1. The Chemical Basis of the Body
CHEMISTRY
The Chemical Basis of the Body

2. MATTER Anything that has mass and occupies space Solid - liquid - gas
Made up of ELEMENTS

3. Atoms
The smallest unit of Matter
Two basic parts
Nucleus
Electrons

4. Nucleus Protons (+ charge) Neutrons (uncharged)
# of protons = element’s Atomic Number
Neutrons (uncharged)
Charge of the Nucleus is +
Electrons - negatively charged particles-orbit around the nucleus
# of electrons always equals the # of protons in an atom

5. Elements
The building blocks of matter

6. Most Abundant Elements
There are 26 elements in the body
Most abundant are CHON
96% of total body mass
O2 is most abundant at 65%

7. Other Elements

8. Ions When an element loses or gains an electron
Potassium( K+) and Sodium(Na+) are important ions
Also called Cations (+ charged)
and Anions (- charged)

9. Electrolytes Ions in the fluids of the body
Essential to many processes in the body
Can be lost through fluid loss

10. Molecules
A molecule is formed when two or more atoms join together chemically. A compound is a molecule that contains at least two different elements. All compounds are molecules but not all molecules are compounds.
Hydrogen (H2), oxygen (O2) and nitrogen (N2) are molecules.
Water (H2O), carbon dioxide (CO2) and methane (CH4) are compounds because each is made from more than one element. 

11. Formed when electrons are Gained, Lost, or Shared
Chemical Bonding
Formed when electrons are Gained, Lost, or Shared

12. Ionic Bonding One loses and one gains an electron
Held together by their attraction
Strongest type of chemical bonding
Example: sodium (1) and chlorine (7)

13. Covalent Bonding The sharing of electron pairs
Single covalent bond = share one pair of electrons
Double covalent bond = share two pairs of electrons
Triple covalent bonds = share three pairs of electrons
Example: CO2, H20

14. Hydrogen Bonds Covalent bond with H and another element
Very weak bond (5%)
Easily broken
Example: water molecules and surface tension

15. Polar Bond Unequal sharing of electrons
Property of water that aids in movement of water

16. pH Describes acidity or alkalinity (basicity) of a solution
Number of H+ ions or OH- ions in solution
Biochemical reactions – sensitive to small changes
Salt is a + and – charged ion bonded together.

17. pH scale Ranging from 0-14. Acid-below 7 Base-above 7
A neutral substance has a pH of 7.0
Average pH of blood
7.35 to 7.45

18. Water in the Body Universal solvent Transports substances Lubricant
Absorbs and releases heat slowly
Aids in chemical reactions
Most important inorganic compound

19. Organic Compounds Contain Carbon, Hydrogen and Oxygen
Are large molecules
Form covalent bonds
Flammable

20. Inorganic Compounds Do not contain carbon Are small molecules
Usually form ionic bonds

21. Carbohydrates Formula is C6H12O6.
Structural units in DNA and cell membrane
MAJOR ENERGY SOURCE for the body.
ONLY energy source for brain and nerve cells.
Blood sugar is known as glucose

22. Lipids (FATS) Insoluble in water
Most common are triglycerides composed of glycerol and fatty acids.
Second source of energy
Protects body organs
Provides insulation and warmth
Absorbs fat soluble vitamins
Forms sex hormones and steroids

23. Proteins Building blocks called Amino Acids (20)
Structure of body tissues
Form enzymes which are catalysts
Antibodies
Regulate Osmotic pressure in the blood
Function as storage molecules

24. Nucleic Acids DNA (deoxyribonucleic acid) and RNA (ribonucleic acid).
Contain the atoms C,H,O,N AND P
DNA stores the genetic code on chromosomes
DNA and RNA assist with protein synthesis

25. Structure of RNA RNA is formed by a single strand of nucleotides
RNA can leave the nucleus
Helps make proteins
Transfers amino acids for proteins

26. Adenosine-TriPhosphate (ATP)
In all living systems
Drives all chemical reactions
Occurs through a process called cellular respiration
ATP + H20 <----> ADP + P + ENERGY
ATP is found in the Mitochondria

27. The End!