Macromolecules
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Most confusing of concepts.
What are they?
Use of Macromolecules
Differentiate
Human need
Etymology
• 1886, from macro- + molecule. Apparently
coined in "On Macro-molecules, with the
Determinations of the Form of Some of
Them," by Anglo-Irish physicist G.
Johnstone Stoney (1826–1911). Originally
of crystals.
Etymology
Macro- meaning “large,” “long,” “great,”
“excessive,”
AND….
Molecule – Combination of elements
Meaning "molecule composed of many
atoms" is from 1935, from German
makromolekul (1922).
A macromolecule
- is a very large molecule commonly created by
polymerization of smaller subunits. In
biochemistry, the term is applied to the four
conventional Biopolymers
• nucleic acids
• proteins
• carbohydrates
• as well as non-polymeric molecules with large
molecular mass such as lipids and
macrocycles.
• The individual constituent
molecules of macromolecules
are called monomers
(mono=single, meros=part).
SPONCH
What is SPONCH?
SPONCH
6 most important
elements to life
•
•
•
•
•
•
S= Sulfur
P= Phosphorus
O= Oxygen
N= Nitrogen
C= Carbon
H= Hydrogen
Matter
• Anything that
occupies space and
has mass
Element
• Simplest form of
matter, cannot be
broken down
chemically into a
simpler kind of matter
Periodic Table of Elements
• Organized table of
elements discovered
so far
• Organized according
to atomic structure
and chemical
characteristics
Atoms and Atomic Structure
• Atoms are the
simplest form of an
element that keeps all
the properties of the
element
Model of the Atom
• Parts of the atom:
– Protons (+), Neutrons
and Electrons (-)
– Nucleus: central core of the
atom that contains
• Protons
• Neutrons
– Electrons orbit the nucleus
Determining Atomic Structure
Using the Periodic Table
• Atomic number = # of
protons and is smaller
number by the symbol
• Atomic mass number
= # of protons + # of
neutrons
• Assume for now that
protons =electrons
Practice
Element
hydrogen
helium
carbon
oxygen
sodium
chlorine
argon
sulfur
# protons
1
# neutrons
0
# electrons
1
Practice
Element
hydrogen
helium
carbon
oxygen
sodium
chlorine
argon
sulfur
# protons #
neutrons
1
0
2
2
6
6
8
8
11
12
17
18
18
22
16
16
#
electrons
1
2
6
8
11
17
18
16
Types of Bonds
• COVALENT – strong bond between
elements
• IONIC- attraction between elements due to
opposite charges (weaker than covalent)
• HYDROGEN – weakest type of bond
Covalent
• Sharing of electrons to fill the valence shell
• Examples– methane (CH4) and carbon
dioxide (CO2)
Ionic
• One element gains electrons becoming
____
• The other element loses electrons
becoming _____________
• Opposites attract
• Ionic compounds
Dissolve easily in water
– EX. NaCl
Hydrogen bonds
• Caused by partial positive and negative
charges
• Water is best example
‫ﮦ‬+
‫ﮦ‬-
How does salt dissolve in
water?
• Na+ and Cl –
• Ions become
attracted to the
partial charges on
water
Today’s
Agenda:
Biology
I know the following…
*atomic mass
*atomic number
*how to find # of protons
*how to find # of neutrons
*how to find # of electrons
*atomic structure (drawings)
*types of bonds
•QUIZ on Basic
Chem.
•2-1
Chemistry Basics Quiz
Element Atomic
Mass
Li
Lithium
He
Helium
B
Boron
Na
Sodium
Atomic # of
# of
# of
Number protons neutron electron
s
s
Draw the following atoms
• Carbon
WATER H2O
• Oxygen
CARBON – the building block of
life!
• DRAW Carbon
Carbon is able to covalently bond with up to four other elements
or form double and triple bonds with other carbon atoms.
Carbon
• Carbon chains make up many structures
of living organisms.
• Varying carbon chains’ structure and/or
adding various atoms and molecules to
the carbon chain will change it’s function
• MAKE CH4
* MAKE C2H6
* MAKE C2H4
Group of 4 Make…
• C4H10 – two different ways
Ring Forms of Carbons
• Make C4H8 with NO DOUBLE BONDS
FUNCTIONAL GROUPS
• Add a hydroxyl group (-OH) to a 2 carbon
chain
•You just made ethanol – an alcohol that
destroys liver cells
MACROMOLECULES
• 4 Large Molecules Important to Life
– Carbohydrates
– Lipids
– Proteins
– Nucleic Acids
Stuff to know!
Chapter 2-1
•Atomic #
•Atomic mass
•Atomic structure
•Ionic bonds
•Covalent bonds
•Hydrogen bonds
•Water chemistry
–Solutions,Solvents,pH
– polarity
Chapter 2-3
•Carbon chem
•Carbohydrates
•Lipids
•Proteins
•Nucleic Acids
CARBOHYDRATES (CH2O)n
•Functions= provides energy (glucose is
energy source for cells
• Monomers = monosaccharides
– Examples = glucose, fructose and galactose
(all 3 = C6H12O6 so they are isomer)
• Two linked = disaccharides
– Examples = sucrose (glucose and fructose)
and lactose
• Polymer = polysaccharides
– Examples = glycogen (animals) starch
(plants)
Why “bulk-up” on carbs?
Why not eat carbs?
