I. Atoms
A.
•
•
•
•
•
B.
C.
D.
Subatomic Particles
Protons (+) in nucleus
Neutrons (0) in nucleus
Electrons (-) in orbitals energy levels
1st- 2electrons 2nd- 8 electrons
3rd orbital 8 or 18 electrons
Atomic number – number of protons
Atomic mass – protons & neutrons
Isotopes – same element w/
different number of neutrons
E. Chemical properties – reactivity,
F. Physical properties – descriptive
solid shape color
G. Elements
1. C H O N Na Cl S Mg K Ca Fe P
2. Periodic table
• 6 – atomic number = # of protons
• C – element symbol
• 12 – atomic mass = # of protons + #
of neutrons
II.Chemical Compounds – 2 or more
elements combined
A. Molecules “compounds”
• H20, O2, NaCl “salt”, CO2,
C6H12O6- monosaccharide (glucose)
• HCl – “hydrochloric acid
•
C12H22O11 – disaccharide (sucrose)
B. Ionic Bonds – elements lose or gain
electrons, become ions
C. Covalent Bonds – shared electrons
III. Water – most common solvent
A. Solubility – how well something
dissolves, like dissolves like
B. Solvent dissolves solute
C. Cohesion-tension – water attracted
to water
• Capillary action – surface
tension, attraction tension H2O
to H2O
D. Specific heat – water has a high
specific heat, it takes a lot of energy
to change water’s temp.
IV. pH – relative concentration of H+
and OH-
A. Acids – pH 1-6, more H+ (hydrogen)
ions, sour taste, urine 5.5, sweat 5.5,
pop 3.5, gastric juice 2.0
B. Bases – “alkaline” pH 8-14, more OH(hydroxide) ions, bitter taste, bile 8,
ammonia 11.5, bleach 12.5, pancreatic
juice 8
C. Neutral – pH 7, H+ = OH-,
water, blood, saliva
D. Buffers – baking soda NaOH,
neutralize excess acid to create pH 7
I. Molecules of living things
A. Organic chemistry – contain
carbon
B. Chemical groups page 38
• Hydroxyl – OH
• Carboxyl – COOH,
in lipids & proteins
• Amino – NH3, NH2,
in proteins
• Phosphates – PO4,
In nucleic acids, DNA, RNA
II. Macromolecules
A. Polymer – repeating monomers “chains”
B. Biological polymers
1. Condensation reactions
Dehydration synthesis,
anabolic = smaller  larger
C6H12O6 + C6H12O6  C12H22O11 + H2O
2. Hydrolysis –
catabolic = larger  smaller, digestion
breaking down
C12H22O11 + H2O  C6H12O6 + C6H12O6
III. Carbohydrates – sugars and starches
used for energy, 4 calories / gram,
contain C, H, O,
2H: 1 oxygen
A. Monosaccharides – single sugars
(C6H12O6)
•
Glucose
•
Fructose – fruit sugar
•
Galactose
Isomers – same formula different arrangement
Test for sugar: Benedicts solution
B. Disaccharides – double sugar
(C12H22O11)
•
•
•
Sucrose – “table” fructose + glucose
Lactose – “milk” glucose + galactose
Maltose – “malt” glucose + glucose
C.Polysaccharides – “many sugars”
1. Starch – breads, potatoes, grains
2. Glycogen – stored glucose in muscles and
liver
3. Cellulose – cell walls “wood”
Test for starches in food: Iodine
IV. Proteins – C H O N & sometimes S,
used for growth maintenance and
repair (4 calories / gram)
Test for protein in food: Biuret
A. Amino acids – (20) base unit of proteins,
examples: lysine, argenine, tyrosine
B. Peptide bonds
• Polypeptides – 3 or more amino acids
form proteins: albumin, keratin,
collagen, enzymes, skin, hair,
muscles, organs
C. Prosthetic groups – another element will
replace H, hemoglobin, H-C-C-C-C-Fe
V. Lipids – C H O (9 calories / gram) fats
,waxes, oils used for energy storage,
insulation, padding Test for lipids: Sudan III
A. Fatty acids – base unit of lipids (linoleic
acid)
Unsaturated – liquid – plants, double bonds,
HDL’s
Saturated – solid – animals, single bonds, LDL’s
B. Triglycerides & neutral lipids – 3 fatty
acids & glycerol, “adipose” fat
C. Phospholipids – cell membranes
D. Sterols – fats in a ring, cholesterol,
