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Chemical Basis of Life
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Basic Chemistry
All matter on Earth is made from approx. 100 elements!!
Element-a substance that cannot be broken down by chemical processes into simpler substances– Atom-smallest form of an element
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Compounds
A substance that is made of two or more elements chemically combined in definite proportions– Ex: H2O (water) Always two hydrogen molecules for every one Oxygen molecule
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Organic Compounds
Generally associated with living things
All contain Carbon!!
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Structure of an Atom
Protons: positively charged particles
Electrons: negatively charged particles
Neutrons: neutral particles
Periodic Table: Atomic Number = the number of protons
H = 1, O = 8
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Atom: Just the facts
Atoms of the same element have the same number of protons and electrons
Atoms of the same element can have different numbers of neutrons = Isotopes
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Radioactive: nucleus splits apart spontaneously (gives off energy)– Releases charged particles and radiation
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Electrons
Orbit around the nucleus in specific energy levels– First energy level requires 2 electrons
– other energy levels require 8 electrons
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Electrons (cont’d)
Atoms are most stable when their outer energy levels are “full”
Atoms will gain or lose electrons in order to fill the outermost level
The remaining atom is called an ion
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Ions
Atoms with a positive or negative charge
Losing electrons = positiveGaining electrons = negative
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Chemical bonds
Attractions that hold two or more atoms together– Whenever a chemical bond is formed or broken energy is absorbed or released (heat)
Three types: Ionic, Covalent, Hydrogen
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1. Ionic Bonds
Formed between ions with opposite charges resulting in a compound that has no electrical charge
IMPORTANT—electrons are lost by one element and gained by another
EX: NaCl (table salt)
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2. Covalent Bonds
Electrons are not gained or lost… they are shared (ex: water)
Covalent bonds create molecules!
See pages 40 & 41
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Polar Molecules
Molecules in which electrons are not shared equally between atoms
This causes the molecules to have one slightly positive end and one slightly negative endO
H HFigure 2.12+ +
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Hydrogen Bonds
Bonds that occur between molecules containing hydrogen
Important—properties of water and the chemistry of living things!
O
H+ +
Opposites attract
H+
+
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Chemical formulas
Shows what type of atoms are in a compound or molecule– Empirical formula: shows simplest
proportions of atoms in compounds– Structural: shows number and type of
atoms as well as how they are bonded– Molecular: Shows number and types
of atoms (most common)
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Simple Variety
Not all living things are as complex as humans
Most living things are made up of only four kinds of chemicals…
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1. Carbohydrates
“chemical energy”– Sugars, starches, and cellulose
– Store energy and provide shape
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Carbohydrates (cont’d)
Three types of sugars1. Monosaccharides 2. Disaccharides
3. Polysaccharides
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Complex Carbohydrates
What do we use them for???Energy storage! In the form of
glycogen (in muscles and liver)
Plants store energy also! In the form of starch! (potatoes, wheat, grains)
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Cellulose
Most abundant molecule on Earth
Storage for simple sugarsFound in desks, paper, pencils,
etc.
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2. Lipids
“long term energy storage”Fats, oils, waxes, steroidsLipids are converted into fat
when too many are consumed
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Lipids are important!!
Cell membranes are made of phospholipids
Waxes repel water– Fruits and leaves retain water– Ducks are waterproof
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3. Proteins
Main control system in your bodyLarge complex molecules
composed of amino acids– Only 20 amino acids combine to make up the countless numbers of proteins that make up all living things!
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The Importance of Protein!
Important for movement, structure, regulation, transport, nutrition, defense
Insects use proteins called pheromones to communicate
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4. Nucleic Acid
Makes you who you are!Large, complex molecules that
contain genetic information
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DNA
Deoxyribonucleic acid– Carries all of the instructions needed to make an organism
Heredity: the passing of genetic information from parent to offspring
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RNA
Ribonucleic Acid– Uses DNA’s instructions to make proteins
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Chemical Reactions
The breaking of bonds to change one or more substancesEx: remember the cracker, as the saliva broke down the starch the cracker began to have a sweet taste!
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How did it do that????
Remember starch is a polysaccharide (carbohydrate)– The saliva breaks down the polysaccharide into simple sugars!
You were a part of a chemical reaction!!
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Chemical Reaction
One or more substances is changed into a new substance by the breaking or forming of chemical bonds
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Chemical Equation
Describes what happens in a chemical reaction
(reactants) (products)C6H12O6 + 6O2 6H2O + 6CO2 +
energy(Glucose)
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Chemical Reactions & Energy
All chemical reactions are either…
1. Absorb energy = endothermic2. Release energy = exothermic
-The energy that is given off when a substance is formed is equal to the energy needed to break it down!!
