Core Organic Chemistry Flashcards by katie puzey

What does nomenclature mean

The system used for naming organic compounds

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What does the term molecular formula mean

The actual number of atoms of different elements in a molecule

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Displayed formula

Shows every atom and bond in a molecule

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Structural formula

Arrangement of atoms in a molecule without showing every bond

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Skeletal formula

Drawn as lines with each vertex being a carbon atom

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Homologous series

Organic compounds with the same functional group but each successive member differing by CH2

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Functional group

A group of atoms responsible for characteristic reactions of a compound

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Aliphatic hydrocarbon

Straight/ branched chained

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Alicyclic hydrocarbon

Arranged in noon aromatic rings with or without side chains

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Aromatic hydrocarbon

Contains at least one benzene ring

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General formula alkanes

CnH2n+2

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General formula alkenes

CnH2n

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General formula alcohols

CnH2n+1OH

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Structural isomers

Same molecular formula but different structural formula

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3 ways structural isomers are formed

Alkyl groups in different places
Functional groups bonded to different parts
Different functional groups

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Stereoisomers

Same molecular formula but different arrangement of atoms in space

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E-Z isomerism

Caused by limited rotation about c=c bonds
If 2 substituents with the highest molecular mass are on the same side of the double bond it’s Z if on different side its E

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Cis-trans isomerism

Type of E/Z isomerism where the 2 substituents on each carbon atom are the same

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Homolytic fission

Each bonding atom receives one electron from the bonded pair forming two radicals

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Heterolytic fission

One bonded atom receives both electrons

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Radicals

Highly reactive neutral species

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What is an alkane

Saturated hydrocarbon with only C-H bonds

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Shape and angle of an alkane

Tetrahedral 109.5°

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Describe the sigma bond in alkanes

Covalent bond with direct overlap of the electron clouds of the bonded atoms

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Intermolecular forces alkanes have

London forces- the bonds are non polar

Boiling point as alkane chain length increases

Increases as there is more surface area and so more London forces so more energy needed to overcome the attraction

Branched molecules boiling points

Lower boiling point than straight b as fewer surface area so less London forces

Are alkanes soluble in water

Insoluble

How reactive are alkanes

Very unreactive

Product of complete combustion of alkanes

CO2 +H2O

How are halogenoalkanes formed

Radical substitution

What is required for alkanes to ready with halogens

UV light

Three stages of radical substitution

Initiation- breaking halogen bond Propagation-products are formed but radicals remain Termination- free radicals removed, stable products formed

What are alkenes

Unsaturated hydrocarbons containing at least 1 c=c bond

How is a pi bond formed

Electrons in adjacent p orbitals overlap above and below carbon atoms

Angle and shape of a double bond

Trigonal planar 120°

Alkenes more or less reactive than alkanes

More due to high electron density of double bond and pi bond is slightly easier to break

What is an electrophile

Species that are electron pair acceptors

Major products will be formed from which kinds of carbocations

Tertiary(or most stable available)

Conditions for electrophilic addition of water to an alkene

Steam in presence of acid catalyst reaction is called hydration

Products of hydration reaction

An alcohol

Conditions for electrophilic addition of a hydrogenhalide to an alkene

Hydrogen halide gases must be at room temperature

Reaction name when a halogen is added to an alkene

Halogenation

How can an alkene be converted into an alkane

Alkene+hydrogen= alkane Hydrogenation 150°c nickel catalyst

What is an addition polymer

Many monomers bonded together via rearrangement of bonds without the loss of any atom or molecule

Ways plastics can be disposed

Landfill Combustion Electricity generation Reuse Recycle Organic feedstock

Functional group in an alcohol

Hydroxyl group OH

Intermolecular forces alcohols have

Hydrogen bonding because of the electronegativity difference in the OH bond

Alcohols boiling points

Higher than alkanes because of hydrogen bonding

Are alcohols soluble

Soluble when short chain but not in long chain

What makes an alcohol primary

The carbon the OH is bonded to is only bonded to one other carbon atom

What makes an alcohol primary

The carbon the OH is bonded to is only bonded to one other carbon atom

What forms if you partially oxidise a primary alcohol

An aldehyde

Conditions to make an aldehyde

Dilute sulphuric acid, potassium dichromate distill product gentle heating

Full oxidation of a primary alcohol

Carboxylic acid

Conditions to make a carboxylic acid

Concentrated sulphuric acid, potassium dichromate, reflux,strong heating

Oxidation of a secondary alcohol

Ketone

Conditions to make a ketone

Concentrated sulphuric acid, potassium dichromate, strong heating

What is a dehydration reation

A reaction where water is lost to form an organic compound

Products of a dehydration reaction (alcohol)

Alkene and water

Conditions dehydration reaction (alcohol)

Conc sulphuric acid/phosphoric and and 170°c

Products halide substitution reaction (alcohol)

Haloalkene and water

What are haloalkanes

Saturated organic compounds containing at least one halogen atom

Intermolecular forces (haloalkanes)

Permanent dipole-dipole and London forces

Most important factor in determining halogen reactivity

The strength of carbon halogen bond

Define nucleophile

Electrons pair donor

Nucleophillic substitution

Nucleophile donates a lone pair to a slightly positive carbon atom and the nucleophile replaces the slightly negative atom

What is hydrolysis

A reaction where water is a reactant

What are CFC's

Chlorine-flouro-carbons

Problem with CFC's

Catalyse the breakdown of ozone via free radical substitution

What happens when a molecule absorbs infrared radiation

Makes covalent bond vibrate/ Stretching or bending motion

Factors affecting amount of vibration of a bond

Bond strength Bind length Mass of each atom in the bond

How does infrared spectroscopy work

Every bond has a unique vibration frequency Bonds absorb radiation of the same frequency as them Infrared radiation emergency from a sample is missing the frequencies that have been absorbed

What do the peaks on an IR spectrum represent

Absorbance of energy from the infrared radiation

Symbol of molecular ion

M+

Is fragmentation predictable

No because it can happen anywhere

In mass spectrometry how is a molecular ion represented

The peak with the highest mass/charge ratio

The molecular mass of the molecular ion is equal to what

The relative molecular mass of the compound

M/Z value of CH3

M/Z value of OH

Advantages of using mass spectrometry

Cheap Small samples required

Disadvantage of mass spectrometry

Sample is completely destroyed