Module 1: OVERVIEW OF ORGANIC CHEMISTRY Flashcards by Aho Tei

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

False

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

False

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Carbon-containing but NOT ORGANIC

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

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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

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The vital force theory is abolished by

Friedrich Wohler

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Ammonium cyanate
(Organic or Inorganic)

Inorganic

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Urea
(Organic or Inorganic)

Organic

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the chemistry of hydrocarbons and their derivatives

Organic Chemistry

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

True

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Organic compounds have simple structures.
(True or False)

FALSE
?? Organic compounds
have complex structures.

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

True

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Organic compounds
are inflammable.
(True or False)

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

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Elements in Organic compounds

Hydrogen
Carbon
Nitrogen
Oxygen
Fluorine
Phosphorus
Sulfur
Chlorine
Bromine
Iodine

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

organic
compounds

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Why study Organic Chemistry?
- make up hair?

Proteins

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

DNA

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Why study Organic Chemistry?

 Foods, medicines
 Examine structures to the right

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The smallest particle of an element that maintains its chemical identity

ATOM

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Building blocks
of atomic structure

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

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The Nuclide Symbol

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

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

Schrödinger Wave Equation

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

Atomic Orbitals (AO)

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Shape of the Orbitals

s spherical
p dumb-bell
d clover leaf
f complex

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“Distribution of electrons”

ELECTRON CONFIGURATION

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

ELECTRON CONFIGURATION

Max e of s

Max e of p

Max e of d

Max e of f

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

Electron Density around the Central Atom of Double bonds

Electron Density around the Central Atom of Triple bonds

Groups Bonded to Carbon of Single Bonds

Groups Bonded to Carbon of Double Bonds

Groups Bonded to Carbon of Triple Bonds

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

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

Module 1: OVERVIEW OF ORGANIC CHEMISTRY Flashcards

(82 cards)