1. What makes up everything in the universe?
2. Name 2 properties of all matter.  
3. Define mass.  
4. How does weight differ from mass?  
5.What are elements?  
6. Name the 4 elements that make up most of a living thing.  
7. What is used to represent an element?  
Matter
Volume and Mass
Quantity of matter an object has
Weight is the pull of gravity on an object
Pure substances that cannot be broken down into simpler kinds of matter
C – H – O – N
Chemical SYMBOL (1 or 2 letters)

2. Nucleus & Energy levels Center & Contains protons & neutrons
8. Name the smallest part of an element.
9. What are the 2 main regions of an atom?  
10. Where is the nucleus of an atom found and what does it contain?  
11. What is the charge on a proton? 
A neutron?  
12. All atoms of the same element have the ________ number of protons.
13. The number of protons in an atom determines the __________________.  
14. What is the charge on an electron?  
Atom
Nucleus & Energy levels
Center & Contains protons & neutrons +
Neutral
same
Atomic # _

3. 15. If you know the number of protons in an atom, how can you determine the number of electrons?  
16. Do all the atoms of the same element have the same number of neutrons?  
17. Atoms of the same element with different numbers of neutrons are called ___________.  
18. The mass of an atom is centered in the ___________.  
19. The number of protons PLUS neutrons in an atom determines its ___________________.  
20. What atomic particle has a negative charge?  
Usually equal No
Isotopes
Nucleus
Atomic Mass
Electrons

4. 22. Where are electrons found?
21. Why isn’t the mass of an electron used to determine the atomic mass of an element?
22. Where are electrons found?
23. Which electrons in an atom have the most energy?  
24. How many energy levels are there & name them?  
25. How many electrons will each energy level hold?  
26. Elements are arranged on a __________________ by their atomic _____________.  
27. What are Periods & what do they tell you about elements?  
28.What are Families & what do they tell you about elements?  
e- have little to no mass
Energy levels
e- in the outer levels
(7) - K – L – M – N – O - P - Q
2(n2) (n=energy level) K-2; L-8; M-18; etc.
Periodic Table #
Rows - # of energy levels
Columns – Valence electrons

5. 29. Two or more elements combined together make a _____________.  
30. Chemical ______________ represent compounds.  
31. _____________ are the smallest part of a compound.  
32. ______________ in chemical formulas tell the number of atoms of each element.  
33. _____________ in a formula tell the number of molecules.  
34. Compounds have ____________ properties than its elements.  
35.  The outermost _______________ in elements determine if they will combine.  
36. Elements with ___________ outer energy levels are stable & won’t react.  
Chemical compound
Formulas
Molecules
Subscripts
Coefficients
Different
Energy
“Full” 2 or 8 e-

6. Chemical Bonds
Ionic
Covalent
NH4
H20
NaCl
KCl
Sharing valence electrons
Single, double or triple bonds can occur
Very strong
Transferring valence electrons
Creates ions (charged particles) that are attracted to each other
Van der Waals (forces)
Attraction between whole molecules
H-bonds are van der Waals attraction between H and other molecules.

7. (breaking down glucose)
Ch.3
Energy in Reactions
Exothermic
Endothermic
Cellular Respiration
(breaking down glucose)
Photosynthesis
(creating glucose)

8. -ASE Enzymes Act as a catalyst Lower the activation energy
2. Are not used up or changed during a reaction
3. Are sensitive to changes in heat & pH
4. Work for only one specific reaction
Enzyme animation

9. Ice is less dense than liquid water
AMAZING WATER!!
Water is fundamental to all life on Earth
The Properties of Water:
Polar molecule
“Universal Solvent”
Ice is less dense than liquid water
Surface Tension
Adhesion (other)
Cohesion (self)

10. Non-polar particles eventually settle out of solution
Mixtures with Water
Homogeneous
Heterogeneous
Suspensions
Colloids
Solutions
Non-polar particles eventually settle out of solution
Non-polar particles do not settle out of solution
Solute
Solvent
Polar molecules dissociate in water (form ions)
Paint
Ink
Milk

11. ACIDS BASES Mixtures with Water pH – measure of H+ ions in solution
Some solutes release H+ ions into solution
ACIDS
Some solutes release OH- (hydroxide) ions into solution
BASES
pH Scale
Acidic
H+ = OH-
Basic (Alkaline)
H+ > OH-
OH- > H+

12. Organic Chemistry

13. -determines some properties and reactions of that class of molecule.
Organic Chemistry
Functional Groups
-determines some properties and reactions of that class of molecule.
*Functional groups will undergo the same type of reactions regardless of the compound of which they are a part
*Functional groups can be used to distinguish similar compounds from each other.
Acetic Acid
Ethanol

14. Organic Chemistry
Functional
Group
Formula
Example
Alcohols
Hydroxyl
R-OH
Carbonyl
R - C
= O
- H
Aldehydes
R –C–R
= O
Ketones
R - C
= O
- OH
R - C
= O
- O
Carboxylic
Acid
Carboxyl

15. Organic Chemistry Group Formula Example
Functional
Group
Formula
Example
R-N
- H
R-N
- H
Amino
Acids
Amino
Sulfhydryl
R-SH
Thiols
Phosphate
R-O-P-O -O O=
Organic
Phosphates

