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Organic Chemistry > Module 1: Introduction > Flashcards

Module 1: Introduction Flashcards

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
Q

The bonding electrons are shared equally between two bonding atoms.

A

Purely Covalent or Non Polar

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26
Q

The electrons are shared between atoms, but unequally, with the electrons spending more time around the morte electronegative form.

A

Polar Covalent

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27
Q

The electrons are not shared.

A

Ionic

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28
Q

Is a measure of the tendency of an atom to attract electrons.

A

Electronegativity

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29
Q

How would you know which has a greater electronegativity value?

A

From bottom to top

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30
Q

What is the highest electronegativity value element?

A

Fluorine 4.0

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31
Q

0-0.4

A

Nonpolar Covalent

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32
Q

0.5-1.4

A

Polar Covalent

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33
Q

1.5-2.0 (NM + NM)

A

Polar Covalent

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34
Q

1.5-2.0 (NM + M)

A

Ionic

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35
Q

2.0+

A

Ionic

36
Q

Which is stronger? Intermolecular or Intramolecular?

A

Intramolecular (connection between two elements)

37
Q

Strongest to weakest intermolecular forces

A

Ionic Interactions
Hydrogen Bonding
Dipole-dipole Interactions
Dispersion Forces

38
Q

Are interactions between charged atoms and molecules

A

Ionic Forces

39
Q

Occurs in molecules containing the highly electronegative elements F, O, N directly bound to hydrogen

A

Hydrogen Bonding

40
Q

Other groups besides hydrogen can be involved in polar covalent bonding with F O N.

A

Dipole-Dipole Interaction

41
Q

Weakest Intermolecular forces

A

London forces

42
Q

Ion-Ion Forces

A

Ionic Bond

43
Q

Ion-Dipole Forces

A

Ionic and Polar

44
Q

Hydrogen Bonding Forces

A

H + FON

45
Q

Dipole-dipole Forces

A

Polar and not H

46
Q

London Dispersion Forces

A

Non-Polar

47
Q

Most common models used in representing molecules in organic chemistry?

A

Lewis Structure

48
Q

What is usually the central element?

A

Thee least electronegativity

49
Q

Total number of electrons shared in the molecule

A

S

50
Q

Total number of valence electrons needed by all the atoms in the molecules to achieve noble gas configuration.

A

N

51
Q

Number of electrons available in the valence shells of all atoms.

A

A

52
Q

It is the charge assigned to an atom in a molecule

A

Formal Charge

53
Q

Also known as mixture of orbitals

A

Hybridization of the Carbon Atom

54
Q

The property of carbon that makes it unique is its ability to form bonds with itself

A

Catenation

55
Q

What is stronger? Sigma bond or Pi bond?

A

Sigma Bond

56
Q

C-H Single Bond, how many no. of sigma and pi bonds?

A

1 Sigma bond

57
Q

C-C Double bond, how many no. of sigma and pi bonds?

A

1 Sigma bond and 1 Pi bond

58
Q

C-C Triple bond, how many no. of sigma and pi bonds?

A

1 Sigma bond and 2 Pi bond

59
Q

What hybridization is 2 steric number?

A

sp, linear, 180

60
Q

What hybridization is 3 steric number?

A

sp2, trigonal planar, 120

61
Q

What hybridization is 4 steric number?

A

sp3, tetrahedal, 109.5

62
Q

Are specific groupings of atoms within molecules that have their own characteristic properties, regardless of the other atoms present in a molecule.

A

Funcitional Groups

63
Q

What does R represent in molecular structures?

A

Rest of the molecule

64
Q

A compound that contains only carbon atoms and hydrogen atoms.

A

Hydrocarbon

65
Q

Hydrocarbons may be divided into two large classes.

A

Saturated and unsaturated hydrocarbon

66
Q

Is a hydrocarbon in which all carbon-carbon bonds are single bonds.

A

Saturated Hydrocarbons

67
Q

Is a hydrocarbon in which one or more carbon-carbon multiple bonds are present.

A

Unsaturated Hydrocarbons

68
Q

Give three examples of saturated hydrocarbons.

A

Alkanes
Cycloalkanes
Haloalkanes

69
Q

Give three examples of unsaturated hydrocarbons.

A

Alkenes
Alkynes
Aromatic

70
Q

A saturated hydrocarbon in which the carbon atom arrangement is acyclic.

A

Alkanes

71
Q

Is a saturated hydrocarbon in which carbon atoms are connected to one another in a cyclic (ring) arrangement.

A

Cycloalkanes

72
Q

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.

A

Haloalkanes

73
Q

Are hydrocarbons that contain one or more double bonds between neighboring carbon atoms.

A

Alkenes

74
Q

Are hydrocarbons that contain one or more triple bonds between neighboring carbon atoms.

A

Alkynes

75
Q

Is a six-carbon ring with alternative double bonds.

A

Aromatic Hydrocarbons or Benzene

76
Q

A functional group that involves an oxygen atom that is bonded to one hydrogen atom and one carbon atom.

A

Alcohol

77
Q

A functional group consisting of an oxygen atom that forms single bonds with two carbon atoms.

A

Ethers

78
Q

A functional group that contains a sulfur atom bonded to a hydrogen atom.

A

Thiols

79
Q

A functional group that consists of a nitrogen atom bonded to some combination of carbons and hydrogens.

A

Amines

80
Q

A carbon atom and an oxygen atom are connected by a double bond.

A

Carbonyl Group

81
Q

Is a carbonyl in which carbon atoms is bonded to at least one hydrogen atom.

A

Aldehyde

82
Q

Involves a carbonyl in which the carbon atom makes single bonds with two r-groups

A

Ketones

83
Q

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.

A

Carboxylic Acids

84
Q

It contains a carbonyl where the carbon is bonded to one additional oxygen atom and one carbon or hydrogen atom.

A

Esters

85
Q

A carbonyl in which the carbon is attached to one nitrogen atom and one carbon or hydrogen atom.

A

Amides

86
Q

Sulfur replaces the oxygen and is connected to one atom and one r group.

A

Thioether

87
Q

ACHAABAETAAKCEAT

A

Organic Chemistry (5 decks)

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