Name: atomic orbitals and quantum numbers
Uploaded: 2023-04-30T18:28:31.000Z
Duration: 2 min 28 s
Channel: JoVE

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-1

Electronic Structure of Atoms

Ein Atom besteht aus drei subatomaren Teilchen – Elektronen, Protonen und Neutronen. Positiv geladene Protonen und elektrisch neutrale Neutronen bilden den Atomkern, in dem sich die gesamte positive Ladung und der größte Teil der Masse eines Atoms befinden.
Elektronen sind die negativ geladenen, massearmen Bestandteile, die sich im leeren Raum um den Kern befinden. Ein Atom ist elektrisch neutral, wenn es so viele Elektronen wie Protonen hat.
Elektronen weisen eine duale Natur auf – Teilchen und Welle. Ihre Lage im Raum und ihre Energie sind komplementäre Eigenschaften. Daher ist die Position eines Elektrons mit einer wohldefinierten Energie unsicher.
Das quantenmechanische Modell eines Atoms sagt voraus, dass die Wahrscheinlichkeit, ein Elektron mit einer bestimmten Energie in einem dreidimensionalen Bereich im Raum zu finden, aus dem Quadrat der Wellenfunktion bestimmt werden kann, das die wellenförmige Natur des Elektrons ausdrückt, auch Elektronenwahrscheinlichkeitsdichte genannt.
Eine Funktion, die die wahrscheinliche räumliche Position eines Elektrons mit spezifischer Energie in einem Atom beschreibt, wird als Atomorbital bezeichnet.
Jedes Orbital entspricht einer einzigartigen Kombination von drei Quantenzahlen. Die Hauptquantenzahl n gruppiert Orbitale in Energieniveaus oder Schalen.
Der Drehimpuls oder die azimutale Quantenzahl l gruppiert Orbitale innerhalb von Schalen in Unterschalen. Jeder Wert von l entspricht entweder einem s-, p-, d- oder f-Orbital unterschiedlicher Form.
Einige Orbitalformen können mehrere mögliche Orientierungen haben, die jeweils mit einer magnetischen Quantenzahl ml verbunden sind. Die Anzahl der Orientierungen für eine gegebene Unterschale ist gleich zwei-l plus eins.
Die vierte Quantenzahl – die Spin-Quantenzahl ms – ist mit den Elektronen verbunden, die ein Orbital besetzen, und hat nur zwei mögliche Werte: "plus die Hälfte" und "minus die Hälfte". Dadurch wird sichergestellt, dass keine zwei Elektronen in einem Atom für alle vier Quantenzahlen die gleichen Werte haben.
Durch die Überlagerung der Orbitale entsteht eine annähernd kugelförmige Form, wie eine "Wolke" aus Elektronen, die den Kern umgibt. Aus diesem Grund werden Atome im Allgemeinen als Kugeln dargestellt.

elektronische struktur von atomen

Ein Atom besteht aus Protonen und Neutronen, die sich in einem dichten, zentralen Kern, dem so genannten Nukleus, befinden, und aus Elektronen, die den Kern umgeben. Unter Berücksichtigung des Welle-Teilchen-Dualismus der Elektronen und der Unbestimmtheit der Position um den Kern liefert die Quantenmechanik ein genaueres Modell für die Atomstruktur. Es beschreibt Atomorbitale als die Bereiche um den Kern herum, in denen Elektronen diskreter Energie existieren, die durch vier Quantenzahlen gekennzeichnet sind: n, l, ml und ms.

Quantenmechanisches Modell

Ein Atom besteht aus einem kleinen, positiv geladenen Kern, der von Elektronen umgeben ist. Der Kern enthält Protonen und Neutronen. Protonen haben eine Ladung von +1 und eine Masse von 1,0073 amu. Neutronen haben keine Ladung und eine Masse von 1,0087 amu. Elektronen haben eine Ladung von −1 und eine Masse von 0,00055 amu. Die Anzahl der Protonen im Kern wird als Ordnungszahl (Z) bezeichnet und definiert die elementare Identität eines Atoms. Die Summe der Anzahl der Protonen und Neutronen im Kern wird Massenzahl genannt und entspricht, ausgedrückt in amu, ungefähr der Masse des Atoms. Ein Atom ist neutral, wenn es die gleiche Anzahl an Elektronen und Protonen enthält.

Zur Beschreibung der Atomstruktur wurden verschiedene Modelle vorgeschlagen, die die Verteilung der Elektronen um den Kern erklären. Die De-Broglie-Relation quantifizierte, dass Elektronen sowohl Eigenschaften eines Teilchens als auch einer Welle haben. Um diesen Welle-Teilchen-Dualismus weiter zu quantifizieren, stellte Heisenberg die Unschärferelation auf: Die Position (verbunden mit der Teilchennatur) und die Geschwindigkeit oder die Energie (verbunden mit der Wellennatur) des Elektrons können nicht gleichzeitig mit voller Präzision bestimmt werden. Das quantenmechanische Modell liefert ein genaueres Bild der Atomstruktur. Es beschreibt die dreidimensionale Position eines in einem Atom enthaltenen Elektrons mit einer bestimmten Energie auf probabilistische Weise anhand des Quadrats der Wellenfunktion ψ2. Atomare Wellenfunktionen oder Atomorbitale beschreiben die Bereiche in einem Atom, in denen sich Elektronen am wahrscheinlichsten befinden.

