Organic Compounds Chapter 12

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Questions and Answers

Which type of intermolecular force is characterized by a strong attraction between molecules containing hydrogen bonded to highly electronegative atoms?

  • Dipole-Dipole Attractions
  • Dispersion Forces
  • Hydrogen Bonds (correct)
  • Ionic Bonds

How are dipole-dipole attractions between polar molecules generated?

  • Due to lone pairs of electrons
  • From the partial positive and negative charges (correct)
  • Through nonpolar molecular interactions
  • By covalent bonding

What is the correct order of increasing electronegativity for the following elements: H, O, N?

  • H < O < N
  • O < N < H
  • O < H < N
  • N < H < O (correct)

Which of the following represents a polyatomic ion?

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

What is the general naming convention prefix for a hydrocarbon containing four carbon atoms?

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

What type of hydrocarbon is characterized by containing only single bonds?

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

In which scenario would you apply the lowest whole number ratio for writing a compound's formula?

<p>When combining ionic compounds like Na⁺ and Cl⁻ (B)</p> Signup and view all the answers

Which of the following is NOT a common pitfall when determining the formula of an ionic compound?

<p>Incorrectly identifying the ionic nature of bonding (C)</p> Signup and view all the answers

What distinguishes an alkene from an alkyne?

<p>Alkenes contain a double bond, while alkynes contain a triple bond. (B)</p> Signup and view all the answers

Which of the following best describes structural isomers?

<p>Compounds that differ only in the arrangement of their atoms. (A)</p> Signup and view all the answers

Which reaction type involves two or more reactants combining to form a single product?

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

What is meant by the term 'limiting reagent' in a chemical reaction?

<p>The reactant that is completely consumed, limiting the amount of product formed. (C)</p> Signup and view all the answers

In an exothermic reaction, what happens to the heat content?

<p>Heat is released to the surroundings. (C)</p> Signup and view all the answers

What is Boyle's Law regarding the relationship between pressure and volume?

<p>At constant temperature, pressure is inversely proportional to volume. (C)</p> Signup and view all the answers

Which change occurs during inhalation in the breathing process?

<p>Lung volume increases, causing pressure to decrease. (A)</p> Signup and view all the answers

What does the Ideal Gas Law equation (PV = nRT) relate?

<p>Pressure, volume, and temperature of a gas. (D)</p> Signup and view all the answers

What effect does an increase in temperature have on gas particles?

<p>Increases the pressure if volume is constant. (C)</p> Signup and view all the answers

In gas solubility, how does temperature typically affect solids and gases?

<p>Solubility of solids increases and that of gases decreases. (D)</p> Signup and view all the answers

Which of the following is a key principle when balancing chemical equations?

<p>Adjust coefficients to reach the simplest ratio. (D)</p> Signup and view all the answers

What is the mole, defined in chemistry?

<p>A unit representing 6.022 x 10^23 particles. (A)</p> Signup and view all the answers

What is a characteristic of cis-trans isomerism?

<p>It results from the rigidity of double bonds in alkenes. (C)</p> Signup and view all the answers

Flashcards

Lewis Structure

A diagram representing the bonding between atoms and lone pairs of electrons in a molecule.

Electronegativity

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

Hydrogen Bonds

Strong attractive forces between molecules with hydrogen bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine.

Dipole-Dipole Attractions

Attractions between polar molecules due to their partial positive and negative charges.

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Dispersion Forces

Weak, temporary attractions between molecules due to fluctuating electron clouds.

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Composition of Organic Compounds

Organic compounds are primarily composed of carbon and hydrogen, sometimes with other nonmetals.

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Bonding in Organic Compounds

Every carbon atom in an organic molecule forms four bonds.

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IUPAC Naming

A standardized system for naming organic compounds.

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Alkenes

Hydrocarbons containing one or more double bonds between carbon atoms, creating a chain of a straight, branched, or cyclic structure.

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Alkynes

Hydrocarbons containing one or more triple bonds between carbon atoms.

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Cycloalkanes

Hydrocarbons where carbon atoms form a closed ring structure. They have a general formula of CnH2n.

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Cis-Trans Isomers

Type of isomerism where molecules have the same molecular formula but differ in the arrangement of atoms around a double bond.

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Structural Isomers

Isomers that differ in the arrangement of atoms or groups, leading to different chemical and physical properties.

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Balancing Chemical Equations

The process of ensuring every element has the same number of atoms on both sides of a chemical equation.

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Limiting Reagent

The reactant that gets completely used up first, limiting the amount of product formed.

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Percent Yield

The ratio of the actual quantity of product obtained to the theoretical yield, expressed as a percentage.

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The Mole

A unit of measurement representing 6.022 x 10^23 particles, such as atoms or molecules.

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Enthalpy Change (ΔH)

The change in heat content during a chemical reaction.

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Exothermic Reactions

Reactions that release heat to the surroundings, resulting in a temperature increase.

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Endothermic Reactions

Reactions that absorb heat from the surroundings, resulting in a temperature decrease.

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Temperature (T) of a Gas

The average kinetic energy of the gas particles.

