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Organic Chemistry > Module 1: Introduction > Flashcards

Module 1: Introduction Flashcards

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1
Q

What century was organic chemistry?

A

18th Century

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2
Q

What was the assumption for organic chemistry?

A

It was assumed that compounds was only found in living organisms and cannot be sythesized in laboratories.

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3
Q

What was this concept called?

A

The Vital Force Theory

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4
Q

Who proposed this concept?

A

Jon Jacob Berzelius

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5
Q

When and who proved it incorrect?

A

In 1828 by Friedrich Wohler

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6
Q

What was the aqueous solution of two inorganic compounds?

A

Ammonium Chloride and Silver Cyanate= Urea-Compound of Urine

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7
Q

What is the study of hydrocarbons and their derivatives?

A

Organic Chemistry

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8
Q

What are the common additional elements found in hydrocarbon derivatives?

A

F P O N S Cl Br

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9
Q

What discipline is organic chemistry normally used?

A

Pharmaceuticals
Biochemistry
Material Science
Metallurgy

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10
Q

It is known for a seemingly unlimited number of compounds

A

Carbon

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11
Q

Chemical compounds are divided into two

A

Organic and Inorganic Compounds

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12
Q

What are examples of Organic Compounds?

A

DNA
Gasoline
Sugar
Alcohol

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13
Q

What are examples of Inorganic Compounds?

A

Salt
Quartz
Hydrochloric Acid
Water

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14
Q

What is stronger? Ionic or Covalent?

A

Ionic

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15
Q

Give some characteristics of organic compounds

A

Low melting point
Low Boiling Point
Low solubility in water
high solubility in non-polar solvents
flammable
aqueous solution does not conduct electricity
exhibit covalent bonding

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16
Q

Give some characteristics of inorganic compounds

A

High melting point
High Boiling Point
High solubility in water
Low solubility in non-polar solvents
non-flammable
aqueous solution conducts electricity
exhibit ionic bonding

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17
Q

Organic Compounds compromise how many percent?

A

90

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18
Q

What is catenation?

A

Self Linking of Ion

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19
Q

What is the tetravalency of carbon?

A

It needs 4 bonds

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20
Q

What is isomerism?

A

Same chemical formula but different chemical structures.

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21
Q

What are the kinds of isomerism?

A

Structural Isomerism
Stereoisomerism

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22
Q

What configuration is the opposite side?

A

E

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23
Q

What configuration is on the same side?

