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organic Flashcards

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1
Q

Structural vs Chain vs Positional Isomers

A
  • Structural Isomers - same molecular formula but different structures
  • Chain Isomers - main chain length is changed
  • Positional Isomers -exist when position of a branch changes
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2
Q

Dispersion forces definition

A

Defined as weak IMFs that occur in non-polar species due to the formation of temporary dipoles which then induce temporary dipoles in the surrounding species

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3
Q

Why do longer alkanes have greater dispersion forces

A

because of increased electrons

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4
Q

Why do straight chain alanes possess stronger dispersion forces than branched alkanes

A

Their shape allows maximum surface contact between the molecules

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5
Q

Why does cis/trans geometric isomerism exist

A

Exists due to inability to rotate around the double bond

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6
Q

Why are alkanes dispersion forces slightly more stronger than alkenes

A

due to stereochemistry

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7
Q

Aldehydes functional group + atoms + suffix

A

Functional group: -CHO (carbonyl - on terminal carbon)
suffix: -al

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8
Q

Dipole-dipole forces definition

A
  • the electrostatic attraction between oppositely charged ends of the overall dipole ,increasing in strength, with the difference in electronegativities between atoms of the molecules
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9
Q

Why does longer chain length aldehydes increases melting and boiling points

A

Increases the amount of electrons, increasing dispersion forces which then then add to the strength of the sum total intermolecular forces taking place between aldehyde molecules

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10
Q

Alcohols functional group + atoms + suffix

A
  • Functional group: -OH (hydroxyl)
  • Suffix: -ol
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11
Q

H-bonding defintion

A
  • Hydrogen bonding is an extreme form of dipole-dipole forces that only occurs when a hydrogen atom bonded to N, O or F interacts with a non-bonding pair of electrons on another N,O or F - either on the same molecule or different polar molecules
    • H-bonding is due to the highly electronegative negative nature of fluorine, oxygen, nitrogen that have a high charge density due to their relatively small size
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12
Q

Why do primary alcohols have higher BP + MP than secondary alcohols than tertiary alcohols

A

Due to the exposure of the hydroxyl

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13
Q

Ketones functional group + atoms + suffix

A
  • Functional group: -C=O (carbonyl - on non-terminal carbon)
    • Double bond oxygen
  • Suffix: -one
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14
Q

Carboxylic Acid functional group + atoms + suffix

A
  • Functional group: -COOH (carboxyl) on the first carbon
  • Suffix: -oic acid
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15
Q

Why does solubility in polar substances decrease with increasing chain length

A

This is because dispersion forces become more significant, preventing solvation in polar substances thus, they then become more soluble in non-polar substances

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16
Q

Amines functional group + atoms + suffix

A
  • Functional group: -NH2 (amine or amino)
  • Suffix: -amine
17
Q

Amides functional group + atoms + suffix

A
  • Functional group: -CONH2 (on starting atom)
    • Double bond oxygen; single bond amine group
  • Suffix: -amide
18
Q

Why is the H-bonding present in amides much stronger than equivalent amines or carboxylic acids (2 reasons)

A
  • Due to a greater number of hydrogen atoms available for hydrogen bonding in an amide compared to an amine or carboxylic acid. Thus, each amide molecule has 3 lone pairs of electrons and two hydrogen atoms that are available for hydrogen bonding
  • Also due to the close proximity of the highly electronegative oxygen atom causes hydrogen atoms from the NH2 group to develop a larger dipole (+) than what would occur on the nitrogen only
19
Q

Esters functional group + atoms + suffix

A
  • Functional group: -COO- (carboxylate - linking two alkane chains)
  • Suffix: -oate
20
Q

What are zwitterions

A
  • The existence of amino acids as a dipolar ion in a solid state or a neutral aqueous solution
    • Has both a positive and negative charge but no net charge
21
Q

What actually happens in a zwitterion on an atomic level

A

In this form, the carboxyl group gives up an acidic proton (leaves a COO-) which is accepted by the amino group (producing -NH3+)

