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Chemistry > AoS2 - Organic Compounds, Naming, Structures and Physical Properties > Flashcards

AoS2 - Organic Compounds, Naming, Structures and Physical Properties Flashcards

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1
Q

Organic Chemistry

A

Study of the compounds of carbon (with some exclusion)

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2
Q

Organic Compounds

A
  • organic molecular compounds
  • comprise over 90% of all known chemicals
  • occur naturally and can be produced in the laboratory.
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3
Q

Hydrocarbons

A
  • simplest class of organic compounds
  • consist of hydrogen and carbon in chains of varying length
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4
Q

Types of Hydrocarbons

A

Aliphatic and Cyclic

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5
Q

Aliphatic Hydrocarbons

A

Carbon and hydrogen atoms are arranged in straight chains or branched chains.

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6
Q

Cyclic Hydrocarbons

A

Carbon atoms arranged in a ring structure.

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7
Q

Saturated Hydrocarbons

A

Contains only single carbon to carbon bonds

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8
Q

Unsaturated Hydrocarbons

A

Contains double or triple carbon to carbon bonds.

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9
Q

Families/Series of Aliphatic Hydrocarbons

A

Alkanes, Alkynes and Alkenes.

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10
Q

Use of Hydrocarbons

A
  • fuels
  • solvents
  • lubricants
  • raw materials for products such as plastics, fibres and explosives.
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11
Q

Homologous Series

A

Series of Hydrocarbons that have a similar chemical structure and similar chemical properties
Each compound in each series differs from the previous one by a CH2 group.

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12
Q

Alkane

A

CnH2n+2
Single Carbon to Carbon bonds only
Saturated

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13
Q

Alkene

A

CnH2n
One double Carbon to Carbon bond
Unsaturated

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14
Q

Alkyne

A

CnH2n-2
I triple Carbon to Carbon bond.
Unsaturated

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15
Q

Molecular Formula

A

Chemical formula that shows the total number and types of atoms in a molecule but not their structural arrangement.

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16
Q

Structural Formula

A

Graphic representation of the molecular structure, showing how the atoms are arranged.
Shows all covalent bonds.

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17
Q

Condensed Formula

A

Compact way of drawing the structural formula of a molecule. Covalent bonds are not shown.

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18
Q

Skeletal Formula

A
  • Representation of the molecular structure in which covalent bonds are shown as line, but the atoms are not shown.
    Other atoms are written in.
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19
Q

Structural Isomers

A

Compounds having the same molecular formula but different structures.
- Have similar chemical properties but can differ in some physical properties.

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20
Q

Straight Chain

A

C atoms bonded in a continuous chain.

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21
Q

Branched Chain

A

C atoms form a branch

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22
Q

What happens to the isomers as the molecules become larger?

A

They are able to form a greater number of isomers.

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23
Q

Naming Hydrocarbons

A

Named according to international union of pure and applied chemistry.

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24
Q

I C

A

Meth

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25
Q

2 C

A

Eth

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26
Q

3 C

A

Prop

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27
Q

4 C

A

But

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28
Q

5 C

A

Pent

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29
Q

6 C

A

Hex

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30
Q

7 C

A

Hept

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31
Q

8 C

A

Oct

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32
Q

9 C

A

Non

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33
Q

10 C

A

Dec

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34
Q

Prefix

A

Indicates number of C atoms in longest chain

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35
Q

Suffix

A

Refers to hydrocarbon type
- ane
- ene
- yne

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36
Q

Naming Alkanes

A
  • identify longest chain
  • identify name of branch
  • number carbon atoms in the longest chain so side groups are on atoms with smallest number
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37
Q

Alkyl Groups

A

An alkane molecule with one less H

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38
Q

Two or more alkyl groups on same/different carbons

A

use
- di
- tri
- tetra

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39
Q

Two or more branches on the same carbon

A
  • identify number for EACH branch
  • List in alphabetical order.
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40
Q

Naming Alkenes + Alkynes

A
  • identify longest chain containing double/triple bond
  • number C’s so double/triple bond has the smallest number
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41
Q

Functional Group

A

An atom (halogen) or groups of atoms (other than hydrogen) that influence the chemical and physical properties of the compounds forming a homologous series.

