Transcript Macromolecules

Macromolecules
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Carbon (C)
• Carbon has 4 valence electrons (bonding
e- in highest energy level)
• Carbon can form covalent bonds with as
many as 4 other atoms.
– 4 Bonds may be single bonds, usually
with C, H, O or N.
– Carbon can also form double and
triple bonds
– Phosphorus and Sulfur will also be in
the bonds to the Oxygen and Carbons2
Macromolecules
• ORGANIC Compounds are carbon
based.
• Macromolecules are LARGE
organic molecules.
• Are also called POLYMERS made
from smaller “building blocks”
called MONOMERS
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Question:
How Are
Macromolecules
Formed?
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ANSWER: Remove WATER
• This process is called
dehydration synthesis which
means to put together by
removing water.
• Remove the hydroxyl ( –OH)
group off of one monomer
• Remove a hydrogen off of
the second monomer
• H with the OH makes H2O
Chemical Reactions
• Chemical Bonds are broken and new Bonds
are formed to form the Macromolecules
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http://cnx.org/content/m47185/latest/
+ H 2O
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Question:
How are
Macromolecules
separated and
digested?
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Answer: Hydrolysis
• Hydro “Water”, Lyse “to break”
– To break apart using water
• Separates polymers by “adding
water”
HO
HO
H
H
H2O
HO
H
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Carbohydrates
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Carbohydrates
• Small and large sugar molecules.
• Function: The main source of energy
for cellular work
• Format: Composed of C, H, and O
where Hydrogen to Oxygen Ratio is 2:1
• Suffix “ose”
Examples: monosaccharides (simplest
sugars), disaccharides, polysaccharides
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Carbohydrates
Monosaccharides these are one
sugar unit
Example: glucose
glucose
Disaccharide: two sugar unit
Example:
glucose
glucose
Sucrose (glucose+fructose)
Maltose (glucose + glucose)
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Carbohydrates
Polysaccharides: many sugar units
Examples:starch (plant’s energy storage)
glycogen (in liver & muscles)
cellulose (plant walls)
glucose
glucose
glucose
glucose
cellulose
glucose
glucose
glucose
glucose
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Example Forming Sucrose
• Balanced Equation
C6H12O6 + C6H12O6
|
glucose
 C12H22O11 + H2O
|
fructose
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ISOMERS – Same Formula, Different
structures due to bonding locations
http://www.elmhurst.edu/~chm/vchembook
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Lipids
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Lipids
• Are nonpolar fats and oils that are not
soluble in water.
• Lipids are soluble in nonpolar solvents which
are hydrophobic solvents which are“water
fearing”
• Format: Composed of C, H, and O but
formula has a greater than 2:1 hydrogen to
oxygen ratio
• Example: C18H36O2
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Major Function of a Lipid
• Major Function: stores energy for long
term
• Examples: Fats, Phospholipids, Oils,
Waxes, Steroid hormones,
Triglycerides
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Lipids
Other Functions of lipids:
1. Long term energy storage
2. insulation
3. cushions organs
4. Chemical messengers (hormones)
5. Major component of membranes
(phospholipids)
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Lipids
Triglycerides:
composed of 1 glycerol and 3
fatty acids.
H
O
H-C----O C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3
O
H-C----O C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3
O
fatty acids
H-C----O C-CH -CH -CH -CH
2
2
2
H
glycerol
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Omega-3 Fatty Acid
Fatty Acids
There are two kinds of fatty acids. (You have
seen these on food labels)
1. Saturated fatty acids: no Carbon to
Carbon double bonds (C=C), carbon is
saturated with hydrogens (bad – solids at
room temp come from ANIMALS)
2. Unsaturated fatty acids: double bonds
between the carbons, so less hydrogens in
the structure (better for your health, liquids
at room temp come from PLANTS)
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Check out the Single vs. Double
bonds…
http://biology.clc.uc.edu/courses/bio104/lipids.htm
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http://biology.clc.uc.edu/courses/bio104/lipids.htm
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Proteins
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Proteins
• Monomer of Proteins are the Amino Acids (20
different kinds of AA)
• AA bond together by peptide bonds
– Attachment is a Carbon to Nitrogen single bond.
• Format: All Contain C, H, O, N some have S.
Contain amino (-NH2) and carboxyl
(–COOH) functional groups.
• Dehydration synthesis removes the H from the
amino group and the OH from the carboxyl
group.
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http://hyperphysics.phy-astr.gsu.edu
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Functions of Proteins
Functions of proteins:
Enzymes: speed up reactions
Aid in Transportation in and out of cell.
Regulates hormones (For example: insulin)
Aid in Movement (controls actions in muscles)
Defense: antibodies of the immune system
Structures of membranes, hair, nails
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Proteins
• Common suffix -ase
• Amylase, protease,
isomerase, ligase, others:
trypsin, pepsin
• Optimal temperature and
pH required for proper
enzyme (protein) function
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Enzymes Speed Up Reactions
http://www.cikguhafiz.com/v1/webcikguhafiz
/images/kuiz/enzyme2.png
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Denaturing Destroys
the Protein
• Too hot, too acidic, too basic
ruins the active site for the
protein.
• Activity graph show a drop
off in rate.
• Go back to previous graph,
where does the enzyme
denature?
• http://highered.mheducation.com/sites/
0072943696/student_view0/chapter2/an
imation__protein_denaturation.html
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Nucleic
Acids
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Nucleic acids
• Two types:
a. Deoxyribonucleic acid (DNAdouble helix)
b. Ribonucleic acid (RNA-single
strand)
• Nucleic acids are composed of long chains of
nucleotides linked by dehydration synthesis.
• Function: genetic programming
• Formula Format: C, H, N, O, and now P
(Phosphorus)
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Nucleic acids
• Monomer is a Nucleotide
– Which includes the following three things:
phosphate group
pentose sugar (5-carbon)
Deoxyribose in DNA
Ribose in RNA
nitrogenous bases:
adenine (A), thymine (T) DNA only,
cytosine (C) guanine (G)
uracil (U) RNA only
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Nucleotide
Phosphate
Group
O
O=P-O
O
5
CH2
O
N
C1
C4
Nitrogenous base
(A, G, C, or T)
Sugar
(deoxyribose)
C3
C2
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5
DNA
double
helix
O
3
3
O
P
5
O
C
G
1
P
5
3
2
4
4
2
3
1
P
T
5
A
P
3
O
O
P
5
O
3
5
P
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Two DNA Strands Connect
Together…
• Cytosine bonds to Guanine
• Adenine bonds to Thymine
• Notice that a purine will connect
with a pyrimidine
• Double helix bonds at nitrogenous bases by
a HYDROGEN BOND
– Not a true “bond”, but an attraction of
one molecule’s slight Positive charge (due
to polar bonding) to a lone pair of
electrons on the opposing molecule.
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Powerpoint Revised from
www.biologycorner.com
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