Welcome to AP Biology
Mrs. Marcum
Big Idea 1: The process of evolution
drives the diversity and unity of life.
Big Idea 2: Biological systems utilize
free energy and molecular building
blocks
to grow, to reproduce, and to maintain
dynamic homeostasis.
Big Idea 3: Living systems store,
retrieve, transmit, and respond to
information
essential to life processes.
Big Idea 4: Biological systems interact,
and these systems and their
interactions possess complex
properties.
Remember!
• Register for AP Central
• Free/Reduced Lunch = 3 = $200 extra
KEES
• AP Exam: Monday, May 9
• December 16 - Open Heart Surgery - $14
• Teacher webpage
• Remind 101: text 81010 message:
@2hca
• Absent: retrieve papers from extra tray
• Bellwork board
Chemistry Topics
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Atomic Structure
Atomic mass, atomic number, isotopes
Chemical Bonding
pH scale
How Matter is
Organized
•Chemical Elements
•Forms all matter
•Substances that cannot be split into simpler substances by ordinary
chemical means.
•Have letter abbreviations called chemical symbols.
•Most common elements in living things  C, H, N, O, P, S (96%)
•Trace elements are present in tiny amounts (Fe, Mn, Cu)
Structure of Atoms
• An element is a quantity of
matter composed of atoms of
the same type.
Atoms contain:
• Nucleus: protons (p+) &
neutrons (neutral charge)
• Electrons (e-) surround the
nucleus as a cloud (electron
shells are designated regions
of the cloud)
http://web.visionlearning.com/custom/chem
istry/animations/CHE1.3-ananimations.shtml
Atomic Number and Mass
Number
• Atomic number is
number of protons in
the nucleus.
• Mass number is the
sum of its protons and
neutrons.
• Isotope  atoms of
same element with
different number of
neutrons (Carbon-14
& Carbon-12)
• A hepatobiliary
iminodiacetic acid
(HIDA) sc
A hepatobiliary iminodiacetic acid (HIDA) scan
Ionic Bonds
•When an atom loses or
gains a valence electron,
ions are formed (Figure
2.4a).
•Positively and negatively
charged ions are attracted
to one another.
Covalent Bonds
– Covalent bonds are
common and are the
strongest chemical bonds
in the body.
• Covalent bonds may be
nonpolar or polar.
– In a nonpolar covalent
bond, atoms share the
electrons equally; one atom
does not attract the shared
electrons more strongly
than the other atom
Van der Waals
interactions
• Electrons are not
always
symmetrically
distributed in
nonpolar
molecules
• Occur only when
atoms and
molecules are
very close to
each other
• Weak
Polar Covalent Bonds
• Unequal sharing of electrons between atoms.
In a water molecule, oxygen attracts the
hydrogen electrons more strongly
Polar Covalent
Bonds
Hydrogen
Bonds
– are weak
intermolecular bonds;
they serve as links
between molecules.
– help determine threedimensional shape of
large molecules
– Important in giving
water its properties
essential for life
Hydrogen Bonds
Biologically important weak bonds helps
stabilize 3 dimensional shape of large
molecules(DNA and proteins).
Because water is polar molecule, it can
form Hydrogen Bonds.
Because of the Hydrogen Bonds, water has
some very UNIQUE Properties!
6 Properties of
Water
• 1. Water is a Powerful
Solvent
– Solute, Solution, Solvent
– Hydrophobic vs Hydrophilic
– Shell of hydration
2. Water is attractive
Water adheres to a surface due to
2 properties:
Adhesion
Cohesion
These 2 properties allow for
capillary action.
• 3. Water has High Surface Tension
– Strong interaction of water molecules
– Water striders, whirly gigs, skipping
rocks
• 4. Water has a High Specific Heat
– High heat is required to increase the
temp. of water and a great deal of heat
must be lost in order to decrease the
temp. of water.
• 5. High Heat of Vaporization
– A great deal of energy must be
present in order to break the Hydrogen
bonds to change water from liquid to
gas
• 6. Water has a high freezing point and lower density
as a solid than a liquid
– Water’s maximum density is 4 degrees Celsius
Normal pH range of arterial
blood 7.35-7.45
Acidosis – blood pH below
7.35
*depression of synaptic
transmission in CNS
Disorientation, coma, death
Alkalosis – blood pH above
7.45
*overexcitability of CNS and
peripheral nerves
Nervousness, muscle
spasms, convulsions
and death
http://nedbook.adam.com/page
s/IPWeb/systems/buildframes.
html?fluids/acihomeo/01
Figure 2.13
Buffers
• Buffers stabilize pH of a solution
by accepting or donating H+.
• Organisms use buffers to maintain
homeostasis.