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42
Q

Homologous Series of Functional Groups include

A

Haloalkanes
Alcohols
Carboxylic acids
Esters

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43
Q

Haloalkanes

A

Functional Group: Cl, Br, F
Prefix: chloro, bromo, fluoro
Dipole - dipole bonding

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44
Q

Alcohol

A

Functional Group (OH-)
- hydroxyl
suffix : “ol”
hydrogen bonding

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45
Q

Carboxylic Acid

A

Functional Group: COOH (carboxyl)
suffix = -oic acid
Hydrogen Bonding

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46
Q

Functional Groups (most important to least important)

A
  • carboxylic acids
  • alcohol
  • alkyne = alkene
  • alkane
  • haloalkane
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47
Q

When naming, if more than one functional group is present

A
  • the most important group determines ending
  • all other groups form the prefix.
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48
Q

Bonding in Hydrocarbons

A
  • non-polar molecules
  • dispersion forces only
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49
Q

Bonding in Haloalkanes

A
  • presence of halogen creates polar molecule
  • dipole-dipole bonding
50
Q

Bonding in Alcohol

A
  • presence of Hydroxyl group creates polar molecule
  • hydrogen bonding
51
Q

Carboxylic Acid

A
  • Presence of Carboxyl group creates polarity
  • Two Hydrogen bonds.
52
Q

Solubility

A

The ability of a substance to dissolve in a solvent

53
Q

For an organic compound to be soluble

A

Intermolecular bonds of the substance and water must be broken
New bonds are formed between molecules.

54
Q

Solubility in water

A

Must be able to break strong hydrogen bonds between water molecules.
Nonpolar molecules: weak dispersion forces hence insoluble.
Small Polar substances with hydrogen bonds are soluble.

55
Q

Solubility with Hydrogen Bonds

A
  • Solubility decreases as size of the molecule increases due to larger non-polar sections (hydrophobic section) that reduces impact of hydrogen bond
56
Q

Chemical Property

A

Characteristic that becomes evident after a substance undergoes a chemical reaction/change.

57
Q

Physical Property

A

Can be observed or measured without changing matter composition.
Melting + boiling points, viscosity, solubility

58
Q

Viscosity

A

The resistance to flow as a liquid

59
Q

Trends of Organic Compounds

A
  • depend on intermolecular forces present
  • strength dependent on: size of molecule, degree of branching and presence of functional groups.
60
Q

Degree of Branching

A

Strength of forces decreases with increasing number of branches
Straight chain molecules are packed close, increasing strength
Branched chain cannot get close, decreasing strength.

60
Q

Size of the molecule

A

Strength of forces increase with increasing size.

61
Q

Presence of functional groups

A
  • Strength increases with addition of dipole-dipole or hydrogen bonding.
62
Q

Why are Carboxyl groups always on the end?

A

The carbon in the carboxyl group already bonded to three other atoms, it only has one bond available and is hence located on the end of the carbon chain.

63
Q

General rule for smaller molecules

A

like dissolves like
polar – polar

64
Q

What is percentage composition?

A

A relative measure of the mass of each different elements present in a compound.

65
Q

Percentage composition formulas

A

Molar mass of element/molar mass of compound
Mass of the element/mass of the sample

66
Q

Calculating mass of an element using percentage composition

A
  • given mass and molecular formula
    molar mass of element (including number)/ molar mass of compound x mass of compound.
67
Q

What is the empirical formula?

A

Simplest whole number ratio of elements in a compound

68
Q

Steps for calculating the empirical formula

A
  1. Determine the mass of each element
  2. Calculate the amount in mol
  3. Divide each element by the lowest mole quantity
  4. Express as a formula
69
Q

Calculating number of mol of an element given mol of the whole compound

A

total mol x number of element atoms in compound

70
Q

What is the molecular formula?

A

Actual number of each element in a compound

71
Q

Steps for calculating molecular formula

A
  1. Determine empirical formula
  2. Determine molar mass
  3. Calculate by dividing molar mass required by molar mass of empirical formula.
72
Q

Define Allotrope

A

Different physical form of the same element

73
Q

What are allotropes of carbon?

A
  • Diamond
  • Graphite
  • Fullerenes
74
Q

Describe diamond

A

Covalent network lattice
- Each atom is covalently bonded to 4 other carbon atoms in 3 dimensions
- highest melting point
- hardest known substance
- chemically inert
- non-conductive
- insoluble in water

75
Q

Provide examples of other network lattices

A
  • Silicon
  • Silicon Carbide
  • Silicon dioxide
76
Q

What carbon allotrope is this?

A

Diamond

77
Q

Describe Graphite

A
  • Covalent layer lattice
  • Each carbon atom is covalently bonded to 3 other carbon atoms
  • conductor of electricity, soft, weak and greasy
  • high melting temperature
78
Q

What intermolecular forces does graphite have?

A

Forces between layers are weak dispersion forces

79
Q

Where is the fourth electron in graphite?

A

Fourth electron is delocalised and free to move between layers

80
Q

What shape does Diamond have?

A

Tetrahedral

81
Q

Why does Graphite conduct electricity while Diamond does not?

