Name: electron filling order in atomic orbitals
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 3 min 2 s
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K12 Standards

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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

נזכיר כי לאורביטלים אטומיים יש אנרגיות שונות והם יכולים להכיל שני אלקטרונים כל אחד. כלל אופבאו מכתיב את הפיזור של אלקטרונים בין תתי קליפות האטום, וחוק הונד של ריבוי מקסימלי מסביר את מילוי האורביטלים בתתי הקליפות. כלל אופבאו קובע כי במצב היסוד, אלקטרונים ממלאים אורביטלים אטומיים מהאנרגיה הנמוכה לגבוהה ביותר כדי להשיג את תצורת האנרגיה הנמוכה ביותר.למרות שבדרך כלל האנרגיה עולה עם מספר הקליפה, החדירה הגדולה יותר של אורביטלי s מובילה לעיתים קרובות לכך שאורביטלי 4-s ו-5-s הם בעלי אנרגיות נמוכות יותר מאורביטלי 3-d ו-4-d בהתאמה. ניתן לזכור את הסדר באמצעות דיאגרמות כמו זו, שבה כיוון החץ מציג את הרצף שבו אלקטרונים מתחלקים לאורביטלים. חשבו על כתיבה של תצורת האלקטרונים של פחמן יסוד עם מספר אטומי שש.ללא ספק, אורביטל 1-s, בעל האנרגיה הנמוכה ביותר אמור להתמלא לפני אורביטל 2-s. כל אורביטל יכול להכיל שני אלקטרונים לכל היותר. האלקטרון החמישי נכנס לתת קליפה 2-p.אך איזה משלושת אורביטלי 2-p היא מאכלסת? טוב, ההנחה היא כי האורביטלים בכל תת קליפה הם מנווונים, מה שאומר שיש להם את אותה האנרגיה. לכן האלקטרון החמישי יכול להיכנס לכל אחד משלושת אורביטלי 2-p המנוונים.מה עם האלקטרון השישי? האם הוא נכנס לאורביטל ה-2-p עם עוד אלקטרון או לאחד מאורביטלי 2-p הריקים? על פי כלל הריבוי המרבי של הונד, האלקטרונים מאכלסים בנפרד את כל האורביטלים ברמת אנרגיה נתונה לפני שהם מתחילים להיקשר, ולאלקטרונים הלא קושרים לא יכולים להיות סיבובים הפוכים:הסיבובים שלהם חייבים להיות מקבילים.לכן, בפחמן, שני אלקטרוני 2-p חייבים לאכלס שני אורביטלים שונים ולהיות בעלי ספינים מקבילים. כך אלקטרונים יכולים להתפזר על פני שטח גדול יותר. זה מקטין את המיסוך שלהם זה מזה ובכך ממזער את האנרגיה של האטום.בחנקן, כל אחד משלושת אורביטלי 2-p מאוכלס בנפרד. בחמצן, ברגע שאורביטלי 2-p המנוונים מתמלאים בנפרד, האלקטרון האחרון חייב להיקשר עם 2-p נוסף. האטום כולל שני אלקטרונים לא קושרים.תצורת האלקטרונים של ניאון מגלה שהקליפה החיצונית ביותר מתמלאת עד לקיבולת המרבית של שמונה אלקטרונים. לניאון יש שני אלקטרונים, הנקראים אלקטרוני ליבה בקליפה הפנימית, ושמונה אלקטרונים, הנקראים אלקטרוני ערכיות, בקליפה החיצונית ביותר.

עקרון האאופבאו וכלל הונד

<div style="direction:rtl">

כדי לקבוע את תצורת האלקטרונים עבור כל אטום מסוים, נוכל לבנות את המבנים לפי סדר המספרים האטומיים. מתחילים במימן, וממשיכים לאורך מחזורים של הטבלה המחזורית, אנו מוסיפים פרוטון אחד בכל פעם לגרעין ואלקטרון אחד לתת-הקליפה המתאימה עד שתיארנו את תצורות האלקטרונים של כל היסודות. הליך זה נקרא עקרון האאופבאו, מהמילה הגרמנית aufbau ("לבנות"). כל אלקטרון שנוסף תופס את התת-קליפה של האנרגיה הנמוכה ביותר הזמינה, בכפוף למגבלות המוטלות על ידי המספרים הקוונטיים המותרים על פי עקרון האיסור של פאולי. אלקטרונים נכנסים לתת-קליפות בעלות אנרגיה גבוהה רק לאחר שתת-קליפות בעלות אנרגיה נמוכה יותר מולאו עד הסוף. איור 1 ממחיש את הדרך המסורתית לזכור את סדר המילוי של אורביטלים אטומיים. 
<img alt="Figure1" src="https://www.jove.com/files/core/CDNSource/lessons/986/986Image_1.png" style="width: 700px;"> 

איור 1 תרשים זה מתאר את סדר האנרגיה עבור אורביטלים אטומיים והוא שימושי עבור גזירת תצורות אלקטרונים במצב יסוד. 

