Bioorganic Chemistry 2nd Assessment
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Questions and Answers

What is the functional group characteristic of thiols?

  • −OH
  • −SH (correct)
  • −S−
  • −COOH

Which prefix is used for compounds with halogen functional groups?

  • oxy-
  • halo- (correct)
  • hydro-
  • alkoxy-

Which example illustrates a compound containing a sulfone functional group?

  • Toluene
  • Bromoethane
  • Dimethyl sulfide (correct)
  • Ethanethiol

What suffix is used in the nomenclature for alcohols?

<p>-ol (C)</p> Signup and view all the answers

Which statement is true about ketones?

<p>They can undergo keto-enol tautomerism. (C)</p> Signup and view all the answers

Which functional group in organophosphates is represented by −PO4?

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

What reaction occurs when alcohols react with carboxylic acids?

<p>Formation of esters (D)</p> Signup and view all the answers

Which compound is an example of an aldehyde?

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

What is the pH when the concentration of H+ ions is $1.8 * 10^{-5}$?

<p>4.744 (C)</p> Signup and view all the answers

Which pH indicates that the concentrations of the acid and its conjugate base are equal in a buffer?

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

In the buffer calculation example with HAc and NaAc, what is the final concentration of HAc after dilution?

<p>0.0400 M (A)</p> Signup and view all the answers

What does the Law of Bouguer – Lambert – Beer describe?

<p>The relationship between absorbance and concentration (D)</p> Signup and view all the answers

What classification of hydrocarbons contains only single bonds?

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

What is the general formula for alkenes?

<p>CnH2n (B)</p> Signup and view all the answers

In which functional group is the hydroxyl group (−OH) present?

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

What parameter is measured in potentiometry?

<p>Potential difference (C)</p> Signup and view all the answers

What is the effect of increasing the concentrations of buffer components on its buffer capacity?

<p>Buffer capacity increases (D)</p> Signup and view all the answers

What functional group is characteristic of carboxylic acids?

<p>−COOH (C)</p> Signup and view all the answers

How do alkenes differ from alkanes?

<p>Alkenes contain one or more double bonds (A)</p> Signup and view all the answers

Which of the following examples represents an alkyne?

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

What is the IUPAC nomenclature change for a ketone?

<p>Replace -e with -one (B)</p> Signup and view all the answers

Which compound contains a carbonyl group at the end of the chain?

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

In the context of amines, which of the following compounds is an example?

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

What type of compounds do lipids primarily consist of?

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

What is a distinguishing feature of fatty acids?

<p>They have both a methyl and a carboxyl group. (A)</p> Signup and view all the answers

What type of reaction produces triacylglycerols?

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

Which of the following best describes amines?

<p>They are classified by the number of alkyl groups attached to nitrogen. (A)</p> Signup and view all the answers

What occurs when amino acids undergo a condensation reaction?

<p>Formation of a peptide bond (C)</p> Signup and view all the answers

How do amides differ from amines structurally?

<p>Amides contain a carbonyl group bonded to nitrogen. (B)</p> Signup and view all the answers

What characterizes essential amino acids?

<p>They must be obtained from the diet. (C)</p> Signup and view all the answers

What specific characteristic do amino acids exhibit at neutral pH?

<p>They exist as zwitterions. (A)</p> Signup and view all the answers

What is keto-enol tautomerism?

<p>A chemical equilibrium between a ketone (or aldehyde) and its enol form. (D)</p> Signup and view all the answers

How are carboxylic acids typically prepared?

<p>By oxidation of primary alcohols and aldehydes. (C)</p> Signup and view all the answers

Which of the following is a characteristic of polyfunctional carboxylic acids?

<p>They have additional functional groups like hydroxy or keto. (A)</p> Signup and view all the answers

Which of the following compounds is an example of a saturated dicarboxylic acid?

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

What type of reaction occurs during decarboxylation of malonic acid?