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How to speed up a chemical reaction…
1. Temperature—an increase in temperature = an increase in chemical reaction rate (why??)
2. Catalyst—a substance that speeds up or slows down a reaction (it is not used or changed in the reaction)
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Catalyst
All living organisms contain catalysts = enzymes!– An enzyme is a protein catalyst that speeds up the chemical reactions within an organism by reducing the amount of activation energy needed
Pg. 44 Figure 2.15
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Enzyme Facts
Names usually end in –aseHave a specific shape so they only
fit one substrate (lock & key)They are never actually used up in
the reactionAllow reactions to occur in an
organisms without increasing the organism’s temperature.
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Enzyme Specifics
A substrate bonds to an enzyme at the active site.
Once the enzyme and substrate are bonded together the enzyme changes shape to ensure the substrate will stay attached = induced fit
The enzyme + substrate = E-S complex
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1. What are enzymes made out of?2. What do enzymes do?3. Molecules that can bind with
enzymes are called_________.4. Why does heating an enzyme
change its function?
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1. What enzyme broke down H2O2?2. Where was the enzyme located?3. What were the products of the
reaction?4. What are enzymes made out of?
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Chemistry in Life Processes
How does the food you eat keep you warm?– Food releases energy when it breaks
down chemically, some is in the form of heat
– energy is stored in the chemical bonds of the food we eat—it is released by chemical reactions (digestion)
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Major life processes
MetabolismCommunicationReproductionHomeostasisGrowth and Repair
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Metabolism
The combination of all of the chemical changes that takes place in an organism– Organisms break chemical bonds
(digestion) in compounds to release energy
– Plants and some organisms can use sunlight to make energy-rich compounds
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– Products of chemical reactions = heat and wastes
– To grow and develop, cells of organisms must make new carbohydrates, proteins, and lipids—also to make repairs
– Regeneration-the process of growing back a lost body part
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Homeostasis
Tendency of an organism to maintain stable internal conditions– Ex: sweat to cool body, panting
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Communication
Internal – neurotransmittersFeedback loop- series of reactions
that help maintain homeostasis by controlling chemical reactions
Pheromones—insects use this protein to communicate(ants form a line to food)
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Water and Solutions
Life processes depend on the properties of water and the characteristics of solutions– Solution: uniform mixture of 2 or more substances; cannot distinguish between the substances
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Water and Solutions (cont’d)
– Solute: the dissolved substance in a solution
– Solvent: the dissolving substance Ex: Ice tea = solvent
Sugar = solute-Suspension: mixture that separates upon standing
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Water-the universal solvent
Water will form a solution with most ionic compounds
Why????Because it is a polar
molecule!(partial charges)
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Water
Cohesion—sticking togetherExpansion—water expands
when it freezes….allowing it to floatWhy is that important???
Allows pond-dwelling organisms to survive
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Acids, Bases, and Salts
When ionic compounds form solutions the compound breaks apart and releases ions– Acid: releases H+ (hydrogen)ionsEx: orange juice, HCl, vinegar
HCl H + Cl
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– Base: releases OH- (hydroxide)ionsEx: NaOH (sodium hydroxide), soaps, ammonia, baking soda
NaOH Na + OH
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– Salt: releases ions other than H+ and OH-Ex: NaCl (table salt)
NaCl Na + Cl
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When water breaks apart (disassociates) in a solution it releases both H+ and OH- ions= Neutralization reactionNaOH + HCl H2O + NaCl
(base) (acid) (water) (Salt)
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pH scale
Measure of the concentration of H+ ions in a solution
So, what mechanism keeps our pH at 7.4?
1 2 3 4 5 6 7 8 9 10 11 12 13 14
ACID Neutral BASE
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Why is this important???
Burning fuels such as coal, oil, and gasoline releases sulfur and nitrogen compounds into the air
What’s also in the air??Water!!
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Acid Rain
When these things mix H+ ions are released…causing the rain to become acidic
Acid rain has a pH of less than 5.6Destroys minerals in the soil vital
to plants…no plants no peopleDecreases the Ph in lakes…killing
aquatic life
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Page 54– Questions 1-5– Write the answers
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Tell me all you know about enzymes and the liver lab.– What is an enzyme? Why does it have an active site? What enzyme did we use in the lab? What substrate did it break down? Etc…
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Read “The Molecules of Life”– Answer post test questions 1-11