Module 1: OVERVIEW OF ORGANIC CHEMISTRY Flashcards
Organic Chemistry deals with substances derived from living things.
(True or False)
False
Organic Chemistry deals with carbon-based molecules.
(True or False)
False
Carbon-containing but NOT ORGANIC
- Carbon (graphite, diamond)
*CO2 - CO
- CN-
- C-4
- CO3-2
Many chemists believed that a “vital force”, a mysterious, presumed
property of living things was needed for the
formation of organic compounds
VITAL FORCE THEORY
The vital force theory is abolished by
Friedrich Wohler
Ammonium cyanate
(Organic or Inorganic)
Inorganic
Urea
(Organic or Inorganic)
Organic
the chemistry of hydrocarbons and their derivatives
Organic Chemistry
Organic compounds are more abundant than inorganic compounds.
(True or False)
True
Organic compounds have simple structures.
(True or False)
FALSE
?? Organic compounds
have complex structures.
Organic compounds
are water-insoluble and nonpolar
(True or False)
True
Organic compounds
are inflammable.
(True or False)
True
?? The words Inflammable and
flammable have the same meaning
Elements in Organic compounds
- Hydrogen
- Carbon
- Nitrogen
- Oxygen
- Fluorine
- Phosphorus
- Sulfur
- Chlorine
- Bromine
- Iodine
Why study Organic Chemistry?
- Living things are
made of?
organic
compounds
Why study Organic Chemistry?
- make up hair?
Proteins
Why study Organic Chemistry?
- controls genetic make-up?
DNA
Why study Organic Chemistry?
Foods, medicines
Examine structures to the right
The smallest particle of an element that maintains its chemical identity
ATOM
Building blocks
of atomic structure
–PROTON (p+)
– NEUTRON (n0)
–ELECTRON (e-)
The Nuclide Symbol
𝐴
𝐸
Z
* E Symbol
* A Mass number
* Z Atomic number
Wave Mechanics
– It estimates the position of electrons and quantifies energy levels (a.k.a. shells).
Schrödinger Wave Equation
Wave Mechanics
– Region of space where an electron is most likely found.
Atomic Orbitals (AO)
Shape of the Orbitals
s spherical
p dumb-bell
d clover leaf
f complex
“Distribution of electrons”
ELECTRON CONFIGURATION
Describes the number and arrangement of
electrons in orbitals, subshells, and shells
in an atom.
ELECTRON CONFIGURATION
Max e of s
2
Max e of p
6
Max e of d
10
Max e of f
14
Outermost electrons
Valence electrons
Different from charge
Valence electrons
A pair of unshared, nonbonding electrons
is called
LONE PAIR
form bonds to achieve 8 valence electrons
OCTET RULE
have a “line” drawn between two atoms indicating a “2-electron” covalent bond.
Kekulé (Line-Bond) Structure
Molecular Representations
– No. of each type of atom
Molecular formula
Molecular Representations
– Atoms and bonds are shown.
Structural formula
Molecular Representations
– Single bond are NOT drawn.
– Groups are clustered
Condensed structural formula
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
Skeletal (Line-angle) Structures
Structures are drawn in “zigzag” manner
Skeletal (Line-angle) Structures
Each corner, bent, endpoint, and intersection represent a C atom.
Skeletal (Line-angle) Structures
C atoms can form 4 covalent bonds. Supply the no. of H atoms mentally.
Skeletal (Line-angle) Structures
form as a result of electron “transfer”
Ionic bonds
form due to sharing of
electrons
Covalent bonds
ability of an atom to attract the shared electrons in a covalent bond
ELECTRONEGATIVITY
- can have ionic character.
- differ on the degree of “sharing”.
– Depends on difference of electronegativity
Covalent bonds
DIFFERENCE IN EN:
??
TYPE OF BOND:
+ Non-polar Covalent
MOST LIKELY FORMED BETWEEN:
+ Two Nonmetals OR Nonmetal and Metalloid
Less than 0.5
DIFFERENCE IN EN:
??
TYPE OF BOND:
+ Polar Covalent
MOST LIKELY FORMED BETWEEN:
+ Two Nonmetals OR
Nonmetal and Metalloid
0.5 – 1.9
DIFFERENCE IN EN:
??
TYPE OF BOND:
+ Ionic
MOST LIKELY FORMED BETWEEN:
+ Metal + Nonmetal
More than 1.9
a.k.a. Electron
Density Model
Electrostatic Map Potential
Arrows indicate direction of bond polarity
Electrostatic Map Potential
Bond Dipole Arrow
Electrostatic Map Potential
Electrostatic Map Potential
- represents low electron density
blue
Electrostatic Map Potential
- represents high electron density
red
Bonding electrons toward the electronegative atom
– C acquires partial positive charge, + (delta plus)
– Electronegative atom acquires partial negative
charge, - (delta minus)
Electrostatic Map Potential
Valence electrons may be involved in the
formation of single, double, or triple bonds
Valence-Shell Electron Pair Repulsion (VSEPR)
Electrons are paired in the “overlapping orbitals” and are attracted to the nuclei of both atoms
Valence Bond Theory
Atomic orbitals combine to form new orbitals called
HYBRID ORBITALS
Sigma (s) bond and Pi () bonds
+ Electrons are centered
between nuclei
Sigma bond
Sigma (s) bond and Pi () bonds
+ Electrons occupy regions above and below the axis joining the nuclei
Pi bond
Energy needed to break or form a chemical bond
Bond Strength (Bond Energy)
Sigma bond is greater than pi bonds
(True or False)
True
Optimum distance between nuclei leading to maximum stability
Bond Length
antibiotic
Benzylpenicillin
Bond angle of Single bond
109.5 degrees
Bond angle of Triple bond
180 degrees
Bond angle of Double bond
120 degrees
Shape of Single bonds
Tetrahedral
Shape of Double bonds
Trigonal Planar
Shape of Triple bonds
Linear
Electron Density around the Central Atom of Single bonds
4
Electron Density around the Central Atom of Double bonds
3
Electron Density around the Central Atom of Triple bonds
2
Groups Bonded to Carbon of Single Bonds
4
Groups Bonded to Carbon of Double Bonds
3
Groups Bonded to Carbon of Triple Bonds
2
Orbital Hybridization of Single Bonds
sp3
Orbital Hybridization of Doubles Bonds
sp2
Type of Bonds to Carbon of Single Bonds
Sigma bond
Orbital Hybridization of Triple Bonds
sp
Type of Bonds to Carbon of Double Bonds
Sigma bond and 1 pi bond
Type of Bonds to Carbon of Triple Bonds
Sigma bond and 2 pi bonds
The charge on an atom in a molecule or polyatomic ion
𝑭𝑪 = # 𝒐𝒇 𝒗𝒂𝒍𝒆𝒏𝒄𝒆 𝒆
− 𝑼𝒏𝒔𝒉𝒂𝒓𝒆𝒅 𝒆
− # 𝒐𝒇 𝒃𝒐𝒏𝒅�
Formal Charge