22
Q

3 characteristics of zwitterions

A
  • Zwitterions have much higher melting points - because they possess ionic bonding
  • Dipolar nature of zwitterions also makes them very soluble in water - interacts through ion-dipole interactions
  • Dipolar nature of zwitterions allows them to act as acids or bases and can also act as buffers
23
Q

What are polymers

A

Polymers consist of long chains of repeating smaller units called monomers

24
Q

What can polymers consist of

A

Can consist of long straight chains or they may have side chains that join to other chains (cross linking)

25
Q

Two types of polymerisation reactions that lead to formation of polymers

A
  • Addition Polymerisation - involve small molecule alkenes acting as monomers joining with use of a catalyst to form a polymer
  • Condensation Polymerisation - involve the joining of monomers to produce the polymer and a small molecule such as water or carbon dioxide
26
Q

Proteins definition

A

Natural polymers formed through the combination of a-amino acids

27
Q

Dipeptide vs Polypeptide vs Protein

A
  • When two a-amino acids combine the structure can be referred to as a dipeptide
  • If more a-amino acids add to the dipeptide, it is referred to as a polypeptide
  • In general, if more than 50 a-amino acids are present in a peptide chain - it is referred to as a protein
28
Q

4 Main structures of proteins

A
  • Primary Structure
  • Secondary Structure
  • Tertiary Structure
  • Quantenary Structure
29
Q

Primary structure of protein definition

A

Specific linear sequence of the individual a-amino acids in the protein

30
Q

Type of bonding in secondary structures of proteins

A

H-bonding occurs between a lone pair of electrons from the oxygen in the carbonyl group and the polar hydrogen atom of an amine group

31
Q

A-Helix vs B-pleated sheets

A

A Helix - interactions within peptide chain between carbonyl group and amine group 4 amino acids away, producing coiled helix structure
B-pleated sheets - Interactions between adjacent polypeptides, resulting in hydrogen bonds within the plane of the sheet structure; all amino groups and carbonyl groups are involved in hydrogen bonds in B-pleated sheets

32
Q

Tertiary Structure definition and explanation for formation

A
  • Interactions that occur between the side chains of the a-amino acids in the proteins
    • May be H-bonding, ionic bonding, dipole-dipole forces, covalent bonding or dispersion forces
    • Gives rise to the protein molecule folding (bending and twisting) in such a way to achieve max stability
33
Q

What happens to tertiary structures in aqeous environments

A
  • protein will orient itself such that the hydrophobic side chains are orientated inwards; thus, hydrophilic side chains are orientated outwards with Disulfide bridges (covalent) often exist in the structure
34
Q

Quantenary Structure definition

A

Involves multiple proteins interacting to form larger conglomerate proteins

35
Q

Why is alcohol soluble in water but alkanes aren’t

A
  • The total alcohol-water forces (dispersion forces, dipole-dipole forces, H-bonding) are strong enough to overcome the total alcohol-alcohol (dispersion forces, dipole-dipole forces, H-bonding) and water-water (dispersion forces, dipole-dipole forces, H-bonding) forces, thus they are miscible
  • Alkanes are non-polar molecules with only dispersion forces
  • Thus, the total alkane-water forces (dispersion forces) are not strong enough to overcome the total alkane-alkane forces (dispersion forces) and water-water forces (dispersion forces, dipole-dipole forces, H-bonding), thus the substances are not miscible
36
Q

Explain why ethanal is soluble in water while octanal is not

A
  • The total ethanal-water forces (dispersion + dipole-dipole + H-bonding) are strong enough to overcome the total ethanal-ethanal (dispersion + dipole-dipole) and water-water (dispersion, dipole-dipole + H-bonding) so they are miscible
  • Octanal is a larger molecule than ethanal with more electrons so stronger dispersion forces
  • So the total octanal-water forces (dispersion, dipole-dipole + H-bonding) are not strong enough to overcome the total octanal-octanal (dispersion, dipole-dipole) and water-water (dispersion, dipole-dipole + H-bonding ) forces

chem (3 decks)

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