1. Levels of Organization
Quarter 2 : Molecules to Organisms

2. Levels of Organization
Biological Levels of Organization
Atom
Molecule
Organelle
Cell
Tissue
Organ
System
Organism
Population
Community
Ecosystem
Biome
Biosphere

4. Atoms The basic unit of matter
(Matter = anything that has mass and takes up space)
There are three subatomic particles that are combined to make each atom.
* Proton (+)
* Neutron (o)
* Electron (-) move around nucleus in electron cloud
Nucleus (+)
Energy Levels
1st = 2
2nd = 8
3rd = 18

5. Molecules When two or more atoms are combined a molecule is formed
When two or more atoms of different elements combine a compound is formed (CO₂)

6. Be able to explain this statement
ALL COMPOUNDS ARE MOLECULES, BUT NOT ALL MOLECULES ARE COMPOUNDS!!!!!!
Be able to explain this statement

7. We can describe the composition of compounds by using a chemical formula
H₂O
(2 atoms of hydrogen, 1 atom of oxygen)
C₆H₁₂O₆ (6 carbon, 12 hydrogen, 6 oxygen)

8. Chemical Bonds Bonds : a force that holds atoms together
Covalent Bonds
Forms when atoms share electrons
Share 2 = single bond
Share 4 = double bond
Share 6 = triple bond
Ex: water

9. (different number of protons/electrons)
Ionic Bonds
a. Formed when atoms lose or gain electrons
b. Creates electrically charged atoms called ions
(different number of protons/electrons)
* if atom loses electron = + ion
* if atom gains electron = - ion
c. Ions with opposite charges are attracted to each other.

10. Hydrogen Bonds
a. Form when the positive end of one molecules is attracted to the negative end of another molecules
b. Form without the interaction of electrons
c. Responsible for the cohesion of water
*allows raindrops to form or water to bead
d. Easily broken

11. VI. Acids/Bases/pH
Acids – a solution with a high concentration of Hydrogen ions (H+)
B. Bases – a solution with a high concentration of hydroxide ions (OH-)
pH – means potential for hydrogen
pH can determine what type of organisms can live in an environment or what types of chemical reactions can take place

12. 2 H₂ + O₂ → 2 H₂O Balancing Equations
Steps to Solve Equation 1. write down elements on reactants side 2. write down elements on product side 3. write number of atoms for each element on each side 4. Begin adding coefficients to balance equation

13. ORGANIC CHEMISTRY
Organic chemistry is the study of compounds that contain bonds between carbon atoms
Carbon atoms have 4 valence electrons; therefore, each electron can join with electrons from another atom to form strong covalent bonds
Carbon can bond with:
* Hydrogen (H) * Phosphorus (P)
* Oxygen (O) * Carbon (C)
* Nitrogen (N) * Sulfur (S)

14. II. Organic Compounds Found in All Living Things
Carbohydrates
Lipids
Proteins
Nucleic acids

15. A. Carbohydrates Made up of C, H, and O in a 1 : 2 : 1 ratio Uses
Energy (quick)
Structural building blocks (cellulose – plant cell walls)
Sugars and Starches
Monosaccharides (one)
Disaccharides (two)
Polysaccharides (many)

16. Monosaccharides Simple sugar Chemical formula: C₆H₁₂O₆
Ex: Glucose, Fructose, and Galactose are 3 isomers of a monosaccharide
= molecules with same chemical formula
but different structure

17. Disaccharides A two-sugar molecule
When 2 carbohydrate monomers are joined, a hydrolysis reaction (removal of H₂O) takes place to form a disaccharide.
Chemical formula: C₁₂H₂₂O₁₁
Ex: glucose + galactose → Lactose
When disaccharides are used for energy, they are digested by enzymes that break them up into monosaccharides which are metabolized in the process of cellular respiration

18. Hydrolysis Reaction glucose + galactose → Lactose
(C₆H₁₂O₆) (C₆H₁₂O₆) (H₂O) = C₁₂H₂₂O₁₁
Monomer = a single unit/molecule
To digest lactose (sugar in dairy), you need lactase enzyme
Lactose intolerant people can’t produce lactase

19. Polysaccharides
Large macromolecules or polymers that can consist of hundreds or thousands of monomers (C₆H₁₀O₅)n
Starches (plant: corn & wheat)
a. Amylase (enzyme) breaks it down into monomers which are absorbed into the bloodstream to be used by the cells.
Glycogen (animal starches)
a. Stored in the liver and muscles when there is excess monosaccharides
Cellulose
a. Can not be digested = roughage

20. B. Lipids Made up mostly of C and H with some O Uses:
Energy – 2x the amount of chemical energy per gram compared to carbohydrates
Making biological membranes
Ex: plasma membrane in cells
Water proof coverings in plants
Physical & thermal insulation to animals

21. Lipids are generally insoluable in water
Formed when a glycerol molecule (C₃H₅O₃) joins a fatty acid
Saturated fats form when each carbon atom in the fatty acid chain is joined to another carbon atom by a single covalent bond
Solid at room temperature
Ex: butter

22. Unsaturated fats form when there is a least one
carbon-carbon double bond
liquid at room temperature
Olive oil
c. Polyunsaturated fats form when there are two or more carbon-carbon double bonds
Corn, sesame & peanut oil

23. Steroids are lipids whose C, H, and O atoms are arranged in rings
Estrogen, Androgen, Cholesterol

24. C. Proteins
1. Made up of C, H, O, and N
Uses:
a. Regulate cell processes and control reaction rates
b. Make up bulk of all solid material in the body (muscle, bone, skin, hair)
c. Transport substances in and out of cell

25. Proteins are polymers of amino acids
a. Amino acids are compounds with an amino group (NH₂) at
one end and a carboxyl group (COOH) at the other.
b. There are 20 different amino acids
c. Amino acids are joined together by peptide
bonds to form a dipeptide or a
polypeptide molecule

26. Enzymes are proteins that are formed during the process of protein synthesis
Enzymes are biological catalysts that control the rate of chemical reactions.
Each type of enzyme catalyzes only one type of reaction.
Names of enzymes usually end in –ase and are named for the reaction they catalyze.
Example: lactase → lactose
protease → protein

27. D. Nucleic Acids Made up of C, H, O, N, and P Uses:
a. Store and transmit genetic information
b. Make proteins
Made up of nucleotides
5 – Carbon sugar
Phosphate group
Nitrogenous base
4. Example: DNA and RNA