Everything is composed of matter
Components of Matter
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Atoms
Elements
Compounds
Mixtures
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Physical – can be changed without
changing the material
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Ie state, temperature, color, shape,
volume, etc
Chemical – can not be changed
without disrupting the material
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PH, density, color, flammability, etc
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Solid – molecules only vibrate, holds own shape and
volume
Liquid- holds the shape of its container, holds volume,
molecules flow.
Gas- no definite shape or volume, molecules not
connected
Plasma – temperature so high, atomic particles
separate
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Nucleus- center of
atom
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Protons (+), Neutrons
(neutral
Orbiting Electrons (-)
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Energy Levels- surround
nucleus
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Organized into Periodic Table
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Atomic Number – number of protons in
nucleus
Atomic Mass – number of protons and
neutrons (mass of atom)
Atomic Symbol- abbreviation for name on
periodic table
Families – columns on table
Periods – rows
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Elements- all one compound
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Found on periodic table
Compounds
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More than one element bonded together
Isotopes – atoms of one element that
have different
numbers of neutrons
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Ionic- transfer of electrons
(btn a metal and
nonmetal)
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Covalent- sharing of
electrons
› Polar Covalent – when one
element gets to spend more
time with electrons
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Hydrogen Bonding – loose
bonds between two
molecules that are partially
charged (caused by a
polar covalent bond)
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Major Properties of Water
› Polarity
› Cohesion
› Adhesion
› Surface Tension
› High Specific Heat
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Water is a highly
polar molecule
Oxygen is very
electronegative,
meaning it pulls the
electrons from the
other atoms in the
bond.
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It is an Electron Hog
This causes on part of
the molecule to be
positive (H), and the
other part to be
negative (O)
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The ability of water to
stick to itself
Caused by the
abundance of
Hydrogen bonding
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Due to the polarity of
water, many H-bonds
form between O and
of one molecule and
the H of another
Allows water to travel
up the xylem of plants
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water molecules get
pulled up as they
evaporate or are used
in leaf cells
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The ability of water to cling
to other substances
 Like Cohesion, adhesion is
caused by H-bonds with
other partially polar and
non-polar molecules
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Allows water to defy gravity
Basic Concept behind the
function of paper towels
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The inability to
stretch or break
the surface of
water
 Another
characteristic of Hbonding btn water
molecules
 Why you can
overfill a glass of
water with out
spilling.
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Heat=the total amount of kinetic (moving)
energy in an object or substance
 Specific Heat- the amount of heat needed
to change 1g of water 1°C
 Water’s high specific heat is due to Hbonding.
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When water is adhering to itself, the molecules
are not allowed to move a freely making is
more difficult to change temperature.
Why a pan on the stove with lukewarm water
can burn your hand.
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Homogenoussame all the way
through (ie
ketchup),
thoroughly mixed
 Heterogeneous- all
parts are visible (ie
salsa)
 Solutions- one
substance broken
into ions in another
(ie salt water)
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require physical changes (usually
phase changes) to separate
components.
Solutions are made of a solvent and
one or more solutes.
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Solute: Substance(s) being dissolved.
Solvent: Base of the solution
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What is doing the dissolving.
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When water is the solvent of a solution, it
is an aqueous solutions.
 Due to the polar properties of water,
many compounds disassociate
(dissolve) in water.
 Breaks the compound into its
components
 Ie. NaCl  Na+ + Cl
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Specialized aqueous
solutions
H+ is the component
released upon
disassociation.
H+ is the most chemically
active ion.
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Binds to almost any anion,
causing chemical changes.
IE. HCl – hydrochloric acid,
HSO4 – Sulfuric Acid
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Specialized aqueous
solutions
OH- is released upon
disassociation.
OH- is also very
highly reactive
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Will bind to most
cations.
IE. NaOH – sodium
hydroxide
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Strong acids are
reacted with weak
bases and vice
versa.
Strength is based
upon the entirety of
the disassociation.
When acids and
bases are reacted, a
salt and water are
formed.
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HCl + NaOH  NaCl +
H2O
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Measure of the
concentration of H+/OHions in the solution.
Logarithmic scale from 0
– 14.
Low pH is an acid, high
pH is a base.
Neutral solutions have a
pH of 7.
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HCl – pH=0.5
NaOH – pH=13
Blood – 7.5
Measured using pH scale
or Litmus Paper.
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Changes in pH affects the homeostasis
of living organisms
Homeostasis- the balance within a living
organism
Enzyme production and function changes
› Protein Denaturation
› Overall health of an organism
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All organic compounds
contain the element
carbon.
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With the exception of CO2.
Everything else is
considered inorganic.
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ie: salts, water, minerals,
most acids
All organic compounds contain
carbon.
Carbon is a unique element
because of its ability to form four
covalent bonds.
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Very strong, stable bonds
always forms four bonds
The shape of C is the cause of the
strength of the covalent bonds.
Small, single C-chains are
considered monomers.
When joined together by
chemical bonds
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Made into polymers
Process known as polymerization
By joining many polymers,
macromolecules are created.
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Basic process behind the making
of a protein.
Four types of organic compounds
make up living things:
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Carbohydrates
Lipids
Proteins
Nucleic Acids
Sugars and Starches
Storage and Structure roles in the cell
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Glycogen - found in the liver, stores fuel for
later use
Cellulose – structural role in plants, makes
up cell walls
“Fuel” of the body

monosaccharide
› fuel for the cell
› made during
photosynthesis
› used during
respiration
AKA: Fats
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Insoluble in water
Does not make polymers
Fatty Acid + Glycerol
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Fatty acid: C-chain with carboxyl group
(COOH)
Glycerol: alcohol with a 3 C-chain
Fatty Acid makes lipids insoluble in water
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Not polar molecules
Saturated Fats contain
nothing but single C-C
bonds.
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They are “saturated” with
hydrogen.
Solid at room temperature.
Cause many health problems
Unsaturated Fats contain
at least one double C-C
bond.
Better fats
Monounsaturated Fats have
one double bond
Polyunsaturated have more
than one.
Liquid at room temperature.
Phospholipids have a
phosphorus containing
head (glycerol).

Phosphorus causes the
glycerol to be polar.
This makes one end of the
molecule to be water soluble.
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Hydrophilic – water liking
head
Hydrophobic – water hating
tail
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The cell membrane is made
of two layers of phospholipids
with the fatty acid tails
toward each other
Polymers of amino acids
Amino acids
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Composed of an amino group, a COOH
group, and an R-group
R-group makes each amino acid different.
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Amino Acids are joined together with
covalent bonds
Bond forms between the amino group and
the COOH group
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Peptide bond
Proteins are also known as polypeptides.
Polymers of nucleotides
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Nucleotides-
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Basic 5-carbon sugar,
phosphate, nitrogenous
base
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2-basic types of nucleic
acids
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2 types of bases
Purines and Pyrimidines
RNA
DNA
Store genetic information

Enzyme – type of protein that acts as
a catalyst
› Speeds up the reaction btn two
molecules
 Lowers the activation energy
 Energy required to make a reaction start
› Does not get used up
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Many reaction in life would
go too slow w/o enzymes
Work by binding to a
substrate
› The reactant that the
enzyme binds to.
› Creates the enzymesubstrate complex

Substrate can only bind to
one site
› Active site of the enzyme
 Special groove or fold in
protein
 EXTREMELY specific

Effects of environmental conditions
› Change the confirmation of protein
(denaturation)
› Break H-bonds and other bonds involved in
protein
› Changes the active site so substrate can no
longer bond
› Ie: high Temperature or change in pH