Module 1.3: Organic Chemistry Flashcards
1
Q
What causes denatured alcohol to be unfit for use in intoxicating beverages?
A
Methanol
Example sentence: This causes the Denatured alcohol unfit for use in intoxicating beverage.
2
Q
It exhibits ability to bond successfully to other carbon atoms to form chains and rings of varying sizes
A
Catenation
3
Q
It exhibits mixing of two or more non equivalent atomic orbitals to form new set of equivalent orbital
A
Hybridization
4
Q
What are the importance of carbon
A
Si carbon maabilidad ang form, flexible pa ang backbone
-Ability to form bonds with other elements including itself
-Gives flexibility to the farm and function of biomolecules can take
-it is the backbone of life on earth
5
Q
What are the importance of organic chemistry
A
For synthesizing medicinal agents
Foundational to biotechnology and bio chemistry
Food technology
For better molecule which can be twist the structure
Survivables like diamonds petroleum
6
Q
Mnemonics: Si carbon maabilidad ang form, flexible pa ang backbone
A
Importance of carbon
- Ability to form bonds with other elements including itself
-Gives flexibility to the farm and function of biomolecules can take
-it is the backbone of life on earth
7
Q
Two types of organic compounds
A
Hydrocarbon and hydrocarbon derivatives
8
Q
What are the components of hydrocarbon
A
Aliphatic automatically cyclic and cationic
9
Q
What are the components of hydrocarbon
A
Aliphatic automatically cyclic and cationic
HNOS
Hydrogen containing
Nitrogen containing
Oxygen containing
Sulfur containing
10
Q
All bonds , etters including single bonds
A
Expanded or kekule
11
Q
All letters are drawn except single bonds but double bonds and triple bonds are shown
A
Condensed formula
12
Q
The whole chemical formula is drawn using points and lines but other atom as substituent are still drawn as
A
Skeletal formula
13
Q
What are the types of structural formulas
A
Expanded/ Kekule
Condensed formula
Skeletal formula
14
Q
What are the types of structural formulas
A
Expanded/ Kekule
Condensed formula
Skeletal formula
15
Q
What are the three types of naming organic nomenclature
A
Systemic or iupac or international union of pure and applied chemist ry
Trivial
Semi systemic
16
Q
What are the three types of naming organic nomenclature
A
Systemic or iupac or international union of pure and applied chemist ry
Trivial
Semi systemic
17
Q
Based on naming rules____
Nickname based on tradition or familiarization of people ___
Combine trivial and systematic__
A
Systematic or iupac
Trivial
Semi- systematic
18
Q
Give example each
Systematic or iupac
Trivial
Say my systematic
A
Ethanoic acid
Vinegar
Acetic acid
19
Q
Does not form a either linear or branch
A
Open chain
20
Q
Does not form a either linear or branch
A
Open chain
21
Q
Forms a ring
A
Cyclic
22
Q
Forms a ring
A
Cyclic
23
Q
Contains only single bond
A
Saturated
24
Q
Has one or more double or triple bond
A
Unsaturated
25
Substituent inside an open chain
Internal
26
Substituent inside an open chain
Internal
27
Subsituent at the end of the open chain
Terminal
28
Carbon directly attached to the functional group
Alpha carbon
29
Carbon holding a double bond
Vinylic or olefenic
30
Alkyl group with a carbonyl group
Acyl group
31
Describe rings
Based on the number of ring members
Based on the number of rings
32
Example of based on the number of members
Homocyclic- all ring members are the same
Heterocyclic-ring members are not the same
33
Example of based on the number of rings
Bicyclic
Tricyclic
34
Differentiating sigma and pi bond
Sigma
-First bond formed
- headways overlapse or collision
-stronger
S/sp orbitals
Pi bond
-bond formed after sigma
-sideways overlap or collision
- weaker
-P orbitals only
35
Electron configuration how much does s, p, d holds
S- 2
P- 6
D- 10
36
What are the requirements for binding
-It needs 2 electron
-Each atom must have an unpaired orbitals
37
Sp3 hybridization
Angle:
Tetrahedral 109.5degrees
38
S+ p+p+p
Sp3 hybridization
39
How can you seperate a SP2 hybridization among others
Presence of the double bond
40
Two hybridized and to unhybridized
Sp hybridization
41
S+p
Sp hybridization
42
4 hybridized 4 unhybridized
Sp3 hybridization
43
Three hybridized one and hybridized
Sp2 hybridization
44
Bond angle of a sp2 hybridization
120°
45
Sp hybridization bond angle
180°
46
