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Questions and Answers

ما هو الشكل الهندسي للمركبات ذات تهيج SP3؟

  • مستوى
  • رباعي السطوح (correct)
  • مربع
  • مثلث

ما هي الزاوية بين الروابط في تهيج SP3؟

  • 109.5 درجة (correct)
  • 120 درجة
  • 90 درجة
  • 180 درجة

ما هي النسبة المئوية للتهجين في حالة تهيج SP2؟

  • 25% SP و 75% P
  • 33.33% SP و 66.67% P
  • 50% SP و 50% P (correct)
  • 75% SP و 25% P

ما هو تأثير التهجين على طول الروابط؟

<p>قوة الربط تزيد مع SP2 (B)</p> Signup and view all the answers

ما هو الشكل الهندسي للمركبات ذات تهيج SP؟

<p>خط مستقيم (B)</p> Signup and view all the answers

ما هي الزاوية المرتبطة بتهيج SP2؟

<p>120 درجة (A)</p> Signup and view all the answers

ما هو التوزيع الذري للنسب المئوية في حالة كيمياء CH3؟

<p>50% SP و 50% P (B)</p> Signup and view all the answers

ما هي الصيغة العامة للتهجين SP3؟

<p>C1H4 (B)</p> Signup and view all the answers

ما هي التركيبة النسبية للتهجين في SP3؟

<p>25% S و 75% P (D)</p> Signup and view all the answers

ما هي النسبة المئوية للخيار (C=C bond) في التفاعل المذكور؟

<p>33.33% (B)</p> Signup and view all the answers

أي من الروابط التالية هو الأقصر من حيث الطول؟

<p>C-H bond (B)</p> Signup and view all the answers

ما هو الصيغه الكيميائية للوحدة (i) المعطاة في الصورة؟

<p>C4H10 (B)</p> Signup and view all the answers

أي من الخيارات لا يمثل رابطة ثنائية؟

<p>CH3-C≡CH (D)</p> Signup and view all the answers

ما هي السالبية الكهربية للمكون الأكثر سالبية في التفاعل؟

<p>أكثر من 2.5 (D)</p> Signup and view all the answers

أي من الخيارات التالية تُستخدم لتحديد القطبية في المركبات الكيميائية؟

<p>السالبية الكهربية (B)</p> Signup and view all the answers

أي مركب من الخيارات التالية يحتوي على رابطة ثلاثية؟

<p>CH3-C≡CH (B)</p> Signup and view all the answers

ما هو الطول المتوقع للرابطة (C=C bond) في المركبات العضوية؟

<p>1.20 A° (C)</p> Signup and view all the answers

أي من الخيارات التالية تشير إلى مركب غير مشبع؟

<p>C2H4 (B)</p> Signup and view all the answers

ما هي النسبة المئوية للرابطة الأحادية (C-C bond) في المركبات المعطاة؟

<p>50% (B)</p> Signup and view all the answers

ما هي الطبيعة الأساسية للرابطة التساهمية؟

<p>رابطة مشتركة (D)</p> Signup and view all the answers

أي من الأوربيتال التالية تشكل رابطة تساهمية مع نوى هيدروجين؟

<p>1S (A)</p> Signup and view all the answers

ما هو مصطلح 'الربط المضاد' في الكيمياء العضوية؟

<p>الرابطة التي تعيق الاستقرار (D)</p> Signup and view all the answers

ما المقصود بتهجين الأوربيتال الذري؟

<p>دمج أوربيتالين لتشكيل جديدة (D)</p> Signup and view all the answers

ما هو الشكل الناتج عن تهجين الأوربيتال SP3؟

<p>رباعي السطوح (C)</p> Signup and view all the answers

ما هي خصائص الرابطة التساهمية؟

<p>تكون روابط قوية (C)</p> Signup and view all the answers

كيف يؤثر التهجين على خصائص المركبات؟

<p>يغير شكل الجزيئات (B)</p> Signup and view all the answers

أي من الجزيئات التالية يحتوي على رابطة تساهمية؟

<p>H2O (B)</p> Signup and view all the answers

ما هي النتيجة عند مزج الأوربيتال 2S و 2P؟

<p>تكوين أوربيتال SP (B)</p> Signup and view all the answers

أي من ذرات العناصر التالية لها احتمال أكبر لتكوين روابط تساهمية؟

<p>الأكسجين (A)</p> Signup and view all the answers

ما هي الجزيئات التي تشترك في تشكيل الرابطة التساهمية؟

<p>الذرات المتماثلة (D)</p> Signup and view all the answers

ما معنى 'الأوربيتال الجزيئي'؟

<p>مستوى طاقة مشترك بين الذرات (B)</p> Signup and view all the answers

هل يمكن أن تتكون رابطة تساهمية بين ذرتين من نوع مختلف؟

<p>نعم، لكن بشكل ضعيف (B)</p> Signup and view all the answers

ما هي العناصر التي تفضل أن تشارك إلكتروناتها في الرابطة التساهمية؟

<p>اللافلزات (D)</p> Signup and view all the answers

Flashcards

Structural isomers

Different compounds with the same molecular formula but different structural arrangements of atoms.

Alkane

A hydrocarbon containing only single bonds.

Alkene

A hydrocarbon containing a double bond.

Alkyne

A hydrocarbon containing a triple bond.

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Bond length (C-C)

Distance between two carbon atoms in a covalent bond.

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Bond length (C-H)

Distance between a carbon and a hydrogen atom in a covalent bond.

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Electronegativity

A measure of an atom's ability to attract electrons in a chemical bond.

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Polarity

