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✅Chemistry Unit 2 > đŸ”´đŸ”¸2.4 -organic Compounds > Flashcards

đŸ”´đŸ”¸2.4 -organic Compounds Flashcards

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1
Q

What is a functional group

A

The atom/ groups of atoms that gives the compound its characteristic properties

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2
Q

What is an homologous series

A

A series of compounds with the same functional group

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3
Q

What is a saturated compound

A

One that contains no C to C multiple bonds

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4
Q

What is a hydrocarbon

A

A compound of carbon and hydrogen only

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5
Q

What is an unsaturated compound

A

One that contains C to C multiple bonds (double bonds)

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6
Q

What are organic chemicals

A

Chemicals produced by living things often containing hydrogen carbon, some oxygen and other elements (nitrogen, sulfur, phosphorous and the halogens)

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7
Q

What does the order of the elements in a functional group determine

A

Determine which homologous series the compound belongs to

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8
Q

What are alkanes

E.g ethane

A

Saturated hydrocarbons

E.g Ethane

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9
Q

What are alkenes

E.g Ethene

A

Unsaturated hydrocarbons with C-C double bond

E.g Ethene

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10
Q

What are halogenalkanes

A

Compounds in which one or more hydrogen’s in an alkane have been replaced by a halogen
E.g iodoethane

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11
Q

What are alcohols

A

Compounds containing -OH as the functional group

E.g Ethanol

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12
Q

What are Carboxylic acids

A

Compounds containing -COOH as the functional group

E.g pentanoic acid

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13
Q

What is the code for 1,2,3,4,5,6,7,8,9 and 10 carbons

A 
Meth
Eth
Prop
But
Pent
Hex
Hept 
Oct 
Non 
Dec
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14
Q

What are the rules for naming compounds

A

1) find longest carbon chain e.g 5 carbons = pent
2) label C atoms starting from 1 where there is a side chain closest
3) if more than 1 side chain use di for 2, tri for 3 or tetra for 4
4) name the side chains e.g CH3= methyl C2H5= ethyl
5) saturated carbons shown by (ane), C=C shown by (ene), -OH shown by (ol), -COOH shown by (oic acid), halogen shown by halogeno

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15
Q

What is the molecular formula

A

Shows the atoms, how many of each type there are, in a molecules of a compound e.g C5H12

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16
Q

What is displayed formula

A 
A formulae showing all of the bonds and atoms in the molecule 
E.g 
 |   |   |   | 
C-C-C-C - 
 |   |   |   |
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17
Q

What is shortened formula

A

Shows the groups in sufficient detail that the structure is unambiguous
E.g CH3C(CH3)2CH2Cl

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18
Q

What is skeletal formula

A

Shows the carbon/hydrogen backbone of the molecule as a series of bonds with any functional groups attached
E.g /\/\/\ =heptane

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19
Q

Name the characteristics for a homologous series

A

1) same general formula e.g (CnH2n+2 for alkanes)
2) differ from neighbour in the series by CH2
3) same functional groups and :: similar chemical properties
4) physical properties that vary as the Mr of the compound varies

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20
Q

Give 5 examples of homologous series

A 
Alkanes (saturated hydrocarbons)
Alkenes (functional group C=C)
Alcohols (functional group -OH)
Halogenoalkanes (functional group -F, -Cl, -Br, -I) 
Carboxylic acids (functional group -COOH)
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21
Q

What 3 things can the functional group vary in particular

A
  • melting temperature
  • boiling temperature
  • solubility in water
22
Q

What is the empirical formula

A

Formula of a compound with the atoms of elements in their simplest ratio

23
Q

Give the empirical formula of ethane

A

Ethan molecular formula = C2H6
Ratio C:H = 2:6
Simplest ratio = 1:3
Empirical formula = CH3

24
Q

What is the equation for the ratio of atoms of each element?