testosterone
E. Waxes – fatty acids & alcohol, resistant
to water
VI. Nucleic Acids – C, H, O, N, and P
A. DNA – deoxyribonucleic acid, genetic
code of life
B. RNA – ribonucleic acid, codes for
proteins
C. Nucleotides & ribose & phosphates
• Guanine
• Adenine
• Thymine
• Cytosine
• Uracil
I. Energy
A. Potential – stored
Chemical – stored in chemical
bonds
B. Kinetic – energy of motion, break
bonds
II. Energy in chemical reactions
A. Reactants and products
(left of equation and right of
Equation will equal each otherbalanced equations
Conservation of matter and
energy
B. Chemical balance of energy
1. ATP – adenosine triphosphate, AP~P~P contains high energy
bonds
2. ADP – adenosine diphosphate, AP~P
3. ATP/ADP cycle – draw diagram
4. Calories & kilocalories
• Calorie = amount of heat
needed to raise 1000 grams of
water 1 degree Celsius
C.Chemical reactions
1. Exergonic – release of energy,
heat, gas, bubbles
2. Endergonic – absorb energy, gets
cooler
3. Activation energy – energy to start
a reaction potential  kinetic
4. Catalyst – speeds up a reaction
lowers the activation energy
required to start reaction
III.Enzymes – organic catalysts speed up
breaking down of food
A. Characteristics
• End in- (ase) amylase lipase sucrase
• Proteins
• Never used up
• Never chemically changed
• Are specific, certain enzymes break
down certain substrates
B. Substrate – substance being broken down
• Active site – where enzyme fits into
substrate “lock and key hypothesis”
C. Enzyme regulation – enzymes reused,
mechanisms to stop enzyme action
D.Cofactors – coenzymes, assist enzymes
“vitamins”
I. Photosynthesis – CO2 + H2O + light
C6H12O6 + O2
A. Energy from sunlight  chemical energy,
wavelengths, longest = red, violet =
shortest
B. Chlorophyll – green pigment traps light
C. carotenes – orange yellow,
D. xanthophylls – red orange
E. Chloroplast – contain chlorophyll
• Thylakoids – light dependent reactions
a)
•
Grana – stacks of membrane absorb light
energy
Stroma – fluid, light independent
reactions
II.Light dependent reactions
• Light  glucose  ATP
• Occur when light is present
Produces oxygen
III.Light independent reactions
• Calvin Cycle – CO2  ATP
Produces sugar
• Mitochondria and chloroplasts –
cellular respiration and
photosynthesis, to produce ATP
I. Metabolism – all chemical
reactions in the body
A. Energy conservation – food
energy  ATP
• Anaerobic – without O2,
glycolysis, fermentation
• Aerobic – with O2,
Kreb’s, electron transport
II. Cellular Respiration- process by
which the energy from food
recharges low energy phosphates to
make ATP
(glycolysis,Krebs & electron transport)
net gain of 36 ATP’s
• C6H12O6 + O2 + 2ATP + 38 ADP +
38( – P)  CO2 + H2O + 38 ATP
A. Glycolysis – anaerobic
Glycogen – (stored glucose)  ATP
lactic acid- formed with no or little O2
• Glycogen stored in muscles and liver
Glycogen + (2ATP)  (4ATP) + pyruvic
acid(citric acid) -formed from
breakdown of glycogen under normal
conditions
•
Net gain of 2 ATP (s)
B. Krebs Cycle
1. Citric acid cycle (gain 2 ATP)
• By products of glycolysis citric
or pyruvic acid  ATP
• Net gain of 1 ATP per cycle 2
cycles
• Excited electrons are left to be
used in electron transport
C. Electron Transport – aerobic
• Glucose  net gain of 32
ATP’s
V.Fermentation – anaerobic “yeasts”
and bacteria
A. Alcohol – sugar or starch  alcohol
+ carbon dioxide
B. Lactate – lactose  lactic acid +
CO2
Pyruvic acid is turned into lactic acid
VI. Energy sources in the human
“Cellular Respiration” total of 36 ATP’s
• Glycolysis – 2 ATP’s anaerobic
• Krebs – 2 ATP’s
aerobic
• Electron transport – 32 ATP’s aerobic