Ein Atomorbital wird durch drei Quantenzahlen charakterisiert. Die Hauptquantenzahl n gruppiert Orbitale nach der Lage des Energieniveaus oder der „Hülle“. Der Drehimpuls oder die azimutale Quantenzahl l gruppiert die Orbitale basierend auf ihrer Form in „Unterschalen“. Sie hat ganzzahlige Werte von 0 bis n–1 und wird durch Buchstaben dargestellt: s (l = 0), p (l = 1), d (l = 2), f (l = 3), g (l = 4) und h (l = 5). Die magnetische Quantenzahl ml mit 2l + 1 Werten im Bereich von –l bis +l beschreibt die Orientierung des Orbitals im Raum. Darüber hinaus hat jedes Elektron eine Spinquantenzahl ms, die ±1/2 betragen kann. Keine zwei Elektronen im selben Atom können die gleichen Werte für alle vier Quantenzahlen haben.

Dieser Text wurde adaptiert von<a href="https://openstax.org/books/chemistry-2e/pages/6-3-development-of-quantum-theory#0"> Openstax, Chemistry 2e, Abschnitt 6.</a>.

Elektronische Struktur von Atomen


Ein Atom besteht aus Protonen und Neutronen, die sich im dichten, zentralen Kern, dem Kern, befinden, wobei Elektronen um den Kern herum vorhanden sind.

Education

Lehre

JoVE Core

Organic Chemistry

Organische Chemie

Unit 1

Einheit 1

Covalent Bonding and Structure

Kovalente Bindung und Struktur

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

atomic orbitals and quantum numbers

Atomic orbitals and quantum numbers describe how electrons are arranged around the nucleus. An atom has a small, positively charged nucleus with electrons surrounding it. The nucleus contains protons and neutrons, and the quantum mechanical model gives a better picture of this structure than older models.

Protons carry a +1 charge and have a mass of 1.0073 amu. Neutrons have no charge and have a mass of 1.0087 amu. Electrons carry a −1 charge and have a mass of 0.00055 amu. The number of protons is the atomic number, Z, and it defines the element. The total number of protons and neutrons is the mass number, and it is approximately equal to the atom’s mass in amu. An atom is neutral when it has equal numbers of protons and electrons.

The quantum model grew from ideas about electron behavior. The de Broglie relation showed that electrons act like both particles and waves. Heisenberg’s uncertainty principle added that an electron’s position and its velocity or energy cannot both be known with full precision at the same time. Because of this, electron location is described in a probabilistic way using the square of the wavefunction, ψ².

Atomic wavefunctions, or atomic orbitals, show the regions where electrons are most likely to be found. Orbitals are described by four quantum numbers. The principal quantum number, n, gives the energy level or shell. The angular momentum, or azimuthal, quantum number, l, describes orbital shape and forms subshells. Its values run from 0 to n − 1, and the labels are s, p, d, f, g, and h for l = 0 through 5.

The magnetic quantum number, ml, describes how an orbital is oriented in space. It has 2l + 1 possible values, ranging from −l to +l. The spin quantum number, ms, can be +1/2 or −1/2. No two electrons in the same atom can have the same set of values for all four quantum numbers.

Atomic Orbitals and Quantum Numbers

what is organic chemistry?

Carbon Compounds in Everyday Life

Organic chemistry focuses on carbon compounds called organic compounds. These compounds may come from living things or be made by chemists. Carbon is the main element in them, and it bonds with other carbon atoms as well as hydrogen, oxygen, nitrogen, and sulfur. Carbon can form up to four strong bonds. That ability lets carbon atoms build chains and rings of many sizes, shapes, and levels of complexity. Not every carbon-containing substance is classified as organic. Carbonates, cyanides, and...

electronic structure of atoms

Atomic orbitals and quantum numbers describe how electrons are arranged around the nucleus. An atom has a small, positively charged nucleus with electrons surrounding it. The nucleus contains protons and neutrons, and the quantum mechanical model gives a better picture of this structure than older models. Protons carry a +1 charge and have a mass of 1.0073 amu. Neutrons have no charge and have a mass of 1.0087 amu. Electrons carry a −1 charge and have a mass of 0.00055 amu. The number of...

electron configurations

How Electrons Fill Atomic Orbitals

Electron filling in atoms follows a set order based on orbital energy. The Aufbau principle says each new electron enters the lowest-energy subshell available. The Pauli exclusion principle says no two electrons can share the same set of four quantum numbers. Hund’s rule of maximum multiplicity says electrons stay unpaired in equal-energy orbitals when possible. The order of filling follows the relative energies of the subshells. A common sequence is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, and so on.

chemical bonds

Chemical Bonds: Types and Strength

Chemical bonds help atoms reach a full valence shell like the nearest noble gas. The main bond types are ionic, covalent, and metallic. Bond energy and bond length also help explain how strong a bond is. An ionic bond forms from electrostatic attraction between cations and anions. In many cases, one atom transfers electrons to another atom, and the ions form from that transfer. Ionic bonds have no defined direction because the attraction spreads evenly through three-dimensional space. A...

