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Organic chemistry > Part 1 > Flashcards

Part 1 Flashcards

(60 cards)

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1
Q

Formal charge formula

A

FC = valence e- - bonding e-

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2
Q

Formal charge:

        | 1.     -  C  -
        |

        \+ 2.     -  C -
        |
A

0 and 1

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3
Q

Difference between isomers and resonance structure

A

Isomers - different arrangement of atoms and electrons

Resonance structure - differ in arrangement of electrons

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4
Q

The only accurate representation of resonance stabilized compounds, due to delocalized e- density

A

Resonance hybrid

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5
Q

Trend for bond length in periodic table

A

/

\/

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6
Q

Which is stronger?

Sigma bond or pi bond

A

Sigma

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7
Q

Label each as Ionic or covalent

A. NaI
B. BrCl
C. HCl
D. CH3NH2
E. NaOCH3
A 
A. Ionic
B. Covalent
C. Covalent
D. Covalent
E. Ionic
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8
Q

The ____ the pKa, the stronger the acid

A

Lower

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9
Q

Acidity in periodic table

A

—->
|
\/

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10
Q

Arrange in increasing bond length

C-H
O-H
N-H

A

BCA

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11
Q

Arrange in decreasing bond length

HF
HCL
HBR

A

HBR>HCL>HF

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12
Q

Steps in drawing Lewis structure

A
  1. Count valence e-
  2. Count e- if there are no bonds (octet)
  3. Count bonded e- (bond e- = 1/2(step 2 - step 1)
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13
Q

Lewis acid

A

e- pair acceptor

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14
Q

Lewis base

A

e- pair donor

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15
Q

Bronsted-Lowry base

A

Proton acceptor

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16
Q

The stronger the acid, the _____ the conjugate base

A

Weaker

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17
Q

In proton transfer reactions, equilibrium favors the _____ acid and _____ base

A

Weaker, weaker

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18
Q

Factors that determine acidity (4)

A
  1. Element effects
  2. Inductive effects
  3. Resonance effect
  4. Hybridization effects
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19
Q

In hybridization effect in acidy, the acidity of HA increases as the percent s character of A _____.

A

Increases

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20
Q

Arrange in increasing acidity

sp
sp2
sp3

A

sp3 sp2 sp

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21
Q

What is the conjugate acid of each base

  1. H20
  2. NH2
  3. HCO3
A
  1. H20 - H30
  2. NH2 - NH3
  3. HCO3 - H2CO3
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22
Q

Rank in order of increasing acidity

NH3, H2O, HF

A

NH3 H2O HF

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23
Q

Rank the ff in order of increasing acidity

HBr, HCl, HF

A

HF < HCl < HBr

Acidity increases down a column

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24
Q

Difference between lewis acid and bronsted-lowry acid

A

A lewis acid is an electron pair acceptor and usually contains a proton of an unfilled valence shell of electrons. A bronsted lowry acid is a proton donor and must contain a hydrogen atom.
(All BL acids are lewis acids, though the reverse may not be true)

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25
Classify each species as a lewis acid, bronsted-lowry or neither H3O+ Cl3C+ BCl3 BF4-
H3O+ both Cl3C+ lewis acid BCl3 lewis acid BF4- neither
26
Types of intermolecular forces of attraction (4)
1. Van der Waals (LDF) 2. Dipole-dipole 3. Hydrogen bonding 4. Ion-ion
27
Cause of dipole-dipole and give examples
It is due to the interaction of permanent dipoles Ex. (CH3)2C=O, H2O
28
This is due to the electrostatic interaction if an H atom in an OH, NH, HF bond with another N, O or F atoms
H-bonding
29
Give example of ion-ion IMFA
NaCl, LiF
30
Van der waals or LDF is due to
Due to the interaction of temporary dipoles Ex. All inorganic compounds
31
Arrange IMFA in increasingr strength
VDW-Dipole dipole-Hydrogen bonding-Ion Ion
32
Relation: Boiling Point and IMFA | 3
- Stronger the forces the higher the BP - for similar functional groups, the larger the area, higher BP - more polarizable atoms, the higher the BP
33
Relation: Melting point and IMFA
- for compounds comaparable in MW, the stronger the forces the higher the MP (same as BP) - with compounds with similar functional group, the more SYMMETRIC, the higher MP
34
Rank in increasing strength of IMFA A. CH3NH2 B. CH3CH3 C. CH3Cl
BCA
35
Rank the compounds in order of increasing strength of IMFA A. CH3Br B. CH3I C. CH3Cl
CAB
36
Rank the compounds in order of increasing strength of IMFA A. NaCl B. CH3OH C. CH3Cl
CBA
37
Rank in increasing boiling point A. CH3(CH2)4I B. CH3(CH2)5I C. CH3(CH2)6I
As is (high SA,high BP)
38
Rank the compounds in order of increasing melting point A. (CH3)2CHOH B. (CH3)3CH C. (CH3)2C=O
BCA
39
Rank the compounds in order of increasing melting point A. CH3F B. CH3Cl C. CH3I
ABC
40
Explain why benzene has a lower boiling point but much higher melting point than toluene
BP is solely determined by the strength of IMFA. Since bezene has a smaller size, it has less SA and weaker VDW interactions and therefore a lower boiling point than toluene. The increased MP for benzene can be explained by symmetry
41
Rank the compounds in order of increasing water solubility A. (CH3)3CH B. CH3OCH2CH3 C. CH3CH2CH2CH3 D. CH3CH2CH2OH
CABD (For A: this nonpolar, hydrophobic molecule is mole compact making it more H20 soluble than its straight chain isomer
42
Molecular formula for alkanes
CnH2n+2 *cycloalkanes CnH2n
43
Alkane conformations can be classified as ____, ____, ____ or ____ depending on the relative orientation of the groups on adjacent carbons
staggered, eclipsed, anti or gauche
44
Staggered dihedral angle
60 degrees
45
Two reperesentation of conformers
Sawhorse and newman
46
Two types of isomers and its definitions
Constitutional isomer - isomers that differ in the way the atoms are connected to each other Stereoisomer - isomers that differ only in the way atoms are oriented in space
47
of carbons gas, liquid, solid phase
Gas C1-C4 Liquids C5-C17 Solids >C18
48
Fuel for get engine
Kerosene (C9-C16)
49
Aka asphalt
Bitumen
50
Bromination - alkane
3* most stable
51
Two types of stereoisomers and its definition
Enantiomer - stereoisomer that are nonsuperimposable mirror images of each other Diastereoisomers - stereoisomer that are not mirror images of each other
52
Difference of chiral and achiral
Chiral- must have 4 different groups attached *chirality - with no plane of symmetry Achiral - plane of symmetry
53
Ability of a compound to rotate plane-polarized light
Optical activity
54
A mixture having equal mixture of two enantiomers
Racemic mixture
55
Meso compunds are
Achiral with plane of symmetry
56
Diastereoisomers are
not mirror images, chiral
57
Number of stereoisomer (formula)
2^(n)
58
Arrange from highest to least priority A. -F B. -OH C. NH2 D. CH3
ABCD
59
Arrange from highest to least priority A. -Cl B. -SH C. -OH D. -CH3
ABCD
60
State at room temp of covalent bond and ionic bond
Covalent bond - gaseous or liquid | Ionic bond - solid

Organic chemistry (4 decks)

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