Name: electron regions in atomic orbitals
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 44 s
Channel: JoVE

K12 Standards

Texas Essential Knowledge and Skills

High School

Chemistry and Physics

IPC.7

IPC.7.E

Atomic Orbitals

전자가 발견될 가능성이 가장 높은 영역인 전자 구름의 밀도가 가장 높은 영역은 원자 궤도로 설명할 수 있습니다. 원자 궤도의 형태는 방위 양자수 엘에 의해 결정됩니다. 엘 값은 주 양자수 n을 기준으로 하며 엘의 가능한 값 범위는 영에서 엔 마이너스 일 입니다.

n이 일보다 크면 여러 개의 하위 준위가 존재합니다. 엘의 값은 s, p, d 또는 f 궤도 중 하나에 해당합니다. 에너지가 가장 낮은 궤도는 엘 에스 궤도입니다.

이것은 구면 대칭 궤도입니다. 엘 에스 궤도의 확률 밀도는 전자가 핵에서 발견될 가능성이 가장 높다는 것을 보여줍니다. 하지만 양성자와 전자 사이의 정전기적인 힘을 고려하면 이것은 가능성이 낮습니다.

확률 밀도에 반지름이 r인 얇은 구면 껍질의 부피를 곱하는 것이 더 잘 표현한 것입니다. 핵에서 r만큼 떨어진 거리에 있는 얇은 껍질 안에서 전자를 찾을 수 있는 총 확률은 방사 분포 함수입니다. 수소의 경우 전자를 발견할 수 있는 가장 큰 확률은 핵으로부터 52.9 피코미터 거리에 있습니다.

따라서 수소의 엘 에스 원자 궤도 형태는 반경이 52.9 피코미터인 구면입니다. 2 에스 와 3 에스 궤도 또한 구면입니다. 크기가 더 크고 마디가 있습니다.

마디에서 전자를 발견할 확률은 0입니다. n이 2 이상인 주 준위는 3개의 p 오비탈을 포함합니다. 이것들은 핵에 노드가 있는 로브모양을 가집니다.

그의 배향은 엠 엘 값으로 설명됩니다. 세 개의 p-오비탈은 서로 직교합니다. n이 3 이상인 주 준위는 5개의 d 오비탈을 가지고 있습니다.

클로버잎 모양의 d 궤도에는 4개의 전자 고밀도 로브와 2개의 수직 노드 면이 있습니다. d 오비탈 에서 하나는 약간 다릅니다. f 오비탈에는 더 많은 로브와 노드가 있습니다.

이러한 오비탈은 n이 4 이상인 주 준위에 존재합니다. 궤도들을 서로 겹쳐놓으면 대략적인 구형의 모양이 나타납니다. 이런 이유로 원자들은 일반적으로 구로 표현됩니다.

원자 궤도

원자 궤도는 전자가 존재할 확률이 가장 높은 원자의 3차원 영역을 나타냅니다. 방사형 분포 함수는 핵으로부터 거리 r에 있는 얇은 껍질 내에서 전자를 발견할 전체 확률을 나타냅니다. 원자 궤도는 각운동량 양자수인 l에 의해 결정되는 독특한 모양을 가지고 있습니다. 궤도는 종종 구름의 가장 밀도가 높은 영역을 둘러싸는 경계면으로 그려집니다.

각운동량 양자수는 l = 0, 1, 2, …, n – 1의 값을 가질 수 있는 정수입니다. 주양자수가 1(n = 1)인 궤도는 하나의 l 값만 가질 수 있습니다( l = 0), 반면 주양자수 2(n = 2)는 l = 0 및 l = 1을 허용합니다. l 값이 동일한 궤도는 부껍질을 정의합니다.

l = 0인 궤도를 s 궤도라고 하며 s 부껍질을 구성합니다. 값 l = 1은 p 궤도에 해당합니다. 주어진 n에 대해 p 오비탈은 p 서브쉘을 구성합니다(즉, n = 3인 경우 3p). l = 2인 오비탈을 d 오비탈이라고 합니다. l = 3, 4, 5인 궤도는 f, g 및 h 궤도입니다.

에너지가 가장 낮은 궤도는 1s 궤도입니다. 이것은 구형 대칭 궤도입니다. 1s 오비탈의 확률 밀도(ψ^2)는 전자가 핵에서 발견될 가능성이 가장 높다는 것을 의미합니다. 그러나 양성자와 전자 사이의 정전기력을 고려할 때 이는 전자가 어디에 위치하는지 정확하게 나타내지 않습니다. 대신에, 주어진 반경 r의 궤도에서 전자를 발견할 전체 확률의 플롯인 방사형 분포 함수가 사용됩니다. 방사형 분포 함수는 확률 밀도에 반경 r을 갖는 얇은 구형 껍질의 부피를 곱하여 구합니다. 수소의 1s 궤도의 경우 방사형 분포 함수는 핵에서 값 0을 가지며, 이는 r이 증가함에 따라 감소하기 전에 52.9피코미터에서 최대값으로 증가합니다.

