1. Five Traditional Branches of Chemistry:
Organic
Analytical
Inorganic
Physical
Biochemistry

2. Organic Chemistry

3. Organic Chemistry references
Morrison & Boyd (6th)
Organic Chemistry by:
William H. Brown
Christopher S. Foote
Brent L. Iverson

4. Organic Chemistry
The study of the compounds of carbon, their properties and the changes that they undergo. 
Include description of –
nomenclature
syntheses
reactions
mechanisms

5. The study of the compounds of carbon Over 10 million compounds have been identified about 1000 new ones are identified each day!
C is a small atom
it forms single, double, and triple bonds
it is intermediate in electronegativity (2.5)
it forms strong bonds with C, H, O, N, and some metals

6. Crude
oil
Coal

7. order of filling

8. Fluorine F (at.no 9) 9p/9e 
1s2,2s2,2p5
 Chlorine Cl (at.no 17) 17p/17e
  1s2,2s2,2p6,3s2,3p5
 Bromine Br (at.no 35) 35p/35e
1s2,2s2,2p6,3s2,3p6,4s2,3d10,4p5
 Iodine I (at.no 53) 53p/53e
  1s2,2s2,2p6,3s2,3p6,4s2,3d10,4p6,5s2,4d10,5p5

9. Atoms and Ions:
Atoms are electrically neutral because they have equal number of (p and e).
Ex; Hydrogen has (1p and 1e )and they cancel each other.
Atoms can gain or lose electrons when they form compounds.
When atoms lose or gain electrons they become charged Atoms having a (+) or (–) charges are called ions .
Sodium (Na) loses an electrons when it forms NaCl and become Na+.

10. Formation of Ions:
We use a single-headed curved arrow to show the transfer of one electron from (Na) to (F).
In forming ( Na+ F-) the single (3s) electron from (Na) is transferred to the partially filled valence shell of (F).

11.  Ionic bond:
Ionic bond formed by the transfer of valence electrons to achieve noble gas electron configurations, resulting in ions held together by electrostatic attraction.
 Covalent bond:
Covalent bond formed by the sharing of valence electrons to achieve noble gas electron configurations.

12. Covalent Bonds The simplest covalent bond is H2
the single electrons from each atom combine to form an electron pair
The shared pair functions in two ways simultaneously; it is shared by the two atoms and fills the valence shell of each atom
The number of shared pairs:
one shared pair forms a single bond
two shared pairs form a double bond
three shared pairs form a triple bond

13. Polar and Non-polar Covalent Bonds:
Although all covalent bonds involve sharing of electrons, they differ widely in the degree of sharing
We divide covalent bonds into
Non-polar covalent bonds
Polar covalent bonds

14. Example of a polar covalent bond is that of (H-Cl)
we show polarity by using the symbols d+ and d-, or by using an arrow with the arrowhead pointing toward the negative end and a plus sign on the tail of the arrow at the positive end.

15. Bond dipole moment (m):
Polar Covalent Bonds
Bond dipole moment (m):

16. Hybridization of atomic orbitals:
sp = linear; 180o
sp2 = trigonal; 120o
sp3 = tetrahedral; 109.5o

17. Hybridizations of carbon

19. Polarity:
Covalent bonds are polar when the two atoms sharing electrons have different electronegativities.
eg. H—Cl
δ+ δ-
A charge separation or a dipole gives a polar bond.
O :O=O: has a non-polar bond

20. Electronegativity
Is the measure of attraction of atom’s for the electrons it shares with another atom in a chemical bond.

21. Intermolecular forces. Attractions between molecules.
Ionic Attractions (very strong) Na+ Cl-
dipole-dipole attractions H—Br
hydrogen bonding ( H attached to N,O,F ) H—O------H—O
van der Waals (London forces) (weak) Br—Br

22. Cl2
CO2
H2O
CH4
KBr
non-polar, covalent => van der Waals
Polar, covalent => dipole-dipole &
Hydrogen bonding
ionic bonding => ionic attractions

23. Prediction of mp/bp (relatively high or low?):
Mg(OH)2
CH3OH
CH2O
CH3CH3
mp bp
350oC --
-94oC 65oC
-920C -21oC
-183oC –89oC
ionic => ionic attractions
polar => (dipole-dipole + H-bond)
polar => dipole-dipole
non-polar => van der Waals
Formaldehyde [CH2O] is a key intermediate in the combustion of fuels like natural gas and methanol,

24. Solubility “like dissolves like”
~ water soluble? must be ionic or highly polar + H-bond
(hydrophilic)
~ water insoluble? must be non-polar or weakly polar
(hydrophobic)

25. Acids historic: sour taste react with metals produce  H2
react with bases  water + salts
change litmus  red
react with limestone rock  CO2
examples: HCl, H2SO4, HNO3, HClO4

26. Bases historic: soapy feel or taste react with acids  water + salts
bases - bitter taste
soapy feel or taste
react with acids  water + salts
change litmus  blue
examples: NaOH, Al(OH)3, K2CO3, NaHCO3

27. Brønsted Acid - a substance that donates a proton (H+) in a chemical reaction.
Brønsted Base – a substance that accepts a proton (H+) in a chemical reaction.
NaOH H2SO4  H2O NaHSO4
base acid acid base

28. Lewis Acid – a substance that accepts an electron pair in a chemical reaction to form a covalent bond.
Lewis Base – a substance that donates an electron pair in a chemical reaction to form a covalent bond.
- +
BF :NH3  F3B:NH3

30. Within the period of the periodic table, acid strength increases with increasing electronegativity:
CH4 < NH3 < H2O < HF
Within a group of elements, acid strength increases with increasing size:
HF < HCl < HBr < HI

31. Which is the stronger acid?
H2O or H2S?
What is the order of base strength?
F Cl Br I-
oxygen & sulfur are in the same group and sulfur is bigger: H2S > H2O
in the halogen family base strength decreases with increasing size:
F- > Cl- > Br- > I-

32. Isomers - different compounds with the same molecular formula.
example: C2H6O
CH3CH2OH CH3OCH3
ethyl alcohol dimethyl ether
boiling point (78oC) boiling point (–24oC)

33. Functional group:
An atom or group of atoms within a molecule that shows a characteristic set of physical and chemical properties
Functional groups are important for three reasons; they are:
1- The units by which we divide organic compounds into classes.
2. The sites of characteristic chemical reactions.
3. The basis for naming organic compounds