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

Um átomo é feito de três partículas subatômicas – elétrons, prótons e nêutrons. Prótons carregados positivamente e nêutrons eletricamente neutros constituem o núcleo atômico, onde residem toda a carga positiva e a maior parte da massa de um átomo.
Os elétrons são os constituintes de baixa massa carregados negativamente localizados no espaço vazio ao redor do núcleo. Um átomo é eletricamente neutro quando tem tantos elétrons quanto prótons.
Os elétrons exibem uma natureza dual - partícula e onda. Sua localização no espaço e sua energia são propriedades complementares. Portanto, para um elétron com uma energia bem definida, sua posição é incerta.
O modelo da mecânica quântica de um átomo prevê que a probabilidade de encontrar um elétron de uma determinada energia em uma região tridimensional no espaço pode ser determinada a partir do quadrado da função de onda que expressa a natureza ondulatória do elétron, também chamada de densidade de probabilidade do elétron.
Uma função que descreve a provável localização espacial de um elétron de energia específica em um átomo é chamada de orbital atômico.
Cada orbital corresponde a uma combinação única de três números quânticos. O número quântico principal, n, agrupa orbitais em níveis de energia ou camadas.
O momento angular, ou azimutal, número quântico, l, agrupa orbitais dentro de cascas em subcamadas. Cada valor de l corresponde a um orbital s, p, d ou f de forma variável.
Algumas formas orbitais podem ter várias orientações possíveis, cada uma associada a um número quântico magnético, ml. O número de orientações para uma determinada subcamada é igual a dois-l mais um.
O quarto número quântico - o número quântico de spin, ms - está associado aos elétrons que ocupam um orbital e tem apenas dois valores possíveis: 'mais metade' e 'menos metade'. Isso garante que dois elétrons em um átomo não tenham os mesmos valores para todos os quatro números quânticos.
A sobreposição dos orbitais uns sobre os outros produz uma forma aproximadamente esférica, como uma "nuvem" de elétrons ao redor do núcleo. É por isso que os átomos são geralmente representados como esferas.

estrutura eletrônica dos átomos

Um átomo compreende prótons e nêutrons, que estão contidos dentro da região central densa chamada núcleo, com elétrons presentes ao redor do núcleo. Levando em conta a dualidade onda-partícula dos elétrons e a incerteza na posição ao redor do núcleo, a mecânica quântica fornece um modelo mais preciso para a estrutura atômica. Ela descreve orbitais atômicos como as regiões ao redor do núcleo onde existem elétrons de energia discreta, caracterizados por quatro números quânticos: n, l, ml e ms.

Modelo de mecânica quântica

Um átomo consiste em um pequeno núcleo carregado positivamente cercado por elétrons. O núcleo contém prótons e nêutrons. Os prótons têm carga de +1 e massa de 1,0073 u. Os nêutrons têm carga zero e massa de 1,0087 u. Os elétrons têm carga de -1 e massa de 0,00055 u. O número de prótons no núcleo é chamado de número atômico (Z) e define a identidade elementar de um átomo. A soma dos números de prótons e nêutrons no núcleo é chamada de número de massa e, expressa em u, é aproximadamente igual à massa do átomo. Um átomo é neutro quando contém números iguais de elétrons e prótons.

Vários modelos foram propostos para descrever a estrutura atômica explicando a distribuição dos elétrons ao redor do núcleo. A relação de Broglie quantificou que os elétrons têm propriedades tanto de partícula quanto de onda. Quantificando ainda mais esta dualidade onda-partícula, Heisenberg forneceu o princípio da incerteza: a posição (associada à natureza da partícula) e a velocidade ou a energia (associada à natureza da onda) do elétron não podem ser determinadas simultaneamente com total precisão. O modelo de mecânica quântica fornece uma imagem mais precisa da estrutura atômica. Descreve a posição tridimensional de um elétron com uma energia específica, contida em um átomo, de forma probabilística em termos do quadrado da função de onda, ψ2. As funções de onda atômicas, ou orbitais atômicos, descrevem as regiões de um átomo onde os elétrons têm maior probabilidade de serem encontrados.

Um orbital atômico é caracterizado por três números quânticos. O número quântico principal, n, agrupa orbitais em termos de localização do nível de energia, ou ‘camada’. O momento angular ou número quântico azimutal, l, agrupa os orbitais com base em suas formas em “subníveis”. Possui valores inteiros de 0 a n–1 e é representado pelas letras: s (l = 0), p (l = 1), d (l = 2), f (l = 3), g (l = 4) e h (l = 5). O número quântico magnético, ml, com valores 2l + 1 variando de –l a +l, descreve a orientação do orbital no espaço. Além disso, cada elétron possui um número quântico de spin, ms, que pode ser igual a ±1/2. Não existem dois elétrons no mesmo átomo que possam ter o mesmo conjunto de valores para todos os quatro números quânticos.

Este texto foi adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/6-3-development-of-quantum-theory#0"> Openstax, Chemistry 2e, Section 6</a>.

Estrutura eletrônica dos átomos


Um átomo compreende prótons e nêutrons, que estão contidos dentro do núcleo central denso chamado núcleo, com elétrons presentes ao redor do ...

Education

JoVE Core

Organic Chemistry

Química Orgânica

Unit 1

Unidade 1

Covalent Bonding and Structure

Ligação Covalente e Estrutura

KEY TERMS AND CONCEPTS

TERMOS-CHAVE E CONCEITOS

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

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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

Lewis Structures, Bonds, and Formal Charge

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

Molecular shape can be predicted from the way electron pairs arrange around a central atom. Valence shell electron-pair repulsion theory, or VSEPR theory, uses a Lewis structure to count bonding pairs and lone electron pairs. The main idea is simple: electron pairs spread out as far as possible to reduce repulsion. In a molecule, the valence electrons around the central atom can be bonding pairs or lone pairs. Bonding pairs are found mainly between bonded atoms. Lone pairs stay on one atom and...

molecular geometry and dipole moments

Predicting Shape and Molecular Polarity

Molecular shape and molecular polarity can be predicted with VSEPR theory and dipole moments. Start by writing the Lewis structure of the molecule or polyatomic ion. Then count the electron groups around the central atom. Lone pairs and bonds both count as electron groups, and a single, double, or triple bond each counts as one region of electron density. Use that count to identify the electron-pair geometry. Next, use the number of lone pairs to determine the molecular structure. If more than...

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

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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

intermolecular-forces-and-physical-properties

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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 - Química Orgânica explica conceitos básicos de estereoquímica, reações e mecanismos usando vídeos de animação concisos e fáceis de entender. Além disso, os vídeos de Cientistas em ação demonstram a aplicação de conceitos relacionados em experimentos de pesquisa clássicos e originais realizados nos laboratórios atuais em todo o mundo.

HS-PS1-2

HS-PS1-3

motion-and-stability-forces-and-interactions

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

C-PS2-6.

Physics

P-PS2-6.

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HS-PS1-4

Atomic Orbitals and Quantum Numbers

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