Geometrical shape of sp2
Trigonal or planar
47
Geometric shape of sp hybridization
Linear
48
How can you determine the hybridization of sp3 sp2 and sp
Sp3 single bond
Sp2 double bond
Sp triple bond
49
What are the intermolecular forces
Van der waals
Ion dipole
Ion induced dipole
Hydrogen bonds
50
It is the weakest intermolecular forces
Van der waals
S- Keesom
Debye
W- London
51
Polar molecules attracted to either positive or negative charges
Ion dipole
52
The forces of attraction included by adults of proximity of a charged ion into a nonpolar molecule
Ion induced dipole
53
Attraction of hydrogen for a strongly electronegative ion
Hydrogen bonds
54
Which is stronger intramolecular or intermolecular
Intramolecular
55
Intramolecular composition based on strongest
1. Ionic
2. Covalent
56
57
KODD
Keesom
Orientation effect
Dipole -
Dipole
58
DIP DID
Debye
Induction effect
Polarization
Dipole
Induced dipole
59
L DIDID
London
Dispersion
Induced dipole
Induced dipole
60
Dipole means
Polar
61
Factors affecting intermolecular forces
Type of intermolecular forces (strength)
Number of carbons
branching
62
BaTaNa si IMF
Factors affecting intermolecular forces
Type of intermolecular forces (strength)
Number of carbons
branching
63
What is the effect of water solubility on the number of carbons
Increase in the number of carbon
= increase Tb= Increase Tm= Increase IMF=Decreases the effect of water solubility
64
What is the effect of water solubility on the branching of compounds
Inc branching= dec IMF = dec Tm and Tb=inc water solubility
65
More branching inc ___
Space for water does more polar and water soluble
66
Which is more soluble carbonyl group or alcohol group
Alcohol group because of the presence of hydrogen
67
VSEPR
Valence shell electron
pair
repulsion
68
What are the types of strain
Ring/ angle
Torsional
Stearic effect
69
Testing of angles due to rain closures
Ring or angle
70
Closing of angles between parallel bonds
torsional
71
Competition for space due to bulky groups; pushing bonds away from expected angle
Stearic effect
72
What happens to stability when the strain increases
Decreases stability
73
Torsional is either staggered or eclipse which of the two is more stable
Staggered
74
It describes the polarity produced in a molecule because of the interaction between a pie bond and a lone pair.
Resonance
75
What is the goal of resonance
To make the structure more stable
76
Re pir, lonely
Resonance interaction between pi bond and lone pair
77
Alternating single and double bonds
Conjugated substance
78
Electron pulls due to the difference in electronegativity
Inductive effects
79
___ alkyl group amide possesses lone pair
Electron donating group
80
Electron donating group___ stability
Increases
81
Electron donating group makes the structure more__
Basic
82
Electronegative atoms like halogens and oxygen
Electron withdrawing group
83
Electron withdrawing group ___ stability
Decreases
84
Electron withdrawing group Makes the structure more
Acidic
85
Cooh groups in inductive effects
Resonance
86
Resonance ___ stability
Increases, can let go of protons better
87
Resonance makes the structure more
Acidic
88
What happens to the stability when the number of carbon increases
Increase in number of carbon also increases the stability
89
What are the aliphatic hydrocarbons
Alkane
alkane
alkyne
90
Other term for alkane alkene alkyne
Alkane -paraffin
alkane -olefin
alkyne- acetylene
91
General chemical formula for alkane
CnH2n + 2
92
General chemical formula for alkene
CnH2n
93
General chemical formula of alkyne
CnHn
94
It is also known as alicyclic
Carbocyclic
95
Change that form a ring that behaves like aliphatic
Carbocyclic/
Alicyclic
96
Requirements to be considered as aromatic hydrocarbon
cyclic or planar
Conjugation
Follows the huckles rule 4n+2= pi electron
97
Huckles rule
4n+2= pi electron, where n should be a whole number
98
Classification of alcohols
Based on the number of r bonded to carbon bearing -OH
Based on the number of OH groups
99
What are their types
Based on the number of r bonded to carbon bearing -OH
Based on the number of OH groups
Based on the number of r bonded to carbon bearing -OH
. Primary
. Secondary
. Tertiary
Based on the number of OH groups
.R-Monohydric
. Dihydric
. Polyhydric
100
R- OH
Alcohol
101
Nag zinc in Cla Lucas, nag Hi Cla miscerable kan?
