Name: ________________________________________
Unit 4: Biochemistry
Review Outline
Per. _______
I. Chemistry
II. Biochemistry
1. composition of matter
 elements
 atom
o protons
o neutron
o electron
 atomic mass
 atomic number
 Periodic Table of Elements
o how do you get the # of...
 protons
 neutrons
 electrons
 isotope
 covalent compounds
o compound
o molecule
o formulas
o diatomic molecules
 ionic compounds
 electron energy level
 inert elements
 ions


2.





energy
states of matter
physical vs. chemical change
reactants
products
activation energy
o hydrolysis
o dehydration synthesis
3. solutions
 mixtures
o solutions
o saturated
o suspensions
 acids and bases
o pH scale

inorganic compounds
properties of water
o polarity
o hydrogen bonding
o adhesion
o cohesion
o capillarity
o temperature moderation
organic compounds
o carbohydrates
 sugars
 monosaccharides
 disasaccharides
 starches
 polysaccharides
 glycogen
 cellulose
 lipids
 glycerols and fatty acids
 fats
 oils
 waxes
 cholesterol
 steroids
 proteins
 amino acids
 peptide bonds
o polypeptide
 enzymes
o organic catalyst
o active site
o enzyme-substrate
complex
 lock and key model
of enzyme action
o effect of
 temperature
 relative amount of
enzyme and
substrate
 pH on enzyme
activity
1
I. Chemistry
1. Composition of Matter
All matter is made up of 92 elements
Element
o a pure substance that cannot be broken down to a simpler substance by ordinary chemical means (see periodic
table)
Carbon
C
Chlorine
Cl
Hydrogen
H
Manganese
Mn
Know
Oxygen
O
Mercury
Hg
names and
Helium
He
Lead
Pb
symbols
Nitrogen
N
Phosphorus
P
Sulfur
S
Silicon
Si
Potassium
K
Tin
Sn
Strontium
Sr
Uranium
U
Copper
Cu
Zinc
Zn
Calcium
Ca
Iron
Fe
Sodium
Na
Magnesium
Mg
Fluorine
F
Iodine
I
Atoms
o smallest units of matter
 made up of:
e-
p+
Protons: found in nucleus, + charge
Subatomic Neutrons: found in nucleus, 0 charge
particles
Electrons: found outside nucleus, - charge




e-
atomic mass = protons + neutrons
atomic number = number of protons
number of electrons = number of protons (atom electrically neutral)
atomic mass – atomic number = number of neutrons
Hydrogen
1
1
H
Deuterium
1
2
1
H
Tritium
Atomic number
1
Atomic mass
1
2
3
# of protons
1
1
1
# of electrons
1
1
1
# of neutrons
(1-1=) o
(2-1=) 1
(3-1=) 2
What do they all have in common? atomic #, # of protons, # of electrons
 atomic number = ID number of the element
 Electrons arranged in energy levels around nucleus
o Describe the electron configuration of the element chlorine
o
3rd
1st
2nd
2
8
nucleus
2
no
18
1
3
1
H
Subatomic Particles Practice
Directions: Using the periodic table provided, use the atomic numbers and/or element symbols to fill in the rest of
the entries below:
atomic
number
element
symbol
element
name
number of
protons
number of
electrons
number of
neutrons
82
Pb
Lead
82
82
207-82
=125
2.
6
C
Carbon
6
6
12-6
=6
3.
26
Fe
Iron
26
26
56-26
=30
4.
8
O
Oxygen
8
8
16-8
=8
5.
50
Sn
Tin
50
50
119-50
=69
6.
11
Na
Sodium
11
11
23-11
=12
7.
16
S
Sulfur
16
16
32-16
=16
8.
53
I
Iodine
53
53
127-53
=74
9.
19
K
Potassium
19
19
39-19
=20
10.
92
U
Uranium
92
92
238-92
=146
1.
3
4
Isotopes
o atoms of the same element having differing numbers of neutrons
ex. carbon-12 and carbon-14
U-235 and U-238 (radioisotopes)
Compounds
o chemical combinations of two or more different elements
 compounds are represented by formulas
ex. H2O
NaCl
C6H12O6

all form molecules = smallest part of a substance that maintains the properties of that substance

when bonds are broken, bond energy is released; takes energy to combine elements into compounds
 Compounds Formed by Covalent Bonding
= sharing of pairs of electrons
 Compounds Formed by Ionic Bonding
= transfer of electrons from one atom to another
ex. NaCl: table salt
Na+



