1. Seminar Seven Introduction to Chemistry

2. Importance of Chemicals Chemicals are responsible for directing virtually all of our bodily functions. It is important to understand the basic chemical reactions that occur in the body. It is important to understand the basic concepts of biochemistry.

3. Atoms and their components Protons Electrons Neutrons Atom = a unit of matter that makes up a chemical element.

4. Terms Nucleus= at the core of each atom Atomic number = # of protons in nucleus of atom Atomic mass = # of protons and neutrons combined.

5. Elements An element is a substance that is composed of only one kind of atom. Elements are represented by symbols. (i.e. periodic table) Do an internet search for the periodic table

6. Question? Which elements are important to our bodies?

7. Carbon = C Nitrogen = N Oxygen = O Phosphorus = P Sodium = Na Hydrogen = H Iodine = I Chlorine = Cl Calcium = Ca

8. From simple to complex Elements = a pure substance Molecules = a group of atoms bound together Compound = substances whose molecules have more than one kind of atom

9. Question? What are the two different ways compounds are formed?

10. Bonding Ionic bonding occurs when one or more electrons are transferred from one atom to another. Pg. 24 i.e. NaCL = sodium chloride Covalent bonds are formed when two atoms share a pair of electrons. Pg. 25 i.e. H 2

11. Bonding ioniccovalent

12. A question for you! What is the primary difference between organic and inorganic compounds?

13. Answer ! Inorganic compounds do not contain carbon- carbon bonds or carbon-hydrogen bonds. [water and some acids, bases, and salts] Organic compounds contain carbon and include carbon-carbon bonds and/or carbon- hydrogen bonds. The human body has both types of compounds!

14. Inorganic compounds Water Water is a solvent (liquid into which solutes are dissolved), forming aqueous solutions in the body Water is involved in chemical reactions Dehydration synthesis (water removed) Hydrolysis ( water added)

15. Inorganic compounds Acids, bases, and salts Water molecules dissociate to form equal amounts of H + (hydrogen ion) and OH – (hydroxide ion) Acid—substance that shifts the H + /OH – balance in favor of H + ; opposite of base Base—substance that shifts the H + /OH – balance against H + ; also known as an alkaline; opposite of acid

16. Acid-Base Balance

17. pH number that indicates the hydrogen ion (H + ) concentration of a fluid pH 7.0 = neutral higher than 7.0 = alkalinity less than 7.0 = acidity

18. 7 Neutral 0 14 AcidsAlkalines(Bases) Normal Human Blood 7.35-7.45 Normal Urine 6.0 Normal stomach acid 1.0

19. pH levels Zwieback 4.84 - 4.94 Watermelon 5.18 - 5.60 Orange, Juice Florida 3.30 - 4.15 Cranberry Juice, canned 2.30 - 2.52 Conch 7.52 - 8.40 Where on the scale would stomach acid be?

20. pH of vomit! Why such a strong acid in stomach?

21. Organic Chemistry More complex than inorganic! Major types found in body: Carbohydrates Lipids Proteins Nucleic acids

22. Questions?