A

Z

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24
Q

Three types of bonds

A

Purely Covalent or Non Polar
Polar Covalent
Ionic

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25
The bonding electrons are shared equally between two bonding atoms.
Purely Covalent or Non Polar
26
The electrons are shared between atoms, but unequally, with the electrons spending more time around the morte electronegative form.
Polar Covalent
27
The electrons are not shared.
Ionic
28
Is a measure of the tendency of an atom to attract electrons.
Electronegativity
29
How would you know which has a greater electronegativity value?
From bottom to top
30
What is the highest electronegativity value element?
Fluorine 4.0
31
0-0.4
Nonpolar Covalent
32
0.5-1.4
Polar Covalent
33
1.5-2.0 (NM + NM)
Polar Covalent
34
1.5-2.0 (NM + M)
Ionic
35
2.0+
Ionic
36
Which is stronger? Intermolecular or Intramolecular?
Intramolecular (connection between two elements)
37
Strongest to weakest intermolecular forces
Ionic Interactions Hydrogen Bonding Dipole-dipole Interactions Dispersion Forces
38
Are interactions between charged atoms and molecules
Ionic Forces
39
Occurs in molecules containing the highly electronegative elements F, O, N directly bound to hydrogen
Hydrogen Bonding
40
Other groups besides hydrogen can be involved in polar covalent bonding with F O N.
Dipole-Dipole Interaction
41
Weakest Intermolecular forces
London forces
42
Ion-Ion Forces
Ionic Bond
43
Ion-Dipole Forces
Ionic and Polar
44
Hydrogen Bonding Forces
H + FON
45
Dipole-dipole Forces
Polar and not H
46
London Dispersion Forces
Non-Polar
47
Most common models used in representing molecules in organic chemistry?
Lewis Structure
48
What is usually the central element?
Thee least electronegativity
49
Total number of electrons shared in the molecule
S
50
Total number of valence electrons needed by all the atoms in the molecules to achieve noble gas configuration.
N
51
Number of electrons available in the valence shells of all atoms.
A
52
It is the charge assigned to an atom in a molecule
Formal Charge
53
Also known as mixture of orbitals
Hybridization of the Carbon Atom
54
The property of carbon that makes it unique is its ability to form bonds with itself
Catenation
55
What is stronger? Sigma bond or Pi bond?
Sigma Bond
56
C-H Single Bond, how many no. of sigma and pi bonds?
1 Sigma bond
57
C-C Double bond, how many no. of sigma and pi bonds?
1 Sigma bond and 1 Pi bond
58
C-C Triple bond, how many no. of sigma and pi bonds?
1 Sigma bond and 2 Pi bond
59
What hybridization is 2 steric number?
sp, linear, 180
60
What hybridization is 3 steric number?
sp2, trigonal planar, 120
61
What hybridization is 4 steric number?
sp3, tetrahedal, 109.5
62
Are specific groupings of atoms within molecules that have their own characteristic properties, regardless of the other atoms present in a molecule.
Funcitional Groups
63
What does R represent in molecular structures?
Rest of the molecule
64
A compound that contains only carbon atoms and hydrogen atoms.
Hydrocarbon
65
Hydrocarbons may be divided into two large classes.
Saturated and unsaturated hydrocarbon
66
Is a hydrocarbon in which all carbon-carbon bonds are single bonds.
Saturated Hydrocarbons
67
Is a hydrocarbon in which one or more carbon-carbon multiple bonds are present.
Unsaturated Hydrocarbons
68
Give three examples of saturated hydrocarbons.
Alkanes Cycloalkanes Haloalkanes
69
Give three examples of unsaturated hydrocarbons.
Alkenes Alkynes Aromatic
70
A saturated hydrocarbon in which the carbon atom arrangement is acyclic.
Alkanes
71
Is a saturated hydrocarbon in which carbon atoms are connected to one another in a cyclic (ring) arrangement.
Cycloalkanes
72
Also known as alkyl halides, are a group of chemical compounds comprised of an alkane with one or more hydrogens replaced by a halogen atom.
Haloalkanes
73
Are hydrocarbons that contain one or more double bonds between neighboring carbon atoms.
Alkenes
74
Are hydrocarbons that contain one or more triple bonds between neighboring carbon atoms.
Alkynes
75
Is a six-carbon ring with alternative double bonds.
Aromatic Hydrocarbons or Benzene
76
A functional group that involves an oxygen atom that is bonded to one hydrogen atom and one carbon atom.
Alcohol
77
A functional group consisting of an oxygen atom that forms single bonds with two carbon atoms.
Ethers
78
A functional group that contains a sulfur atom bonded to a hydrogen atom.
Thiols
79
A functional group that consists of a nitrogen atom bonded to some combination of carbons and hydrogens.
Amines
80
A carbon atom and an oxygen atom are connected by a double bond.
Carbonyl Group
81
Is a carbonyl in which carbon atoms is bonded to at least one hydrogen atom.
Aldehyde
82
Involves a carbonyl in which the carbon atom makes single bonds with two r-groups
Ketones
83
Are another carbonyl-containing functional group, in which the carbon atom is bonded to an OH group on one side and either a carbon or hydrogen atom on the other.
Carboxylic Acids
84
It contains a carbonyl where the carbon is bonded to one additional oxygen atom and one carbon or hydrogen atom.
Esters
85
A carbonyl in which the carbon is attached to one nitrogen atom and one carbon or hydrogen atom.
Amides
86
Sulfur replaces the oxygen and is connected to one atom and one r group.
Thioether
87
ACHAABAETAAKCEAT

Organic Chemistry (5 decks)

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