Organic Chemistry Flashcards

Vocabulary flashcards based on lecture notes for exam preparation.

Carbon, Hydrogen, Oxygen, Nitrogen, Sulfur, Phosphorous, Silicon, Fluorine, Chlorine, Bromine, Iodine

Elements commonly found in organic compounds

Systemic Approach

A method that gives satisfactory results in identifying elements in inorganic compounds using qualitative chemical changes

Organoleptic Approach

A method where qualitative chemical tests highly rely on for observation of test results

Cupric Oxide (CuO)

A compound used to detect carbon and hydrogen by strongly heating

Carbon Dioxide and Water

The products of oxidizing carbon and hydrogen when heated with cupric oxide

Lime Water

Used to detect carbon dioxide (CO₂)

Clear solution turns turbid

Positive result for carbon dioxide detection

Anhydrous CuSO₄

Used to detect water (H₂O)

White powder turns blue

Positive result for water detection

Fusing compounds with Sodium Metal

The process to convert elements into inorganic ions for qualitative analysis

Lassaigne’s Extract (Sodium Extract)

The alkaline solution obtained by extracting the fused mass in water

Soda Lime Test for Amide Nitrogen

A test limited for organic compounds with amino (NH₂) group only

Beilstein Test

A test used to detect halogens

Green Colored Flame

Positive result for Beilstein Test

Cupric Halide

The compound formed in the Beilstein test, responsible for the color of the flame

Silver Nitrate Test

A test used to detect halogens by reacting with silver nitrate

White to Light Yellow Precipitate

Positive result for Silver Nitrate Test

Lead Acetate Test

A test used to identify the presence of sulfur

Brownish-Black Acetate

Positive result for Lead Acetate Test

Lead Sulfide

The compound formed in Lead Acetate test when sulfur is present

Cysteine

An amino acid containing sulfhydryl group

Ferrox Test

A test used to detect oxygen

Red to Reddish Purple Color Solution

Indication for a positive result in the Ferrox Test

Iron (III) hexathiocyanatoferrate or Ferrox paper

Reagent used in the Ferrox Test

Ferrox Paper

A paper prepared by soaking filter paper in methanol for Oxygen detection.

Arrhenius Theory

A theory where acid is any species that can increase the concentrations of hydrogen ions in an aqueous solution and base increases the concentration of hydroxide ions

Bronsted-Lowry Theory

A theory where acid donates a proton and base accepts a proton

Conjugate Acid

Formed after base accepts a proton

Conjugate Base

Formed after an acid donates its proton

Stronger Acids

React almost completely with water

Weak Acids

Reacts only slightly with water

Lewis Electron Pair Theory

A theory where acid accepts a pair of non-bonding electrons, and base donates a pair of non-bonding electrons

Acid-Base Complex or Complex Ion

The product of reaction between a Lewis Acid and Lewis Base

pH

Negative logarithm of hydrogen ions

pOH

Negative logarithm of hydroxide ions

pH Paper

Measures pH of the solution by changing its color depending on the concentration of H⁺ and OH⁻

Flavin, an Anthocyanin

A plant pigment commonly found in red cabbages and used as an indicator on pH paper

pH Meter

An accurate method to measure pH using a probe that measures voltage

Sensor electrodes and Reference electrode

Parts of the glass pH probe

Boiling and Melting Points

Physical properties that can help identify and characterize unknown compounds and function as an index of purity of substances

Intermolecular Forces of Attraction

Force affecting boiling point that happens between one molecule and another, influencing directly the boiling point

Van Der Waals Dispersion Forces, Dipole-Dipole Interaction, Hydrogen Bonding, Ionic Bonding

Types of Intermolecular Forces of Attraction

Van der Waals Dispersion Forces

Weak intermolecular attraction formed by induced polarization of molecules

Van der Waals Dispersion Forces

Occurs only among hydrocarbon groups and within short distances in between molecules

Dipole-Dipole Interaction

Happens among partially ionic or polar molecules

Hydrogen Bonding

Formed between partially positive hydrogen (H⁺) and an adjacent electronegative atom that has the partial negative charge

Ionic Bonding

Happens between molecules having opposite charges

Amines and Carboxylic Acids

The functional groups that ionizes easily

Melting Point

A pure crystalline compound has a sharp melting point and completely melts within a narrow range temperature NMT 0.5 – 1° C

Solubility

A physicochemical property that refers to the ability of a given solute to be dissolved in a given amount of solvent