• Blood pH is 7.4
• Carbonic Acid helps to maintain
this pH
Friday November 13, 2015
• Bellwork: crossword puzzle
Isomers – compounds that have
the same chemical formula but
differ in structure
differ in covalent arrangements
differ in spatial arrangements
Mirror images of each other pg. 62
Tuesday
November 17
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Grab A Worksheet from the Bellwork Tray
Matching:
A. Phosphate
1. donates Hydrogen ions
B. Sulfhydrl
2. aldehyde
C. Carboxyl
3. transfer energy
D. Amino
4. stabilizes protein structure
E. Hydroxyl
5. alcohol; polar
F. Carbonyl
6. accepts Hydrogen ions
Sulfhydryl Group
Tryptophan
All living organisms require 4 types
of Organic Compounds:
1.
2.
3.
4.
Carbohydrates
Lipids
Proteins
Nucleic Acids
**All contain**:
Carbon
Hydrogen
Oxygen
1. Carbohydrates
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All carbs contain
C,H,O in a 1:2:1
ratio
Functions: Energy &
structural support
Exist as:
a. Monosaccharides
b. Disaccharides
c. polysaccharides
a. Monosaccharide
“simple sugar”
3 Forms
1. Glucose - made by plants;
source of energy
2. Fructose - found in fruits;
Sweetest!!
3. Galactose – found in milk
These are ISOMERS – same
chemical formula but
different structures.
b. Disaccharide
“double sugar”
3 Forms
1. Sucrose – Table Sugar
glucose + fructose
2. Maltose - Malt Sugar
glucose + glucose
3. Lactose – Milk Sugar
glucose + galactose
•How do monosaccharides form
disaccharides?
https://www.youtube.com/watch?v=ZMTeq
ZLXBSo
• Hydrolysis
• Dehydration synthesis (condensation reaction)
– Glycosidic linkage – covalent bond between 2 mono’s
c. Polysaccharide
“Many Sugars”
3 Forms – All composed of repeating
units of glucose.
1.
Glycogen – Energy storage in
animals. (Liver & Muscles)
2.
Starch - Energy storage in plants
(Roots, Stems, Leaves)
3.
Cellulose - Gives strength &
rigidity to plant cell
(Fiber  Prevents Colon Cancer)
Monosaccharide vs
Polysaccharide
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Add a pipette full of each food to each test tube
Add a 15 drops of Benedicts to each tube
Heat for 3-5 minutes, orange, green, red = +
Wash out test tubes
Load tubes again
Add a 4 drops of iodine
Dark blue, purple, blackish = +
Wash test tubes
Record data on board
Functional group Quiz
2. Lipids
• Nonpolar / insoluble / hydrophobic
• 5 types: triglycerides, phospholipids,
steroids, waxes, glycolipids
• Fx: insulation, cushion, energy storage,
hormones, membrane structure, protection
against pathogens, repel water, water
conservation
Four Ring Structure of Steroids
Glycolipid
• 3rd Carbon in glycerol is
bound to a carb chain
instead of a phosphate
group.
• Behaves like a
phospholipid because the
carbohydrate is
hydrophilic
• Found in cell membrane
and functions in
identification of the cell
Waxes
December 1
Tuesday
• Get out
multiple
choice
review sheet
from
yesterday
3. Proteins
• Found in: meat, eggs,
nuts, beans, tofu
• Uses in body: muscle,
hormones, enzymes,
energy, transport of
oxygen (hemoglobin),
support, hair, nails,
skin, blood clots (fibrin)
• Monomers of proteins
are amino acids
• Amino acids join
together by peptide
bond
Formation of a Dipeptide Bond
• Dipeptides formed from 2 amino acids joined by a
covalent bond called a peptide bond
– dehydration synthesis
• Polypeptides chains contain 10 to 2000 amino acids.
Copyright 2009, John Wiley &
Sons, Inc.
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Primary Structure:
ex.: lysozome
Catalyzes hydrolysis of carbohydrates
Secondary Structure:
Alpha helix: ex. hair
stabilized by hydrogen bonds
Beta pleat
ex. silk
Tertiary
Structure:
Protein
channels
Quaternary Structure:
ex.: hemoglobin
Enzymes
• Most enzymes are
proteins; some RNA
• Speed up chemical rxn;
biological catalyst
• Shape of protein allows
it to bond to specific
molecules called
substrates, causes a
change in shape
• maltase: maltose  2 glucose
• lipase: lipids fatty acids
• protease: proteins  amino
acids
**works best under certain
temperatures
Enzymes
4. Nucleic Acids
DNA and RNA
• Oganic molecules that contain
carbon, hydrogen, oxygen,
nitrogen, and phosphorus.
• Deoxyribonucleic acid (DNA) =
Genetic Code.
• Ribonucleic acid (RNA) relays
instructions from the genes in
the cell’s nucleus to guide
each cell’s assembly of amino
acids into proteins by the
ribosomes.
• ATP – energy molecule
• Monomers = nucleotides
Nucleic Acids
• There is a base-pairing rule:
– A always bonds across from T
– C always bonds across from G
• A and G, called purines, are structures
composed of two rings
• C and T are pyrimidines – singled-ringed
structures
• A purine always pairs with a pyrimidine
and vice versa
Nucleic Acids
• Because of this, if one strand of DNA is
known, the other strand can be deciphered
• If we know that one strand of DNA has the
sequence:
ATCGGCA
• The other side must be:
TAGCCGT