Classification of Hydroxyl and Carbonyl Compounds

<p>Secondary alcohols can be oxidized using mild oxidizing agents. (B)</p> Signup and view all the answers

<p>Increase in the number of C-H bonds. (D)</p> Signup and view all the answers

<p>Small molecule, usually water. (B)</p> Signup and view all the answers

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

<p>A halogen atom (D)</p> Signup and view all the answers

<p>Store it in a cool dry place. (A)</p> Signup and view all the answers

<p>It can cause skin irritation. (A)</p> Signup and view all the answers

<p>60 degrees Celsius (D)</p> Signup and view all the answers

<p>It loses effectiveness over time. (A)</p> Signup and view all the answers

<p>Formation of a yellow precipitate. (C)</p> Signup and view all the answers

<p>Wait for at least 15 minutes. (B)</p> Signup and view all the answers

<p>Heat the solution to boiling. (B)</p> Signup and view all the answers

<p>To form a cloudy suspension or two layers. (C)</p> Signup and view all the answers

<p>Decreases solubility significantly after three carbons (A)</p> Signup and view all the answers

<p>Number of sulfur groups (A)</p> Signup and view all the answers

<p>Alcohols engage in hydrogen bonding (C)</p> Signup and view all the answers

<p>Tollens’ Silver Mirror Test (C)</p> Signup and view all the answers

<p>Alcohols can undergo ester formation (D)</p> Signup and view all the answers

<p>All alcohols can be oxidized using acidic potassium dichromate. (C)</p> Signup and view all the answers

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

<p>It increases with the number of hydroxyl groups (B)</p> Signup and view all the answers

<p>To facilitate the miscibility of alcohol with water. (B)</p> Signup and view all the answers

<p>It is miscible with water. (D)</p> Signup and view all the answers

<p>Carboxylic acid, alcohol, and concentrated sulfuric acid. (D)</p> Signup and view all the answers

<p>60 degrees Celsius. (A)</p> Signup and view all the answers

<p>It acts as a catalyst for the reaction. (C)</p> Signup and view all the answers

<p>Formic acid and ethyl alcohol - Rum. (B)</p> Signup and view all the answers

<p>Cool the test tube in cold water. (B)</p> Signup and view all the answers

<p>Waft gently without inhaling deeply. (A)</p> Signup and view all the answers

<p>C12 aldehyde (A)</p> Signup and view all the answers

<p>Presence of alkyl groups (C)</p> Signup and view all the answers

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

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

<p>Condensation reaction with a secondary alcohol (C)</p> Signup and view all the answers

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

<p>Aldehydes and ketones with fewer than six carbon atoms are soluble in water. (C)</p> Signup and view all the answers

<p>Tollens' test (B)</p> Signup and view all the answers

<p>To create a reagent suitable for testing (A)</p> Signup and view all the answers

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

<p>Aldehydes and ketones have higher boiling points. (A)</p> Signup and view all the answers

<p>Formation of a yellow precipitate (D)</p> Signup and view all the answers

<p>Straight-chain saturated aldehyde (A)</p> Signup and view all the answers

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

<p>35-50 degrees Celsius (A)</p> Signup and view all the answers

<p>To oxidize the sample (B)</p> Signup and view all the answers

<p>Prepare it fresh before each use (C)</p> Signup and view all the answers

A functional group containing an oxygen atom bonded to a hydrogen atom.

A functional group containing a carbon atom doubly bonded to an oxygen atom.

An organic compound containing a hydroxyl (-OH) group.

The ability of alcohols to dissolve in water. Shorter alcohol chains dissolve more readily.

Alcohols have higher boiling points than alkanes with similar sizes, due to hydrogen bonding.

Organic compound containing a carbonyl group at the end of the carbon chain.

Organic compound containing a carbonyl group in the middle of the carbon chain.

Laboratory procedures to distinguish between hydroxyl- and carbonyl-containing compounds.

The reaction of an alcohol with oxygen, producing carbon dioxide and water.

A chemical reaction where water is removed from the same alcohol molecule, forming an alkene.

A reaction where water is removed between two alcohol molecules, creating an ether.

A reaction where atoms or groups are removed from a molecule, creating a double or triple bond.

A reaction that increases the number of C-O bonds and/or decreases the number of C-H bonds in alcohols, using oxidizing agents like potassium permanganate or dichromate.

Substituting a halogen atom for the hydroxyl group in an alcohol, resulting in an alkyl halide.

Two molecules combining to form a larger molecule and releasing a small molecule, often water.

A temperature of 180 degrees Celsius and presence of Sulfuric Acid (catalyst) are ideal to perform intramolecular dehydration.

A reaction between a carboxylic acid and an alcohol in the presence of a strong acid catalyst (like sulfuric acid) to produce an ester and water.

Heating the reaction mixture accelerates the rate of ester formation, allowing the reaction to reach completion more quickly.