16. Organic Chemistry 3. Identify Which group(s) What group is do you see?
boxed in?
Which group(s)
do you see?
Ketone
Carboxyl
Aldehyde
Amino
5. Which group(s)
do you see?
RNA
4. Which group(s)
do you see?
Amino
Phosphate
Carboxyl
Hydroxyl

17. Biological Macromolecules
Polymers
Monomers
H2O
Condensation
Reaction
Carbohydrates
Monosaccharides
Fatty Acids & Glycerol
(Dehydration
Synthesis)
Lipids
H2O
Hydrolysis
Proteins
Amino Acids
Nucleic Acids
Nucleotides

18. Biological Macromolecules
Amino Acids
Polypeptide
Hydrolysis/enzyme animation

19. Carbohydrates

20. Carbohydrates Small sugar molecules to large sugar molecules.
Examples:
A. monosaccharide
B. disaccharide
C. polysaccharide

21. Carbohydrates Monosaccharide: one sugar unit
Examples: glucose (C6H12O6)
deoxyribose
ribose
Fructose
Galactose
glucose

22. Carbohydrates Disaccharide: two sugar unit Examples:
Sucrose (glucose+fructose)
Lactose (glucose+galactose)
Maltose (glucose+glucose)
glucose

23. Carbohydrates Polysaccharide: many sugar units
Examples: starch (bread, potatoes)
glycogen (beef muscle)
cellulose (lettuce, corn)
glucose
cellulose

24. Lipids

25. Lipids General term for compounds which are not soluble in water.
Lipids are soluble in hydrophobic solvents.
Remember: “stores the most energy”
Examples: 1. Fats
2. Phospholipids
3. Oils
4. Waxes
5. Steroid hormones
6. Triglycerides

26. Lipids Six functions of lipids: 1. Long term energy storage
2. Protection against heat loss (insulation)
3. Protection against physical shock
4. Protection against water loss
5. Chemical messengers (hormones)
6. Major component of membranes (phospholipids)

27. Lipids Triglycerides: composed of 1 glycerol and 3 fatty acids. = =H
H-C----O
glycerol O
C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3 = O
C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3 =
fatty acids O
C-CH2-CH2-CH2-CH
=CH-CH2-CH2-CH2-CH2-CH3 =

28. C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3
Fatty Acids
There are two kinds of fatty acids you may see these on food labels:
1. Saturated fatty acids: no double bonds (bad)
2. Unsaturated fatty acids: double bonds (good) O
C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3 =
saturated O
C-CH2-CH2-CH2-CH
=CH-CH2-CH2-CH2-CH2-CH3 =
unsaturated

29. Proteins

30. Proteins (Polypeptides)
Amino acids (20 different kinds of aa) bonded together by peptide bonds (polypeptides).
Six functions of proteins:
1. Storage: albumin (egg white)
2. Transport: hemoglobin
3. Regulatory: hormones
4. Movement: muscles
5. Structural: membranes, hair, nails
6. Enzymes: cellular reactions

31. Proteins (Polypeptides)
Four levels of protein structure:
A. Primary Structure
B. Secondary Structure
C. Tertiary Structure
D. Quaternary Structure

32. Primary Structure
Amino acids bonded together by peptide bonds (straight chains)
aa1
aa2
aa3
aa4
aa5
aa6
Peptide Bonds
Amino Acids (aa)

33. Secondary Structure
3-dimensional folding arrangement of a primary structure into coils and pleats held together by hydrogen bonds.
Two examples:
Alpha Helix
Beta Pleated Sheet
Hydrogen Bonds

34. Tertiary Structure
Secondary structures bent and folded into a more complex 3-D arrangement of linked polypeptides
Bonds: H-bonds, ionic, disulfide bridges (S-S)
Call a “subunit”.
Alpha Helix
Beta Pleated Sheet

35. Quaternary Structure Composed of 2 or more “subunits”
Globular in shape
Form in Aqueous environments
Example: enzymes (hemoglobin)
subunits

36. Nucleic Acids

37. Nucleic acids Two types: a. Deoxyribonucleic acid (DNA- double helix)
b. Ribonucleic acid (RNA-single strand)
Nucleic acids are composed of long chains of nucleotides linked by dehydration synthesis.

38. Nucleic acids Nucleotides include: phosphate group
pentose sugar (5-carbon)
nitrogenous bases:
adenine (A)
thymine (T) DNA only
uracil (U) RNA only
cytosine (C)
guanine (G)

39. Nucleotide O O=P-O Phosphate Group N Nitrogenous base (A, G, C, or T)
CH2 O C1 C4 C3 C2 5
Sugar
(deoxyribose)

40. DNA - double helix P O 1 2 3 4 5 P O 1 2 3 4 5 G C T A

41. C, O & H in straight chains or chains of rings
Carbohydrates
C, O & H in straight chains or chains of rings
Lipids
C, O & H
Fatty acids held together by a glycerol or rings and chains

42. Proteins Nucleic Acids
(Amino Acids)
Look for an Amino group and carboxyl group
Nucleic Acids
(Nucleotides)
Look for a sugar ring, phosphate, and amino group