Biochemistry is the study of biomolecules in living organisms and their chemical reactions. It includes cell biology, molecular biology, and molecular genetics. The goals of biochemistry are to describe and explain all chemical processes in cells on a molecular level and to understand the origins of life. Biochemistry is essential to medicine, as many diagnostic techniques and drugs are developed based on biochemical discoveries and processes. The basic units of life, cells, can be either eukaryotic or prokaryotic. Biomolecules include carbohydrates, proteins, lipids, nucleic acids, minerals, vitamins, and water, which are held together by covalent and non-covalent bonds.

2. By Dr. Elrasheed Eltaher Osman

3. Biochemistry
Definition
Is the science concerned
with various biomolecules
that occur in the living cell
and organism and their
chemical reactions

4. Components of biochemistry :
1- cell biology
2- molecular biology
3- molecular genetics

5. Aims of biochemistry
1- is to describe and explain in
molecular terms all chemical
processes of living cell
2- To understand how life is began
3- knowledge of biochemistry is
essential to all life sciences

6. Bio-medicine relationship
 Most Biomedical of biomedical
techniques
reaction used for has diagnosis been
of
discovered diseases
after following
a course of a disease
 All diseases have
biomedical bases
Biochemistry used for
formulation of drugs

7. In order to study biochemistry a little
information should be known about
the cell
The cell smallest unit of live capable
of doing all living processes
Cell divided into :
1- eukaryotic cell
2- prokaryotic cell

9. Biomolecules
Complex molecules that is formed living
organisms they include:
1- carbohydrates
2- protein
3- lipids
4- nucleic acids
5- minerals
6- vitamins
7- water

10. All are composed of atoms
 All except minerals contain
elements of water
 All except minerals and water
are organic molecules
 All except minerals ,water and
vitamins yield energy

11. • WATER IS BLESS FROM GOD
~ USE IT DON’T ABUSE IT

12. Homeostasis
Is the maintenance of composition of the
internal environment for good health and
this include:
1- water distribution
2- pH
3- electrolytes concentration

13. WATER , pH and BUFFERS
Water
Is the principle end product of
oxidative catabolism of food
Is the most important molecule
for life
No life without water
All elements and processes in
some how needs water

14. Water distribution
This depends on
Control of thirst by hypothalamus
Anti-diuretic hormone
Retention or excretion of water by
-Kidney (micturition)
- skin (perispiration)
-Lung (respiration)

15. Water disbalance
occurs when there is state of water
depletion or excess
Water depletion (dehydration)
Result from
1- decrease intake (comma)
2- increase loss (severe
sweating, renal loss, diarrhea
cholera …

16. Water excess
May be due to:
 Increase intake
(excessive I/V fluids)
 Decrease output
(renal failure)

17. WHAT MAKES WATER AN
IDEAL SOLVENT FOR THE
LIFE ?
This is due to its ideal
properties

18. Physical properties of water
1- high heat of vaporization
2- high melting
3- low freezing point
4- neutral pH

19. solvent Melting
point
Boilin
g
point
Heat of
vaporizatio
n
1 water 0 100 2260
2 methanol -98 65 1100
3 ethanol -117 78 854
4 acetone -95 56 523
5 benzene 6 80 394
6 chloroform -63 61 247
7 Hexane -98 69 423

20. Chemical properties of water
1- tetrahedral
2- bipolar
3- formation of hydrogen bonds
4- Partial dissociation
5- React as acid or base
6- high ionic product

21. pH
Potential hydrogen
Hydrogen ion concentration
Is –log [H+]
pH scale 1—14
7 neutral
Normal pH 7.35 – 7.45

22. • pH < 7 acidic
• In blood pH<7.35
acidosis
•Acidosis can be
1- metabolic
2- respiratory

23. • pH > 7 alkaline
• In blood pH>7.45
alkalosis
• Alkalosis can be
1- metabolic
2- respiratory

24. Buffers
 Molecules that resist
change in pH when acid
or alkaline are added to a
solution
 They are week acids
and their conjugated
base

25. Normal occurring buffers
inside human body include:
1- carbonic acid and
bicarbonate
2- organic phosphoric acid
and phosphate
3- proteins

26. Week acid
HX H++X-Conjugate
base
AX A++X-

27. If we add acid
(H+)
+ H+
H+
HX H++X-H
AX A+ + X-

28. Not like this
Wake up

29. Forces stabilizing bimolecules
These Include:
1- covalent bonds
2- non- covalent bonds

30. Covalent bonds
 Strong bonds
 Needs high energy to be broken
 Examples are
Peptide bonds
Glycosidic bonds
Ester bonds
Disulfide bridge

32. Peptide bonds
 Covalent bond
 Form between amino group
of one molecule and carboxyl
group on another molecule

34. Glycosidic bond
 Covalent bond
 Form between two different
alcohol groups
 Can be
1- N-glycosidic
2- O-glycosidic
3- S-glycosidic

36. O-glycosidic bond
Occur when the two
alcoholic groups are
OH-

37. -CH2OH + OHCH2-
-CH2-O-CH2- H2O

38. N-glycosidic bond
Occur when one
of the alcohol
group is NH3

39. -CH2NH2 + OHCH2-
-CH2-N-CH2- H2O
IH

40. S-glycosidic
Occur when one
of the alcohol
group is SH

41. -CH2SH + OHCH2-
-CH2-S-CH2- H2O

42. Ester bond
Occur between alcohol
group and carboxyl group
Phosphoester
Thioester

44. 2O
-COH +H OOC-H
II
-C-O-C-O

45. Disulfide bridge
Occur between two SH
group

46. 2H+
-SH + HS-
―S―S―

48. The non-covalent bonds
This include
1- hydrogen bond
2- hydrophobic interaction
3- Electrostatic bond
4- Van Der Waal forces

49. Hydrogen bond
 Non-covalent bond
 Occur between positive
hydrogen ion in a molecule ad
negative ion in another one
Is very week bond

52. The hydrophobic interaction
Is tendency of a molecule for
folding around it self to hide
the non-polar part from water
when put in solution
In this case the polar
part come to the out side
to contact water

54. Electrostatic interaction
(ionic bridge,salt bridge)
 Non-covalent bond
 Occur between a positive
ion in one molecule and most
negative ion in another
molecule

56. Van Der Waal forces
Is the attractive and
repulsive forces that
occur between two
adjacent atoms in a
molecule