Biochemistry primer for exercise science

1. Biochemistry
Chapter 1
Presented by
Yaser Alikhajeh

2. History of biochemistry
• he history of biochemistry can be said to have
started with the ancient Greeks who were interested
in the composition and processes of life , although
biochemistry as a specific scientific discipline has its
beginning around the early 19th century.

3. What is Biochemistry
• The term “biochemistry” itself is derived from the
combining form bio-, meaning "life", and chemistry.
• Biochemistry is the application of chemistry to the study of
biological processes at the cellular and molecular level.
• It emerged as a distinct discipline around the beginning of
the 20th century when scientists combined chemistry,
physiology and biology to investigate the chemistry of living
systems by:

4. A. Studying the structure and behavior of the complex
molecules found in biological material
B. the ways these molecules interact to form cells, tissues
and whole organism
C. Biochemistry has become the foundation for
understanding all biological processes. It has provided
explanations for the causes of many diseases in humans,
animals and plants."

5. Elements of the human body
96% (O, C, H & N)
• 3/8 % (P, S, Cl, Mg, Ca, Fe, K & Na)
• 0.8 ( Al, B, Cr, Co, Cu, F, I, Mn, Mo,
Se, Si, Sn, V& Zn)
 Carbohydrates
 Protein
 Lipids
 Water
 Mineral
Vitamin

6. Atom
• Atomic number
• is the number
of protons found in
the nucleus
• Mass number
• is the total number of
protons and neutrons

7. Electron shell Isotopes

8. Atomic mass unit
• Dalton or atomic mass unit
• 1/12 of the mass of an
unbound neutral atom of carbon-12.
• 1 Da=m(12C)/12 (1/66g × 10 -24 )
Base 10Prefix
symbolName
10 6Mmega
10 3Kkilo
10 -1ddeci
10 -2ccenti
10 -3mmilli
10 -6μmicro
10 -9nnano
10 -12ppico

9. Structural formula Molecular formula
• The structural formula of a
chemical compound is a grap
hic representation of the m
olecular structure, showing
how the atoms are possibly
arranged in the real three -
dimensional space .
• Indicate the simple numb
ers of each type of atom
in a molecule, with no info
rmation on structure.
• C6H12O6

10. Ion
• An ion is an atom or molecule that has a net electrical charge .
• A cation is a positively charged ion, with fewer electrons than
protons, while an anion is negatively charged.
• Na → Na+ + e− Cl + e− → Cl−

11. Chemical compound
• A chemical compound is a chemical substance composed of many
identical molecules composed of atoms from more than one elem
ent held together by chemical bonds.
• H+ + OH- → H2O
-Ơ
+Ơ

12. Chemical bond
• Covalent bonds
• Polar and Nonpolar
• Ionic bonds

13. Functional group
• In organic chemistry, functional groups are specific
substituents moieties within molecules that may be responsible
for the characteristic chemical reactions of those molecules.

14. chemical reaction Equilibrium constant
• A chemical reaction is a
process that leads to the
chemical transformation of
one set of chemical
substances to another.
• The equilibrium constant of a
chemical reaction is the value of
its reaction quotient at chemical
equilibrium, a state approached
by a dynamic chemical system
after sufficient time has elapsed
at which its composition has no
measurable tendency towards
further change.

15. PH
• pH is defined in terms of the activity of the hydrogen
ion.
• pH = −log10 {H+}
HA →H+ + A -
HA H + + A -

16. Acid-base reactions
• In the Brønsted–Lowry acid–base theory, an acid-base reaction
involves a transfer of protons (H+) from one species (the acid)
to another (the base).

17. Cell (biology)
• The cell is the basic structural, functional, and biological unit of
all known organisms.

18. Mitochondrion
Surrounded by a double membrane with a series of folds
called cristae. Functions in energy production through metabolism.
Plasma Membrane
A lipid/protein/carbohydrate complex, providing a barrier and
containing transport and signaling systems.
Nucleus
Double membrane surrounding the chromosomes and the nucleolus.
Pores allow specific communication with the cytoplasm. The
nucleolus is a site for synthesis of RNA making up the ribosome

19. .
Rough endoplasmic reticulum (RER)
A network of interconnected membranes forming channels within the
cell. Covered with ribosomes (causing the "rough" appearance) which
are in the process of synthesizing proteins for secretion or
localization in membranes.
Ribosomes
Protein and RNA complex responsible for protein synthesis
Smooth endoplasmic reticulum (SER)
A network of interconnected membranes forming channels within the
cell. A site for synthesis and metabolism of lipids. Also contains
enzymes for detoxifying chemicals including drugs and pesticides.
Golgi apparatus
A series of stacked membranes. Vesicles (small membrane
surrounded bags) carry materials from the RER to the Golgi
apparatus. Vesicles move between the stacks while the proteins are
"processed" to a mature form. Vesicles then carry newly formed
membrane and secreted proteins to their final destinations including
secretion or membrane localization.
Lysosymes
A membrane bound organelle that is responsible for degrading
proteins and membranes in the cell, and also helps degrade materials
ingested by the cell.

21. Metabolism
• Metabolism is the set of life-
sustaining chemical reactions in
organisms.
• Metabolic reactions may be
categorized as catabolic –
the breaking down of compounds (the
breaking down of glucose to pyruvate
by cellular respiration); or anabolic –
the building up (synthesis) of
compounds (such as proteins,
carbohydrates, lipids, and nucleic
acids). Usually, catabolism releases
energy, and anabolism consumes
energy.

22. ATP
• ATP + H2O → ADP + Pi + (−7.3 kcal/mol)
• ADP + Pi + energy ATP synthase ATP + H2O
• calorie =The calorie is a unit of energy defined as the amount of heat
needed to raise a quantity of water by one degree of temperature.
• 1 cal ( 4/184 joule)
• ATP + H 2O → AMP + PPi ΔG° = −45.6 kJ/mol (−10.9 kcal/mol)
ATPase
ΔG= ΔH-T ΔS

24. Oxidations and reductions
Oxidation : Loss of Electrons
Reduction: Gain of Electrons
Many redox reactions involve the breaking of a C-H bond and the
loss of two bonding electrons
Y + H O C
R
R
H
N
R
NH2
OH
+
Y H
R
NH2
O
R
R
O
HH
+ +

25. Reduction of NAD+ to NADH

26. Reduction of NADP+ to NADPH

27. Reduction of FAD to FADH2