A property of a molecule where one side of the molecule has a slight positive charge and the other side has a slight negative charge.

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Hydrocarbon

An organic compound consisting entirely of hydrogen and carbon atoms.

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Isomerism

The phenomenon where multiple molecules have the same chemical formula but different chemical structures, leading to different properties.

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SP hybridization

A type of hybridization involving one s-orbital and one p-orbital, resulting in two sp hybrid orbitals.

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SP3 hybridization

A type of hybridization involving one s-orbital and three p-orbitals, resulting in four sp3 hybrid orbitals.

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SP2 hybridization

A type of hybridization involving one s-orbital and two p-orbitals, resulting in three sp2 hybrid orbitals.

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Hybridization

The mixing of atomic orbitals to form new hybrid orbitals that are used to form chemical bonds.

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Bond strength

The strength of a chemical bond: higher strength means more energy is required to break it.

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Bond length

The distance between the nuclei of two atoms in a covalent bond.

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Percentage contribution (S and P)

The portion of s and p orbitals that makes up the hybrid orbital (like Sp, Sp2, or Sp3); determines the characteristics of the bond.

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Bond Angle

The angle between two bonds in a molecule

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Tetrahedral

A three-dimensional geometric shape with four equivalent faces and four identical corners.

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Sigma and Pi bonds

Types of covalent bonds. Sigma bonds are strong single bonds formed by head-on overlapping of orbitals. Pi bonds are weaker multiple bonds formed by side-to-side overlapping of orbitals.

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Organic Chemistry

The branch of chemistry dealing with carbon-containing compounds.

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Covalent Bond

A chemical bond formed by the sharing of electron pairs between atoms.

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Molecular Orbital

A region in a molecule where electrons are likely to be found.

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Bonding Molecular Orbital

A molecular orbital formed by combining atomic orbitals that lowers the energy.

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Antibonding Molecular Orbital

A molecular orbital formed when atomic orbitals combine that raises the energy.

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σ (sigma) bond

A covalent bond formed by head-on overlap of atomic orbitals.

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π (pi) bond

A covalent bond formed by sideways overlap of atomic orbitals.

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Atomic Orbital

A region of space around an atom where an electron is likely to be found.

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Hybridization

The mixing of atomic orbitals to form new hybrid orbitals.

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Ground State

The lowest energy state of an atom or molecule.

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sp3 hybridization

The combination of one s and three p atomic orbitals to form four sp3 hybrid orbitals.

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H2 molecule

Diatomic molecule formed by a covalent bond between two hydrogen atoms.

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HCl molecule

Molecule formed by the bonding between hydrogen and chlorine atoms.

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Cl2 molecule

Diatomic chlorine molecule formed by a covalent bond between two chlorine atoms.

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Formation of covalent bond

Process of atoms sharing electrons to achieve a stable configuration.

