organic chemistry a chapter 1 introduction by prof. dr. adel m. awadallah
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Organic chemistry A Chapter 1 Introduction By Prof. Dr. Adel M. Awadallah Islamic University of Gaza. Chapter 1 Bonding and Isomerism Organic chemistry is the chemistry of the compounds of carbon Atoms consist mainly from Nucleus: (containing Protons and Neutrons) - PowerPoint PPT PresentationTRANSCRIPT
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Organic chemistry A
Chapter 1
Introduction
By Prof. Dr.
Adel M. Awadallah
Islamic University of Gaza
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Chapter 1
Bonding and IsomerismOrganic chemistry is the chemistry of the compounds of carbon
Atoms consist mainly froma) Nucleus: (containing Protons and Neutrons)
Protons (positive particles, Atomic Number)
Neutrons (Neutral particles)
Protons + Neutrons (Atomic weight)
b) Electrons: negatively charged particles
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Electronic Configuration (review)1) Shells (n = 1,2,3,4, ….)2) (Subshells , s, p, d, f)3) (orbitals: rgions of space around the nucleus containing
electrons)4) each orbital contains only 2 electrons with different spins
SubshellNumber of orbitals (electrons)Name of orbitals
S1 (2)s
P3 (6)Px, py, pz
d5 (10)Dxy, dyz, dxz, dz2,
dX2
-y2
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Examples:Filled Shells
Play almost no role in chemical reaction
Valence Electrons
They are the outermost electrons and they are mainly involved in chemical bonding
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Ionic CompoundsThey are formed by the transfer of one or more valence
electrons from one atom to another
Electropositive atoms: give up electrons and form cations.
Electronegative atoms: accept electrons and form anions
Ionic compounds: are composed of positively charged cations and negatively charged cations
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Covalent compoundsA covalent bond: is formed when two atoms share one or more electron
pairs. A molecule consists of two or more atoms joined by covalent bonds
Bond energy: is the energy necessary to break a mole (6.022 x 1023)of covalent bonds.
Bond length: is the average distance between two covalently bonded atoms
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• Valence and bonding in organic compounds
O
O
Cl
N
CH3
H
H
H
H
H
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• Polarity of Bonds: depends on the electronegativity difference
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• Examples:
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• Polarity of Molecules: depends on the sum of the polarity of bonds (geometry)
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• Isomers: different compounds having the same molecular formula
CH3CH2OH CH3OCH3
ClI
Br
H
ICl
Br
HCH3 CH3CH3CH3
CH3
Et
Cl
Cl HH
CH3
Et
Cl
ClH
H
ClH
Cl H
ClH
H Cl
Cl H
ClH
Cl Cl
HH
IsomersDifferent compounds that have the same molecular formula
Constitutional isomers Stereoisomers
Atoms are attached to one another in different ways
Atoms have the same constitution but different arrangement in space
Enantiomers Diasteriomers
Non superimposable mirror- image stereoisomers
Non mirror-image stereoisomers
Conformational Configurational
Interconvertable by rotation
Interconvertable by bond breaking
SR
cis- trans-
cis trans
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• Abbreviated structural formulas
CH3CH2CH2OH OH OH
H
HH
H
H
H
H
CH2
CH2
CH2
CH2
CH2
= =
=
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• Formal Charges: are the charges that each atom carries, and can be calculated as follows
• Formal charge = Valence electrons – bonds – electrons
• Example:
• Resonance: arises whenever we can write two or more structures for a molecule with different arrangements of electrons but identical arrangement of atoms
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• Arrows:
CH3 CH3
Reaction
equilibrium reaction
Resonance
Movement of two electrons
Movement of one electron
straight arrow
double headed straight arrow
Pair of straight arrows with half heads
Curved arrow
Fishhook
2CH3.
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• The orbital view of bonding
+
H. H. H - H
H.
+
F. H - F
+
F.F. F - F
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• Orbital picture of Methane and ethane
•
The bond formed by end-to-end overlap is called a sigma bond.
