Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Core Organic Chemistry > Flashcards

Core Organic Chemistry Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What is an hydrocarbon?

A

It is a compound that has ONLY carbon and hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is an aliphatic hydrocarbon?

A

It is a compound containing carbon and hydrogen joined together in straight chain, a branched chain or non-aromatic rings

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is an alicyclic hydrocarbon

A

It is an aliphatic compound arranged in non-aromatic rings, with or without side chains

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is an aromatic hydrocarbon?

A

It is an unsaturated hydrocarbon that contains benzene rings(C6H6)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is a functional group?

A

It is a group of atoms responsible for the characteristics reaction of a compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is a homologous series?

A

It is a series of organic compounds that have the same functional group but with each successive member differing by CH2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What does “saturated mean”?

A

It means having single carbon-carbon bonds ONLY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What does “unsaturated” mean?

A

It means having multiple carbon-carbon bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is a molecular formula?

A

It tells you the actual number of the atoms of the element in the compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is an empirical formula?

A

It is the simplest whole number ratio of the atoms of each element in a compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is a structural formula?

A

It is the minimal detail that shows the arrangement of an atom in a molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is a displayed formula?

A

It shows the relative positioning of atoms and the bonds between them

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is a skeletal formula?

A

It is shown by leaving just a carbon skeleton and associated functional group

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is isomerism?

A

It is when compounds have the same molecular formula but different arrangements of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are structural isomers?

A

It is when compounds have the same molecular formula but different structural formulae

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is electronegativity?

A

It is the ability of an atom to attract the bonded pair of electrons in a covalent bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Factors affecting electronegativity

A

Nuclear charge
Atomic radius
Number of electron shielding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

How does nuclear charge affect electronegativity?

A

As the nuclear charge ⬆, the electronegativity ⬆. This is because the increased positive charge increases the attraction between the electrons in the outer shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

How does Atomic radius affect electronegativity?

A

As atomic radius ⬇, the electronegativity ⬆. This is because the outer shell is closer to the nucleus and so the atom is easily attracted to the electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

How does number of shielding affect electronegativity?

A

As number of shielding ⬆, the electronegativity ⬇. This is because the inner shells are blocking the outer shells from being attracted by the nucleus and so the outer shell gets further away from the nucleus.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is a dipole?

A

A dipole is a separation of partial charges in a molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is IMF?

A

IMF is a weak force of attraction between molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What are the types of IMF?

A

Induced dipole-dipole forces/London forces
Permanent dipole-dipole forces
Hydrogen Bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is an instantaneous dipole?

A

It is caused by the random movement of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

How are London forces formed?

A

They are formed when the random movement of electrons form a temporary dipole and that causes an induced dipole in the neighbouring molecule and these induced dipoles attract each other resulting in an attraction between the molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What are some key features of London forces?

A
  1. They are weak and easily broken
  2. Their strength depends on the number of electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

How does permanent dipole-dipole interactions form between molecules?

A

permanent dipole-dipole forms when the electrons get more attracted to the more electronegative atom and forms a polar bond and this attracts the less EN atom in another polar molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Why does F2 have a higher BP than O2, but a lower BP than HCl?

A

F2 has a higher BP than O2 because it has more electrons
F2 has non-polar molecules and has London forces only. HCl has polar molecules and will also have permanent dipole-dipole interactions and so the total IMF in HCl are stronger

29
Q

How does hydrogen bonding forms?

A
  1. It forms when H bonds with a more electronegative atom
  2. The electronegative atom must have a lone pair
30
Q

What are Alkanes?

A

Alkanes are compounds with saturated hydrocarbons

31
Q

What are the type of covalent bond in alkanes called?

A

Sigma bonds

32
Q

How are sigma bonds formed?

A

Sigma bonds are formed when the electron orbitals from adjacent atoms directly overlap

33
Q

What is the general formula of an alkane?

A

CnH2n+2

34
Q

What are some properties of alkanes?

A
  1. they are insoluble in water because they are non-polar molecules(because of the similar electronegativity in C and H)
  2. They are generally unreactive (because of the strong covalent bonds between them)
35
Q

What is the trends in BP for straight chain alkanes?

A

As the length of the chain ⬆, the BP ⬆ because of the electrons ⬆ which ⬆ the strength of the London forces

36
Q

What is the trends in BP for branched chain alkanes?

A

As the number of branches ⬆ the BP ⬇. This is because there is less contact between the molecules and so the London forces get weaker

37
Q

What are some reactions of alkanes?