<p>Formation of acetic acid and CO2. (B)</p> Signup and view all the answers

Which of the following descriptions best defines chirality in molecules?

<p>A molecule that exists as non-superimposable mirror images. (B)</p> Signup and view all the answers

What type of acids are classified as oxo acids?

<p>Acids that contain hydrogen atoms capable of dissociating to form H+ ions. (B)</p> Signup and view all the answers

Which statement is true about mono- and polyfunctional compounds?

<p>Polyfunctional compounds contain several identical functional groups. (C)</p> Signup and view all the answers

What defines an Arrhenius acid?

<p>Dissociates to produce hydrogen ions (H+) in water (C)</p> Signup and view all the answers

Which of the following compounds is an example of a non-electrolyte?

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

If a solution has a pH of 12, what is the relationship between H3O+ and OH- concentrations?

<p>OH- concentration is higher than H3O+ (B)</p> Signup and view all the answers

What is the formula to calculate pOH?

<p>pOH = -log[OH-] (D)</p> Signup and view all the answers

What characterizes a buffer solution?

<p>Contains a weak acid and its salt or a weak base and its salt (C)</p> Signup and view all the answers

How do you calculate the hydronium ion concentration from pH?

<p>[H3O+] = 10^-pH (B)</p> Signup and view all the answers

In a pH calculation, if the concentration of H3O+ is 0.01 M, what is the pH?

<p>2 (C)</p> Signup and view all the answers

What is the pH of a solution with a hydroxide ion concentration of 0.01 M?

<p>12 (D)</p> Signup and view all the answers

Flashcards

Arrhenius Acid

A substance that produces hydrogen ions (H+) when dissolved in water.

Brønsted-Lowry Acid

A substance that donates a proton (H+).

pH

A measure of the hydrogen ion concentration in a solution, expressed as the negative logarithm (base 10) of the hydrogen ion concentration.

pH of 7

Neutral solution, the concentration of H3O+ ions is equal to the concentration of OH– ions.

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Electrolyte

A substance that dissolves in water and conducts electricity due to the presence of ions.

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Buffer Solution

A solution that resists changes in pH when small amounts of acid or base are added.

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Dissociation Constant (Ka)

Numerical value showing how much a weak acid dissociates into ions in solution.

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pH Calculation

Calculating pH from concentration of hydrogen ions (-log[H+])

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Buffer Capacity

The amount of acid or base a buffer can absorb without significantly changing its pH.

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Halogen Functional Group

A functional group containing a halogen atom (F, Cl, Br, or I) bonded to a carbon atom.

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Thiol Functional Group

A functional group containing a sulfur atom bonded to a hydrogen atom (-SH).

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Buffer Range

The pH range over which a buffer effectively maintains a relatively constant pH.

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Sulfide Functional Group

A functional group containing a sulfur atom bonded to two carbon atoms (-S-).

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Henderson-Hasselbalch Equation

An equation used to calculate the pH of a buffer solution.

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Primary Alcohol

Alcohol with the -OH group attached to a primary carbon atom (bonded to only one other carbon atom).

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Secondary Alcohol

Alcohol with the -OH group attached to a secondary carbon atom (bonded to two other carbon atoms).

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Spectroscopy

A technique that uses electromagnetic radiation to analyze materials and chemicals.

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Tertiary Alcohol

Alcohol with the -OH group attached to a tertiary carbon atom (bonded to three other carbon atoms).

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Law of Bouguer-Lambert-Beer

The absorbance of light is directly proportional to the concentration and path length of the absorbing substance.

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Oxidation of Alcohol

The process of converting a primary or secondary alcohol to an aldehyde, ketone, or carboxylic acid.

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Potentiometry

A method of measuring the potential difference between two electrodes for analyte concentration determination.

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Chromatography

A technique used to separate components of a mixture based on their different interactions with a stationary and mobile phase.

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Ester Formation

Reaction between an alcohol and a carboxylic acid to form an ester, releasing water as a byproduct.

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Alkane General Formula

The general formula for alkanes is CnH2n+2, where 'n' is the number of carbon atoms.

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Alkene General Formula

The general formula for alkenes is CnH2n, where 'n' is the number of carbon atoms. Alkenes contain one or more carbon-carbon double bonds.

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Alkyne General Formula

The general formula for alkynes is CnH2n−2, where 'n' is the number of carbon atoms. Alkynes contain one or more carbon-carbon triple bonds.

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Alcohol Functional Group

The functional group for alcohols is -OH (hydroxyl group).

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Example of Alcohol

Ethanol is an example of an alcohol.

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Ether Functional Group

The functional group for ethers is -O- (oxygen bridge).

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Aldehyde Functional Group

The functional group for aldehydes is -CHO (carbon bonded to an oxygen and hydrogen; located at the end of the molecule).

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Amine Functional Group

The functional group for amines is -NH2, -NHR, or -NR2, where R represents a hydrocarbon group.

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Keto-enol Tautomerism

A reversible interconversion between a ketone and an enol form, driven by the migration of a proton from the α-carbon to the carbonyl oxygen.

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What are lipids?

Organic compounds containing hydrocarbons, essential for cell structure and function. They are nonpolar, making them soluble in nonpolar environments like fats and oils.

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Fatty Acids: Saturated

Fatty acids with only single bonds between carbon atoms, making them solid at room temperature.

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Fatty Acids: Unsaturated

Fatty acids with at least one double bond between carbon atoms, making them liquid at room temperature.

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Triacylglycerols (TAGs)

Esters formed by the reaction of glycerol and three fatty acid molecules, commonly known as fats and oils.

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Amides

Organic compounds with a carbonyl group directly bonded to a nitrogen atom (C=O-N).

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Amines: Basic Properties

Amines are organic compounds that contain a nitrogen atom. Their nitrogen atom is basic and can accept a proton (H+) to form ammonium salts.

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Amino Acids: Essential

Amino acids that cannot be synthesized by the body and must be obtained from the diet.

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Carboxylic Acids: Properties

Carboxylic acids are weakly acidic, forming carboxylate salts when reacting with bases. For example, CH3COOH + NaOH → CH3COONa + H2O.

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Carboxylic Acids: Preparation

Carboxylic acids can be prepared by oxidizing primary alcohols and aldehydes.

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Polyfunctional Carboxylic Acids

Carboxylic acids with additional functional groups like hydroxy (-OH) or keto (=O). Examples include lactic acid and citric acid.

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Heterofunctional Carboxylic Acids

Carboxylic acids with different functional groups, like carboxyl and amino groups, including oxo acids (like pyruvic acid) and amino acids.

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Dicarboxylic Acids: Saturated

Dicarboxylic acids with single bonds between carbons. Examples include oxalic acid (HOOC-COOH) and succinic acid (HOOC-CH2)2-COOH.

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Dicarboxylic Acids: Unsaturated

Dicarboxylic acids with double or triple bonds between carbons. Examples include maleic acid and fumaric acid (cis-trans isomers of butenedioic acid).

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Dicarboxylic Acids: Reactions

Dicarboxylic acids undergo reactions such as decarboxylation (losing CO2), salt formation (with bases), and esterification (with alcohols).

