1. Biochemistry

2. Biochemistry is the study of the molecules of life.
What materials actually comprise the “building blocks of life”?

3. I. Matter
Everything in the universe exists as either matter or energy.

4. A. Energy = the capacity to do work.
This is what allows changes in matter to happen!
Examples: Sound, light, heat

5. A. Energy (cont’d)
Energy can be stored (Potential) – roller coaster at the top of a hill
Energy can be in action (kinetic) – roller coaster moving down a hill

6. B. Matter = anything that has mass and takes up space
1. Matter exists in 4 states: solid, liquid, gas, and plasma (a high temperature gas-like state on stars)

7. B. Matter 2. Atoms
2. The smallest unit of matter is the atom. There are approximately 110+ types of atom (we call them elements) which we are aware of on earth. Atoms are composed of smaller, subatomic particles

8. 2. Atoms (cont’d)
Draw a Bohrs Diagram of a carbon atom

9. 2. Atoms (cont’d) Charge Mass Proton +1 1 amu
= atomic #/# electrons when neutral
B. Neutron
0 (Neutral)
Neutrons + protons = mass
C. Electron -1
0 (Insignificant)

10. 2. Atoms (cont’d)
It is the electrons which determine how atoms bond to form compounds (with new properties). They occupy “levels” or “shells”, sometimes even called orbitals.
They “fill” orbitals in this order: 2, 8, 8, … and like to travel in pairs. The “outermost” electrons (available for bonds) are called valence electrons.
Atoms prefer to have 8 electrons in their outer orbitals, even if it means they gain a charge.

11. 2. Atoms (cont’d)
Ionic Bond – Electrons are transferred from one atom to another. (example: NaCl, sodium chloride… salt!)

12. 2. Atoms (cont’d)
Covalent Bond – Electrons are shared between atoms. (Example: H20, sugar)
Water is called the Mickey Mouse molecule. It is polar, meaning electrons are not shared evenly.
Draw a water molecule including Protons, neutrons, electrons, and location of charges.

13. 2. Atoms (cont’d)
Hydrogen Bond (example: what holds the rungs of DNA together; what holds water molecules together in a crop…) These are weaker than ionic and covalent bonds.

14. 3. Atoms have special forms, under certain circumstances:
A. Ions – atoms with a charge (gained or lost electrons)
B. Isotopes – Atoms of the same element with a different number of neutrons and therefore different mass.
Draw the diagrams for carbon-12 and carbon-14.

15. 4. A simple look at the way atoms may combine
Atoms represented by elements; chemically combine -> molecules, which is the basic unit of a compound (ex. H2O).
Atoms and molecules may also physically mix (ex. Saltwater)

16. 4. Atoms combine (cont’d)
Two mixtures involving water are:
1. Solutions – a solute (sugar or Kool-Aid) is dissolved in water (which is known as the universal solvent).
2. Suspensions – particles of a substance do not dissolve, but as so small they remain suspended between the molecules of another substance.
Water promotes the circulation, secretion, and excretion of essential substances throughout an organism.

17. 5. We can show the structure of molecules using:
A. Molecular (chemical) formulas – ingredients (H2O)
B Structural formulas – arrangement of atoms

18. 6. Some molecules have an uneven distribution of charge
(water, for example); they are polar.
When these molecules are attracted and held to each other, this is called cohesion.
When molecules of different substances are attracted to each other, this is called adhesion.

19. 7. Building and breaking down molecules:
A. Why must we learn this stuff? Protoplasm, all the stuff that collectively makes cells, is constantly building and breaking apart life’s molecules!
B. Dehydration Synthesis – removing water to put two molecules together.
This is used to build complex carbohydrates, proteins, and lipids (fats).

20. 7. Building/breaking molecules (con’t)
Example: Dehydration Synthesis
Glucose Glucose → Maltose Water
C6H12O C6H12O → C12H22O H2O

21. 7. Building/breaking molecules (con’t)
C. Hydrolysis – adding water to split molecules
Example: Hydrolysis
Maltose Water --→ Glucose Glucose
C12H22O H2O → C6H12O C6H12O6