Name: electron filling order in atomic orbitals
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 3 min 2 s
Channel: JoVE

K12 Standards

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

NC K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.1.3

The Aufbau Principle and Hund's Rule

原子の軌道は 異なるエネルギーを持ち それぞれ2つの電子を受け入れる ことを思い出してください アウフバウの原理は 原子の各殻間の 電子の分布を規定し フントの最大多重度の法則は 各殻内の軌道の充填を 説明しています アウフバウの原理において 基底状態では 電子は最低エネルギー軌道から 最高エネルギー軌道を埋めていき 最も低いエネルギーの配置を 実現するとしています 一般的にエネルギーは 殻の数が増えるにつれて 増加しますが s軌道の透過が大きいため 4s軌道は3d軌道よりも低く 5s軌道は4d軌道よりも低い エネルギーになることが多くなります このような図を使って 順番を覚えることができ 矢印のパスは電子の 軌道に割り当てられた 順番を示しています 原子番号6の元素である 炭素の電子配置を 書いてみましょう 確かに エネルギーが 最も低い1s軌道は 2s軌道の前に 埋めなければなりません それぞれの軌道は最大2個の 電子を保持することができます 5個目の電子は 2-p部分殻に入ります しかし 3つの2-p軌道のうち どの軌道に入るのでしょうか？そうですね どの部分殻の軌道も 縮退していると推定されますが これは同じエネルギーを 持っていることを意味します したがって 5番目の電子は 3つの縮退した2-p軌道の どれにでも入ることができます 第6電子はどうでしょうか？電子と一緒に 2-p軌道に入るのか それとも空いている2-p軌道の 1つに入るのでしょうか？フントの最大多重度の 法則によれば 電子はペアリングを始める前に あるエネルギー準位の すべての軌道を 単数で占有しています したがって 炭素の場合 2個の2-p電子は 2つの異なる軌道を占有し 平行なスピンを 持っていなければなりません このようにして 電子はより広い 面積に広がることができます これはお互いの遮蔽を減少させ それによって原子の エネルギーを最小化します 窒素の場合 3つの 2-p軌道のそれぞれが 単数で占有されています 酸素の場合 いったん縮退した 2-p軌道が1つになったら 最後の電子は別の2-p電子と 対にならなければなりません 原子は2つの 不対電子を持っています ネオンの電子配置を見ると 一番外側の殻が 8個の電子の最大容量まで 満たされていることがわかります ネオンは内殻に2つの電子 コア電子と呼ばれる）を持ち 外殻には8つの電子 価電子と呼ばれる）を 持っています

アウフバウの原理とフント則

特定の原子の電子配置を決定するために、原子番号順に構造を構築していくことができます。水素から始まり、周期表の周期をまたがり、一度に1つの陽子を原子核に加え、1つの電子を適切な小軌道に加えて、すべての元素の電子配置を記述します。この方法は、ドイツ語の「アウフバウ（積み上げる）」から「アウフバウの原理」と呼ばれています。追加された電子は、パウリの排他原理により許容される量子数の制限を受けながら、最もエネルギーの低い小軌道を占めます。電子がより高いエネルギーの小軌道に入るのは、低いエネルギーの小軌道がいっぱいになった後です。図1は、原子軌道の充填順序を覚えるための伝統的な方法を示したものです。
 
 <img alt="Figure1" src="https://www.jovecore.com/CDNSource/lessons/986/986Image_1.png" style="width: 700px;" />
 
 図 1この図は原子軌道のエネルギー順を表したもので、基底状態の電子配置を導き出すのに役立ちます。 
 
 原子番号6の元素である炭素の電子配置を書くことを考えてみましょう。4つの電子が1sと2sの軌道を占めています。残りの2つの電子は、2p小軌道を占めています。ここで、2p軌道の1つを埋めて電子を対にするか、電子を対にしないで2つの異なるが縮退したp軌道に残すかを選択することになります。縮退した軌道の中に電子を持つ原子の最もエネルギーの低い配置は、最大数の不対電子を持つ配置であるというフントの法則に従って、軌道が埋められます。したがって、炭素の2p軌道にある2つの電子は、n、l、msの量子数が同じで、 mlの量子数が異なります（パウリの排除原理に合致する）。電子配置が1s22s21p2である炭素の軌道図は次のようになります。
 
 <img alt="Figure2" src="https://www.jovecore.com/CDNSource/lessons/986/986Image_2.png" style="width: 300px;" />
 