transfer
e-
Cl-
explosive metal
poisonous gas
gain or loss of electrons causes the atom to become charged = ions
Na+ ion is attracted to the Cl- ion
chemical reactivity of an atom depends on the # of electrons it can share or transfer
2. Energy
States of Matter
 depends on rate of molecular movement: solid, liquid, gas
 change in state = physical change
ex. H2O(s)  H2O(l)  H2O (g)
 change in composition = chemical change
ex. steak (proteins)  amino acids
Energy and Chemical Reactions
 reactions are represented by equations:
ex. CO2 + H2O

H2CO3
reactants
products
 many chemical reactions require activation energy in order to occur
 catalysts reduce the amount of activation necessary to start a reaction
Catalyst speeds up the reaction without changing itself

enzymes are required for many reactions in living systems
ex.
end in “-ase” : lactase, lipase, maltase, protease
5
Types of Reactions
hydrolysis: reaction in which large molecules are broken down into smaller molecules. Chemical digestion is an
example of a hydrolysis reaction
synthesis: the combining of simpler molecules to form a more complex molecule
Biochemical processes, both breakdown (hydrolysis) and synthesis, are made possible by enzymes. Enzymes and
other molecules, such as hormones and antibodies, have specific shapes that influence both how they function and
how they interact with other molecules.
3. Solutions
o two or more substances blended together but not chemically combined (= mixture)
 Solutions are formed when solute evenly dispersed (dissolved) in solvent
ex. sugar = solute
water = solvent
 Saturated solution can dissolve no more solute
 Aqueous solutions (solutions dissolved in water) are very important in living systems



Acids and Bases
H2O covalently bonded, but 2/billion dissociate into ions
+
 Acid solutions sour
 Basic (alkaline) solutions bitter, slippery OHNaOH
pH scale
H
stomach acid
blood, saliva
<H+ 0------------------------------7-------------------------------14 <OHacidic
neutral
basic
 acid/base indicators = litmus paper, pH meters, phenolphthalein
 most biochemical reactions very sensitive to changes in pH
ex. blood and body fluid- pH 7.4
stomach acid- pH 2
 buffers help to maintain body fluids at normal and safe pH values
ex: Tums
6
Litmus
Red = Acid
Blue = Base
7
II. Biochemistry
1. Water
o most common compound in living systems
 unique properties of water:
i.
ii.
water molecule is polar
 has a slightly negative oxygen end and slightly positive hydrogen ends
hydrogen bonding
 positive region of one water molecule is attracted to hydron region of another
 weak bonding; easily broken
 causes water to cling to itself (cohesion) and other substances
(adhesion)

ex. cohesion – surface tension
adhesion – water moving up stem
 capillarity = adhesion and cohesion working together to pull water up narrow tube
temperature moderation
i.
takes great energy gain or loss for water to change temperature
because it requires breaking all of the hydrogen bonds before temperature change can take
place
allows stability in temperature of cells, therefore homeostasis

ii.
2. Carbon Compounds
Inorganic vs. Organic Compounds
 Organic compounds must contain carbon and hydrogen
 Inorganic Compounds
ex. H20- water
ex. CO2- supplies C in organic compounds
 green plants use it in photosynthesis
ex. minerals
compounds of P, Ca, Fe, Mg, Zn from soil, water
***Green plants converter INORGANIC to ORGANIC compounds***

Organic Compounds



all contain carbon (and hydrogen)
all produced by organisms
carbon can form 4 covalent bonds; links to form long chains/rings
ex. C6H12O6 = molecular formula for glucose, fructose, galactose
carbon bonds with itself, forming many different compounds
most organic compounds have functional groups
ex. hydroxide (-OH) = functional group attached to carbon atom



i.
ethanol: causes liver and brain cell death
ii.
methanol: (wood alcohol) causes blindness and death
iii.
glycerol: forms part of lipid
monomers
(small)
8
vs.
polymers
(long chains)
H
CH4:
H
C
H
H
3. Molecules of Life
 Four classes of organic compounds:
i.
carbohydrates
ii.
proteins
iii.
lipids
iv.
nucleic acids
CARBOHYDRATES
 contain C, H, O
2 hydrogen: 1 oxygen
 ex. sugars, starches, cellulose
Indicators:

energy & structure
Benedict’s

Sugars
blue

monosaccharides (C6H12O6)
Iodine
ex. glucose, fructose, galactose (isomers)
amber