Lucas test
Reagent: zinc chloride
Reactant: hydrochloride
Positive results:
Two immiscible layers 3> 2
1 no reaction
102
OC MR ParaHBen
Ortho catechol
Meta- Resorcinol
Para- hydroquinone and benzoquinone
103
R-OH
Alcohol
104
R-OR
Ether
105
Ether is classified into
Open chain
Cyclic
106
Types of Open chain in ether
Symmetrical
Mixed
107
Cyclic in ether : types are
Epoxide/ Oxacyclopropane/ Oxirane
More than 3 members included in the ring system
108
Gemfibrosil use
Lowers TG
109
R- NH2
Amine
110
Organic compounds derived fim ammonia
Amine
111
It is the most basic amine
Secondary amine
112
Test for amine
Hinsberg test
113
Hindi 2 aamine
Hinsberg test for amine. 2ary amine is the most basic
114
What are the catecholamine?
Norepinephrine
Epinephrine
Dopamine
114
Hindi 2 aamine kay BSC
Hinsberg test for amine. 2ary amine is the most basic.
Reagent: benzenesulfonyl Chloride
115
C= O
Carbonyl group
116
R= OH
Aldehyde
117
Aldehyde is oxidized to form __
Reduced to form__
Carboxylic acid
Primary alcohol
118
Identification test of aldehyde
Jone's oxidation test
Tollen's test
Fehling's test
Brady's test
119
Alden, Feeling body Builder Joke To
Aldehyde tests
Fehling's test
Brady's test
Jone's oxidation test
Tollen's test
120
Also known as knock out drops
Chloral hydrate
121
Keton is reduced to form __
2ary alcohol
122
na Ketong Idin uncle Boy
Ketone Tests
Brady's test
Iodoform Test
123
124
Simplest ketone
Propan - 2 - one or 2 propanone
125
Aldehyde: tollen's test
reagent and
positive result
Ammoniacal Siver nitrate
Gray
126
Aldehyde: Fehling's test reagent and positive result
Cupric sulfate and
Sodium Potassium tartrate/. Sodium tartrate
Red
127
Aldehyde and ketone:
Brady's
test reagent and positive result
2,4- dinitrophenylhydrazine
Red
128
Methyl ketoses ONLY: Iodoform test reagent and positive result
Alkaline Iodine Solution
Yellow
129
C=OOH
Carboxyl groups
130
Kinds of Acids
Monicarboxylic acids
Dicarboxylic acids
131
Saturated FA, one Carboxylic acid
Monicarboxylic
132
Saturated FA, two Carboxylic acid
Dicarboxylic acid
133
Oh My Such Good Apple Pie, Sweet as Sugar
Example of Dicarboxylic
134
Oh My Such Good Apple Pie, Sweet as Sugar meaning
Oxalic acid-2 carbon, 2 COOH
Malonic acid-3
Succinic acid4
Glutaric acid5
Adipic acid6
Pinelic acid 7
Suberic acid8
Azelaic acid9
Sebabic acid10
135
Aldehyde: Jone's oxidation test reagent and positive result
Chromic acid in sulfuric acid
Green
136
Monocarboxylic: prefix
12C-
14C
16C
18C
20C
Lauric
Mystic
Palmitic
Stearic
Arachidic
137
LaMig Pa Sa Australia
Monocarboxylic: prefix
Lauric
Mystic
Palmitic
Stearic
Arachidic
138
RC=OOC=OR
Anhydride
139
RC=OOR
Ether
140
RC=OX
Acyl halide/ ex. Alkanoyl halide
141
RC=ONH2
Alkanamide/ amide
142
C triple bond N
Nitrile
143
Compounds with identical chemical formula but different in properties and arrangement of atoms in the molecule
Isomers
144
Types of Isomers
Constitutional isomers and stereoisomers
145
What are the three types of constitutional isomers
Skeletal
Positional
Functional
146
What are the two types of stereoisomers
Configurational isomers
Confirmational isomers
147
Two types of configurational isomer
Optical and geometry
148
Two types of optical isomer
Enantiomer and diastereomers
149
Types of geometric isomers
Cis or trans
Z/E
150
What are the unique difference of stereoisomers and constitutional isomers
*stereoisomers- with connectivit
*constitutional isomers- without connectivity
151
DIFFERENT IN DEGREE OF BRANCHING OR PARENT CHAIN LENGTH
Skeletal or structural isomers
152