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Study Notes

Organic Chemistry

  • This branch of science studies carbon compounds.
  • All organic compounds contain carbon.
  • Most organic compounds consist of molecules with covalent bonds, although some contain ionic bonds.
  • Carbon atoms can connect to form long, continuous, branched, acyclic, or cyclic chains.
  • Hydrogen is a common element present with carbon, as in hydrocarbons.
  • Oxygen is also found with carbon and hydrogen in compounds like alcohols, aldehydes, and ketones.
  • Nitrogen can combine with carbon and hydrogen, as in amines, nitriles, nitro compounds, and others.
  • Halogens can also be present with carbon and hydrogen, forming alkyl halides or dihalogenated derivatives, among others).
  • Other elements like sulfur, phosphorus, and certain metals can also be part of organic compounds.
  • Organic compounds are used in various applications, including dyes, antibiotics, synthetic fibers, pesticides, plastics, and fragrances.

Formation of Covalent Bonds

  • Molecular Orbital: Covalent bonds form through the overlap of atomic orbitals.

  • This overlap creates a new orbital, called a molecular orbital, which surrounds both atoms.

  • The overlap leads to bonding and antibonding molecular orbitals.

  • Bonding orbitals (sigma (σ) bonds) have high electron density between the atoms.

  • Antibonding orbitals have lower electron density.

  • Head-to-head overlap of atomic orbitals (on a straight line) forms sigma (σ) bonds.

  • Example: H₂ is formed from S-S overlap.

  • Example: HCl is formed from S-P overlap.

  • Example: Cl₂ is formed from P-P overlap (lateral overlap creating pi (π) bonds).

  • Pi (π) bonds occur in unsaturated compounds with double bonds (as in ethylene) or triple bonds (as in acetylene).

  • Bond strength and length depend on orbital overlap and atomic distance.

Hybridization of Atomic Orbitals

  • Carbon's electron configuration in its ground state doesn't account for its tetravalency.
  • To achieve tetravalency, carbon undergoes hybridization.
  • Hybridization mix or blend) atomic orbitals to create new orbitals with equivalent energy.
  • SP³ hybridization: Mixing the 2s and three 2p orbitals creates four new SP³ hybrid orbitals.
  • SP³ hybridized orbitals are tetrahedral, with a bond angle of roughly 109.5°.
  • Each SP³ orbital has 25% 2s character and 75% 2p character.
  • SP² hybridization: Mixing the 2s orbital and two 2p orbitals forms three SP² hybrid orbitals in a plane, with a bond angle of approximately 120°.
  • The remaining p orbital is perpendicular to the plane of the SP² hybrid orbitals and has 67% 2p character.
  • SP hybridization: Mixing the 2s orbital and one 2p orbital gives two SP hybrid orbitals in a linear arrangement, with a bond angle of 180°.
  • Each SP orbital has 50% 2s character and 50% 2p character.
  • These three types of hybridization (SP, SP³, SP²) are important in determining the characteristics of organic compounds.

Classification of Organic Compounds

  • Aliphatic Hydrocarbons: These compounds consist of carbon and oxygen.
    • Saturated hydrocarbons (alkanes) with single bonds.
    • Unsaturated hydrocarbons (alkenes) with double bonds.
    • Unsaturated hydrocarbons (alkynes) with triple bonds.
  • Naming Alkanes: Methods to name alkanes with five or more carbons
  • Isomers: Compounds with the same molecular formula but different structural formulas (e.g., n-butane and iso-butane).
  • Alkyl Groups: Groups formed by removing a hydrogen atom from an alkane.
  • Naming with IUPAC: A systematic method for naming organic compounds.

Functional Groups

  • Alcohols: Contain the hydroxyl (-OH) functional group.
  • Aldehydes: Contain the carbonyl group (C=O) bonded to a hydrogen atom.
  • Ketones: Contain the carbonyl group (C=O) bonded to two alkyl groups.
  • Carboxylic Acids: Contain the carboxyl group (-COOH).
  • Amines: Derived from ammonia (NH3) by replacing one or more hydrogens with alkyl groups.
  • Ethers: Contain an oxygen atom bonded to two alkyl groups.
  • Thiols: Contain a sulfur atom bonded to a hydrogen atom.
  • Thioethers: Contain a sulfur atom bonded to two alkyl groups.

Reactions of Functional Groups

  • Note various reactions including additions, substitutions, eliminations, and rearrangements.
  • These are described in detail for each functional group, including the conditions required for each.

Isomerism

  • Chain Isomerism: Isomers with different carbon-chain arrangements.
  • Positional Isomerism: Isomers with the same carbon chain but different positions of a functional group or substituent.
  • Functional Group Isomerism: Isomers with different functional groups.

Optical Isomerism

  • Chirality: A property of molecules that have non-superimposable mirror images.
  • Enantiomers: Non-superimposable mirror images of a chiral molecule.

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