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Study Notes

Bioorganic Chemistry 2nd Assessment

  • Acids and Bases:
    • Arrhenius: Acids donate H+ ions in water, bases donate OH⁻ ions in water.
    • Brønsted-Lowry: Acids donate protons (H+), bases accept protons.
    • Lewis: Acids accept electron pairs, bases donate electron pairs.
  • Electrolytes and Non-Electrolytes:
    • Electrolytes: Compounds that dissolve into ions and conduct electricity in solutions. Examples include HCl, NaCl, H₂SO₄, KOH, etc.
    • Non-Electrolytes: Compounds that dissolve in water but do not conduct electricity. Examples include CO₂, alcohols, sugars, organic solvents.
  • Dissociation constant, Hydrogen ions and pH:
    • pH 7: Concentration of H₃O⁺ = OH⁻
    • pH below 7: Concentration of H₃O⁺ is greater than OH⁻
    • pH above 7: Concentration of OH⁻ is greater than H₃O⁺
    • Calculation of pH: -log[H₃O⁺]
    • Calculation of pOH: -log[OH⁻]
    • pH + pOH = 14.00
    • Calculate [H₃O⁺] from pH: [H₃O⁺] = 10⁻pH
    • Calculate [OH⁻] from pOH: [OH⁻] = 10⁻pOH
  • Buffer solutions:
    • Solutions that resist changes in pH when small amounts of strong acid or base are added.
    • Composed of a weak acid and its conjugate base (or a weak base and its conjugate acid).
    • Buffer capacity: Amount of acid or base that can be added before significantly changing pH.
  • Spectroscopy:
    • Spectroscopy is used to study the structure of materials by analyzing their interaction with electromagnetic radiation.
    • Law of Bouguer-Lambert-Beer: The absorbance of light by a sample is proportional to the concentration of the sample and the path length of the light through it.
  • Functional Groups in Organic Compounds:
    • Hydrocarbons: Contain only carbon and hydrogen.
    • Alcohols: Contain a hydroxyl group (-OH).
    • Phenols: Contain a hydroxyl group (-OH) attached to an aromatic ring.
    • Ethers: Contain an oxygen atom (-O-) bonded to two hydrocarbon groups.
    • Aldehydes: Contain a carbonyl group (-CHO) at the end of the carbon chain.
    • Ketones: Contain a carbonyl group (-CO-) within the carbon chain.
    • Carboxylic acids: Contain a carboxyl group (-COOH).
    • Esters: Contain a carbonyl (-CO-) group between a carbon and an oxygen from an alcohol group.
    • Amines: Contain a nitrogen atom bonded to one or more alkyl groups.
    • Amides: Contain a carbonyl (-CO) group bonded to a nitrogen atom.
    • Nitro compounds: Contain a nitro group (-NO₂).
    • Halogen compounds: Contain a halogen atom (F, Cl, Br, or I).
    • Thiols: Contain a sulfhydryl group (-SH).
    • Sulfides: Contain a sulfur atom (-S-) bonded to two hydrocarbon groups.
    • Phosphorus compounds: Contain phosphorus and oxygen.
  • Lipids:
    • Organic compounds containing primarily hydrocarbons.
    • Nonpolar, therefore not soluble in water.
    • Includes saturated and unsaturated fatty acids.
    • Triacylglycerols are a type of lipid.
  • Fatty Acids:
    • Carbon chains with a carboxyl group at one end.
  • Triacylglycerols:
    • Formed by the esterification of glycerol with three fatty acids.
  • Oxidation: Chemicals can be turned into other chemicals through reaction with oxidizing agents.
  • Keto-enol tautomerisation: A chemical equilibrium between two isomers that differ in the position of a double bond and a hydroxyl group.

Additional Topics

  • Amino Acids:
    • Contain an amino group (-NH₂) and a carboxyl group (-COOH).
    • Form peptides and proteins via peptide bonds.
    • Some are essential, meaning they must be obtained from the diet.
  • Chirality (Optical Isomerism):
    • Molecules that are not superimposable on their mirror images (enantiomers)
  • Polyols: Contain multiple hydroxyl groups (-OH)
  • Buffer Capacity: Affects how much acid or base a solution can neutralize.

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Bioorganic Chemistry 2nd Assessment PDF

Description

Test your knowledge on acids, bases, and their properties in the context of bioorganic chemistry. This assessment covers key concepts like Arrhenius, Brønsted-Lowry, and Lewis definitions, as well as electrolytes and the calculation of pH and pOH. Prepare to apply your understanding of ionic dissociation and the behavior of different compounds in solutions.

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