CONDENSATION REACTION
HOW WOULD THIS GET BROKEN
DOWN?
H20
HYDROLYSIS
PROTEINS
• Monomers = amino acids
• All amino acids have
– Amine group (NH2)
– Carboxyl group (COOH)
• R-groups differ
Dipeptide
FUNCTIONS of PROTEINS
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Structural
Hormones
Transport
Histones
ENZYMES!!!
Lock and Key Model
What symptoms would you have if
you had sickle cell anemia?
1 amino acid is wrong in the hemoglobin
sequence = mis-shaped RBCs
LIPIDS
• MONOMERS = fatty acids
• Saturated
• Unsaturated
COMPLEX
• TRIGLYCERIDES
• PHOSPHOLIPIDS
• WAXES
FUNCTIONS
• TRIGLYCERIDES – insulation and energy
storage
• PHOSPHOLIPDS – main component in
cell membranes
HARDENING OF THE ARTERIES
• Fats such as cholesterol and saturated
fatty acids build up in arteries
• What other factors contribute to
arteriosclerosis?
Concept Map
Section 2-3
include
that consist of
that consist of
that consist of
that consist of
which contain
which contain
which contain
which contain
Concept Map
Section 2-3
Carbon
Compounds
include
Carbohydrates
Lipids
Nucleic acids
Proteins
that consist of
that consist of
that consist of
that consist of
Sugars and
starches
Fats and oils
Nucleotides
Amino Acids
which contain
which contain
Carbon,
hydrogen,
oxygen
Carbon,
hydrogen,
oxygen
which contain
which contain
Carbon,hydrogen,
oxygen, nitrogen,
phosphorus
Carbon,
hydrogen,oxygen,
nitrogen,
WATER CHEMISTRY
2-2
Section Outline
Section 2-2
•
2–2
Properties of Water
A.The Water Molecule
1. Polarity
2. Hydrogen Bonds
B.Solutions and Suspensions
1. Solutions
2. Suspensions
C.Acids, Bases, and pH
1.
2.
3.
4.
The pH Scale
Acids
Bases
Buffers
Hydrogen bonds
• Caused by partial positive and negative
charges
• Water is best example
‫ﮦ‬+
‫ﮦ‬-
Figure 2-9 NaCI Solution
Section 2-2
ClCl-
Na+
Na+
Water
Water
Figure 2-9 NaCI Solution
Section 2-2
ClCl-
Na+
Na+
Water
Water
Solutions
• Ions break away from each other and form
hydrogen bonds with water (because its
polar)
• Solute- the substance that is dissolved
• Solvent- almost always water, substance
in which the solute is dissolved
• Ex. Koolaid
– Solute- koolaid powder
– Solvent- water
Suspension
• Materials do not dissolve when placed in
water, instead the water molecules keep
them floating
• Blood- cells are floating in water solution
H2O sometimes breaks down into
H+ and OH-
pH Scale indicates the
Section
2-2
concentrion
of H+ ions in water
Acids have higher
concentration of
H+, bases have
higher
concentration of
OH-
Increasingly Basic
Oven cleaner
The higher the pH,
the more BASIC the
solution. The lower
the pH, the more
ACIDIC the
solution.
Increasingly Acidic
Neutral
Bleach
Ammonia solution
Soap
Sea water
Human blood
Pure water
Milk
Normal
rainfall
Acid rain
Tomato
juice
Lemon juice
Stomach acid
Buffers
• Weak acids and bases that reacts with
other acids and bases to change the pH.
• In the body, buffers help maintain
homeostasis
• Ex. Blood needs to stay within 6.5 to 7.5.
Stomach needs to stay around 3.
Peptobismo (buffer) raises stomach acid if
your stomach is too acidic.
Interest Grabber continued
• 1. What are the reactants when wood burns?
2-4
•Section
Reactants
are oxygen and cellulose.
• 2. What are the products when wood burns?
• Products are carbon dioxide and water
• 3. What kinds of energy are given off when wood burns?
• Light and heat are given off. Some students may also mention
sound (the crackling of a fire).
• 4. Wood doesn’t burn all by itself. What must you do to start a
fire? What does this mean in terms of energy?
• To start a fire, you must light it with a match and kindling. You
are giving the wood some energy in the form of heat.
• 5. Once the fire gets started, it keeps burning. Why don’t you
need to keep restarting the fire?
• Once the fire gets going, it gives off enough heat to start more of
the wood burning.
Section Outline
Section 2-4
•
2–4 Chemical Reactions
and Enzymes
A.Chemical Reactions
B.Energy in Reactions
1. Energy Changes
2. Activation Energy
C.
D.
Enzymes
Enzyme Action
1. The Enzyme-Substrate Complex
2. Regulation of Enzyme Activity
Effect of Enzymes
Section 2-4
Reaction pathway
without enzyme
Activation energy
without enzyme
Reactants
Reaction pathway
with enzyme
Activation
energy
with enzyme
Products
Figure 2-19 Chemical Reactions
Section 2-4
Energy-Absorbing Reaction
Energy-Releasing Reaction
Activation
energy
Products
Activation energy
Reactants
Reactants
Products
Figure 2-19 Chemical Reactions
Section 2-4
Energy-Absorbing Reaction
Energy-Releasing Reaction
Activation
energy
Products
Activation energy
Reactants
Reactants
Products
Enzyme/Substrate Complex
CATALASE AND H2O2