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1
Q
  • the study of molecules that have carbon atoms
A

Organic Chemistry

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2
Q
  • First coined the term “organic chemistry” for the study of compounds derived from biological sources
A

Jons Jacob Berzelius (1806)

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3
Q

Organic chemistry referred to the study of chemical compounds that could only be extracted from living things, but not made

A

Vital Force Theory

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4
Q
  • Discover organic matter on meteorites
A

Friedrich Wöhler (1828)

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5
Q
  • First person to isolate the elements yttrium, beryllium, and titanium
A

Friedrich Wöhler (1828)

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6
Q
  • Most well known for his discovery that an inorganic salt, ammonium cyanate, could be used to make urea without living organisms.
A

Friedrich Wöhler (1828)

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7
Q
  • Discovered the benzene ring structure
A

Friedrich August Kekule von Stradonitz (1865)

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8
Q

characterized by three double bonds alternating with single bonds between carbon atoms and in concept double bonds are shorter than single bonds,

A

benzene ring

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9
Q
  • Demonstrated the concept of electron dot structure
A

Gilbert Newton Lewis

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10
Q

Responsible for the concepts of nature of chemical bond, resonance, hybridization, and molecular orbital theory

A

Linus Pauling

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11
Q

➢ Atoms with the same number of protons but different numbers of neutrons

A

isotopes.

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12
Q

➢ Atomic mass unit (amu) - based

A

Carbon 12

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13
Q

Electrons that are bound to nuclei are found in

A

orbitals

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14
Q

we can never determine the exact location of the electron, but we can determine the electron density

A

Heisenberg Uncertainty Principle

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15
Q

the probability of finding the electron in a particular part of the orbital

A

electron density

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16
Q

Orbitals with identical energies

A

degenerate orbitals.

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17
Q

electrons that are in the outermost shell

A

valence electron

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18
Q

represents a nonbonding (lone) pair of electrons that are not involved in a covalent bond and “belong to” only one atom

A

A pair of dots

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19
Q

an atom will be most stable when surrounded by 8 electrons in the valence shell

A

Octet Rule

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20
Q

bond with the electrons shared equally between the two atoms

A

Nonpolar Covalent Bond

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21
Q

unequally shared pair of bonding electrons

A

Polar Covalent Bond

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22
Q

symbolized by an arrow with its head at the negative end of the polar bond and a plus sign at the positive end.

A

Bond polarity

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23
Q

The bond polarity is measured by its

A

dipole moment (µ)

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24
Q

defined to be the amount of charge separation (𝛿+ and 𝛿–) multiplied by the bond length (d).

A

dipole moment (µ)

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25
chemical property that describes the tendency of an atom or a functional group to attract electrons toward itself.
Electronegativity
26
is useful for predicting the polarity of covalent bonds.
Pauling Electronegativity Scale
27
more attraction for bonding electrons
Higher EN
28
the charge a bonded atom in a molecule would have if the bonding electrons are shared equally.
Formal Charge
29
process of combining two atomic orbitals (AOs) to create a new type of hybridized orbitals (HOs).
Hybridization
30
explains covalent bonds as the results of overlapping atomic orbitals from different atoms from which the unpaired electrons interact, form bonds, and share electron pairs
Valence Bond Theory
31
molecular geometry model that helps predict the shape of a molecule from the electron pairs that surround the central atoms of the molecule.
VSEPR (Valence Shell Electron Pair Repulsion Theory)
32
produces linear molecules at a 180° angle
sp hybridization
33
“diagonal hybridization”
sp hybridization
34
a hybrid orbital of one ‘s’ and one ‘p’ orbitals of equal energy 50% s, 50% p
sp hybridization
35
120° angle
sp2 hybridization
36
a hybrid orbital of one ‘s’ and two ‘p’ orbitals
sp2 hybridization
37
“trigonal hybridization”
sp2 hybridization
38
109.5° angle
sp3 hybridization
39
“tetrahedral hybridization”
sp3 hybridization
40
a hybrid orbital of one ‘s’ and three ‘p’ orbitals 25% s, 75% p
sp3 hybridization
41
head-on overlap of orbitals.
Sigma (σ) bonds
42
overlap of unhybridized p-orbitals.
Pi (π) bonds
43
Way of describing delocalized electron with certain molecules where the bonding cannot be expressed by one Lewis Structure
Resonance
44
It occurs because of the delocalization of pi electrons
Resonance
45
the movement of electrons from electron rich atom to electron poor atom.
curved arrow formalism
46
proton donor
Acid
47
proton acceptor
Base
48
A group of atoms responsible for the characteristic reactions of a particular compound. It serves as the site of organic reactions.
Functional Groups
49
The carbons present in alkanes are sp3 hybridized.
Alkanes
50
The_______ of alkanes depend on the no. of carbon present in the compound.
Physical Properties
51
This will dictate primarily the reactivity of organic molecule particularly hydrocarbon or any carbon-containing molecule
Degree of Substitution of C
52
This force is present in all molecules. It has the weakest force. However, if the molecules have more electrons, the force is stronger.
London Dispersion Force or Van Der Waals
53
The force between polar nonmetal bonds
Dipole-Dipole
54
It occurs when hydrogen is bonded with fluorine, oxygen, or nitrogen (FON)
Hydrogen Bond
55
The force when metals bond to nonmetals.
Ion-Dipole
56
The strongest force which occurs when a metal bonds to another metal.
Ion-ion
57
Process of combining alkanes with oxygen
COMBUSTION
58
It is a gateway to the rest of organic synthesis.
HALOGENATION
59
decomposing or separating the halogen molecule into its corresponding radical.
Initiation
60
step in producing more radicals, specifically alkyl radicals and halogen radicals.
Propagation
61
all the remaining radicals in the propagation step must be combined in all possible manner to form a more stable product.
Termination
62
The stability of Benzene is due to the _________________ across its ring structure.
delocalization of electrons
63
are a special class of organic molecules that exhibit unique properties due to their specific structural characteristics.
Aromatic Compounds
64
a ring of atoms
cyclic
65
all atoms in the molecule lie in the same plane
fully planar
66
p orbitals at every atom in the ring
conjugated
67
Huckel's Rule
4n+2=π electrons
68
Three-dimensional arrangement of atoms
Stereochemistry
69
It deals with the spatial arrangement of atoms and groups in molecules
Stereochemistry
70
has sedative effect
(R)-Thalidomide
71
- has teratogenic effect
(S)-Thalidomide
72
same molecular formula and chemical bonds but they have different spatial arrangements.
Stereoisomers
73
Stereoisomers can be subdivided into two parts
configurational conformational
74
non-superimposable and non-interconvertible by rotation around single bonds.
Configurational
75
They can be interconverted by breaking and making bonds
Configurational
76
2 types of Configurational
Enantiomers and Diastereomer
77
non-superimposable but easily interconvertible by rotation about single bonds.
Conformational
78
Also termed as handedness
Chirality
79
Means that molecules cannot be superimposed with its mirror image by any rotations or translations
Chirality
80
Has four (4) unique substituents
Chiral Carbon
81
Only applicable if the atoms on the left are not the same and the atoms on the right are not the same.
Cis-trans Isomers

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