1. Monday August 15, 2016 Bell Ringer
Copy and answer the following:
What chemicals do you think are found in all organisms?

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The Chemistry of Life
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Water Foldable
PROPERTIES OF WATER BOOK
INSTRUCTIONS FOR MAKING A BOOK:
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Number the pages
Title page is the front page.
Page 1 is the back of the title page
Page 2 is the next page, then pages 3, 4, 5, 6
Page 7 is the back of the booklet
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5. Pages 1 and 7 Instructions
Write the Page Title SOLUTIONS AND SUSPENSIONS centered at the top of the page
Page 7
Write the Page Title, pH, centered at the top of the page
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Page 1 instructions
Make a bullet named SOLUTIONS
Copy the following questions, leaving room to answer them.
What are the two parts to a solution?
How are the two parts different?
How would you describe the ions in the solution?
Give two examples of solutions.
Make a bullet named SUSPENSIONS
How are suspensions different than solutions?
What are two examples of suspensions.
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Page 7 Instructions
Copy the following questions, leaving room to answer them.
What happens when a water molecule dissociates?
What is an acid?
What is a base?
What does the pH scale measure?
Draw the pH scale.
acid neutral base
acidic alkaline 14
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Properties of Water
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The Water Molecule
Neutral Charge – ZERO
Have no charge
Have an Equal number of p+ and e-
Charges aren’t evenly distributed
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The Water Molecule
Polarity
A water molecule is polar because there is an uneven distribution of electrons between the oxygen and hydrogen atoms.
(-)
(+)
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Hydrogen Bonds
Polar water molecules act like magnets and attract each other
Hydrogen Bonds
The attraction of the Hydrogen end (+) of one molecule for the Oxygen end (-) of another water molecule.
They are strong bonds that form between molecules (CO2, H2O, …)
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Hydrogen Bonds
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Cohesion
The attraction between molecules of the same substance (e.g. water).
H2O attracting other H2O molecules
Allows some insects and spiders to walk on water.
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14. Adhesion & Capillarity
Adhesion - Attraction between H2O molecules and different molecules
Cohesion & adhesion produce Capillarity (upward movement against gravity of water through small tubes)
Question: How do plants make use of Capillarity?
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15. Solutions & Suspensions
Water is usually part of a mixture.
Because so many things dissolve in water, it is called the Universal Solvent
There are two types of mixtures:
Solutions
Suspensions
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16. Properties of Solutions
Ionic compounds disperse as ions in water (+ions & -ions spread out among polar water molecules)
Solutions are Evenly distributed mixtures
SOLUTE
Substance that is being dissolved
SOLVENT
Dissolving Substance for the solute
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Ionic Solutions
Na+ ions will be attracted to WHAT END of the water molecule?
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Suspensions
Substances that don’t dissolve but separate into tiny pieces.
Water keeps the pieces suspended so they don’t settle out.
Blood & Cytoplasm are suspensions
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Acids, Bases & pH
1 water molecule in 550 million naturally dissociates into a Hydrogen Ion and a Hydroxide Ion
Hydrogen Ion Hydroxide Ion
Acid Base
H2O  H+ + OH-
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20. How much stronger is a pH3 than a pH of 5?
The pH Scale
Indicates the concentration of H+ ions
Ranges from 0 – 14
pH of 7 is neutral
pH 0 up to 7  acid … H+
pH above 7 to 14  base… OH-
Each pH unit represents a factor of 10X change in concentration
How much stronger is a pH3 than a pH of 5?
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Acids
Strong Acid = pH 1-3
High in H+ ions
Lower number of OH- ions
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Bases
Strong Base = pH 11 – 14
High in OH-ions
Lower in number of H+ ions
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23. Bell Ringer 8/19/16:
Use the information from the graphs to answer the
questions.

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Macromolecules
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26. Monday August 22, 2016 Bell Ringer
Copy and answer the following: 1. What are the four macromolecules that we are studying? 2. What property of water molecules makes water have surface tension?
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Carbon (C)
Carbon has 4 electrons in outer shell.
Carbon can form covalent bonds with as many as 4 other atoms (elements).
Usually with C, H, O or N.
Example: CH4(methane)
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Organic Compounds
Compounds that contain CARBON are called organic.
Macromolecules are large organic molecules.
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Macromolecules
Large organic molecules.
Also called POLYMERS.
Made up of smaller “building blocks” called MONOMERS.
Examples:
1. Carbohydrates
2. Lipids
3. Proteins
4. Nucleic acids (DNA and RNA)
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Carbohydrates
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Carbohydrates
Small sugar molecules to large sugar molecules.
Examples:
A. monosaccharide
B. disaccharide
C. polysaccharide
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Carbohydrates
Monosaccharide: one sugar unit
Examples: glucose (C6H12O6)
deoxyribose
ribose
Fructose
Galactose
glucose
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Carbohydrates
Disaccharide: two sugar unit
Examples:
Sucrose (glucose+fructose)
Lactose (glucose+galactose)
Maltose (glucose+glucose)
glucose
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Carbohydrates
Polysaccharide: many sugar units
Examples: starch (bread, potatoes)
glycogen (beef muscle)
cellulose (lettuce, corn)
glucose
cellulose
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35. Tuesday August 23, 2016 Bell Ringer
Copy the following graphic organizer:

36. Wednesday August 24, 2016 Bell Ringer
Copy the following definitions:
Isomerism- two molecules share the same formula, but have different structures
Dehydration Synthesis- process where a molecule of water is lost when forming molecules
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Lipids
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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
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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)
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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 =
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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
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Proteins
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43. 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
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44. Proteins (Polypeptides)
Four levels of protein structure:
A. Primary Structure
B. Secondary Structure
C. Tertiary Structure
D. Quaternary Structure
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Primary Structure
Amino acids bonded together by peptide bonds (straight chains)
aa1
aa2
aa3
aa4
aa5
aa6
Peptide Bonds
Amino Acids (aa)
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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
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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)
Called a “subunit”.
Alpha Helix
Beta Pleated Sheet
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Quaternary Structure
Composed of 2 or more “subunits”
Globular in shape
Form in Aqueous environments
Example: hemoglobin
subunits
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Nucleic Acids
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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.
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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)
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Nucleotide O
O=P-O
Phosphate
Group N
Nitrogenous base
(A, G, C, or T)
CH2 O C1 C4 C3 C2 5
Sugar
(deoxyribose)
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DNA - double helix P O 1 2 3 4 5 P O 1 2 3 4 5 G C T A
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