A

Moles (n) = Mass (g) / Ar

25
Q

Name 2 types of isomerism

A

Structural and E/Z

26
Q

What is structural isomerism

A

Compounds with the same molecular formula but different structural formula

27
Q

Name the 3 types of structural isomerism

A

Chain isomerism
Position isomerism
Functional group isomerism

28
Q

When does chain isomerism usually occur

A

When carbon chain is arranged differently, usually one is a straight chain and the others branched
E.g CH3CH2CH3 (butane) and 2-methylpropane

29
Q

When does positional isomerism occur

A

When the functional group is in a different position in the molecule e.g 1 -chloropropane (CH2ClCH2CH3) and 2 -chloropropane (CH3CHClCH3)

30
Q

When does functional isomerism occur?

A

When the functional group in compounds is different e.g C3H6O could be propanal (aldehyde) or propanone (ketone)

31
Q

What is E-Z isomerism

A

Isomerism that occurs in alkenes due to restricted rotation about the double bond

32
Q

Why is E-Z isomerism possible in alkenes but not alkanes

A

Single bonds in alkanes allow the atoms/groups at either end to rotate freely
The double bond in alkenes restrict rotation due to the π bond

33
Q

What is a π bond

A

A bond formed by the overlap of p orbitals on adjacent atoms, often represented as double bonds (C=C)

34
Q

What is a sigma bond

A

Strongest type of covalent chemical bond formed by head on overlapping between 2 atomic orbitals. Represented by (C-C)

35
Q

What is a (Z) isomer

A

An isomer where groups of the higher priority (highest Ar) are on the same side of the carbon double bond
E.g (Z)-1,2 -dibromoethene

36
Q

What is an (E) isomer

A

An isomer where groups with the higher priority (highest Ar) are attached to the carbons on opposite sides of the double bond
E.g (E)-1,2 -dibromoethene

37
Q 
What happens if the groups attached are different e.g 
     Br     Cl
       \       /
       C = C
      /        \
    H         H
A

Bromine has a higher priority than Hydrogen
Chlorine has a higher priority than Hydrogen
Both groups with highest priority are on the same side of double bond :: z isomerism
This is called (Z)1-bromo 2-chloroethene

38
Q

What effect does the double bond have on the isomers

A

still take part in characteristic reactions of alkenes as still have double bond

39
Q

What effect does the restricted rotation have on the substituent groups attached to double bond

A

Can cause them to behave differently because In the E form the substituent groups are held too far apart to interact, in Z form they are closer

40
Q

Why do E isomers normally have higher melting/ boiling points than Z isomers

A

Shape of E molecules means they can fit together more closely :: have stronger intermolecular forces and :: higher melting/boiling temperatures

41
Q

Give an example of the melting points in an E isomer and Z isomer

A

(Z) -Butenedoic acid = 130 degrees Celsius

(E) -Butenedioc acid = 286 degrees celcius

42
Q

What are Van der Waals forces?

A

Dipole-dipole or temporary dipole-temporary dipole Interactions between atoms and molecules

43
Q

What states do small hydrocarbon chains have at room temperature?

A

Gases

44
Q

What state do longer hydrocarbons have at room temperature?

A

Liquids and even larger hydrocarbons are solid at room temperature

45
Q

What structure do all hydrocarbons have, what does this mean

A

Hydrocarbons are simple covalent molecules, non polar

This mean only temporary dipole-temporary dipole Van der Waals forces are present between molecules (weak)

46
Q

Why do the van der Waals forces affect melting/boiling temperatures

A

Intermolecular temporary dipole-temporary dipole forces act between he surfaces of hydrocarbons meaning the more surface there is in contact the more forces will act and the more energy is needed to overcome these forces

47
Q

What are intermolecular forces

A

Forces between molecules

48
Q

What are intramolecular forces

A

Forces within the same molecule

49
Q

Why do ‘sausage shaped’ molecules e.g pentane (straight carbon chain saturated with hydrogen’s) have a greater boiling temperature than more spherical molecules with the same molecular formula e.g 2,2 -Dimethylpropane

A

When bonds are in a spherical formation often very branched (2,2 -dimethylpropane) the area available for surface area contact is very small meaning the lower its boiling temperature as less van der Waals forces can form

50
Q

Give the boiling points of pentane and 2,2 dimethyl propane

A

Pentane = 36 degrees

2,2 -dimethylpropane = 10 degrees

✅Chemistry Unit 2 (8 decks)

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