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chemistry > Module 4.1 Basic concepts and hydrocarbons > Flashcards

Module 4.1 Basic concepts and hydrocarbons Flashcards

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1
Q

Homologous series

A

A series of organic compounds having the same functional group but with each successive member differing by CH2

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2
Q

Functional group

A

Part of a molecule which determines how it reacts

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3
Q

How do we name a alkane?

A
  • add the prefix (first part of name) depending on how many carbon atoms
  • then add -‘ane’ to the end
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4
Q

How do we name a alkene ?

A
  • add the prefix determined my how many carbon atoms there are
  • number carbon atoms from the side where the double c=c bond will be the lowest
  • add the c=c number
  • end with ‘ene’
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5
Q

How do we name branched chained hydrocarbons ?

A
  • identify the longest carbon atoms
  • number the carbon chain so the functional group sits on the lowest carbon number possible
  • look at the side groups and determine which akyl group there are in and what carbon the sit on
  • if there is more than one identical functionial group/side chain put di-2, tri-3 tetra-4
  • name by the number on side group and alkyl name, the carbon chain name, carbon number the functional group is on and the suffix.
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6
Q

General formula

A

The simplest algerbraic formula of a member of a homologous series

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7
Q

Alkane general formula

A

CnH2n+2

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8
Q

Alkene general formula

A

CnH2n

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9
Q

Alcohols general formula

A

CnH2n+1OH

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10
Q

Structual formula

A

The minimal detail that shows the arrangement of atoms in a molecule without showing bonds

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11
Q

Sketetal formula

A

Shows just a carbon skeleton and functional groups. Hydrogen is not shown

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12
Q

Display formula

A
  • the relative positioning of atoms and bonds between them
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13
Q

Prefix’s naming molecules

A 
1- meth
2-eth
3-prop
4-But
5-pent
6-Hex
7-hept
8-oct
9-non
10-dec
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14
Q

Alkyl groups

A

Hydrocarbon branches with the general formula CnH2n+1

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15
Q

Aromatic compounds

A
  • contains a benzene ring. They may have functional groups and alkyl groups coming from this
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16
Q

Aliphatic compounds

A
  • straight, branched chains or non aromatic rings with or without side chains
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17
Q

Alycyclic compounds

A
  • a aliphatic compound arranged in non-aromatic rings with or without side chains
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18
Q

Unsaturated compound

A
  • multiple carbon-carbon bonds
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19
Q

Saturated compounds

A
  • single carbon-carbon bond
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20
Q

Structural isomers

A
  • conpounds with the same molecular formula but differnt structural formulae. There are 3 types: chain, positional and functional group
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21
Q

Chain isomerism

A
  • compounds with the same molecular formula but different arrangement of the carbon skeleton
22
Q

Positional isomerism

A
  • compounds with the same molecular formula but different position of functional group on the carbon skeleton
23
Q

Functional group isomerism

A

-compounds with the same molecular formula but different functional group

24
Q

Homolytic fission

A

Each bonding atoms reveives one electron from the bonded pair,
forming two radical

25
Q

Heterolytic fisson

A

One bonding atom receiving both electrons from the bonded pair

26
Q

Radicals

A

A species with an unpaired electron

27
Q

What does the dot represent in a reaction mechanism?

A
  • radicals
28
Q

What does a curly arrow represent?

A

The movement of electrons

29
Q

Properties of alkanes

A
  • saturated hydrocarbon. Each carbon is bonded 4 times
  • form a tetrahedral shape (109.5 degrees) because all the bonds repel each other equally.
  • larger molecules (longer carbon chain) have more induced dipole-dipole forces due to having a larger electron cloud and more surface contact. so a higher boiling point.
  • branched molecules have fewer induced dipole attraction due to fewer surface area interaction between molecules so have a lower boing point.
30
Q

Why do alkanes have a low reactivity with many reagents?