polar covalent bonds

Electronegativity in Polar Covalent Bonds

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lewis structures and formal charges

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Lewis structures show how atoms share electrons in covalent bonds and in polyatomic ions. Lewis symbols help draw these structures, and the periodic table helps predict how many valence electrons an atom has and how many bonds it can form to reach an octet. Group 18 elements, such as argon and helium, already have filled electron configurations. They rarely take part in chemical bonding. Atoms in group 17, such as bromine and iodine, need one more electron to reach an octet, so they can form...

vsepr theory

Molecular Shapes from Electron Pairs

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molecular geometry and dipole moments

Predicting Shape and Molecular Polarity

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resonance and hybrid structures

Resonance in Nitrite and Carbonate Ions

Resonance explains why some Lewis structures do not match the measured properties of a molecule or ion. When two or more Lewis structures have the same atom arrangement, the real electron distribution is an average of the structures shown. The nitrite anion, NO2−, is one example. It can be drawn in two ways, with the N–O and N=O bonds in different places. If nitrite had one single bond and one double bond, the two bond lengths should be different, because a double bond is shorter and stronger...

valence bond theory and hybridized orbitals

valence-bond-theory-and-hybridized-orbitals

Covalent Bond Overlap and Orbital Hybridization

Covalent bonds form when orbitals on two atoms overlap and their single electrons pair up. The bond is stronger when the overlap is greater. Maximum overlap happens when the orbitals meet along a direct line between the two nuclei. A sigma bond, or σ bond, is the kind of covalent bond found in a single bond in a Lewis structure. In a σ bond, electron density is concentrated along the internuclear axis. A pi bond, or π bond, forms when two p orbitals overlap side by side. In a π bond, the...

mo theory and covalent bonding

Bond Order and Molecular Orbitals

Molecular orbital theory explains how electrons are arranged in molecules. It treats electron regions in a molecule much like atomic orbitals in an atom. A molecular orbital is the region of space where a valence electron is most likely to be found. Molecular orbitals form through the linear combination of atomic orbitals, or LCAO. When atomic wave functions combine in phase, they create regions with high electron density. When they combine out of phase, they create nodes, or regions with no...

intermolecular forces and physical properties

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How Intermolecular Forces Affect Matter

Intermolecular forces are the attractions between molecules, and they help explain how matter behaves. These forces influence melting points, boiling points, and whether substances mix with one another. Water has a much higher boiling point than hexane, which shows that water has stronger intermolecular forces. Three main kinds of intermolecular interactions are covered here. They include ion-dipole forces, dipole-dipole interactions, and van der Waals forces, which include London dispersion...

solubility

Why Some Substances Dissolve in Water

Solution formation depends on how solutes and solvents interact. A solution is a homogeneous mixture made of a solvent, which is the larger part, and a solute, which is the smaller part. The physical state of a solution is usually the same as the solvent. Concentration is often described as dilute for a low amount of solute or concentrated for a high amount of solute. When a solute dissolves, its particles are surrounded by solvent species. This process is called solvation. If water is the...

introduction to functional groups

Functional Groups and Organic Molecules

Functional groups are groups of atoms with specific chemical properties that appear within organic molecules. They are sometimes shown as "R." These groups sit along the carbon backbone of macromolecules, which can form chains or rings of carbon atoms. Functional groups help functionalize a compound. That means they can give the molecule different physical and chemical properties. In organic chemistry, this change in group structure can strongly affect how a compound behaves. Common...

overview of advanced functional groups

Advanced Functional Groups in Organic Chemistry

Advanced functional groups are atom clusters in organic molecules that give those molecules specific chemical properties. They are sometimes shown as "R" in formulas. By changing the atoms attached to a carbon skeleton, a functional group can make a compound behave differently in physical and chemical reactions. This topic covers several major classes of organic compounds with advanced functional groups. Aromatic hydrocarbons include benzene. Phenol is another example and is also called...

key terms and concepts

Learn how atomic orbitals, shells, subshells, and the four quantum numbers describe electron arrangement in atoms through the quantum mechanical model.

Atomic Orbitals and Quantum Numbers | JoVE K12

organic chemistry

JoVE Core Organic Chemistry explains basic concepts of stereochemistry, reactions, and mechanisms using concise and easy-to-understand animated video lessons. Additionally, the scientist-in-action videos demonstrate the application of related concepts in classical and original research experiments performed in today's laboratories worldwide.

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HS-PS1-3

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Motion And Stability: Forces And Interactions

HS-PS2-6

Virginia  Standards of Learning

HIgh School

CH.2

CH.2.d

Next Generation Science Standards

Physical Science

Matter and Its Interactions

Florida Department of Education

SC.912.P.8

SC.912.P.8.5

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South Carolina College and Career Ready Science Standards

C-PS1-1

C-PS1-3.

Motion and Stability: Forces and Interactions

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Physics

P-PS2-6.

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HS-PS1-4

Atomic Orbitals and Quantum Numbers

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