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Chem - Gr11 > Organic Chem > Flashcards

Organic Chem Flashcards

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1
Q

Explain s character and bond length relation

A
  1. sp orbital = more s character = closer to nucleus = shorter and stronger bonds
  2. sp3 orbital = least s character = further from nucleus = longer and weaker bonds
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2
Q

3D representation of organic molecules

A
  • Bonds in paper
  • Dashed wedge - bonds away from observer
  • Solid wedge - bond towards observer
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2
Q

Explain s character and electronegativity

A

Greater the s character = greater the electronegativity

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3
Q

Why are such electrons being easily available to attacking reagents

A
  • In pi bond, parallel orientation of two p orbitals on adjacent atoms is necessary for sideways overlap
  • Electron cloud of pi bond is located above and below the plane of bonding atoms
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4
Q

Alicyclic compounds

A

Carbon atoms joined in a ring (Cyclopropane, cyclohexane)

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4
Q

Aliphatic compounds

A

Straight or branched chain compounds (CH3 - CH3)

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5
Q

Suffix of:
1. aldehydes
2. Ketones
3. nitriles
4. Caboxylate ions
5. Esters
6. Acyl Halides
7. Amines
8. Amides

A
  1. -al
  2. -one
  3. nitrile
  4. oate
  5. -oate
  6. -oyl halide
  7. amine
  8. amide
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6
Q

Common name of:
1. Methylbenzene
2. Methoxybenzene
3. Aminobenzene

A
  1. Toulene
  2. Anisole
  3. Aniline
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7
Q

Structural Isomer + Example

A

Isomers having same molecular formula but different structures
Eg:
chain (CH3CH2CH2CH3 and CH3 - CH2 - CH3
|
CH3)
Position (CH3 - CH2 - CH2 - OH and CH3 - CH - CH3
|
OH)

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8
Q

Stereoisomers

A

Isomers that have same constition and sequence of covalent bonds but differ in relative positions of their atoms - cis and trans

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8
Q

Functional Isomer Example

A

Refers to the type of isomer where same moleculr formula but different functional groups - aldehyds and ketones for example

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9
Q

Explain carbocations

A
  • Bond broken in a manner to form a carbon atom with a positive charge
  • Tertiary > Secondary > Primary
  • Trigonal planar shape - sp2 hybridized
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10
Q

Metamerism

A

Refers to the different alkyl chains on either side of the functional group in the molecule
C4H10O –> CH3OC3H7 and C2H5OC2H5

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11
Q

Carbanion

A
  • Negative charge on carbon atom
  • sp3 hybridized having distorted tetrahedron
  • Primary > Secondary > Tertiary
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12
Q

Free radicals

A
  • Formed by homolytic cleavage
  • tertiary > secondary > primary
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13
Q

Substrate

A

A substrate refers to a molecule or compound that undergoes a chemical reaction, whether catalyzed by an enzyme, a catalyst, or an inhibito

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14
Q

Reagent

A

In chemistry, a reagent is a substance or compound added to a system to cause a chemical reaction or test if a reaction occurs.

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15
Q

How can electron pairs shift

A
  • From pi bond to adjacent bond position
  • From pi bond to adjacent atom
  • From atom to adjacent bond position
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16
Q

Inductive Effect

A
  • Polarization of sigma bond caused by the polarization of adjacent sigma bond
  • Permanent effect
  • More the inductive effect = More the polarity
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17
Q

Explain how inductive effect works

A
  • Polarization in a way that carbon - 1 gains positive charge (since the electronegative atom pulls the electrons towards itself)
  • Then carbon 2 also experiences such a pull but lesser
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18
Q

Electron withdrawing vs Electron donating groups

A

Electron withdrawing: Halogens, NO2, -CN , -COOH, COOR
Electron donating:
-CH3, -CH2 - CH3, etc.

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19
Q

Resonance structure

A
  • Refers to the structure as the bonds contain an intermediate value of energy and are of different bond lengths
  • In between single and double bond length
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20
Q

Resonance stabilization energy

A

Difference between the actual structure and the lowest energy resonance structure

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21
Q

+ and - Resonance

A

+ –> Transfer of electrons from an atom attached to the conjugated system
- –> Refers to the transfer of electrons towards the atom or substiuent group

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22
Q

Electomeric

A
  • Temporary
  • Complete transfer of a shared pair of pi electrons to one of the atoms joined by a multiple bond on the demand of an attacking reagent
  • Annulled as soon as the attacking reagent is removed
23
Q

Which is stronger electomeric or inductive effect?

