way to explain Bohr’s quantized electron orbits. He suggested that an electron could be treated as a circular standing wave instead of only as a particle. In that model, only an integer number of wavelengths can fit exactly around the orbit. For a circular orbit of radius r, the circumference is 2πr, so de Broglie’s condition requires n whole wavelengths, where n can be 1, 2, 3, and so forth.

The wave nature of electrons was later shown in an experiment at Bell Laboratories by C. J. Davisson and L. H. Germer. They aimed a beam of electrons at a crystalline nickel target. The spacing of atoms in the crystal lattice was about the same as the de Broglie wavelengths of the electrons. The regularly spaced atomic layers acted like slits used in other interference experiments.

At first, when only a few electrons were recorded, the result looked particle-like. As more electrons were collected, a clear interference pattern appeared. That pattern is a sign of wavelike behavior. The experiment showed that electrons are localized particles, but their motion does not follow classical mechanics. Instead, it is described by a wave equation. This wave-particle duality, first seen with photons, is a basic feature of quantum particles.

Electron Waves and Standing Orbits

the wave nature of light

Measuring Light with Wavelength and Frequency

Light can be described as an electromagnetic wave, and its behavior helps explain many patterns seen in science. For centuries, scientists have tried to understand light. Newton used lenses and prisms to show that white light is made of the colors of the rainbow mixed together. He explained light as tiny particles moving at high speed. Other scientists, including Christiaan Huygens, showed that reflection and refraction could also be explained by treating light as a wave. At the time, people...

the electromagnetic spectrum

Electromagnetic Waves: Uses Across the Spectrum

The electromagnetic spectrum includes all electromagnetic radiation arranged by frequency and wavelength. Visible light is only a small part of it, and each color of visible light has its own frequency and wavelength. Different parts of the spectrum also use different units. Radio waves are usually measured in MHz, while the visible range is often measured in nm or angstroms. The spectrum is organized from radio waves to gamma rays as frequency increases and wavelength decreases. Radio waves...

interference and diffraction

Wave Patterns from Light and Slits

Light can form wave patterns through interference and diffraction. When two electromagnetic waves meet with their peaks and troughs lined up, they combine into a larger wave. This is constructive interference, and the waves are in phase. When a peak of one wave meets a trough of the other, the waves reduce each other. This is destructive interference, and the result has a much lower amplitude. Diffraction is another wave behavior. When light passes through a slit that is about the same size as...

photoelectric effect

Why Light Ejects Electrons from Metals

Light can eject electrons from a metal surface when it has the right frequency. This process is called the photoelectric effect. Each metal has its own threshold frequency, which is the minimum light frequency needed to free electrons. Light below the threshold frequency cannot cause emission, even if it is very bright. When the light frequency is above the threshold, electrons are ejected. In that case, the number of electrons released is directly proportional to the intensity, or brightness,...

the bohr model

Bohr’s Quantized Atomic Orbits

Bohr’s quantized atomic orbits explain why hydrogen atoms can stay stable. Early in the twentieth century, Ernest Rutherford and his colleagues described atoms as tiny dense nuclei with lighter electrons moving around them. This picture was called the planetary model because it compared the atom to a miniature solar system, with electrons orbiting the nucleus like planets around the sun. The simplest atom is hydrogen. It has one proton in the nucleus and one electron moving around it. In the...

emission spectra

Line Spectra from Heated Gases

Line spectra are produced when heated gases give off light at specific wavelengths. In contrast, hot solids, liquids, or condensed gases radiate excess energy as a continuous spectrum. That spectrum contains an unbroken range of wavelengths. A gas at low partial pressure can produce a line spectrum when it is excited by an electric current or heated. Fluorescent light bulbs and neon signs work in this way. Each element has its own characteristic set of lines, and molecules can also produce...

the de broglie wavelength

Electron waves and standing orbits explain how tiny particles can behave like waves. Large objects in the macroscopic world, like a billiard ball on a table, follow classical physics. A ball keeps moving in a straight line unless it hits another ball or a force such as friction acts on it. It also has a well-defined position, velocity, and momentum, where momentum is mass times velocity. Waves behave differently from macroscopic particles. When waves interact, they can form interference...

the uncertainty principle

Electron Position and Momentum Limits

Heisenberg’s uncertainty principle sets a limit on how precisely we can know an electron’s position and momentum at the same time. Momentum is the motion of a particle, and the two measurements affect each other. If the momentum is known more accurately, the position becomes less certain, and the reverse is also true. Heisenberg described this limit with an equation that uses Planck’s constant. The equation shows the smallest possible uncertainty for position and momentum together. It explains...

