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

تتكون الذرة من ثلاثة جسيمات دون ذرية - الإلكترونات والبروتونات والنيوترونات. تشكل البروتونات موجبة الشحنة والنيوترونات المحايدة كهربائيا النواة الذرية ، حيث توجد كل الشحنة الموجبة ومعظم كتلة الذرة.
الإلكترونات هي المكونات سالبة الشحنة ومنخفضة الكتلة الموجودة في المساحة الفارغة حول النواة. تكون الذرة محايدة كهربائيا عندما تحتوي على عدد من الإلكترونات مثل البروتونات.
تظهر الإلكترونات طبيعة مزدوجة - الجسيم والموجة. موقعها في الفضاء وطاقتها هي خصائص تكميلية. لذلك ، بالنسبة للإلكترون ذو طاقة محددة جيدا ، فإن موقعه غير مؤكد.
يتنبأ النموذج الميكانيكي الكمومي للذرة بأنه يمكن تحديد احتمال العثور على إلكترون لطاقة معينة في منطقة ثلاثية الأبعاد في الفضاء من مربع الدالة الموجية التي تعبر عن طبيعة الإلكترون الشبيهة بالموجة ، والتي تسمى أيضا كثافة احتمال الإلكترون.
تسمى الوظيفة التي تصف الموقع المكاني المحتمل لإلكترون ذو طاقة معينة في الذرة بالمدار الذري.
يتوافق كل مدار مع مجموعة فريدة من ثلاثة أرقام كمية. الرقم الكمي الرئيسي ، n ، يجمع المدارات في مستويات طاقة أو قذائف.
الزخم الزاوي ، أو السمت ، الرقم الكمي ، l ، يجمع المدارات داخل الأصداف في أغلفة فرعية. تتوافق كل قيمة ل مع مدار s أو p أو d أو f بأشكال مختلفة.
قد يكون لبعض الأشكال المدارية اتجاهات محتملة متعددة ، كل منها مرتبط برقم كمي مغناطيسي ، ml. عدد اتجاهات غلاف فرعي معين يساوي اثنين لتر زائد واحد.
يرتبط الرقم الكمي الرابع - الرقم الكمي للدوران ، ms - بالإلكترونات التي تحتل مدارا وله قيمتان محتملتان فقط: "زائد النصف" و "ناقص النصف". هذا يضمن عدم وجود إلكترونين في الذرة لهما نفس القيم لجميع الأعداد الكمومية الأربعة.
ينتج عن تراكب المدارات فوق بعضها البعض شكل كروي تقريبا ، مثل "سحابة" من الإلكترونات المحيطة بالنواة. هذا هو السبب في أن الذرات يتم تمثيلها بشكل عام على شكل كرات.

البنية الإلكترونية للذرات

<div style="direction:rtl">
تتكون الذرة من البروتونات والنيوترونات الموجودة داخل النواة المركزية الكثيفة التي تسمى النواة، مع وجود الإلكترونات حول النواة. وبالأخذ في الاعتبار ازدواجية موجة الإلكترونات والجسيمات وعدم اليقين في موضعها حول النواة، توفر ميكانيكا الكم نموذجًا أكثر دقة للبنية الذرية. وتصف المدارات الذرية بأنها المناطق المحيطة بالنواة حيث توجد إلكترونات ذات طاقة محددة، وتتميز بأربعة أعداد كمية: n، l، ml، وms.
<h4>النموذج الميكانيكي الكمي</h4>

تتكون الذرة من نواة صغيرة موجبة الشحنة محاطة بالإلكترونات. تحتوي النواة على بروتونات ونيوترونات. البروتونات لها شحنة +1 وكتلتها 1.0073 amu. النيوترونات لها شحنة صفرية وكتلتها 1.0087 amu. تمتلك الإلكترونات شحنة −1 وكتلة قدرها 0.00055 amu. يُطلق على عدد البروتونات في النواة اسم العدد الذري(Z) ويحدد الهوية العنصرية للذرة. يسمى مجموع أعداد البروتونات والنيوترونات في النواة بالعدد الكتلي، ويعبر عنه بـ amu، ويساوي تقريبًا كتلة الذرة. تكون الذرة متعادلة عندما تحتوي على أعداد متساوية من الإلكترونات والبروتونات.

تم اقتراح نماذج مختلفة لوصف البنية الذرية موضحة توزيع الإلكترونات حول النواة. حددت علاقة دي برولي أن الإلكترونات لها خصائص كل من الجسيم والموجة. وعند التعمق في الازدواجية الموجية-الجسيمية بشكل أكبر، قدم هايزنبرغ مبدأ عدم اليقين: لا يمكن تحديد الموقع (المرتبط بطبيعة الجسيم) والسرعة أو الطاقة (المرتبطة بالطبيعة الموجية) للإلكترون في وقت واحد وبدقة كاملة. يعطي النموذج الميكانيكي الكمي صورة أكثر دقة للبنية الذرية. فهو يصف الموقع ثلاثي الأبعاد للإلكترون ذي الطاقة المحددة، الموجود في الذرة، بطريقة احتمالية بدلالة مربع الدالة الموجية، ψ2. تصف الدوال الموجية الذرية، أو المدارات الذرية، المناطق الموجودة في الذرة التي من المرجح أن توجد فيها الإلكترونات.

يتميز المدار الذري بثلاثة أعداد كمية. يقوم عدد الكم الرئيسي، n، بتجميع المدارات من حيث موقع مستوى الطاقة، أو "الغلاف". يقوم العدد الكمي الزاوي أو السمتي، l,، بتجميع المدارات بناءً على أشكالها في "أغلفة فرعية". تحتوي على قيم أعداد صحيحة من 0 إلى n – 1 ويتم تمثيلها بالأحرف: s(l = 1), d (l = 2), f (l = 3), g (l = 4), and h (l = 5). عدد الكم المغناطيسي، ml، بقيم 2l + 1 تتراوح من –l إلى +l، يصف اتجاه المدار في الفضاء. بالإضافة إلى ذلك، كل إلكترون لديه عدد كمي مغزلي، ms، يمكن أن يساوي ±1/2. لا يمكن لأي إلكترونين في نفس الذرة أن يكون لهما نفس مجموعة القيم لجميع الأعداد الكمية الأربعة.

هذا النص مقتبس من<a href="https://openstax.org/books/chemistry-2e/pages/6-3-development-of-quantum-theory#0"> Openstax, Chemistry 2e, Section 6</a>.

</div>


تتكون الذرة من البروتونات والنيوترونات ، والتي توجد داخل النواة المركزية الكثيفة المسماة النواة ، مع وجود الإلكترونات حول ...

Education

JoVE Core

Organic Chemistry

الكيمياء العضوية

Unit 1

الوحدة الأولى

Covalent Bonding and Structure

الترابط التساهمي والبنية

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

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

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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...

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chemical bonds

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intermolecular forces and physical properties

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introduction to functional groups

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HS-PS1-2

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

C-PS2-6.

Physics

P-PS2-6.

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HS-PS1-4

Atomic Orbitals and Quantum Numbers

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