The odor of an ester can provide information about its structure and can be used to identify different esters based on their unique smells.

A chemical test that differentiates between primary, secondary, and tertiary alcohols based on their reactivity with a mixture of concentrated hydrochloric acid and zinc chloride (Lucas reagent).

The Lucas reagent generates a carbocation intermediate, which reacts with chloride ions to form a chloroalkane. The rate of reaction depends on the stability of the carbocation.

The rate of the Lucas test is influenced by the stability of the carbocation. Tertiary alcohols react fastest, followed by secondary alcohols, and lastly primary alcohols.

The Lucas test can be used to distinguish between primary, secondary, and tertiary alcohols because they react with the Lucas reagent at different rates, which can be observed visually.

Aldehydes and ketones have intermediate boiling points compared to similar-sized alkanes and alcohols. They boil higher than alkanes due to dipole-dipole interactions, but lower than alcohols due to weaker hydrogen bonding.

Smaller aldehydes and ketones (less than 6 carbons) are soluble in water due to their ability to form hydrogen bonds. Larger aldehydes and ketones are primarily soluble in organic solvents.

Lower molecular mass aldehydes have a pungent, penetrating, and unpleasant odor. This is often described as a sharp, irritating smell.

Higher molecular mass aldehydes (above C8) have a fragrant odor. These often have pleasant, floral, or fruity scents.

Ketones typically have pleasant odors. They are often described as sweet, fruity, or minty.

Oxidation is a chemical process where a substance loses electrons. In organic chemistry, it often involves gaining oxygen atoms or losing hydrogen atoms.

Tollens' Test is a chemical test that distinguishes aldehydes from ketones. It uses a silver mirror reagent to oxidize aldehydes, forming a silver mirror on the inside of the reaction vessel.

Benedict's Test is another method used to distinguish aldehydes from ketones. It uses a copper(II) reagent that is reduced in the presence of an aldehyde, changing the solution from blue to brick red.

Reduction is a chemical process where a substance gains electrons. In organic chemistry, it often involves gaining hydrogen atoms or losing oxygen atoms.

Hemiacetal formation is an addition reaction between an aldehyde or ketone and an alcohol. The result is a hemiacetal, containing a carbon atom bonded to both a hydroxyl and an alkoxy group.

A mixture of anhydrous zinc chloride (ZnCl2) in concentrated hydrochloric acid (HCl) used in the Lucas test to differentiate between primary, secondary and tertiary alcohols.

A chemical reaction that increases the number of C-O bonds and/or decreases the number of C-H bonds in an alcohol molecule. Oxidizing agents like potassium dichromate are often used.

A powerful oxidizing agent used in the oxidation of alcohols. It is prepared by dissolving potassium dichromate (K2Cr2O7) in water and adding concentrated sulfuric acid (H2SO4).

A chemical test used to detect the presence of carbonyl groups (aldehydes and ketones) in a compound. It forms a yellow or orange precipitate upon reaction with compounds that have carbonyl groups.

A solution of 2,4-dinitrophenylhydrazine in a mixture of concentrated sulfuric acid, water, and ethanol. It is used in the 2,4-Dinitrophenylhydrazine test to detect carbonyl groups.

A yellow, orange, or orange-red precipitate forms if carbonyl groups (aldehydes or ketones) are present in the sample. If no precipitate forms, it indicates the absence of carbonyl groups.

Many chemical reagents used in organic chemistry experiments are corrosive, toxic, or hazardous. Proper handling techniques and safety precautions are essential to prevent injuries or accidents.

A chemical test used to differentiate between aldehydes and ketones, based on their reaction with a copper(II) complex. Aldehydes (reducing sugars) react with Fehling’s reagent to form a red precipitate of copper(I) oxide, while ketones do not.

Fehling's reagent is a mixture of two solutions: Fehling's A (copper sulfate) and Fehling's B (potassium sodium tartrate and sodium hydroxide). Equal volumes of both solutions are mixed before use.

A chemical test used to differentiate between aldehydes and ketones based on their reaction with silver ions. Aldehydes reduce silver ions to metallic silver, forming a silver mirror on the inner surface of the reaction vessel. Ketones do not react.

Tollens' reagent is prepared by mixing a solution of silver nitrate with sodium hydroxide, followed by the addition of ammonia solution until the precipitate dissolves. Excess ammonia should be avoided.

A chemical test used to detect the presence of methyl ketones (ketones with a CH3 group attached to the carbonyl group). The test involves reacting the sample with iodine and a base, forming a yellow precipitate of iodoform.

The silver ions in Tollen's reagent react with aldehydes to form a silver mirror on the surface of the test tube. This reaction is due to the aldehyde's ability to reduce silver ions.

Excess ammonia in Tollens' reagent can form an explosive silver compound. It is important to add just enough ammonia to dissolve the initial precipitate.

Fehling's Test uses copper(II). Tollen's Test uses soluble silver ions. Iodoform Test uses iodine and a base.