MOD 4 Flashcards by Clary Dricu

alkenes are _________ hydrocarbons and their general formula is __________

Alkenes are unsaturated hydrocarbons which the formula CnH2n

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Alkanes are _______ hydrocarbons meaning they have _______ CC bonds with the general formula _________

Alkanes are saturated hydrocarbons meaning they have single CC bonds, with the general formula CnH2n+2

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Define homologous series

Families of organic compounds with the same functional group which differs by a -CH2

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Define functional group

Part of organic molecules that is largely responsible for the molecules chemical properties.

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Functional groups to remember

Alcohol
Carboxylic acid
Ester
Alky group
Amine
Amide
Aldehyde
Ketone
Haloalkane

Functional groups to remember

Alcohol> C-OH
Carboxylic acid> C-COOH
Ester> COOR
Alky group> R=
Amine> C-NH2
Amide>O=C-NH2
Aldehyde> -CHO
Ketone> C-CO-C
Haloalkane> -halide

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Functional groups to remember

Alcohol
Carboxylic acid
Ester
Alky group
Amine
Amide
Aldehyde
Ketone
Haloalkane

Functional groups to remember

Alcohol> C-OH
Carboxylic acid> C-COOH
Ester> COOR
Alky group> R=
Amine> C-NH2
Amide>O=C-NH2
Aldehyde> -CHO
Ketone> C-CO-C
Haloalkane> -halide

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Define aliphatic hydrocarbons

Hydrocarbon with carbon atoms joined together in straight or branched chains

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Define alicyclic hydrocarbons

Hydrocarbons with carbon atoms joined together in a ring structure

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Define aromatic hydrocarbon

Hydrocarbon that contains at least one benzene ring in the structure

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Define empirical formula

Simplest whole number ratio of the element in a compound

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Define molecular formula

How many atoms of each element that makes up the compound

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Define general formula

The simplest algebraic formula for a homologous series

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Define structural formula

Shows the arrangement of atoms in a molecule. It is a short hand way of writing the displayed formula with no bonds between the atoms

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Define displayed formula

Shows the relative position of all the atoms in a molecule and all the bonds between them

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Define skeletal formula

Simplified organic formula with hydrogen atoms removed from the allkyl chains. This just leaves the carbon skeleton with associated functional groups

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What is meant by homolytic fission

When a covalent bond breaks and each of the bonded atoms take one of the shared electrons from the shared bonds.
Each atom now has a single unpaired electron—>This is called a radical

Describe heterolytic fission

A covalent bond is broken and one of the bonded atoms takes both the electrons from the bond
The atom taking both the electrons becomes negative while the atom that does not take electrons becomes positive

_______________ are electron pair acceptors (therefore something that is positively charged)

Electrophiles are electron pair acceptors (therefore something that is positive )

What is a neucleophile

Neucleophiles are electron pair donors (therefore something positively charged )

What does IUPAC stand for

The INTERNATIONAL UNION of PURE and APPLIED CHEMISTRY

Identify and describe 3 types of structural isomers

Alkyll groups in different places
Functional group bonded to a different part of the parent chain
Functional group can be different

Definition difference between structural isomers and stereoisomers

Structural isomers have the same molecular formula but different structural formulae

Stereoisomers- organic compound with the male molecular AND STRUCTURAL formula but different arrangements of atoms in space.

__________ are a homologous series of saturated hydrocarbons

Alkanes are a homologous series of saturated hydrocarbons

as an alkene chain gets __________ its relative molecular mass increases. Larger molecules have more _________ __________ __________ between adjacent molecules. this ______________ the number of induced dipole-dipole forces. so ___________ energy is needed to overcome the intermolecular attraction in order that the alkene can change state

as an alkene chain gets LONGER its relative molecular mass increases. Larger molecules have more SURFACE AREA CONTACTS between adjacent molecules. this INCREASES the number of induced dipole-dipole forces. so MORE energy is needed to overcome the intermolecular attraction in order that the alkene can change state

Branched hydrocarbons have ________ BP than straight chain isomer because there is _______ chain isomerism. _________ __________ _______________forces. Fewer ___________ ______________.Thus _______ energy needed to overcome these forces.

Branched hydrocarbons have LOWER BP than straight chain isomer because there is MORE chain isomerism. WEAK LONDON forces. Fewer induced dipole-dipole interactions. Thus LESS energy needed to overcome these forces.

Alkanes and rigidity

Alkanes are not rigid because each sigma bond acts as an axis around which the atom can rotate freely

why does methane have a tetrahedral shape with an angle of _____- ???

tetrahedral angle = 109.5 each sigma bond exerts an equal amount of repulsion on the other bonds causing a 3D tetrahedral structure as all electron pairs are at equal distances between eachother.

Cis vs Trans isomerism

Cis- same side groups placed on the same side of the double bond Trans-molecules with the same side groups placed on opposite sides of a double bond.

Define E\Z isomerism

Type of stereoisomerism caused by the restricted rotation around the double bond- 2 different groups are attached to both carbon atoms of the double CC bond

Comment on the reactivity of alkanes

Alkanes have LOW reactivity because all the covalent bonds in alkane molecules have high bond enthalpies which require a large amount of energy to break Carbon-hydrogen sigma bonds have low polarity because electronegativity of H and C are almost the same

General reactions of incomplete and complete combustion for alkanes

INCOMPLETE Alkane+Oxygen----> Carbon Monoxide+ Water Alkane+Oxygen----> Carbon + Water COMPLETE Alkane+Oxygen----> Carbon Dioxide+ Water

General reactions of incomplete and complete combustion for alkanes

INCOMPLETE Alkane+Oxygen----> Carbon Monoxide+ Water Alkane+Oxygen----> Carbon + Water COMPLETE Alkane+Oxygen----> Carbon Dioxide+ Water

Outline the process of Halogenation

STEP 1 INITIATION-UV light used to cause the covalent bond in bromine to break up via homolytic fission. Formation of radicals STEP 2 PROPAGATION- 2 repeated steps (a & b) that build up the desired product in a side-reaction a. Bromine radical reacts with C-H bond in methane. A methyl radical forms and a hydrogen bromide. b. Methyl radical reacts with the other bromine molecule forming the product of bromoethane and a bromine radical. STEP 3 TERMINATION- when 2 radicals collide, both radicals are removed from the reaction mixture stopping it . Mixture of products produced by random collisions between radicals. Only one product is desirable thus the reaction has low economy.

Define radical

Species with one or more unpaired electrons

Define reaction mechanism

Models that show the movement of electron pairs during a reaction