Macromolecules
• 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
• S= Sulfur• P= Phosphorus• O= Oxygen• N= Nitrogen• C= Carbon• H= Hydrogen
6 most important elements to life
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
PracticeElement # protons # neutrons # electrons
hydrogen 1 0 1
helium
carbon
oxygen
sodium
chlorine
argon
sulfur
Practice
Element # protons # neutrons
# electrons
hydrogen 1 0 1
helium 2 2 2
carbon 6 6 6
oxygen 8 8 8
sodium 11 12 11
chlorine 17 18 17
argon 18 22 18
sulfur 16 16 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 compoundsDissolve 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
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
Today’s Agenda:
•QUIZ on Basic Chem.
•2-1
Chemistry Basics Quiz
Element Atomic Mass
Atomic Number
# of protons
# of neutrons
# of electrons
Li
Lithium
He
Helium
B
Boron
Na
Sodium
Draw the following atoms
• Carbon • Oxygen
WATER H2O
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
• Monomers = monosaccharides– Examples = glucose, fructose and galactose
(all 3 = C6H12O6 so they are isomer)
•Functions= provides energy (glucose is energy source for cells
• 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?
HYDROLYSISH20
PROTEINS
• Monomers = amino acids
• All amino acids have– Amine group (NH2)
– Carboxyl group (COOH)
• R-groups differ
Dipeptide
FUNCTIONS of PROTEINS
• 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?
include
that consist of
which contain
that consist of that consist of that consist of
which contain which contain which contain
Section 2-3
Concept Map
CarbonCompounds
include
that consist of
which contain
that consist of that consist of that consist of
which contain which contain which contain
Section 2-3
Concept Map
Carbohydrates Lipids Nucleic acids Proteins
Sugars and starches
Fats and oils Nucleotides Amino Acids
Carbon,hydrogen,
oxygen
Carbon,hydrogen,
oxygen
Carbon,hydrogen,oxygen, nitrogen,
phosphorus
Carbon,hydrogen,oxygen,
nitrogen,
WATER CHEMISTRY
2-2
• 2–2 Properties of WaterA.The Water Molecule
1. Polarity
2. Hydrogen Bonds
B.Solutions and Suspensions1. Solutions
2. Suspensions
C.Acids, Bases, and pH1. The pH Scale
2. Acids
3. Bases
4. Buffers
Section 2-2
Section Outline
Hydrogen bonds
• Caused by partial positive and negative charges
• Water is best example
+ ہ- ہ
Cl-
Water
Cl-
Na+
Water
Na+
Section 2-2
Figure 2-9 NaCI Solution
Section 2-2
Figure 2-9 NaCI Solution
Cl-
Water
Cl-
Na+
Water
Na+
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-
Oven cleaner
Bleach
Ammonia solution
Soap
Sea water
Human bloodPure waterMilkNormalrainfall
Acid rainTomatojuice
Lemon juice
Stomach acid
NeutralIn
crea
sing
ly B
asic
Incr
easi
ngly
Aci
dic
Section 2-2
pH Scale indicates the concentrion of H+ ions in water
Acids have higher concentration of H+, bases have higher concentration of OH-
The higher the pH, the more BASIC the solution. The lower the pH, the more ACIDIC the solution.
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.
• 1. What are the reactants when wood burns?
• 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 2-4
Interest Grabber continued
• 2–4 Chemical Reactions and EnzymesA.Chemical Reactions
B.Energy in Reactions1. Energy Changes
2. Activation Energy
C. Enzymes
D. Enzyme Action1. The Enzyme-Substrate Complex
2. Regulation of Enzyme Activity
Section 2-4
Section Outline
Reaction pathwaywithout enzyme Activation energy
without enzyme
Activationenergywith enzymeReaction pathway
with enzyme
Reactants
Products
Section 2-4
Effect of Enzymes
Energy-Absorbing Reaction Energy-Releasing Reaction
Products
Products
Activation energy
Activation energy
Reactants
Reactants
Section 2-4
Figure 2-19 Chemical Reactions
Energy-Absorbing Reaction Energy-Releasing Reaction
Products
Products
Activation energy
Activation energy
Reactants
Reactants
Section 2-4
Figure 2-19 Chemical Reactions
Enzyme/Substrate Complex
CATALASE AND H2O2
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