the quantum-mechanical model of an atom

Electron Orbitals in Quantum Mechanics

Quantum mechanics explains how electrons behave in atoms using waves and probability. Erwin Schrödinger built on de Broglie’s idea that an electron in hydrogen could act like a circular standing wave instead of moving in fixed circular paths. He then derived the Schrödinger equation, which became a major step in modern atomic theory. When Schrödinger applied his equation to hydrogen-like atoms, it matched Bohr’s energy expression and the Rydberg formula for hydrogen spectra. He described...

quantum numbers

Electron Orbitals and Spin

Electron orbitals are described by quantum numbers that show where an electron is most likely to be found around the nucleus. These numbers come from the quantum mechanical model, which is based on solutions of the Schrödinger equation. They also help explain why electron energy comes in set values instead of changing smoothly. The principal quantum number, n, labels the energy level. It can be 1, 2, 3, and so on, and higher n values usually mean higher electron energy. This number also tells...

atomic orbitals

Electron Regions in Atomic Orbitals

Electron regions in atomic orbitals show where an electron is most likely to be found in an atom. These three-dimensional regions are often drawn as boundary surfaces around the densest part of the cloud. The shape of an orbital depends on the angular momentum quantum number, l. This value can range from 0 to n - 1, where n is the principal quantum number. For n = 1, only l = 0 is allowed. For n = 2, both l = 0 and l = 1 are allowed. Orbitals with the same value of l form a subshell. The l =...

the pauli exclusion principle

Electron Spin and Orbital Pairing

Electron spin and orbital pairing explain why only two electrons can fit in one atomic orbital. Electron configuration describes how electrons are arranged in an atom’s orbitals. It is written with three parts: the principal quantum number, n, the orbital type, or subshell, and a superscript that shows how many electrons are in that subshell. For example, 2p4 means four electrons in a p subshell with n = 2, and 3d8 means eight electrons in a d subshell with n = 3. The three quantum numbers...

the energies of atomic orbitals

Shielding and Orbital Penetration

Shielding and orbital penetration help explain why electrons in an atom have different energies. Electrons are attracted to the positive nucleus, but they also repel one another in atoms with more than one electron. The strength of these forces depends on the charge and the distance between the particles. Opposite charges attract, like charges repel, and the force gets weaker as the particles move farther apart. An electron that stays closer to the nucleus is held more tightly. That means...

the aufbau principle and hund's rule

Electron Filling Order in Atomic Orbitals

Electron filling order in atomic orbitals follows the aufbau principle and Hund's rule. To write an electron configuration, we build atoms in order of atomic number. Starting with hydrogen and moving across the periods of the periodic table, one proton is added to the nucleus and one electron is placed into the correct subshell. This process describes the ground-state electron configurations of the elements. The aufbau principle comes from the German word aufbau, which means "to build up." It...

electron configuration of multielectron atoms

electron-configuration-of-multielectron-atoms

Valence Electrons and Noble Gas Shorthand

Valence electrons and noble gas shorthand help show how electrons are arranged in multielectron atoms. Sodium, the alkali metal with atomic number 11, has one more electron than neon. That extra electron goes into the lowest-energy subshell available, the 3s orbital, so sodium has the configuration 1s2 2s2 2p6 3s1. Electrons in the outermost shell, where n is highest, are called valence electrons. Electrons in the inner shells are called core electrons. Because core electrons often match a...

key terms and concepts

Learn how de Broglie linked electrons to waves, explained Bohr’s quantized orbits with standing waves, and how electron interference confirmed the idea.

Electron Waves and Standing Orbits | 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.

Tennessee Academic Standards

High School

waves-and-their-applications-in-technologies-for-information-transfer

Waves and Their Applications in Technologies for Information Transfer

CHEM1.PS4.1

Virginia  Standards of Learning

HIgh School

CH.2

CH.2.e

PS.2

PS.2.a

Physics

PH.9

PH.9.a

Texas Essential Knowledge and Skills

CHEM.6

CHEM.6.A

CHEM.6.B

Florida Department of Education

SC.912.P.8

SC.912.P.8.3

SC.912.P.10

SC.912.P.10.9

PHYS.9

PHYS.9.C

PHYS.9.D

Chemistry and Physics

IPC.7

IPC.7.E

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-7.

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 ...

molecular-comparison-of-gases-liquids-and-solids

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 ...

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.

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 ...

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 ...

Alkali Metals

Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

Halogens

Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. ...

Noble Gases


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were ...

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

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 ...

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 ...

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 ...

Construct an explanation to classify the type of chemical bond that occurs (covalent, ionic, or metallic) in a given substance.

PS.PSc.2.1

Understand types, properties, and structure of matter.

Electron Waves and Standing Orbits

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