Different placement or local of the functional group
Positional isomer
153
Different in functional group itself
Functional isomer
154
Mirror image
Enantiomer
155
the rotation of the chiral compound is opposite of the other
Enantiomer
156
Example of enantiomer
D and L glyceraldehyde
D and L alanine
157
What are the requirements for a carbon to be chiral
4 substituent
The four substitution must be different from each other
158
A substituent with a higher atomic number will receive greater priority than a substituent with a lower atomic number
Cahn- Ingold- Prelog rule
159
Counterclockwise and clockwise configuration
R configuration- clockwise
S-configuration- counterclockwise
160
Not mirror image
Diastereomers
161
Not all chiral carbons rotate in opposite direction compounds with more than one chiral carbon
Diastereomers
162
Compounds having two adjacent carbons with subsequents which happens when there is a double bond or when the compound is cyclic
Geometric isomers
163
Cis Trans
Cis- same side
Trans- opposite side
164
Cis
*Polarity
* Solubility
* Boiling point
* Melting point
*Polarity increases
* Solubility increases
* Boiling
point increases
* Melting point decreases
165
Trans
*Polarity
* Solubility
* Boiling point
* Melting point
*Polarity decreases
* Solubility decreases
* Boiling point decreases
* Melting point increases
166
Which of which more stable and more steering effect cis or trans
Cis- stearic effect
Trans- more stability
167
Z and E means
Zusamen - same side
Entgen- opposite side
168
Stereo are summers of the same compound with temporary differences in bond rotation
Confirmational isomers
169
What is the most stable form of cyclohexane
Chair confiormation
170
Neutrophile versus electrophiles
Neutrophile
Nu-
Electron reach
Proton loving
Nucleus loving
(- )charged
Ex: alkyl, nitrogen, sulfur
Electrophiles
E+
Electron poor
Positively charged
Electron loving
Ex: X, O, H
171
Free radical substitution of alkanes
Initiation
propagation
termination
172
Free I Pan Ta
Free radical substitution of alkanes
Initiation
propagation
termination
173
What sign you can see if there is complete combustion and incomplete combustion
Incomplete combustion is the presence of CO
Complete combustion- CO2
174
Most of the time in complete combustion is
Alkane
175
Markovnicov's rule
Major product: More stable
176
What is the product of hydration in electrophilic addition of alkenes
Alcohol
177
Metabolism process in electrophilic addition of alkenes
Hydrogenation
Halogenation
Hydrohalogenation
Markovnicov's rule
Hydration
178
For hydrogenation of alkynes a ___ is required to limit it to an alkene while __ alkane
Alkene - lindlar catalyst
Alkyne- palladium
179
Metabolism process in electrophilic addition of alkynes
Hydrogenation
Hydration
180
It is also known as ketone formation
Keto-enol tautomerization
181
If it is electrophilic substitution there is always a
Leaving group
182
What is the product of halogenation in electrophilic substitution of aromatic compounds
Halogenated benzene or halobenzene
183
What is the product of nitration in electrophilic substitution of aromatic compounds
Nitrated benzene or nitrobenzene
184
What is the product of Friedel-Craft Alkylation in electrophilic substitution of compounds
if CH3Cl is added
Alkylated benzene/ Alkyl benzene
185
What is the product of Friedel-Craft Alkylation in electrophilic substitution of compounds
if CH3C=OCl is added
Ketone
186
What is the product of Sulfonation in electrophilic substitution of
Benzene Sulfonic a.