Solute

Dissolved to create a solution

Solvent

Dissolving medium

Solution

Liquid mixture of the solute with the dissolved solvent

Dissolution

Process of dissolving

Saturated Solution

Maximum amount of solute dissolved in the given solvent

Supersaturated Solution

More amount of solute than solvent

Unsaturated Solution

Less amount of solute than solvent

Miscibility

Wherein substances mix in all proportions Forming a HOMOGENEOUS MIXTURE

Rule of Solubility

Pertains to the polarity of compounds; "Like dissolves like"

Recrystallization

Fractional Crystallization

Selection of an Appropriate Solvent

Most critical step in Recrystallization

Decolorization with Activated Charcoal

Removes high molecular weight impurities, which are often colored and relatively less soluble

Activated charcoal

Universal antidote

Seeding

Crystal of the original solid is added to the solution to induce crystallization

Scratching

A glass rod is to rub the inside surface of the crystallization vessel at or just above the air/solution interface

Oiling Out

Solute separates as oil instead of a solid, an undesirable purification

Melting Point Determination

Purity of the crystals are usually assessed using melting point determination.

Silver Nitrate Test

Used to detect any sodium chloride impurity left on the purified crystals.

Sublimation

Direct conversion of solid to gas without passing through the liquid phase.

Sublimate

The crystals, deposit, or material obtained when a substance is heated during sublimation

Residue

The solid particle that remained on the dish during sublimation

Barium Chloride Test

Test employed to differentiate the organic substance from inorganic residue during sublimation

Simple Distillation

Involves the process of separating 2 or more liquids homogenously mixed but with different boiling points (at least 20° difference)

Fractional Distillation

Same technique as simple distillation, just repeated several times

Ignition Test

Separation of the liquid mixture can be detected through this test

Sodium Nitroprusside Test

Acetone (a ketone) will react with sodium nitroprusside and sodium hydroxide to form a wine red solution due to the formation of acetone-nitroprusside ion complex.

Chromatography

The process of separating the substances in a complex mixture by their different affinities to an adsorbent.

Stationery Phase

Liquid or solid that is fixed in a place during the chromatography process

Mobile Phase

Either liquid or gas which moves the samples through the stationary phase during the chromatography process.

Retention Factor (Rf Value)

The extent of separation in chromatography is measured by this value.

Thin Layer Chromatography

Stationary phase (adsorbent like silica gel on aluminum), coated over an inert solid plate and a mobile phase made up of a solvent system (solvent mixture) is involved

Paper Chromatography

Largely depends on adhesion and cohesion forces which allows the mobile phase to move along the stationary phase due to surface tension.

Ruhemann’s Purple

Ninhydrin solution reacts with amino acids giving colored compounds usually brown or purple

Saturated Hydrocarbon

Compound with carbon atoms bonded with a single bond

Unsaturated Hydrocarbon

Compound with carbon atoms are bonded with double or triple bonds

Open-Chain Hydrocarbon

Could be straight or branched chains (Acyclic or Linear structure)

Closed-Chain Hydrocarbon

Could be aliphatic or aromatic (Cyclic or Ring structure)

Aliphatic Hydrocarbons

Alkanes, Alkenes, and Alkynes

Aromatic Hydrocarbons

Cyclic hydrocarbons with delocalized pi electrons between carbon atoms of ring

Combustion Reaction

Hydrocarbon reacts with oxygen to produce carbon dioxide, water and heat.

Baeyer’s Test

Used as a qualitative test for unsaturation.

Baeyer’s Reagent

Alkaline solution of potassium permanganate.

Bromine Test for Unsaturation (Addition Reaction)

An alkene/alkyne reacts with Br₂ producing products of a dibromo for alkene and ultimately a tetrabromo for alkyne

Nitration Test

Used to produce Nitrobenzene.

Alcohols

Organic compounds composed of an aliphatic carbon atom with a hydroxyl (-OH) functional group

Boiling Point of Alcohols

Higher boiling points compared to hydrocarbons with the same molecular mass, due to intermolecular H-bonding

Acidity of Alcohols

Acidic in nature because of their ability to react with active metals (Sodium, Potassium) forming Alkoxide

Jones’ Test (Chromic Acid Test)

Used to distinguish primary and secondary alcohols from tertiary alcohols

Chromium oxide (CrO₃) in sulfuric acid (H₂SO₄)

Reagent used in Jones' Test

Blue-green solution

Positive result for Jones' Test