특정 궤도에 위치한 전자를 찾을 확률 밀도가 0이 되는 핵으로부터 특정 거리가 있습니다. 즉, 이 궤도에 대한 이 거리에서 파동함수 ψ의 값은 0입니다. 이러한 r 값을 방사형 노드(radial node)라고 합니다. 궤도의 방사형 노드 수는 n - l - 1입니다. n = 1인 2s 궤도의 경우 방사형 노드가 1개 있는 반면, 3s 궤도는 방사형 노드가 두 개 있습니다.

n = 2 이상의 각 주 준위에는 3개의 p 궤도가 포함됩니다. 세 개의 p 오비탈에는 핵에 노드가 있는 두 개의 돌출부가 있습니다. 공간에서 p 오비탈의 방향은 m_l 값으로 설명됩니다. 세 개의 p 오비탈은 서로 수직(직교)합니다. 더 높은 p 오비탈(3p, 4p, 5p 이상)은 모양이 비슷하지만 방사형 노드가 추가되어 크기가 더 큽니다.

n = 3 이상의 주준위에는 5개의 d 궤도가 포함됩니다. 이 궤도 중 4개는 클로버잎 모양으로 구성되며 4개의 전자 밀도가 높은 돌출부가 있습니다. 핵에서 교차하는 두 개의 수직 절점 평면이 있습니다. 이 노드 평면에서 전자 밀도는 0입니다. d 오비탈 중 하나는 모양이 약간 다르며 xy 평면에 도넛 모양의 고리가 있는 z축 방향으로 두 개의 돌출부가 있습니다. n = 4 이상의 주준위에는 복잡한 모양을 갖는 7개의 f 오비탈이 포함되어 있습니다. 이 궤도에는 d 궤도보다 더 많은 노드와 로브가 있습니다.

<img alt="Figure1" src="https://www.jove.com/files/core/CDNSource/lessons/983/983Image 1.png" style="width: 700px;" />

Figure 1: 대표적인 s, p, d 및 f 궤도.

원자 궤도의 이러한 다양한 모양은 전자가 발견될 가능성이 있는 3차원 영역을 나타냅니다. 모든 궤도는 함께 대략 구형 모양을 구성하므로 원자는 일반적으로 구로 표시됩니다.

이 문서는 에서 발췌되었습니다 <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>

원자 궤도(atomic orbital)는 전자가 존재할 확률이 가장 높은 원자의 3차원 영역을 나타냅니다. 방사형 분포 ...

Education

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JoVE Core

Chemistry

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하나

Electronic Structure of Atoms

원자의 전자 구조

KEY TERMS AND CONCEPTS

주요 용어 및 개념

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 = 0 orbitals are s orbitals, and they make up s subshells. The l = 1 orbitals are p orbitals, which form a p subshell such as 3p when n = 3. The l = 2 orbitals are d orbitals. The l = 3, 4, and 5 orbitals are called f, g, and h orbitals.

The lowest-energy orbital is the 1s orbital. It is spherically symmetric. The probability density, ψ², suggests that an electron is most likely found at the nucleus. But this does not fully match electron behavior. The radial distribution function gives the total probability of finding an electron at a distance r from the nucleus. It is found by multiplying the probability density by the volume of thin spherical shells.

For the 1s orbital of hydrogen, the radial distribution function is zero at the nucleus. It rises to a maximum at 52.9 picometers and then decreases as r increases. Some distances from the nucleus have zero probability density for a given orbital. These points are called radial nodes. The number of radial nodes is n - l - 1. A 2s orbital has one radial node, and a 3s orbital has two.

Each principal level with n = 2 or more contains three p orbitals. Each p orbital has two lobes and a node at the nucleus. Their orientation in space is described by m_l. The three p orbitals are mutually perpendicular. Higher p orbitals, such as 3p, 4p, and 5p, have the same general shape but are larger and contain additional radial nodes.

Principal levels with n = 3 or more contain five d orbitals. Four of them have a cloverleaf shape with four electron-dense lobes. They also have two perpendicular nodal planes that meet at the nucleus. The fifth d orbital has two lobes along the z-axis and a donut-shaped ring in the xy plane.

Principal levels with n = 4 and greater contain seven f orbitals. These orbitals have complex shapes with more nodes and lobes than d orbitals. Together, s, p, d, and f orbitals help explain why atoms are often drawn as spheres, even though the electron regions inside them have distinct shapes.

Electron Regions in Atomic Orbitals

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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 ...

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 ...

Melting Points

Melting Points in Organic Chemistry
The melting point of a compound is the temperature at which the solid phase transitions into the liquid phase at a ...

Boiling Points

Source: Lara Al Hariri at the University of Massachusetts Amherst, MA, USA

	Preparation of the LaboratoryExpand
	Here, we show the laboratory preparation ...

Explain how physical and chemical properties of substances are related to their usage in everyday life such as in sunscreen, cookware, industrial applications, and fuels.

IPC.7.C

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 ...

Metal Flame Emission

Metal Flame Emission
Flame testing is an analytical technique where a sample is placed in a flame, and the characteristic flame color is used to identify ...

Explain how electrons can transition from a high energy level to a low energy state, emitting photons at different frequencies for different energy transitions.

Science concepts. The student knows that relationships exist between the structure and properties of matter. The student is expected to:

Electron Regions in Atomic Orbitals

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