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Organic Chemistry Lec > Module 1: OVERVIEW OF ORGANIC CHEMISTRY > Flashcards

Module 1: OVERVIEW OF ORGANIC CHEMISTRY Flashcards

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1
Q

Organic Chemistry deals with substances derived from living things.
(True or False)

A

False

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2
Q

Organic Chemistry deals with carbon-based molecules.
(True or False)

A

False

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3
Q

Carbon-containing but NOT ORGANIC

A
  • Carbon (graphite, diamond)
    *CO2
  • CO
  • CN-
  • C-4
  • CO3-2
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4
Q

Many chemists believed that a “vital force”, a mysterious, presumed
property of living things was needed for the
formation of organic compounds

A

VITAL FORCE THEORY

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5
Q

The vital force theory is abolished by

A

Friedrich Wohler

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6
Q

Ammonium cyanate
(Organic or Inorganic)

A

Inorganic

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7
Q

Urea
(Organic or Inorganic)

A

Organic

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8
Q

the chemistry of hydrocarbons and their derivatives

A

Organic Chemistry

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9
Q

Organic compounds are more abundant than inorganic compounds.
(True or False)

A

True

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10
Q

Organic compounds have simple structures.
(True or False)

A

FALSE
?? Organic compounds
have complex structures.

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11
Q

Organic compounds
are water-insoluble and nonpolar
(True or False)

A

True

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12
Q

Organic compounds
are inflammable.
(True or False)

A

True
?? The words Inflammable and
flammable have the same meaning

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13
Q

Elements in Organic compounds

A
  • Hydrogen
  • Carbon
  • Nitrogen
  • Oxygen
  • Fluorine
  • Phosphorus
  • Sulfur
  • Chlorine
  • Bromine
  • Iodine
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14
Q

Why study Organic Chemistry?
- Living things are
made of?

A

organic
compounds

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15
Q

Why study Organic Chemistry?
- make up hair?

A

Proteins

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16
Q

Why study Organic Chemistry?
- controls genetic make-up?

A

DNA

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17
Q

Why study Organic Chemistry?

A

 Foods, medicines
 Examine structures to the right

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18
Q

The smallest particle of an element that maintains its chemical identity

A

ATOM

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19
Q

Building blocks
of atomic structure

A

–PROTON (p+)
– NEUTRON (n0)
–ELECTRON (e-)

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20
Q

The Nuclide Symbol

A

𝐴
𝐸
Z
* E  Symbol
* A  Mass number
* Z  Atomic number

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21
Q

Wave Mechanics
– It estimates the position of electrons and quantifies energy levels (a.k.a. shells).

A

Schrödinger Wave Equation

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22
Q

Wave Mechanics
– Region of space where an electron is most likely found.

A

Atomic Orbitals (AO)

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23
Q

Shape of the Orbitals

A

s spherical
p dumb-bell
d clover leaf
f complex

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24
Q

“Distribution of electrons”

A

ELECTRON CONFIGURATION

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25
Q

Describes the number and arrangement of
electrons in orbitals, subshells, and shells
in an atom.

A

ELECTRON CONFIGURATION

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26
Q

Max e of s

A

2

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27
Q

Max e of p

A

6

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28
Q

Max e of d

A

10

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29
Q

Max e of f

A

14

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30
Q

Outermost electrons

A

Valence electrons

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31
Q

Different from charge

A

Valence electrons

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32
Q

A pair of unshared, nonbonding electrons
is called

A

LONE PAIR

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33
Q

form bonds to achieve 8 valence electrons

A

OCTET RULE

34
Q

have a “line” drawn between two atoms indicating a “2-electron” covalent bond.

A

Kekulé (Line-Bond) Structure

35
Q

Molecular Representations
– No. of each type of atom

A

Molecular formula

36
Q

Molecular Representations
– Atoms and bonds are shown.

A

Structural formula

37
Q

Molecular Representations
– Single bond are NOT drawn.
– Groups are clustered

A

Condensed structural formula

38
Q

C and H atoms usually are “NOT” shown.
– H atoms attached to all “non-carbon” atoms must be shown
- All heteroatoms (atoms other than carbon and hydrogen) must be drawn, and any H atoms attached to a heteroatom must also be drawn

A

Skeletal (Line-angle) Structures

39
Q

Structures are drawn in “zigzag” manner

A

Skeletal (Line-angle) Structures

40
Q

Each corner, bent, endpoint, and intersection represent a C atom.

A

Skeletal (Line-angle) Structures

41
Q

C atoms can form 4 covalent bonds. Supply the no. of H atoms mentally.