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Volume (V) of a Gas

The space occupied by the gas, which is determined by the container.

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Amount (n) of a Gas

The number of moles of gas present in a sample.

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Study Notes

Lewis Structures and Electronegativity

  • Lewis structures depict atomic bonding and electron pairs in molecules.
  • Electronegativity quantifies an atom's attraction for bonding electrons, impacting bond polarity.

Intermolecular Forces

  • Hydrogen bonds are strong dipole-dipole interactions in molecules with H bonded to highly electronegative atoms (O, N, F).
  • Dipole-dipole attractions occur between polar molecules with partial positive and negative charges.
  • Dispersion forces are weak intermolecular forces due to temporary dipoles in molecules.

Polyatomic Ions and Prefixes

  • Hydroxide: OH⁻
  • Sulfate: SO₄²⁻
  • Nitrate: NO₃⁻
  • Ammonium: NH₄⁺
  • Carbonate: CO₃²⁻
  • Electronegativity differences: 0-0.3 (nonpolar), 0.4-2 (polar), >2 (ionic).
  • Covalent compound naming prefixes: mono(1), di(2), tri(3), tetra(4), penta(5), hexa(6), hepta(7), octa(8), nona(9), deca(10).

Organic Compounds (Chapter 12)

  • Organic compounds primarily contain carbon and hydrogen, sometimes other nonmetals.
  • Found in various products: oil, gasoline, medicines, plastics, etc.
  • Every carbon atom forms four bonds.

IUPAC Naming Conventions (Chapter 12)

  • IUPAC system for naming organic compounds.
  • Carbon Chain Base Names: meth-(1), eth-(2), prop-(3), but-(4), pent-(5), hex-(6), hept-(7), oct-(8), non-(9), dec-(10).
  • Suffixes: alkane(-ane), alkene(-ene), alkyne(-yne).

Types of Hydrocarbons (Chapter 12)

  • Alkanes: Saturated hydrocarbons with single bonds.
  • Alkenes: Unsaturated hydrocarbons with double bonds.
  • Alkynes: Unsaturated hydrocarbons with triple bonds.
  • Cycloalkanes: Hydrocarbons arranged in ring structures.

Isomerism (Chapter 12)

  • Cis-trans isomers: Alkenes with restricted rotation due to double bonds.
  • Structural isomers: Same molecular formula, different bonding arrangements.

Identifying Alkenes and Alkynes (Chapter 12)

  • Look at the molecular formula (C and H count).
  • Double bond (C=C) indicates an alkene.
  • Triple bond (C≡C) indicates an alkyne.
  • Alkenes and alkynes are unsaturated (fewer hydrogens than alkanes).

Chemical Reactions (Chapter 7)

  • Combustion: Example: CH₃CH(OH)C(O)OH + O₂ → CO₂ + H₂O.
  • Synthesis: A + B → AB (reactants combine).
  • Decomposition: AB → A + B (compound breaks down).
  • Exchange: AB + CD → AC + BD (components swap).

Balancing Chemical Equations (Chapter 7)

  • Balance atoms for each element on both sides.
  • Start balancing atoms within compounds.
  • Adjust coefficients to balance individual elements.

Limiting Reagents and Percent Yield (Chapter 7)

  • Limiting reagent is completely consumed, limiting product.
  • Percent yield = (actual yield / theoretical yield) × 100%.

Mole Calculations (Chapter 7)

  • Moles are 6.022 × 10²³ particles (Avogadro's number).
  • Converting between mass and moles.

Common Oxidation States (Chapter 7)

  • Oxygen (O) = -2
  • Hydrogen (H) = +1
  • Alkali metals (+1)
  • Alkaline earth metals (+2)

Types of Chemical Reactions (Chapter 7)

  • Synthesis, Decomposition, Exchange reactions.

Gases (Chapter 8)

  • Temperature (T): Average kinetic energy of gas particles.
  • Volume (V): Space occupied by the gas.
  • Amount (n): Number of moles of gas.
  • Pressure (P): Gas particle collisions with container walls.

Gas Laws (Chapter 8)

  • Boyle's Law: P₁V₁ = P₂V₂ (Pressure and volume, constant temperature).
  • Gay-Lussac's Law: P₁/T₁ = P₂/T₂ (Pressure and temperature, constant volume).
  • Charles's Law: V₁/T₁ = V₂/T₂ (Volume and temperature, constant pressure).

Breathing and Gas Exchange (Chapter 8)

  • Inhalation: Lung volume increase, pressure decrease.
  • Exhalation: Lung volume decrease, pressure increase.

Ideal Gas Law (Chapter 8)

  • PV = nRT

Standard Temperature and Pressure (STP) (Chapter 8)

  • 0°C (273 K) and 1 atm (760 mmHg)

Solubility and Solutions (Chapter 9)

  • Solubility of most solids increases with temperature, gases decrease.
  • Osmotic pressure is crucial for red blood cells.

Solutions (Chapter 9)

  • Preparing Solutions: Calculate solute mass using molarity (M) = moles of solute / liters of solution.
  • Dilution: M₁V₁ = M₂V₂ for concentration changes.

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