1. 01
Chapter 2
Lesson 1
Basic Chemistry

2. Matter anything that has mass and occupies space Examples: ? ?

3. Elements all of the atoms w/ the same atomic number
Living organisms require about 20 w/ C, H, O, and N making up more than 95% of the human body!
composed of atoms: the smallest stable unit of matter
chemical symbols (oral review)

4. Atomic Structure Atom Diagram WKST A
Concept Map
Atomic Structure
Atom Diagram
WKST A

5. Isotopes
forms of an element whose atoms contains the same # of protons (p+) but different numbers of neutrons ( n )
are distinguished by mass # : total # of p+ and n in the nucleus

6. Isotopes cont’
All isotopes of a particular element have the same number of e- and react chemically the same.
Therefore, any of the isotopes of oxygen can play the same role in an organism’s metabolic reactions.

7. Isotopes cont’ Unstable isotopes  aka: radioactive
Atomic fragments/energy
aka: atomic radiations
The three forms of atomic radiations are alpha (α) beta (β) & gamma (γ) which is the most penetrating.

8. Isotopes cont’
Half-life: time required for isotope to lose ½ of its radioactivity
Half-life of I days
P days
Co years
Ra years

9. Isotopes cont’ Uses: inflammatory disease
Radioactive substances can by introduced into and organism and traced as it enters into metabolic activities
Uses:
I-131 thyroid
Tl-201 heart conditions
Ga-67 certain cancers &
inflammatory disease
Co-60 cancer

10. Atomic Weight the average mass of an element’s atoms Carbon 12.01
Hydrogen 1.01
Oxygen 16.00
Nitrogen 14.01

11. Electron Shells The charge on atoms is neutral!
Chemical behavior of an atom results from the number of e- in the outer shell.
An atom with full outer shell of e- :
stable, inert, unreactive
An atom with an incomplete outer shell tends to react w/ other atoms
unstable, reactive

12. Bonding of Atoms
Chemical bond: connection between atoms after a reaction
produces molecules: chemical structures that contain more than one atom bonded together by shared e-
or compounds: any chemical substance made up of atoms of 2+ elements regardless of the type of bond joining them

13. Bonding of Atoms cont’
Electrically charged atoms and molecules are: ions
Cations = ion w/ positive charge
Anion = ion w/ negative charge
Most common in body fluids:
Na + Cl -
K + HCO3 -
Mg ++ HPO4 3-
Ca ++ SO4 2-

14. Types of Bonds
IONIC
:molecular bond created by attraction btw. ions w/ opposite charges
COVALENT
:a chemical bond btw. atoms that involves e- sharing
HYDROGEN
:weak interaction btw. H atom on one molecule and negatively charged portion of another molecule

15. WKST D: Ionic Bonds
WKST C: Covalent Bonds

17. Chemical Reactions
bonds form between atoms or existing bonds break btw. atoms
Reactants GO INTO a chemical reaction.
Products ARE PRODUCED. [come out of]
described using chemical shorthand or chemical notation ex. water H2O glucose C6H12O6
table salt NaCl oxygen O

18. WKST H: Chemical Reactions

19. Chemical Reactions cont’
Decomposition reaction involving the addition of a H2O molecule: hydrolysis
Cells can harness energy to power essential functions from the decomposition of complex molecules.
This process is catabolism

20. Chemical Reactions cont’
A reaction that is opposite of hydrolysis is dehydration synthesis aka: condensation
Catabolism supports the process of anabolism!

21. Chemical Reactions cont’
Acid-Base reactions are examples of exchange reactions in the body.
Reversible reactions are 2 reactions occurring at the same time
If balanced equilibrium

22. Enzymes
Activation energy is the amount of energy required to start a reaction.
Enzyme aka: catalyst: compounds that accelerate chemical reactions w/o being permanently changed in the reaction
Function: lower activation energy which in turn speeds up chemical reactions

23. Enzymes cont’
If energy released is greater than activation energy: exergonic
If more energy is required to begin the reaction than is released: endergonic
Enzymatic binding depends on shape of moleculed.

24. Figure 2-19
WKST R: Enzymes

25. Water and Physiological Systems
single most important constituent of the body
accounts for nearly 2/3 of body weight
Properties
Essential reactant
heat capacity: ability to absorb and retain heat
Excellent solvent

26. Acids, Bases, and pH
Acid: compound dissociates in solution releasing H+ ; pH & excess of H+
HCl  H Cl
Base: compound whose dissociation releases OH- or removes H+ from solution
OH- ions react quickly w/ H+ to form H2O
NaOH  Na OH-

27. Acids, Bases, and pH cont’
Salts: ionic compound consisting of any cation except H+ and any anion except OH-
Salts are examples of electrolytes!
Alterations in concentration can disturb almost every vital function!

28. Acids, Bases, and pH cont’
pH: expressed in moles/ L; solutions are acidic if below 7; basic if above 7 and neutral if 7
The difference in concentration per whole number on the scale is tenfold!
A solution with a pH of 6 has 10X the hydrogen ion concentration of a solution with a pH of 7

29. That should blow the cobwebs out of your brain!!

30. Coming Soon: to an Anatomy class near you
Biochemistry !