187
Product of Nucleophilic ( alkoxide )substitution of alkyl halides
Ether
188
Product of Nucleophilic ( alcohol )substitution of alkyl halides
Alcohol
189
190
191
192
193
194
195
product of Hydration of alkene
Alcohol
196
Product of Dehydration of alcohol
Alkene
197
Aldehyde+ primary amine =
Imine
198
Ketone + secondary amine =
Enamine
199
Oxidation process of alkane
Alkane --> alcohol --> carbonyl --> Carboboxylic acid
200
Reduction process of Carboxylic
Alkane <-- alcohol <--carbonyl <-- Carboboxylic acid
201
Difference between oxidation and reduction in terms of
Oxygen
Hydrogen
Bonds
Oxidation
Oxygen+
Hydrogen -
Bonds increases
Reduction
Oxygen -
Hydrogen +
Bonds decreases
202
Mild oxidizing agent
PCC or pyridinium chlorochromate
Periodinane
203
Strong oxidizing agent
Chromic acid H2CrO4
Potassium permanganate KMnO4
204
Strong reducing agent
Lithium aluminum Hydride
205
Mild reducing agent
Sodium borohydride NaBH4
206
Reactivity and the symbol of alkane
Free radical substitution
SR
207
Reactivity and the symbol of alkenes and alkynes
Electrophilic addition
AE
208
Reactivity and the symbol of aromatics
Electrophilic substitution
SE
209
Reactivity and the symbol of alcohols and alkyl halide
Nucleophilic substitution
SN
210
Reactivity and the symbol of carbonyl compounds
Nucleophilic addition
AN
211
Reactivity and the symbol of carboxylic acid and its derivatives
Necrophilic acid substitution
SN acyl
212
Reactivity and the symbol of oxygen containing compounds
Redox loop
213
Bro si Bae alkene lang
Bromine and Baeyer is test for alkenes
214
Brominne test for alkene
Reagent;
Results
Carbon tetrachloride CCl4
Disappearance of orange
215
Baeyer
test for
alkene
Reagent;
Results
Potassium permanganate
Disappearance of violet + brown precipitate
216
Xanthoproteic test for aromatics
Reagent;
Results
Nitric acid
Yellow
216
What is the flame color of bellstein test for halogenated compounds
Green
217
Nitrogen containing compounds test
Test
Reagent
Results
Test: hinsberg test
Reagent: benzenesulfonyl Chloride
Results:
Primary amine- clear solution
Secondary amine- white precipitate
Tertiary amine- no reaction
218
Ferric chloride is a test for
Reagent Result
Phenols
FeCl3/ ferric chloride
Blue or purple
219
Jones oxidation is a test for
Reagent Result
All
Chromic acid in sulfuric acid or jones reagent
Green
220
Tollen's is a test for
Reagent Result
All
Ammonium silver nitrate
Silver mirror
221
Fehling's is a test for
Reagent Result
All
Fehling's A: cupric sulfate
Fehling's B: sodium potassium tartrate
Red precipitate
222
Brady's is a test for
Reagent
Result
Carbonyl compounds
2 4 dinitrophenylhydrazine
Red precipitate
223
Iodoform is a test for
Reagent
Result
Methylketone
Alkaline iodine solution
Pale yellow precipitate