 窒素（原子番号7）は、フント則に従い、1sおよび2s小軌道を満たし、3つの2p軌道にそれぞれ1つの電子を持っています。この3つの電子は不対スピンを持っています。酸素（原子番号8）は、2p軌道のいずれか1つに一対の電子を持ち（電子のスピンは逆）、他の2つの軌道にはそれぞれ1つの電子を持ちます。フッ素（原子番号9）は、不対電子を含む2p軌道を1つだけ持っています。希ガスであるネオン（原子番号10）の電子はすべて対になっていて、n=1とn=2の殻のすべての軌道が満たされています。
 
 この文章は <a href="https://openstax.org/books/chemistry-2e/pages/6-4-electronic-structure-of-atoms-electron-configurations">、 Openstax, Chemistry 2e, Section 6.4: Electronic Structure of atoms から引用したものです。</a>

特定の原子の電子配置を決定するために、原子番号の順に構造を構築できます。水素から始まり、そして...

Education

JoVE Core

化学

Electronic Structure of Atoms

原子の電子構造

KEY TERMS AND CONCEPTS

主要用語と概念

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 &quot;to build up.&quot; It says that each added electron enters the lowest-energy subshell available. The Pauli exclusion principle still applies, so electrons must follow the allowed quantum numbers. Higher-energy subshells do not fill until lower-energy subshells reach capacity.

A common filling-order diagram helps show the energy sequence of the atomic orbitals. Carbon is a useful example because it has atomic number 6. Four electrons fill the 1s and 2s orbitals, and the remaining two electrons go into the 2p subshell. At that point, the electrons can either pair in one 2p orbital or stay unpaired in two different p orbitals.

Hund's rule gives the lower-energy choice for degenerate orbitals, which are orbitals with the same energy. The rule states that electrons in a set of degenerate orbitals occupy the arrangement with the maximum number of unpaired electrons. In carbon, the two 2p electrons have the same n, l, and m_s quantum numbers, and they differ in m_l, which matches the Pauli exclusion principle.

Nitrogen, with atomic number 7, fills the 1s and 2s subshells and places one electron in each of the three 2p orbitals. These three electrons are unpaired. Oxygen, atomic number 8, has one pair of electrons in one 2p orbital and one single electron in each of the other two. Fluorine, atomic number 9, has only one 2p orbital with an unpaired electron.

Neon, atomic number 10, has all paired electrons. Its n = 1 and n = 2 shells are completely filled. This pattern shows how electron configurations build step by step across the first ten elements.

Electron Filling Order in Atomic Orbitals

electron-filling-order-in-atomic-orbitals

the wave nature of light

Measuring Light with Wavelength and Frequency

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the electromagnetic spectrum

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the bohr model

Bohr’s Quantized Atomic Orbits

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emission spectra

Line Spectra from Heated Gases

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the de broglie wavelength

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the uncertainty principle

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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

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atomic orbitals

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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

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the aufbau principle and hund's rule

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 electron configurations build by atomic number, why lower-energy orbitals fill first, and how Hund's rule shapes carbon, nitrogen, oxygen, fluorine, and neon.

Electron Filling Order in Atomic Orbitals | JoVE K12

chemistry

JoVE Core 化学は、簡潔で理解しやすいアニメーションビデオレッスンを使用して、一般的な化学の概念を生き生きとしたものにします。さらに、活動する科学者のビデオでは、現在世界中の実験室で行われている古典的そして独創的な研究・実験をお見せします。

Louisiana Student Standards for Science

High School

Matter And Its Interactions

HS-PS1-1

HS-PS1-2

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Structure And Properties Of Matter

Atomic structure

Tennessee Academic Standards

Matter and Its Interactions

CHEM1.PS1.12

Virginia  Standards of Learning

HIgh School

CH.2

CH.2.e

Physical Science

PS.2

PS.2.a

Arizona Science Standards

HS.P1

HS.P1U1.1

Texas Essential Knowledge and Skills

CHEM.6

CHEM.6.B

Alabama Course of Study Science

9-12.C.1.1.c

Next Generation Science Standards

Florida Department of Education

SC.912.P.8

SC.912.P.8.5

SC.912.P.10

SC.912.P.10.9

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-1.

HS. Chemical Reactions

HS-PS1-7.

Georgia Standards of Excellence

SC1.

electron-configuration-and-chemical-properties

Electron Configuration and Chemical Properties

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PS.Chm.1.1

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PS.Chm.1.2

Atomic Orbitals

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The Energies of Atomic Orbitals

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Electron Configuration of Multielectron Atoms

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Periodic Classification of the Elements

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The Periodic Table

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Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.Chm.2.1

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Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

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Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

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Analyze the structure of atoms and isotopes.

Electron Filling Order in Atomic Orbitals

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