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intro to organic chem Flashcards

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1
Q

stem –> no. of carbon atoms (1-10)

A

1: meth-
2: eth-
3: prop-
4: but-
5: pent-
6: hex-
7: hept-
8: oct-
9: non-
10: dec-

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2
Q

Common prefixes ( alkyl, -NH2, -Br, -Cl, -CN, -F, -OH, -I, -NO2, -C6H5)

A

alkyl: methyl, ethyl, propyl, butyl, pentyl..

-NH2: amino

-Br: bromo

-Cl: chloro

-CN: cyano

-F: fluoro

-OH: hydroxy

-I: iodo

-NO2: nitro

-C6H5: phenyl

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2
Q

functional group from highest priority to lowest priority

A

carboxylic acids, esters, acid chlorides/acyl chlorides, amides, nitrile, aldehydes, ketones, phenols, alcohols, amines, arenes, alkyne, alkenes, alkanes

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3
Q

commas (,) in IUPAC

A

separate numbers

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4
Q

hyphens (-) in IUPAC

A

separate numbers and letters

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5
Q

effect on hybridisation on bond length and bond strength

A

e in s orbitals are closer to the nucleus compared to the p orbitals

bond length:
sp3 > sp2 > sp

bond strength:
sp3 < sp2 < sp

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6
Q

homologous series

A

-organic compounds with similar general formula
successive members:
1. are represented by a general formula

  1. differ by a constant -CH2- units in the carbon skeleton
  2. have diff phy properties cuz diff imf cuz diff e cloud size
  3. similar chem properties cuz same functional group
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6
Q

what is the organic series: free radical?

A

highly reactive, not influenced under a electric field atoms/grp of atoms with 1 unpaired electron

attack another atom in molecule to form another radical and another molecule

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7
Q

what is the organic series: nucleophile?

A

electron pair donor :Nu -

  • negatively charged ion
  • neutral molecules with a lone pair of electrons

attracted to electron-deficient sites (S+)

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8
Q

what is the organic series: electrophile?

A

electron pair acceptor E+

  • positively charged ion
  • atom with a partial positive charge (S+) in a polar bond

attracted to electron-rich sites

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9
Q

homolytic fission

A
  • shared pair of e are split equally between 2 atoms after the bond breaking process
  • forms free radicals
  • 2 half-arrows
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10
Q

heterolytic fission

A
  • shared pair of e are split unequally between 2 atoms after the bond breaking process
  • 1 cation & 1 anion
  • 1 full-arrow
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11
Q

types of reaction: addition

A

2 reactants -> 1 product

1 pi bond broken ->2 sigma bonds formed

opposite of elimination

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12
Q

types of reaction: substitution

A

replacement

1 sigma bond broken -> 1 sigma bond formed

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13
Q

types of reaction: elimination

A

remove atoms /grp of atoms from bigger molecule

2 sigma bonds broken -> 1 pi bond formed

opposite of addition

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14
Q

types of reaction: hydrolysis

A

reaction with water/H+/OH-

15
Q

types of reaction: condensation

A

2 molecules react to form a larger molecule with the elimination of a small or simple molecule like H2O or HCl

16
Q

constitutional (structural) isomerism

A

same molecular formula, diff structural formula

  1. chain (diff arrangement of C chain)
  2. positional (diff positions of a functional grp on C chain or ring
  3. functional group ( same molecular but diff functional groups)
17
Q

stereoisomerism

A

same molecular formula and structural formula, diff arrangement of atoms

  1. Cis-trans isomerism (pi bond must break to rotate)
    - restricted rotation of bond due to presence of pi bond
    - 2 diff atoms or grp of atoms attached to each C of the bond
    - 2^m (m=no. of C=C bonds)
  2. enantiomerism
    - non-superimposable mirror img (do not give the same structure when placed on top of each other)
    - no plane of symmetry (also no internal plane of symmetry!! when cutting molecule through the middle)
    - chiral centre (4 diff atoms/substituents, sp3 hybridized)
    -2^n (n=no. of C*)

-same physical(except in direction in which they rotate plane-polarised LIGHT) and

  • same chem(except differ in interaction with other chiral compounds)
  • diff bio (eg. Drug action - enzymes having active sites than can accept ONLY 1 of the 2 enantiomers!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!)
18
Q

meso compounds

A

mirror img + superimposable = achiral

optically inactive

got internal plane of symmetry

19
Q

Why cis-isomer has a lower mp, density, stability but higher bp, solubility and dipole moment?

A

CIS HAVE HIGH BP:
Both molecules have simple molecular structures. More energy is required to overcome the stronger pd-pd interactions between the polar cis- molecules than the weaker id-id interactions between non-polar trans- molecules

TRANS HAVE HIGH MP:
Both molecules have simple molecular structures. The trans- molecules have higher symmetry and can pack more closely in its lattice structure than cis- molecules. More energy is required to overcome the more extensive id-id interactions in trans- during melting

20
Q

describe sp3 hybridisation in CH4

A

-tetrahedral in shape
- bond angle 109.5
- all C-H bonds have equal bond lengths -> identical sigma bonds formed

  • x1 2s orbital + x3 2p orbitals = 4 degenrate 2sp3 hybrid orbitals (tetrahedral,109.5)
  • each of the x4 2sp3 hybrid orbitals of C atom overlaps head-on with the 1s orbital of H atom
21
Q

describle sp2 hybridisation in C2H4

A

-trigonal planar in shape
- bond angle 120
- all C-H bonds have equal bond lengths -> identical sigma bonds formed

  • x1 2s orbital + x2 2p orbitals = 3 degenrate 2sp2 hybrid orbitals (trigonal planar,120)
  • unhybridised p orbital is perpendicular to the plane of the x3 2sp2 hybrid orbitals
  • has a C=C bond which consists of 1 sigma bond + 1 pi bond. Each C atom uses one 2sp2 hybrid orbital to overlap head-on to form the sigma bond. The unhybridized p orbital of each C atom overlaps side-on to form pi bond. Each C atom’s 2 remaining 2sp2 hybrid orbitals overlap head-on with the 1s orbital of H atom to form C-H sigma bonds.
  • 4 C-H bonds formed
22
Q

describe sp hybridisation in C2H2

A
  • linear in shape
  • bond angle 180
  • all C-H bonds have equal bond lengths -> identical sigma bonds formed
  • x1 2s orbital + x1 2p orbitals = 2 degenrate 2sp hybrid orbitals (linear, 180)
  • unhybridised 2pz and 2py orbital is perpendicular to the plane of the x2 2sp hybrid orbitals
  • has a C=C bond which consists of 1 sigma bond + 2 pi bond. Each C atom uses one 2sp hybrid orbital to overlap head-on to form the sigma bond. The unhybridized 2pz and 2py orbital of each C atom overlap side-on to form 2 pi bond. Each C atom’s 1 remaining 2sp hybrid orbitals overlap head-on with the 1s orbital of H atom to form C-H sigma bonds.
  • 2 C-H bonds formed

chem (20 decks)

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