topic 10/20 Flashcards by Lavi R

define a homologous series

a series of compounds of the same family, with the same general formula, which differ from each other by a common structural unit (CH2, methylene group)

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explain the trend in boiling points and density of members of homologous series

boiling point/density increases as length of carbon chain increases:
- molecular mass increases/no of C atoms increases
- London forces increase as the molecules get bigger

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describe and explain the trend in solubility of members of a homologous series

less soluble as homologous series is ascended:
hydrocarbon chain is non-polar (hydrophobic) and as no of carbons increase, this increases the percentage of the molecule that is unattractive to water.

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what does the solubility of a compound in water depend on?

solubility in water depends on the ability of the water molecules to attract dipoles in the organic compound.

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describe physical and chemical properties of homologous series

physical properties change gradually as the length of the carbon chain increases
similar chemical properties

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general formula of alkanes

CnH2n+2

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general formula for alkenes

CnH2n

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general formula for alkynes

CnH2n-2

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general formula for ketones

CnH2nO

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general formula for alcohols

CnH2n+1OH

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general formula for aldehydes

CnH2n+2

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general formula for carboxylic acids

CnH2n+1COOH

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define an empirical formula

the simplest ratio of the atoms within a molecule of the compound

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define the molecular formula

shows the actual number of atoms of each type in the molecule

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define the structural formula

shows the actual arrangement of the atoms in a molecule by drawing the bonds as lines between letters representing the atoms

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define a skeletal formula

each carbon is represented by an angle, or termination in a line and the hydrogen atoms are just assumed

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state the two ways that structural formulae can be represented.

full format
condensed format

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describe alkanes as a class of organic compounds

saturated hydrocarbons

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describe alkenes as a class of organic compounds

unsaturated hydrocarbons- carbon and hydrogen atoms with one or more carbon-carbon double bond in their chemical structure

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describe alkynes as a class of organic compounds

organic molecules made of the functional group carbon-carbon triple bonds

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describe halogenoalkanes as a class of organic compounds

organic compounds that contain one or more halogen atom (chlorine, bromine, fluorine, or iodine) attached to a carbon atom in an alkane molecule
- RX, where R=alkyl group, H= halogen

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describe alcohols as a class of organic compounds

one or more hydroxyl (―OH) groups attached to a carbon atom of an alkyl group (hydrocarbon chain).

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describe ethers as a class of organic compounds

characterized by an oxygen atom bonded to two alkyl or aryl groups
R−O−R′

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describe aldehydes as a class of organic compounds

a carbon atom shares a double bond with an oxygen atom, a single bond with a hydrogen atom, and a single bond with another atom or group of atoms
R−CH=O

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describe ketones as a class of organic compounds

R−C(=O)−R'

describe esters as a class of organic compounds

any of a class of organic compounds that react with water to produce alcohols and organic or inorganic acids R-C(=O)-O

describe carboxylic acids as a class of organic compounds

any of a class of organic compounds in which a carbon atom is double bonded to an oxygen atom and to a hydroxyl group (―OH) by a single bond R−COOH

describe amines as a class of organic compounds

organic compounds that contain nitrogen atoms with a lone pair R-CO- NH2

describe amides as a class of organic compounds

R(CO)NR2

describe nitriles as a class of organic compounds

any of a class of organic compounds having molecular structures in which a cyano group (―C ≡ N) is attached to a carbon atom (C) R-C[triple]N

describe arenas as a class of organic compounds

aromatic hydrocarbons- implies a particular sort of delocalized bonding CnH2n−6

define functional groups

a group of atoms that determines a molecule's reactivity

describe phenyl as a functional group

a benzene ring, minus a hydrogen

describe hydroxyl as a functional group

- OH

describe carbonyl as a functional group

[C=O]

describe carboxyl as a functional group

−COOH

Describe a carboxamide as a functional group

-CO-NH2

Describe aldehydes as a functional group

−CH=O

Esters as a functional group

-COO-

Ethers as a functional group

R−O−R

Amines as a functional group

-NH2

Nitrile as a functional group

−C≡N

Alkyl functional group

−C≡N

Alkyl as a functional group

formed by removing a hydrogen atom from the molecule of alkane.

Alkenyl group

Hydrocarbon group formed when a hydrogen atom is removed from an alkene group

Alkynyl group

Obtained by the removal of one hydrogen atom that is linked to a triply bonded carbon atom

Define structural isomers

Compounds with the same molecular formula but different arrangement of atoms

Define stereoisomers

Have the same structural formula but differ in their spatial arrangement

Describe the different types of stereoisomerism

- Stereoisomerism: Configurations isomerism (cis/trans E/Z, optical isomerism), conformational isomerism - Structural isomerism: Positional isomers, functional group isomers, chain isomerism

Describe the difference between conformational isomers and configurational isomers

Conformational: can interconvert by rotation about a sigma bond Configurational: can only interconvert by breaking and reforming a bond

why do alkanes only undergo free radical substitution?

they have a low reactivity due to the: - strength of the C-C and C-H bonds - lack of polarity

incomplete combustion of alkanes

C, CO, H2O

complete combustion of alkanes

CO2, H2O

combustion of alkanes is ...

highly exothermic

describe heterolytic fission

results in the formation of a positive and negative ion

describe homolytic fission

results in the formation of two radicals

what condition is necessary for free radical substitution?

UV light

define free radical substitution

a type of substitution reaction where a radical replaces a different atom or group of atoms

what bonds can UV light break/not break?

it can break bonds between halogens but not between C-H bonds (too strong)

why would excess methane be needed in free radical substitution?

to reduce further substitution

describe the free radical substitution mechanism

check notes

give 3 limitations of free radical substitutions

- any of the hydrogens can be substituted so a number of products can be formed - multi-substitutions may occur - it is not effective to create a specific halogenoalkane

topic 10/20 Flashcards

(62 cards)