A

Electomeric effect predominates

24
Q

Positive vs Negative Electomeric

A
25
Q

Hyperconjugation

A
  • Delocalization of sigma electrons of C-H bond of an alkyl group directly attached to an atom of unsaturated system or to an atom with an unshared p orbital
  • Permanent effect
26
Q

Draw hyperconjugation of propene and ethene

A

-

27
Q

Sublimation

A

On heating, solids changing to gaseous state directly

28
Q

Crystallization

A
  1. Impure compound dissolved in a solvent where it is sparingly solublr
  2. Heated and concentrated to get a nearly saturated solution
  3. Impurities removed by adsorbing over active charcoal
29
Q

Normal distillation

A
  • Sufficient different in boiling points, hence are heated
  • Vapours of lower boiling component are formed first
  • Aniline and Chloroform
30
Q

Fractional distillation

A
  • Vapours of a liquid mixture are passed through a fractionating column before condensation
  • Higher BP condense before as they reach up first and are more volatile
  • Application: crude oil in petroleum
31
Q

Distillation under reduced pressure

A
  • Purify liquids having very high BP and decompose below BP
  • They are made to boil at a temp lower than normal
  • Eg: glycerol separated from spent-lye
32
Q

Steam distillation

A
  • Separate substances which are steam volatile and immiscible with water
  • Mixture of steam and volatile organic compound is condensed and collected
  • Atmospheric pressure = vapour pressure + water pressure
  • Eg: aniline-water
33
Q

Why does steam distillation have organic liquid vapourizing at a lower temp than BP

A

Atmospheric pressure = pressure due to organic liquid and due to water (hence since p1 lower than p, it will vaporize at a lower point)

34
Q

Give examples of all distillations

A
  • Normal: Chloroform and aniline
  • Fractional: Crude oil from petroleum
  • Distillation under reduced pressure: Glycerol from spent-lye in soap industry
  • Steam distillation: Aniline and water
35
Q

Adsorption chromatography

A

Different compounds are adsorbed on an adsorbent to different degrees

36
Q

Commonly used adsorbents

A

Silica gel and alumina

37
Q

Column Chromatography

A
  • Separation of a mixture over a column of adsorbent
  • Mixture adsorbed is on top of the column
  • Most readily adsorbed substances are retained near the top
38
Q

Thin Layer chromatography

A
  • Separation over a thin layer of an adsorbent coated on glass plate
  • Silica gel or alumina is spread over a glass plate
39
Q

Partition chromatography

A
  • Based on continuous differential partitioning of components of a mixture between stationary and mobile phases
  • Solvent acts as mobile phase
39
Q

Test for Nitrogen

A
  • Na + C + N –> NaCN
  • Sodium fusion extract boiled with FeSO4 and acidified with conc. H2SO4
  • Prussian blue colour confirms presence of nitrogen
40
Q

R value

A

Retardation factor = Dist. moved by substance from base line / Distance moved by solvent from base line

41
Q

Detection of carbon and hydrogen

A

C + CuO –> Cu + CO2
H + CuO –> Cu + H2O
CO2 + Ca(OH)2 –> CaCO3 + H2O
H2O + CuSO4 –> CuSO4.5H2O

42
Q

Lassaigne’s test

A
  • Nitrogen, sulphur, halogens and phosphorus present in an organic compound are detected by Lassaigne’s test
  • Elements present are converted from covalent form into ionic form by fusing compound with sodium metal
43
Q

Test for sulphur

A

Na + S –> Na2S
* Sodium fusion extract is acidified with acetic acid and lead acetate added (Black ppt)
* Sodium fusion extract with sodium nitroprusside forms a violet colour

44
Q

What happens when nitrogen and sulpur are both present

A

Na + C + N + S –> NaSCN
Sodium thiocynate is formed and gives blood red colour and no prussian blue

45
Q

What happens when sodium fusion is carried out with excess of sodium

A

Thiocynate decomposes to yield cyanide and sulphide

46
Q

Test for halogens

A
  • Sodium fusion extract is acidified with nitric acid and treated with silver nitrate
    white ppt soluble in NH4OH = chlorine
    yellow ppt sparingly sol. in NH4OH = bromine
    yellow ppt, insoluble in NH4OH = iodine
47
Q

What happens for the halogen test when nitrogen or sulphur is present

A
  • Sodium fusion extract is first boiled with conc. HNO3 to decompose cyanide or sulphide of sodium
48
Q

Phosphorus test

A
  • Compound heated with an oxidising agent (sodium peroxide)
  • Solution boiled with HNO3 and treated with ammonium molybdate
  • yellow ppt = phosphorus
49
Q

Carbon and Hydrogen percentage

A

Percent C = (12 m * 100) / 44w
Percent H = (2m * 100)/18w

50
Q

Dumas method

A

28 * (P1V1 * 273/ 760 * T) * 100 / 22400 w

51
Q

Kjeldahl Method

A

(1.4/w * (2MV1 - MV2)
MV1 –> Molarity H2SO4, volume
MV2 –> Molarity of NaOH

52
Q

When is kjeldahl’s method not applicable

A

Compounds containing nitrogen in nitro and azo groups and nitrogen present in the ring as nitrogen does not change to ammonium sulphate under these conditions

53
Q

Carius method for halogen

A

atomic mass of X * m1 * 100 / molecular mass of AgX * m

54
Q

Sulphur estimation

A

32 * m * 100 / 233 * w

55
Q

Phosphorus estimations

A

62m * 100 / 222

56
Q

Percentage oxygen estimation

A

32m * 100 / 88 w

57
Q

Does double bond or triple bond get higher preference in naming

A

Double bond gets a higher preference

58
Q
A

Chem - Gr11 (8 decks)

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