: tests for glucose
 orange
: tests for starch
 black
disaccharides (C12H22O11)
ex. sucrose, maltose



o

2 molecules of monosaccharide combined = 1 molecule of disaccharide + water
monosaccharides can also form long chains to form polysaccharides
= dehydration synthesis: take water away to form new links
Starches
polysaccharides in long branched chains
ex. potato starch
cellulose in potato
animal starch = glycogen
 produced and stored in liver
cellulose- forms plant cell wall
animals break down starches into simple sugar to get energy
= hydrolysis: add water to break down
Practice Questions:
_____1. Which substances are inorganic compounds?
A. water and salts
C. fats and oils
B. proteins and carbohydrates
D. enzymes and hormones
_____2. Which term best describes a solution with a pH of 5?
A. acidic
B. neutral
C. basic
_____3. A simple sugar such as glucose is classified as a
A. monosaccharide
B. polysaccharide
D. colorless
C. disaccharide
D. nucleotide
_____4. In which process are simple materials chemically combined to form more complex materials?
A. synthesis
B. pinocytosis
C. hydrolysis
D. cyclosis
_____5. Which formula represents an organic compound?
A. Mg(OH)2
B. NaCl
C. C12H22O11
D. NH3
9
10
LIPIDS
 contain C,H,O
ratio of H to O much greater than 2:1
 ex. fats, oils, waxes
 made up of glycerols and fatty acids, usually in a 3 to 1 ratio
 dehydration synthesis releases 3 molecules of water
 fats (triglycerides) are hydrolyzed when needed; stored when not needed; do not dissolve in water
ex. butterfat – in milk
Indicator
oils - energy source in plants
waxes - usually protective
Brown Paper turns
 steroids- complex lipids that form many hormones
oily
&
greasy
ex. testosterone – male hormone
cholesterol – needed for nerve cell function but may block blood vessel walls
PROTEINS and AMINO ACIDS

contain C, H, O, N

building blocks = amino acids

each contains an amino group (NH2) and a carboxyl group
(COOH)
20+ amino acids, depending on “R” group
amino acids group in long chains to form polypeptides by
dehydration synthesis
(also called condensation
reaction)
C-N bonds = peptide bonds
hamburger protein broken down by hydrolysis into amino
acids and reassembled into yours




ENZYMES
o proteins that act as organic catalysts,
affecting reaction rates in organisms without being changed
themselves
 only active site on enzyme involved in reactions; dependent on shape
 enzyme and molecule (substrate) form enzyme-substrate complex causing reaction to occur
 enzymes are very specific, similar to a lock and key system
 names of enzymes end in –ase
ex. maltase breaks down maltose
11