A

Combustion (complete& incomplete)

38
Q

What is the word equation for the COMPLETE combustion of alkanes?

A

Alkane + oxygen➡Carbon dioxide + water

39
Q

What is the word equation for the INCOMPLETE combustion of alkanes?

A

Alkane + 1/2 oxygen ➡ Carbon monoxide + water + soot

40
Q

What are radicals?

A

Radicals are species with unpaired electrons

41
Q

Describe the reaction of alkanes with halogens

A

UV light is used to initiate the reaction
Successive substitution of the H atom in the alkane with either Br/Cl
Produces a mixture of bromo-/chloro- alkane

42
Q

What are the three stages in free radical substitution?

A

Initiation
Propagation
Termination

43
Q

Describe the initiation process

A

UV light is shone at the reaction mix
UV light then breaks the covalent bond between the bromine atoms and each electron goes to one bromine atom each forming two free bromine radicals

44
Q

Diagram of the initiation process between Br and methane

A

Br2➡2Br*

45
Q

Describe the 2 steps in propagation process

A

Step 1: the free bromine radical reacts with the methane atom and takes a hydrogen and an electron from the methane atom to form a free methyl group and hydrogen bromide
Step 2: the free methyl group reacts with an bromine molecule to form bromomethane and a free bromine radical

46
Q

Diagram of the propagation process

A

Step 1: CH4 + Br➡CH3+HBr
Step 2: CH3+ Br2➡CH4Br+Br

47
Q

Describe the termination process

A

Removes the free radical from the system by replacing them with new ones

48
Q

Possible termination products

A

Br+Br➡Br2
2CH3* ➡ C2H6
CH3* + Br* ➡ CH3Br

49
Q

What are some problems with the free radical substitution?

A

It produces a wide range of side-products so we need to separate out the product molecule

50
Q

What are alkene

A

Alkenes are unsaturated hydrocarbons

51
Q

What is the general formula of alkenes?

A

CnH2n

52
Q

What are the types of covalent bonds in alkenes?

A

π-bonds and sigma σ-bonds

53
Q

What are π-bonds?

A

π-bonds are formed when sideway orbitals overlap above and below the bonding C atoms

54
Q

Explain the reactivity of alkenes

A

Alkenes are reactivity because:
1. the double bond is a region of high electron density which will attract an electrophile
2. The π-bond has a lower bond enthalpy than σ-bonds and so less energy is needed to break the π-bonds

55
Q

What are σ-bonds?

A

They are formed when the orbitals overlap between the bonding atoms

56
Q

Explain the shape and bond angles around the C atoms of a C=C bond

A

Each carbon atom has 3 regions of electron density which repel each other forming a trigonal plane with bond angles of 120 °

57
Q

What is an electrophile?

A

An electrophile is an electron pair acceptor from a region of high electron density.

58
Q

What is the reaction that alkenes are involved in?

A

Addition reactions

59
Q

What happens in an addition reaction?

A

a small molecule breaks the π-bond forming a new σ-bond
unsaturated to saturated

60
Q

What is formed when a hydrogen halide reacts with a symmetrical alkene?

A

Hydrogen halide + symmetrical alkene=one product

61
Q

What is formed when a hydrogen halide reacts with an unsymmetrical alkene?

A

Hydrogen halide + unsymmetrical alkene= two product (one is usually a major product while the other is a minor product)

62
Q

Why are major and minor products formed?

A

They are formed because the stability of the carbocations depend on the number of alkyl groups that the carbon with the positive charge is bonded to.

63
Q

What is a carbocation?

A

It is a positive charged specie with the positive charge on the carbon atom

64
Q

What is a primary carbocation?

A

It is when the carbon with the positive charge is bonded to only one alkyl group

65
Q

What is a secondary carbocation?

A

It is when the carbon with the positive charge is bonded to 2 alkyl groups

66
Q

What product ends up being the major product?

A

The secondary carbocation because it is more stable so it’s more likely to form more products

67
Q

What is Markovnikov’s rule?

A

When a hydrogen halide reacts with an asymmetric alkene, the hydrogen atom of the hydrogen halide is more likely to get attracted to the carbon atom which has a greater number of hydrogen atoms

68
Q

Describe the test for unsaturation

A

In a test tube, add the unknown substance and add bromine water and gently mix the mixture
RESULTS: if the mixture is unsaturated, then the mixture will turn colourless and this is because of the bromine molecule getting added across the C==C bond

Chemistry (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions