Ch. 2 - Chemistry of Life -...
Transcript of Ch. 2 - Chemistry of Life -...
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Chemistry of Life
Chapter Two
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Biology and Chemistry
Biology = study of life
Chemistry = study of matter
and the changes it undergoes
Matter – anything that takes up
space and has mass
Life is made up of atoms
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2.1 Atoms, Ions, and Molecules
Atoms
Building blocks of
matter
Tiny
Models
Help explain structure
and properties
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Atomic Structure
Three subatomic particles:
Protons (p+)
Neutrons (no)
Electrons (e-)
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Subatomic Particles
Protons
Same size as no
Inside nucleus
Positive charge
Same number as e-
Identifies element
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Subatomic Particles
Neutrons
Same size as p+
Inside nucleus
No charge
Helps hold nucleus
together
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Subatomic Particles
Electrons
Smallest
Outside nucleus
Negative charge
Same number as p+
Involved in chemical reactions
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Atomic Review
Nucleus
Core of atom
Dense
p+ and no
e- are outside the
nucleus
Atoms are neutral
Same # of p+ as e-
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Elements
Pure; made of just one
kind of atom
>100 different kinds
91 natural
~25 found in organisms
Represented by chemical
symbols
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Elements Differ in # of p+ in atoms
Atomic number = # of p+ in atom
Ex:
Carbon = 6
Oxygen = 8
Hydrogen = 1
What element is shown?
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Elements
Atomic Mass – sum
of p+ and no in an
atom
“atomic weight”
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Isotope
Atoms of the same element that differ in
the # no
Same element
Same # p+
Same # e-
Different # no
Ex: Hydrogen
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Mystery Atom
How many protons?
How many electrons?
What is the atomic number?
What is the name?
What is its chemical symbol?
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In Your Own Words: Differentiate between an
atom and an element:
What is an atom?
What is an element?
How are they related?
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Compounds Made up of two or more different
kinds of atoms joined together represented by chemical formulas
Formulas tell type of elements and proportion (# of atoms of each element)
Ex: Water = H2O
Sodium chloride = NaCl
Carbon dioxide = CO2
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Chemical Bonding Atoms join with other atoms to form compounds
Force that holds the atoms together = chemical bond
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Chemical Bonds
Atomic “Glue”
Three basic types:
Ionic bonds
Covalent bonds
Hydrogen bonds
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Ion An atom that has gained or
lost one or more electron
Now different # of p+ and e-
Not neutral
Has a charge!
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Ions
Cation – an atom that
has lost one or more
electrons
positive charge
Anion – an atom that
has gained one or
more electrons
negative charge
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Atoms Want Stability
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Ionic Bonding
Ex: NaCl = Table Salt
Na gives up an e-
Becomes cation
Cl takes in an e-
Becomes anion
Opposites attract and
BOND
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Ionic Bonding
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Covalent Bonding
Atoms share e- to gain
stability
Fill outer shell with e-
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Covalent Bonds
Molecule – two or more
atoms held together by
a covalent bond
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Covalent Molecules
Ex:
Water
Carbon dioxide
Oxygen
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2.2 Properties of Water
~70% of your body is water
~2/3 of molecules in your body
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Hydrogen Bonding
Weak bond between
polar molecules
Holds molecules
together
Water = good example
Often between slightly
positive H atom and
slightly negative N or O
atom
Opposite charges attract
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Polar Molecules
Overall molecule is
neutral
e- shared unequally
One end positive
One end negative
Ex: Water
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Hydrogen Bonding in Water
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Water in Living Things Your cells: filled AND surrounded by water
All living things need water
Properties of water 7 min British
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Properties Related to H bonding
1) Specific heat
2) Cohesion
3) Adhesion
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1)High Specific Heat
Water:
Heats up slowly
Cools down slowly
Helps regulate body
temperature
Evaporation
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2) Cohesion
Force of attraction between similar substances
Ex: Hydrogen bonding in water
Creates surface tension
surface doesn’t break easily
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3) Adhesion
Attraction between different substances
Ex: Water is attracted to other polar substances
Adhesion is stronger than cohesion in water molecules
Explains water meniscus
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Adhesion
Powers capillary action
Water moves upward
through tiny tubes against
gravity
Ex: water moving up a
plant
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Aqueous Solutions Solution of a substance dissolved in water
Solution - mixture of evenly distributed
substances (homogeneous)
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Solution Parts
Solvent – does the dissolving
Solute- gets dissolved
Concentration – the amount of solute
dissolved in solvent
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Polarity of Water
Review:
Overall molecule = neutral
One end = positive
One end = negative
Opposites attract
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“Like Dissolves Like”
Water dissolves ionic
compounds and polar
molecules best
Ionic compounds
break apart into ions
in water
Ions have charges
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Sodium Chloride in Water
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Sodium chloride is an example of :
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Oil and Water do NOT mix!
Nonpolar and polar do
NOT mix
Nonpolar substances
do not dissolve well in
water
Important to organisms
Nonpolar membranes
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Acid
Compound that releases a hydrogen
ion (H+) - when dissolved in water
H+ is a proton
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Bases Compounds that form hydroxide ions
(OH-) when dissolved in water
Reduces concentration of H+
OH- react with H+ to form H2O
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Acids and Bases
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pH Scale Measures concentration
of H+ in a solution
pH scale runs from 0-14
below 7 = acidic
above 7 = basic
pH equal to 7 is neutral
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pH Scale Each step is a ten fold change in H+ concentration!
Ex: pH 4 is ________x more acidic than pH of 6?
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pH of Common Household Items
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pH Range in organisms
Very narrow
Ex:
human blood pH 7.35-7.45
Azalea plant pH 4.5
Buffers – help regulate pH
binds to H+ when too many, and releases H+
when not enough
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Thinker. . .
Cells have a higher concentration of
Hydrogen ions than blood.
Which has a higher pH – blood or a cell?
Why?
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2.3 Carbon Compounds
= Organic compound
Contain C
“building block
of life”
Usually forms:
4 covalent
bonds
Long chains or
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Carbon Molecules
Monomer – subunit of the molecule
Polymer – Many monomers bonded
together
large molecule (macromolecule)
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Classes of Organic Compounds
1) Carbohydrates
2) Lipids
3) Proteins
4) Nucleic Acids
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1) Carbohydrates
Made of C, H, and O
Often 1:2:1 ratio
Most have 5 or 6 C
atoms
Key energy source
Monomer (building
block) =
monosaccharides
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A) Monosaccharides
Simple sugars
Mono = “one”
Saccharide =“sugar”
Examples:
Glucose
Fructose
Galactose
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B) Disaccharides
Double sugars
Di = “two”
Two
monosaccharides
joined
Ex: Sucrose =
table sugar
glucose + Fructose
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C) Polysaccharides Poly = “many”
Polymers of monosaccharides
Macromolecules
Macro = “big”
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Polysaccharides
Some store energy
Plants = starch
Animals = glycogen
In plants, they also
provide support
Ex: Cellulose in cell
walls
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2) Lipids
Not soluble in water
Nonpolar
Examples:
Fats
Oils
Waxes
Steroids
Cholesterol
Phospholipids
Cell membranes
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Lipids include Fats Store lots of energy
Building blocks:
1) Fatty acids – chain of C bonded to H
2) Glycerol
Triglyceride = 3 fatty acids + glycerol
Many lipids
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Saturated Fatty Acids
Lots of C – H single
bonds
Generally solids at room
temp
Ex: Animal fats
Butter
Lard
Grease
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Unsaturated Fatty Acids
Some double bonds
Bends molecule
Can’t pack tightly together to become solid
Generally liquids at room temp
Most plant oils
Some fish oils
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Hydrogenated fats
“Trans Fats”
Made when unsaturated fat has H added Becomes more solid
More “saturated” with H
Tastes better. Lasts longer. Not good for you!
Not natural!
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Phospholipids
Make up cell
membranes
Contain
Glycerol
2 fatty acids
Nonpolar “tails”
Phosphate group
(PO4-)
Polar “head”
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Cholesterol
Ring structure
Too much = not good
Necessary for:
Cell membrane structure
Steroid hormone production
Ex: testosterone, estrogen
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3) Proteins
Important to life
Ex: enzymes
Promote chemical
reactions
Ex: structural proteins
Collagen
Keratin
Fibrin
Hemoglobin 69
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Proteins Large molecules = macromolecules
Building blocks = Amino acids (aa)
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Amino Acids
Twenty different aa
Some polar
Some nonpolar
Fold into shapes
Our body makes 12
Get other 8 from food
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Amino Acids
Contain C,H,O,N and sometimes S
Most varied organic compound
All have:
C bonded to H
Amino group (NH2)
Carboxyl group (COOH)
Only differ in R-group (side chain)
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Examples of aa
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AA Bonding
Form Peptide bonds
covalent bonds
Linked chains =
polypeptides
Protein = 1 or more
polypeptides
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Proteins
AA sequence
determines structure
and function
Ex: hemoglobin
In RBCs
One incorrect aa = sickle
cell anemia
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4) Nucleic Acids
long chain-like
molecule
Nucleotides =
building blocks
(monomer)
Store protein making
info
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Nucleotides
3 parts
Phosphate
group
Sugar
Nitrogen
base
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Two kinds
1) DNA
Two strands
Spiral shape
Stores hereditary info
makes up chromosomes
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Two kinds of nucleic acids
2) RNA
One strand
3 different types
Key role in making proteins
Can act as enzyme
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ATP
Adenosine triphosphate
Single nucleotide with 2
extra phosphate groups
Energy “currency”
Fuels cell activities
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ATP
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2.4 Chemical Reactions
Change substances into different
substances by making and breaking bonds
Reactants – substances changed
Products – substances made
Bond Energy – amount of energy needed to
break a bond between 2 atoms
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Energy
Ability to move or
change matter
Many forms:
Light
Heat
Chemical
Electrical
Mechanical (motion)
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Energy Conversions
can change from one
form to another
Ex:
Kicking a ball
Frying an egg
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Chemical Reactions Energy stored or
released
Atoms rearranged
1000s of reactions
per cell per second!
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Chemical Reactions
Reactants
Starting materials
Before reaction
Products
Ending materials
After reaction
Arrow = “yields”
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Energy in Chemical Reactions
Involve energy changes
Bonds are broken and formed
Energy is either absorbed or released
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Energy-Releasing Reaction
Exothermic
Gives off energy
Ex:
Squid and firefly
light
Water freezing
Cellular respiration
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Energy-Absorbing Reaction
Endothermic
Takes in energy
Ex:
Melting of ice
Photosynthesis
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Metabolism
Sum of all chemical
reactions in
organism
Energy comes from
food
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Activation Energy Energy needed to
start a chemical
reaction
Energy absorbed
“chemical push”
Amount needed varies
Analogy: To get a
boulder to roll
downhill, First you
must push it up
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2.5 Enzymes Act as catalysts
Speed up chemical
reactions (rxs) in cells
Lower activation
energy
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Cells and Energy
Cells must have “fuel”
Chemical rxs in cells occur:
Quickly
Low temperatures
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Enzymes Required for Life
Help maintain
homeostasis
w/o enzymes rxs
would be too slow
Life could not exist
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Carbonic Anhydrase
Enzyme in blood
Helps convert CO2
and H2O into carbonic
acid
Carried to lungs
Converted back into
carbon dioxide and
water
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Do not write; just an example Without Carbonic
anhydrase
Slow rx
2000 molecules per hour
converted
Not fast enough
Millions of cells release
CO2
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Do not write; just an example
With enzyme
600,000 molecules
per second
Increases rate a
million times!
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Do not write; just an example
Catalase
enzyme
Helps breakdown
hydrogen peroxide
(toxic to cells)
Reduce activation
energy
quicker
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Enzyme Specificity Each enzyme acts only on a specific substrate
(reactant)
Substrate
Substance on which an enzyme acts
“Lock and key” model
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Active Sites
Shape is everything!
Enzymes bend
slightly around
substrate
Active site - site on
enzyme where
substrate temporarily
binds
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Enzymes
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Factors That Affect Enzymes
1)Temperature
Operate best within
certain range
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Factors That Affect Enzymes
2) pH
Operate best within
certain range
Thinker: If the HCl in
the stomach has a pH
of ~2, which enzyme
on the chart would
function best here?
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Enzyme Activity
Many different ones
Each for different rx
Not used up
Used over
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