A

Skeletal (Line-angle) Structures

42
Q

form as a result of electron “transfer”

A

Ionic bonds

43
Q

form due to sharing of
electrons

A

Covalent bonds

44
Q

ability of an atom to attract the shared electrons in a covalent bond

A

ELECTRONEGATIVITY

45
Q
  • can have ionic character.
  • differ on the degree of “sharing”.
    – Depends on difference of electronegativity
A

Covalent bonds

46
Q

DIFFERENCE IN EN:
??
TYPE OF BOND:
+ Non-polar Covalent
MOST LIKELY FORMED BETWEEN:
+ Two Nonmetals OR Nonmetal and Metalloid

A

Less than 0.5

47
Q

DIFFERENCE IN EN:
??
TYPE OF BOND:
+ Polar Covalent
MOST LIKELY FORMED BETWEEN:
+ Two Nonmetals OR
Nonmetal and Metalloid

A

0.5 – 1.9

48
Q

DIFFERENCE IN EN:
??
TYPE OF BOND:
+ Ionic
MOST LIKELY FORMED BETWEEN:
+ Metal + Nonmetal

A

More than 1.9

49
Q

a.k.a. Electron
Density Model

A

Electrostatic Map Potential

50
Q

Arrows indicate direction of bond polarity

A

Electrostatic Map Potential

51
Q

Bond Dipole Arrow

A

Electrostatic Map Potential

52
Q

Electrostatic Map Potential
- represents low electron density

A

blue

53
Q

Electrostatic Map Potential
- represents high electron density

A

red

54
Q

Bonding electrons toward the electronegative atom
– C acquires partial positive charge, + (delta plus)
– Electronegative atom acquires partial negative
charge, - (delta minus)

A

Electrostatic Map Potential

55
Q

Valence electrons may be involved in the
formation of single, double, or triple bonds

A

Valence-Shell Electron Pair Repulsion (VSEPR)

56
Q

Electrons are paired in the “overlapping orbitals” and are attracted to the nuclei of both atoms

A

Valence Bond Theory

57
Q

Atomic orbitals combine to form new orbitals called

A

HYBRID ORBITALS

58
Q

Sigma (s) bond and Pi () bonds
+ Electrons are centered
between nuclei

A

Sigma bond

59
Q

Sigma (s) bond and Pi () bonds
+ Electrons occupy regions above and below the axis joining the nuclei

A

Pi bond

60
Q

Energy needed to break or form a chemical bond

A

Bond Strength (Bond Energy)

61
Q

Sigma bond is greater than pi bonds
(True or False)

A

True

62
Q

Optimum distance between nuclei leading to maximum stability

A

Bond Length

63
Q

antibiotic

A

Benzylpenicillin

64
Q

Bond angle of Single bond

A

109.5 degrees

65
Q

Bond angle of Triple bond

A

180 degrees

66
Q

Bond angle of Double bond

A

120 degrees

67
Q

Shape of Single bonds

A

Tetrahedral

68
Q

Shape of Double bonds

A

Trigonal Planar

69
Q

Shape of Triple bonds

A

Linear

70
Q

Electron Density around the Central Atom of Single bonds

A

4

71
Q

Electron Density around the Central Atom of Double bonds

A

3

72
Q

Electron Density around the Central Atom of Triple bonds

A

2

73
Q

Groups Bonded to Carbon of Single Bonds

A

4

74
Q

Groups Bonded to Carbon of Double Bonds

A

3

75
Q

Groups Bonded to Carbon of Triple Bonds

A

2

76
Q

Orbital Hybridization of Single Bonds

A

sp3

77
Q

Orbital Hybridization of Doubles Bonds

A

sp2

78
Q

Type of Bonds to Carbon of Single Bonds

A

Sigma bond

78
Q

Orbital Hybridization of Triple Bonds

A

sp

79
Q

Type of Bonds to Carbon of Double Bonds

A

Sigma bond and 1 pi bond

80
Q

Type of Bonds to Carbon of Triple Bonds

A

Sigma bond and 2 pi bonds

81
Q

The charge on an atom in a molecule or polyatomic ion

𝑭𝑪 = # 𝒐𝒇 𝒗𝒂𝒍𝒆𝒏𝒄𝒆 𝒆
− 𝑼𝒏𝒔𝒉𝒂𝒓𝒆𝒅 𝒆
− # 𝒐𝒇 𝒃𝒐𝒏𝒅�

A

Formal Charge

Organic Chemistry Lec (5 decks)

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