שקול לכתוב את תצורת האלקטרונים עבור פחמן - יסוד עם מספר אטומי שש. ארבעה אלקטרונים ממלאים את האורביטלים של 1s ו-2s. שני האלקטרונים הנותרים תופסים את התת-קליפה 2p. כעת יש לנו אפשרות למלא את אחד מהאורביטלים של 2p ולשייך את האלקטרונים או להשאיר את האלקטרונים בלתי מזווגים בשני אורביטלים p שונים, אך מנוונים. האורביטלים ממולאים כמתואר על ידי הכלל של הונד: תצורת האנרגיה הנמוכה ביותר עבור אטום עם אלקטרונים בתוך קבוצה של אורביטלים מנוונים היא זו בעלת המספר המרבי של אלקטרונים בלתי מזווגים. לפיכך, לשני האלקטרונים באורביטלי הפחמן 2p יש מספרים קוונטיים זהים n, l ו-ms והם שונים במספרם הקוונטי ב-ml (בהתאם לעקרון האיסור של פאולי). דיאגרמת האורביטל של פחמן, עם תצורת אלקטרונים של 1s22s21p2 היא: 

<img alt="Figure2" src="https://www.jove.com/files/core/CDNSource/lessons/986/986Image_2.png" style="width: 300px;"> 

חנקן (מספר אטומי 7) ממלא את התת-קליפות 1s ו-2s ויש לו אלקטרון אחד בכל אחד משלושת האורביטלים של 2p, בהתאם לכלל הונד. לשלושת האלקטרונים הללו יש ספינים לא מזווגים. לחמצן (מספר אטומי 8) יש זוג אלקטרונים בכל אחד מהאורביטלים של 2p (לאלקטרונים יש ספינים מנוגדים) ואלקטרון בודד בכל אחד מהשניים האחרים. לפלואור (מספר אטומי 9) יש רק אורביטל אחד של 2p המכיל אלקטרון לא מזווג. כל האלקטרונים בניאון הגז האציל (מספר אטומי 10) מזווגים, וכל האורביטלים בקליפות n = 1 ו-n = 2 מלאים.

טקסט זה מותאם מ- <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.</a></div>

כדי לקבוע את תצורת האלקטרונים עבור אטום מסוים, אנו יכולים לבנות את המבנים לפי סדר המספרים האטומיים. החל ממימן, ו...

Education

JoVE Core

כימיה

אחד

Electronic Structure of Atoms

מבנה אלקטרוני של אטומים

KEY TERMS AND CONCEPTS

מונחים ומושגים מרכזיים

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

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

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the de broglie wavelength

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...

the uncertainty principle

Electron Position and Momentum Limits

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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

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 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

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Matter And Its Interactions

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Structure And Properties Of Matter

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New York State Science Learning Standards

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Georgia Standards of Excellence

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electron-configuration-and-chemical-properties

Electron Configuration and Chemical Properties

Scientific Laws and Theories

Scientific Laws

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Classifying Matter by State

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Classifying Matter by Composition

Matter: Pure Substances and Mixtures
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The Atomic Theory of Matter

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Subatomic Particles

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Elements: Chemical Symbols and Isotopes

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Radioactivity and Nuclear Equations

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Types of Radioactivity

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Nuclear Binding Energy

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Radioactive Decay and Radiometric Dating

Radioactivity is a spontaneous disintegration of an unstable nuclide and is a random process, as all the nuclei in the sample do not decay simultaneously. ...

Nuclear Fission

Many heavier elements with smaller binding energies per nucleon can decompose into more stable elements that have intermediate mass numbers and larger ...

Nuclear Power

Controlled nuclear fission reactions are used to generate electricity. Any nuclear reactor that produces power via the fission of uranium or plutonium by ...

Nuclear Fusion

The process of converting very light nuclei into heavier nuclei is also accompanied by the conversion of mass into large amounts of energy, a process ...

Nuclear Transmutation

Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with ...

Use models to compare nuclear reactions including alpha decay, beta decay and gamma decay; nuclear fusion and nuclear fission.

PS.Chm.1.2

Atomic Orbitals

An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution ...

The Pauli Exclusion Principle

The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that ...

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are ...

To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and ...

Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the ...

Use models to explain how electrons are distributed in atoms.

Periodic Classification of the Elements

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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 ...

Atomic Mass

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Molar Mass

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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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Atomic Radii and Effective Nuclear Charge

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Ionic Radii

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Ionization Energy

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Electron Affinity

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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

Types of Chemical Bonds

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Lewis Symbols and the Octet Rule

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Ionic Bonding and Electron Transfer

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The Born-Haber Cycle

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An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

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 ...

Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity.&#xA0;

Electronegativity values of ...

bond-polarity-dipole-moment-and-percent-ionic-character

Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

The absolute value of the difference in electronegativity (&Delta;EN) of two bonded atoms provides a rough measure of the polarity to be ...

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

PS.Chm.3.1

Analyze the structure of atoms and isotopes.

Electron Filling Order in Atomic Orbitals

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