Rates of enzyme action dependent on:
i.
temperature
 rate of enzyme action generally low at low temperatures and increases as temperature rises
 BUT at a maximum temperature, enzyme loses effectiveness
 enzyme gets denatured
ii.
relative amounts of enzyme and substrate
 in a given amount of enzyme, addition of substrate will increase enzyme activity until all enzyme is
“busy”
iii.
pH
 each enzyme acts most effectively within a specific pH range
ex. gastric protease – pH 2
pancreatic protease – pH 8
NUCLEIC ACIDS
 building blocks = nucleotides
 each nucleotide contains:
o phosphate molecule
o nitrogenous base
o 5-carbon sugar
 Several types of nucleic acids, including:
o DNA: deoxyribonucleic acid
 Genetic material, double stranded helix
o RNA: ribonucleic acid
 Genetic material, single stranded
o ATP: adenosine triphosphate
 High energy compound
12
Name: ___________________________________________
Per. _____
Carbohydrates
Sugar
-ose
Saccharides
Monosaccharide
Disaccharide
Polysaccharide
glucose
starch
Lipids
Proteins
Amino acids
Peptide
Dipeptide
polypeptide
N
enzymes
Nucleic Acids
DNA
RNA
ATP
fat
oil
waxes
Regents Questions:
_____ 1. Which formula represents an organic compound?
1. NH3
2. NaCl
3. H2O
4. C6H12O6
_____ 2. The reactions involving most chemical compounds in living systems depend upon the presence of
1. sulfur as an enzyme
3. water as a solvent
2. salt as a substrate
4. nitrogen as an energy carrier
_____ 3. Small soluble food molecules are converted to larger, insoluble molecules by the process of
1. hydrolysis
3. dehydration synthesis
2. respiration
4. fermentation
_____ 4. Which organic compound is correctly matched with the subunit that composes it?
1. maltose - amino acid
3. protein - fatty acid
2. starch - glucose
4. lipid - sucrose
_____ 5. In most carbohydrate molecules, the ratio of hydrogen atoms to oxygen atoms is
1.
1:2
2.
3:1
3.
2:1
4.
_____ 6. Which compound is inorganic?
1. amino acid
2. nucleic acid
3. protein
1:3
4. water
_____ 7. Which metabolic waste is produced as the result of the synthesis of maltose from two glucose
molecules?
1. water
2. salt
3. carbon dioxide
4. urea
13
_____ 8. To be used by muscle cells, starch must be chemically converted to
1. amino acids
3. fatty acids
2. simple sugars
4. simple proteins
_____ 9. What are the end products of carbohydrate hydrolysis?
1. amino acids 2. simple sugars
3. hydrogen ions
4. fatty acids
____ 10. The complete digestion of animal starch results in the formation of
1. glucose molecules
3. fatty acids
2. amino acids
4. glycogen molecules
____ 11. Which formula represents a carbohydrate?
1. NaHCO3
2. NH2CH2COOH
3. C18H36O2
4. C12H22O11
____ 12. A specific organic compound contains only the elements carbon, hydrogen, and oxygen in the ratio of 1:2:1.
This compound is likely a
1. nucleic acid 2. monosaccharide
3. protein
4. lipid
____ 13. The complete hydrolysis of carbohydrates results directly in the production of
1. glycogen
2. carbon dioxide
3. urea
4. simple sugars
____ 14. Which element is present in all lipids and proteins?
1. iron
2. nitrogen
3. carbon
4. calcium
____ 15. The process by which proteins are made from amino acids is known as
1. dehydration synthesis
3. intracellular digestion
2. ingestion
4. hydrolysis
____ 16. An organic compound that has hydrogen and oxygen in a 2:1 ratio would belong to the group of compounds
known as
1. lipids
2. proteins
3. fatty acids 4. carbohydrates
____ 17. Which substance is an inorganic compound that is necessary for most of the chemical reactions to take
place in living cells?
1. glucose
2. water
3. starch
4. amino acid
____ 18. If a specific carbohydrate molecule contains ten hydrogen atoms, the same molecule would most probably
contain
1. one nitrogen atom
3. five oxygen atom
2. ten nitrogen atoms
4. twenty oxygen atoms
____ 19. A chemical reaction involves the production of a dipeptide from two amino acids. This is an example of
1. hydrolysis
3. dehydration synthesis
2. digestion
4. carbon fixation
____ 20. An organic compound has both an amino group and a carboxyl group. It is most probably a (an)
1. amino acid
2. monosaccharide
3. fatty acid
4. glycerol
____ 21. A carbon to nitrogen bond may also be called a (an)
1. peptide bond
2. hydrogen bond
3. ionic bond
14
4. polymer
____ 22. Which of the following may be used as a building block for proteins?
1. monosaccharide
2. fatty acid
3. glycerol
4. amino acid
____ 23. Which organic compound is a building block of a triglyceride, containing three carbon atoms, five
hydrogen atoms, and three hydroxyl groups?
1. glycerol
3. saturated fatty acid
2. amino acid
4. unsaturated fatty acid
____ 24. Which process produces peptide bonds?
1. digestion
2. hydrolysis
3. dehydration synthesis
4. enzyme deactivation
Base your answers to questions 25 through 29 on the diagram below which represents steps in the enzymecatalyzed breakdown of maltose and on your knowledge of biology.
