1. Atoms Atoms are the basic unit of matter
Atoms are composed of protons, neutrons and electrons
These subatomic particles are charged….

2. Atoms make elements… Elements can’t be broken down into anything simpler.
Examples:
Carbon= C
Sodium = Na
Hydrogen= H
Nitrogen= N

3. Subatomic particles have specific locations…
Protons and the neutrons are found in the nucleus of the atom and electrons whizz around the outside of the nucleus
Electrons are always moving.
The atomic shell or orbital is the distance from the nucleus that the electron spins.

4. Valence shells… The outermost shell is called the valence shell.
To be “happy” and full, the valence shell must have 8 electrons.
The electrons in the outermost shell are the only ones that react with other atoms. If the valence shell is full, the atom does not react.
Carbon only has four valence electrons (8 is the max) so carbon can bond with up to four other atoms.

5. Ions A normal atom is neutral (same number of electrons and protons)
Ions have a different number of electrons than the neutral atom
Sodium has only one valence electron… it would like to give that up so it can have a full outer shell.
Chloride needs one electron to have a full outer shell.
Sodium loses an electron and becomes Na+
Chloride becomes negative when it gains an electron… Cl-

6. Bonding= trying to be a happy, FULL atom
Some atoms can easily lose electrons to be full
Some atoms can easily gain electrons to become full

8. Ionic bonds A good example of an ionic bond is NaCl.
Sodium really wants to lose an electron and becomes a positive ion (cation).
Chloride really wants to gain an electron (high electronegativity) and becomes a negative ion (anion).

9. Covalent bonds
If the two atoms have partially fill shells then the two atoms will probably just share the electrons. A good example of this methane

10. More covalent examples

11. Polar Covalent Bonds
Polar Covalent means that two atoms share electrons but the electrons may spend a majority of their time with one particular atom. (joint custody)
An example: WATER

12. Hydrogen Bonds
The hydrogen ends of water are slightly positive because the electrons spend most of their time with oxygen.
This means that the H’s are attracted to the O’s of other water molecules. The dotted lines show hydrogen bonds forming.
Hydrogen bonds form in other molecules like DNA

14. MACROMOLECULES important to living things!
_____________
Carbohydrates
Lipids- fats, oils, waxes steroids
Proteins
Nucleic acids

15. Introductory Terms Macromolecule = “giant” molecule of living matter
Monomer = subunits that are the building blocks of a polymer
Example: Lego block
Polymer = monomers linked together
Example: Lego castle

16. Macromolecular Reactions 
Dehydration Synthesis:
2 monomers become bonded to each other to make a polymer
Lose water
Hydrolysis:
Water is used to break up polymers into monomers
Using water to break bonds

17. Carbohydrates Structure: Functions: C:H:O in a 1:2:1 Ratio
Example: C6H12O6 which is glucose
Functions:
Short-term energy-
-Pasta dinner before the big race, game, etc.
Structural Support

18. Lipids Structure: Functions:
Made up of carbon, hydrogen, and a few oxygens
Do not dissolve in water
Functions:
Long-term energy storage
Chemical messengers (hormones)
Insulation around your nerve cells and to keep you warm!
Waxes (plant leaves to prevent water loss)

19. Lipids-Triglycerides
Fats
Made of glycerol and 3 fatty acids tails
Connect via dehydration synthesis to make triglycerides
Triglycerides are fat molecules… clogging arteries…

21. ___________________ (lipid tails + glycerol/phosphate head)
PHOSPHOLIPIDS
___________________ (lipid tails + glycerol/phosphate head)
Polar head
Non-polar
tails

22. Lipids Steroids Made up of 4 interconnected rings Examples:
Cholesterol
Testosterone
Estrogen

23. Proteins Most of a cell is made up of proteins
Instrumental in almost everything organisms do
Structure:
All proteins are created from unique combinations of 20 different amino acids
C,H,O,N (S)
Major Functions:
Structure
Defense (antibodies)
Enzymes- we will discuss these later!

24. Proteins Amino Acids Amino acids are the monomers of proteins
Organic molecules possessing both carboxyl and amino groups ( get it AMINO…. ACID)
20 types of AAs that make up 1000s of different proteins
AAs are linked together by peptide bonds to make polypeptides

26. Proteins Denaturation:
When pH, salt concentration, temperature, and/or other environmental factors are altered, the protein may unravel and lose its shape
Biologically inactive
Structure + function

27. Nucleic Acids Structure Made of a chain of Nucleotides
Nucleotides are made of a sugar, a phosphate and a nitrogen base
Function
Carries genetic material from one generation to the next
Builds RNA and DNA

28. NUCLEOTIDES
2 SUGARS can be used:
DEOXYRIBOSE for DNA
RIBOSE for RNA

29. 5 NITROGEN BASES Adenine= A Guanine= G Cytosine= C
Thymine = T (only in DNA)
Uracil= U (only in RNA)
A,G= Purines
C,T,U= pyrimidines

31. RNA vs. DNA RNA DNA Sugar is ribose Contains Uracil not Thymine
Single stranded
DNA
Sugar is Deoxyribose
Contains A,T, C, G
Double stranded

32. ONE SPECIAL KIND of NUCLEOTIDE is used by cells to store and transport energy!
ATP
Sugar =_____________
Nitrogen base =__________
+___ PHOSPHATE groups
That’s why it is called adenosine triphosphate
RIBOSE
ADENINE 3

33. When you use up energy or ATP…

34. ATP ADP Cycle
So, ATP has three phosphates but energy is released when ATP turns to ADP by losing a phosphate
Hydrolysis
Cycles back and forth

35. Cohesion Water sticks to water (hydrogen bonds)
Helps plants transport water through vessels

36. Adhesion Water sticks to other molecules (like the side of a glass)
Also helps keep water moving up against gravity in plants.

37. Surface Tension Related to cohesion
Molecules resist being pulled apart due to strong hydrogen bonds… form a “film”

38. Density Why can’t you fill a water bottle completely when you want to freeze it?
What occurs to the structure of water when it freezes?
Insulation for life below the surface…

39. pH Scale- ever heard of it?
An acid is a compound that releases protons (H+) when dissolved in water
A base is a compound that adds OH- when dissolves in water.
We measure the these reactions on the pH scale

40. The pH Scale- ranges from 0-14
pH of 1 means lots of H+ ions and SUPER ACIDIC
pH of 14 means lots of OH- (or low H+) and SUPER BASIC
Water is neutral with a pH of 7

42. Enzymes are special proteins