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Bond Angles in Methane
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• Bonding in Ethylene (ethene)
1s2
sp2 sp2 sp2
p
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A pi bond is one in which the electrons in the p orbitals are held above and below the plane of the molecule.The sigma bond is stronger than the pi bond.A double bond is formed from a sigma bond and a pi bond, and so it is stronger than a single bond.
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• Bonding in acetylene (ethyne)
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• Classification of organic compounds according to functional groups
OHO
R H
O
SHS
R OH
O
R OR
O
R R
O
R X
O
R NH2
O
R NH2 R CN
Alkane Alkene Alkyne Aromatic
Alcohol Thiol Ether Thioether
Aldehyde Ketone Carboxylic acid Ester Acid halide Amide
Amine Nitrile
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Intramolecular Forces
Bond Dissociation Energy: The amount of energy consumed or liberated when a bond is broken orformed
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Intermolecular ForcesIntermolecular forces: attractive forces between molecules.
•Intramolecular forces: hold atoms together in a molecule.(chemical bonding)
•Intramolecular forces stabilize individual molecules, whereas intermolecular forces are primarily responsible for the bulk properties of matter (i.e. melting point and boiling point).
•Intermolecular vs Intramolecular•41 kJ to vaporize 1 mole of water (inter)
•930 kJ to break all O-H bonds in 1 mole of water (intra)•Generally, intermolecular forces are much weaker than intramolecular
forces .•The boiling points of substances often reflect the strength of the
intermolecular forces operating among the molecules. At the boiling point, enough energy must be supplied to overcome the attractive intermolecular forces between liquid molecules. The same is true for melting a solid
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• Types of Intermolecular forces:• 1- Dipole-Dipole Forces: are attractive forces that act between polar
molecules•
• The larger the dipole moments, the greater the force.
• The Hydrogen Bond: is a special type of dipole-dipole interaction between the hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom.
• Aــــ H---B or Aــــ H---A• A & B are N, O, or F• The average energy of a hydrogen bond is quite large for a dipole-dipole
interaction (up tp 40KJ/mol). Thus, hydrogen bonds are a powerful force in determining the structure and properties of many compounds.
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• 2- Ion-Dipole Forces: Attractive forces between an ion (either a cation or an anion) and a polar molecule.
•
• 3- Dispersion (London) force: arise as a result of temporary dipoles induced in the molecules or atoms.
• - act between all molecules.• - only force between nonpolar molecules and noble gas
atoms.• - strength depends primarily on size of molecule, very weak
for small molecule but fairly strong for large ones. (Shape plays a role too.)
- +
Na+
+ -
I -
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- +
-
-
(a)
+
Cation Induced dipole
- +
-
Induced dipole
(b)
- +
(c)
Dipole
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•Melting points• Melting is the change from the highly ordered arrangement
of particles in the crystalline lattice to the more random arrangement that characterizes a liquid
•Mp NaCl = 801
•Mp CH4 = -183
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Boiling point: The temperature at which the vapor pressure of a liquid equals the external pressure
Boiling involves the breaking away from the liquid of individual molecules or pairs of oppositely charged ions
Associated liquids
(Hydrogen bonded liquids)
Have relatively high bp.
HF boils 100 oC higher than HCl
H2O boils 160 oC higher than H2S
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Solubility: Like dissolve likeIonic Solutes are dissolved in water or very polar
solvents. They form ion-dipole bonds
Non-ionic solutes: solubility depends on polarityMethane (London forces ) in CCl4 (London forces )
Methanol (hydrogen bonding) in water (hydrogen bonding)
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Acids and bases:Arrhenius Definition Acid: H+ donor, Base: OH- donor
HCl + NaOH → NaCl + H2O
Lowry-Brønsted Acids and Bases:
Acid: H+ donor , Base: H+ acceptor
HCl + :OH- → Cl- + H2O
HCl + :NH3 → Cl- + NH4+
Lewis Definition: Acid: e acceptor, base: electron donor
H+ + :OH- → H2O
F3B + :NH3 → F3B:NH3
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