A
  • all covalent bonds in alkanes have high bond enthalpies
  • the carbon-hydrogen sigma bonds have very low polarity as the electronegatibites of crabon and hydrogen are almost the same.
31
Q

Complete combustion of alkanes

A
  • burns completely in oxygen wgen there is a plentiful supply forming CO2 and H20.
32
Q

Incomplete combustion of alkanes

A
  • burns with a limited supply of oxygen producing carbon monoxide( CO) and carbon particles (soot)
33
Q

3 main stages of radical substitution ( alkanes react with chlorine and bromine forming halogenated organic compound)

A
  • inititation: radicals are produced normally using visible or UV light (photochemical reactions)
  • propagation: when a radical reacts woth a non-radical molecules forming new radicals which go on to react with other non- radicaks.
  • termination: two radicals react to make a stable non-radical molecule (chloromethane) ends reaction
34
Q

Limitations of radical substitution

A
  • forms a mixture of organic products. and side products ( multiple substitutions) therefore there is a low atom economy

Adding excess of the reactant can reduce the amount of substitutions. There is a greater chance of radical reacting with the product than another substance

  • isomers are formed as free radical substitution can occur abywhere on a hydrocarbon chain
35
Q

steroisomerism

A

molecules with the molecular formula but different arrangement of atoms in space

36
Q

cis-trans isomerism

A
  • naming isomer system
  • carbon atoms on each side of the double bond must be bonded to 2 different groups and at least one of theses groups must be the same on both sides of the carbons on the double bond.
  • find the group the same on both sides if the group are on the same side it is a CIS isomer
  • if the group are on opposite sides its a TRANS isomer
37
Q

using CIP rules to determine E/Z isomers

A
  • assign priority to the highest atomic number group on both sides of the carbon atoms
  • if the priority groups are on the same side its a Z isomer and on different sides its a Z isomer
38
Q

Properties of alkenes

A
  • trigonal planar shape (120 degree) The three bonding pair of electrons are in the plane of the molecule and repel each other equally
  • stereoisomerism
  • very reactive due to the Pi bonds having a high electron density and low bond enthaplys
39
Q

E/Z isomerism

A

An example of steroisomerism, in terms of restricted rotation about a double bond and the reuirement for two different groups to be attached to each carbon atom of the C=C group

40
Q

Cis-trans isomerism

A

A special case of E/Z isomerism in which two of the substituent groups attached to each carbon atom of the C=C group are the same.

41
Q

Electrophile

A

An electron pair acceptir

42
Q

The use of bromine to detect the presence of a double C=C bond

A
  • Bromine is polarised as the electrons in the double repel the electrons in Br2 moving them to one side creating a dipole
  • an electron pair in the double bond is attracted to the slighly positive bromine and form a bond. This breaks the Br-Br (heterlytic fission)
  • a carbon cation intermediate is formed and Br is attracted to the C+
  • this forms colourless dibromoethene
43
Q

Hydrogenation

A

-hydrogen is added across a C=C bond. At 150 degree temp with a nickel catalyst. This saturated the alkene forming a alkane.

44
Q

Hydrogen halides to form haloalkanes

A
  • H-X is permanently polarised e.g HBR
  • heterlytic fission breaks the bonds between HBR
  • a carbon intermediate is formed and the Br- is attrated to the C+
45
Q

addition reaction with steam

A
  • addition reaction between gaseous alkene and steam. Used to make alcohols.
  • conditions involve high temperatures and high pressures with a phosphoric acid catalyst
  • reversible reaction with a inital reaction yield of only 5%. Any unreacted alkene is recycled through and an overall yield at 90-95% can be obtained overall
46
Q

Markownikoffs rule

A

when H-X is added to an unsymmetrical alkene, the hydrogen becomes attached to the carbon with that is most stable than those with hydrogen atoms attached

47
Q

reactions of alkenes

A
  • very reactive due tom the pi bond which have a high electron density
  • then Pi electrons are on the outside of the double bond this makes it easier to break as they are more exposed
  • because the double bond breaks it is possible to add atoms/groups to the alkene
  • undergo addition reactions with:
  • hydrogen
  • halogens
  • hydrogen halides
  • steam
48
Q

combustion of energy production

A
  • plastic can be burnt in power stations. the chemical energy transferred can be used to drive turbines and generate electricity.
49
Q

organic feedstock

A
  • waste polymers are broken down by chemical and thermal processes into monomers. Which can be used as the raw materials in the production of new polymers and other organic chemicals.
  • benefit is it works well with unsorted and unwashed polymers
50
Q

the benefits of biodegradable and photodegradable polymers

A
  • biodegradable polymers can be broken down over time by microorganisms
  • photodegradable polymers contain bonds that are weakened by absorbing light/visible radiation breaking down the polymer,.
  • compostable polymers are commonly plant based .they degrade naturally leaving no harmful residues.
  • bioplastics are polymers that are made from plant starch

chemistry (9 decks)

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