_____ 25. Which substance is represented by letter A?
1. sucrose
2. maltase
_____ 26. The substrate in this process is a (an)
1. disaccharide
2. amino acid
3. lipase
3. monosaccharide
4. protease
4. lipid
_____27. Which chemical reaction occurs between steps 1 and 5?
1. fermentation
3. hydrolysis
2. carbon fixation
4. dehydration synthesis
_____ 28. Which statement best describes step 2?
1. An enzyme is undergoing denaturation.
2. An enzyme is being hydrolyzed.
3. A water molecule is being synthesized.
4. An enzyme-substrate complex is being formed.
_____ 29. Steps 1 through 5 best illustrate
1. that substrate concentration affects enzyme action
2. a model of enzyme specificity
3. that enzymes are composed of protein
4. the role of coenzymes in chemical reactions
_____ 30. Compound X increases the rate of the reaction below.
Compound X is most likely
1. an enzyme
2. a lipid molecule
3. an indicator
4. an ADP molecule
15
Base your answers to 31 through 33 on the diagram of the chemical equation which represents a metabolic activity
and your knowledge of biology.
_____ 31. Which chemical substance is labeled C?
1. a lipid
2. a dipeptide
3. a disaccharide
4. a nucleotide
_____ 32. Which substance is represented by letter D?
1. water
2. salt
3. ammonia
4. carbon dioxide
_____ 33. Molecule C belongs in the general class of substances known as
1. vitamins
2. minerals
3. inorganic acids
4. organic compounds
_____ 34. The equation below summarizes the process that produces the flashing light of a firefly.
The molecule luciferin is broken down, and energy is released in the form of heat and light. In this process,
luciferase functions as
1. a reactant
2. a substrate
3. an inorganic catalyst
4. an enzyme
Base your answer on the graph and on your knowledge of biology
_____ 35. Which is a true statement about the relationship between pH and enzyme action?
1. All enzymes work best at a neutral pH.
2. Adding more acid does not affect the rate of activity of an enzyme.
3. Enzymes function only in a pH range of 4.0 to 5.5.
4. The activity of an enzyme is affected by pH.
_____ 36. Which substance found in the cytoplasm of an ameba is an inorganic compound?
1. nucleic acid
2. amino acid
3. water
4. glucose
16
Base your answers for 37 through 39 on the diagram shows a model of a biochemical reaction.
_____ 37. The process represented in the diagram is known as
1. dehydration synthesis
2. carbon fixation
3. photolysis
4. hydrolysis
_____ 38. Molecule A can best be described as a
1. dipeptide
2. disaccharide
3. starch
4. fat
_____ 39. The bond that exists between alanine and phenylalanine is known as
1. an ionic bond
2. a peptide bond
3. a hydrogen bond
4. a phosphate bond
_____ 40.
According to the graph in the diagram, at what temperature will the denaturation of lipase begin?
A. below 0°C
B. between 0°C and 38°C
C. at 40°C
D. at 68°C
_____ 41. Which enzyme regulates the reaction represented by the word equation:
lipid + water = fatty acids + glycerol
1. amylase
2. lipase
3. ATPase
4. protease
_____ 42. A process that occurs in the human body is shown in the diagram. What would happen if a temperature
change caused the shape of the active site to be altered?
1. The dipeptide would digest faster.
3. The amino acids would combine faster.
2. The dipeptide would digest slower or not at all.
4. The amino acids would combine slower or not at all.
17
Base your answers to 43 through 47 on the chemical equation shown in the diagram and your knowledge of biology.
_____ 43. The reaction indicated by arrow E illustrates
1. hydrolysis
2. dehydration synthesis
3. photolysis
_____ 44. A molecule containing a peptide bond is represented by
1. A
2. B
3. C
_____ 45. Amino groups are found in molecules of
1. A, only
2. A and B, only
4. aerobic respiration
4. D
3. A, B, and C, only
4. A, B, C, and D
_____ 46. The end products resulting from the complete digestion of a protein molecule is represented by both
1. A and D
2. B and C
3. C and D
4. A and B
_____ 47. A dipeptide is represented by
1. A
2. B
3. C
4. D
_____ 48. The rate of the enzyme action of the enzyme protease is affected by
1. temperature, particle size, and lipase concentration 3. pH, particle size and amylase concentration
2. temperature, pH, and protein concentration
4. pH, temperature, and carbohydrate concentration
_____ 49. Base your answer on the reactions shown in the graphic.
The X in each reaction represents various
1. energy sources
2. final products
3. reactants
4. enzymes
_____ 50. Which statement best describes the enzyme represented in the graphs above?
1. This enzyme works best at a temperature of 35°C and a pH of 8.
2. This enzyme works best at a temperature of 50°C and a pH of 12.
3. Temperature and pH have no effect on the action of this enzyme.
4. This enzyme works best at a temperature above 50°C and a pH above 12.
18