A
  • Graphite has free moving delocalised electrons
  • For electricity to be conducted, there must be free moving charged particles.
82
Q

Why is diamond so hard?

A
  • strongest form of intramolecular forces due to network lattice in which atoms are arranged
  • Each carbon atom is covalently bonded to 4 other carbons
83
Q

Practical uses for Diamond

A

Cutting tools and jewelry

84
Q

Why does diamond have a high melting point compared to graphite?

A
  • Diamond has carbon atoms arranged in a network lattice and has strong bonds in all three dimensions
  • A network lattice is stronger than the intermolecular forces of graphite as more energy required to break these bonds
85
Q

Why can graphite be used as a lubricants?

A
  • Layer lattice structure
  • Layers are held together by weak dispersion forces so they can readily slide past one another
  • Has a very high melting point
86
Q

Reactivity of hydrocarbons order

A
  1. Alkynes
  2. Alkenes
  3. Alkanes
    The presence of a double or triple bond makes a hydrocarbon more reactive.
87
Q

What are esters?

A
  • a homologous series which contain an ester functional group
  • creates a polar molecule which leads to dipole dipole bonding
88
Q

What homologous series are esters made from?

A

Alcohols and carboxylic acids.

89
Q

Naming esters

A

(alcohol)(acid-oate)

90
Q

Why does boiling point increase with increasing chain length?

A
  • number of dispersion forces increase
  • results in stronger intermolecular forces which require more energy to break
91
Q

Why are cyclic hydrocarbons insoluble in water?

A
  • both substances have to be polar according to the like dissolves like rule
  • hydrogen bonds are unable to be broken by the weak dispersion forces
92
Q

Where are hydrocarbons found?

A
  • crude oil
  • processing oil produces useful substances
93
Q

Why does the addition of a functional group change the properties?

A
  • creates dipole or hydrogen bonding
  • polar
  • increases intermolecular force strength, melting and boiling points.
94
Q

Why are carboxyl groups always on the end of the longest chain?

A
  • Carbon is already bonded to 3 other atoms, it only has one bond available.
95
Q

Properties affecting viscosity

A
  • smaller molecules that have less atoms form less dispersion forces
  • ## molecules require less energy to break bonds and can flow over one another easier
96
Q

Largest source of crude oil

A

Fossil fuels

97
Q

Crude oil is also known as

A

Petroleum that contains different length hydrocarbons

98
Q

Distillation

A

separating two or more liquid components on the basis of boiling point differences

99
Q

Fractional distillation

A

process used to refine (seperate) crude oil into its components
Hydrocarbons have different length chains so are seperated based on boiling points

100
Q

Distillation in the laboratory

A
  • process used to separate and purify liquids in the laboratory based on boiling points.
101
Q

Substitution reaction

A

Atom in an alkane is replaced by a halogen in the presence of UV light and high temperatures

102
Q

How many products are formed in a substitution reaction?

A

Two

103
Q

Why is UV light required for a substitution reaction?

A

UV light provides the energy to break the covalent bond in the halogen molecule to produce two reactive halogen atoms each with an unpaired electron

104
Q

Combustion reaction

A
  • hydrocarbons are fuels that react with oxygen gas in a combustion reaction
105
Q

complete combustion reaction

A

excess oxygen

106
Q

incomplete combustion

A

limited oxygen (monoxide)
CO

107
Q

Addition reactions

A

Alkene reacts with another substance to form a single product
- must be unsaturated
- often requires a catalyst

108
Q

Bromine test

A
  • bromine water has a characteristic orange colour
  • loses this when combined with an unsaturated hydrocarbon
109
Q

How are esters produced

A

Condensation reaction

110
Q

Condensation reaction

A
  • carboxylic acid and alcohol
  • water is the product
  • hydroxyl group must be on carbon 1
  • acid required as a catalyst
111
Q

Cracking/Decomposition

A
  • process where large alkanes are broken down into smaller more useful hydrocarbons
112
Q

Weak acids

A
  • carboxylic acids
  • in water, partially ionize to produce hydrogen ions
113
Q

pH scale

A
  • measures how acidic a substance is
114
Q

Acidity

A

Measure of concentration of hydrogen ions
- the more hydrogen ions the more acidic

115
Q

Alcohol pH

A

6

116
Q

Carboxylic acid pH

A

3 - 4

117
Q

Reactions of haloalkanes

A

made from alkanes using substitution or alkenes using addition
- starting material for synthesis
- creates polar bond

118
Q

To produce a haloalkane

A
  • react with hydroxide ions in a substitution reaction to produce an alcohol
119
Q

Hydrolysis

A
  • addition of water
  • presence of water and heat
120
Q

catalyst

A

speeds up chemical reaction

Chemistry (6 decks)

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