1. Matter Matters! Hydrogen Oxygen 1 proton 1 electron 8 protons
8 neutrons
8 electrons
Proton +
Neutron
Electron –

2. The Periodic Table K C N O Na Mg P S Ca

3. Interactions between atoms
Electrons are key!
chemical behavior of an atom depends on # valence electrons
What’s the magic number??

4. A little more on electrons…
What do you notice about the # of electrons in each element?
Elements in same row have same # shells & those in same column have same valence & chemical properties

5. Bonds to know… Little heat needed to break hydrogen bonds
attraction between + and –
hydrophobic & hydrophilic interactions
interaction with H2O
ionic bonds (transfer of electrons)
Van der Waals forces
Inter or intramolecular attractions (forces of millions of H2O molecules, Ar2, (HF2))
Sharing of electrons
covalent bonds(nonpolar, polar)

6. Van der Waal(sum of the attraction and repulsion forces between molecules)
Collectively, such interactions can be strong, as between molecules of a gecko’s toe hairs and a wall surface

7. Chemical reactions are the making and breaking of chemical bonds
The starting molecules of a chemical reaction are called reactants
The final molecules of a chemical reaction are called products
Chemical equilibrium is reached when the forward and reverse reaction rates are equal
Energy! & Reactions

8. What is Energy? capacity to do work/supply heat Many faces of energy:
Potential energy (EP) – stored
Kinetic energy (EK) – motion; aka thermal energy of molecular motion
amount of thermal energy in an object is its temperature

9. EP high EP transformed to EK Original EP transformed:
Mechanical energy breaks rocks
Heat; thermal energy increases rock temp
Sound
Same type of energy transfer occurs within atoms and drives reactions

10. LawS of Thermodynamics
First - Energy NEVER created or destroyed – changes form
Second – entropy always increases in an isolated system
**Entropy – amount of order, disorder, of
chaos in a system (∆S) Ex: “a neat room is more organized but less stable than a messy room, which is disorganized but more stable” (Mader page 106)

11. Spontaneity of Reactions
Spontaneous! – ONLY when products have ↓ EP than reactants AND products have ↑ entropy
Spontaneous nail rusting, wood burning
Nonspontaneous: recharging a battery
Spontaneous reactions are exergonic (exothermic); nonspontaneous rxns are endergonic (endothermic) – require LARGE amt of energy

12. Paired rxns that involve (-) or (+) of electrons
Redox reactions
Paired rxns that involve (-) or (+) of electrons
**Follow the H’s in living systems!**
Oxidation
Atom loses Electron
Remove H’s
Reduction
Atom gains Electron
Add H’s
LEO the lion goes GER!
o l x a l e
s e i i e d
e c d n c u
t i t c
r z r e
o e o
n n

13. Example: Cellular Respiration
Oxidation
Reduction
Glucose is oxidized (loss of electrons) and oxygen
is reduced (gains electrons)
C6H12O6 is high energy molecule and CO2 and H2O are
low energy which is why energy is released

14. Versatility of Carbon! 4 covalent bonds (to itself and other atoms)
single, double, triple bonds
Form straight and branched chains along with rings
Nearly endless variety & complexity
Can form polymers (protein, carbs, nucleic acids)

15. STRUCTURE DETERMINES FUNCTION!
Structural isomers
Effective
Enantiomer
Ineffective
Enantiomer
Drug
Condition
Pain;
inflammation
Ibuprofen
S-Ibuprofen
R-Ibuprofen
Albuterol
Asthma
R-Albuterol
S-Albuterol
STRUCTURE DETERMINES FUNCTION!

16. Functional Groups-they direct the chemical behavior of a compound
Has acidic properties
Acts as a base
Is polar and can form hydrogen bonds with H2O
Found in sugars
At end of carbon skeleton
Within carbon skeleton

17. Contributes a negative charge, can react with H2O releasing energy
2 groups can form cross-linking
Methyl (CH3) – can affect the expression of genes (attached to DNA)

19. Water, water, everywhere
H2O molecules form H-bonds with one another
+H attracted to –O
creates a sticky molecule

20. Elixir of Life Polarity allows for… 1. cohesion & adhesion
surface tension, capillary action
2. good solvent
many molecules dissolve in H2O
hydrophilic vs. hydrophobic
3. lower density as a solid
ice floats!
4. high specific heat
water stores heat
5. high heat of vaporization
heats & cools slowly

21. What’s the Water Property?
Direction
of water
movement

22. Two types of water-conducting cells
Figure 3.3
Adhesion
Two types of
water-conducting
cells
Cohesion
Direction
of water
movement
Figure 3.3 Water transport in plants.
300 m 22