BIOCHEMISTRY

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BIOCHEMISTRY
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CHEMISTRY OF LIFE

• Elements simplest form of a substance - cannot
  be broken down any further without changing what
  it is
• Ex. C, H, O, N, Fe
• Atom the actual basic unit - composed of
  protons, neutrons, and electrons

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THE ATOM

• Just like cells are the basic unit of life, the
  ATOM is the basic unit of matter.
• They are very small. If placed side by side one
  million would stretch a distance of 1cm.
• The atom is made up of 3 particles.

Particle Charge
PROTON
NEUTRON NEUTRAL
ELECTRON -
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• Electrons are not present within the atom,
  instead THEY REVOLVE AROUND THE NUCELUS OF THE
  ATOM FORM THE ELECTRON CLOUD

PROTONS
NEUTRONS


ATOMIC 2 (PROTONS) ATOMIC MASS 4 (PROTONS
NEUTRONS)
-
-
ELECTRONS
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ISOTOPES

• atoms of the same element that HAVE A DIFFERENT
  NUMBER OF NEUTRONS
• Some isotopes are radioactive. This means that
  their nuclei is unstable and will break down at a
  CONSTANT RATE over time.
• There are several practical uses for radioactive
  isotopes
• CARBON DATING
• TRACERS
• KILL BACTERIA / CANCER CELLS

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COMPOUNDS

• a substance formed by the chemical combination of
  2 or more elements in definite proportions
• Ex water, salt, glucose, carbon dioxide

H20
CO2
NaCl
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Elements and Life

• The cell is a COMPLEX CHEMICAL FACTORY containing
  some of the same elements found in the nonliving
  environment.
• carbon (C), hydrogen (H), oxygen (O), and
  nitrogen (N) are present in the greatest
  percentages

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TWO TYPES OF COMPOUNDS

• Organic - Contain CH in some ratio (usually
  referred to as chemicals of life)
• Carbohydrates, Proteins, Lipids, Nucleic Acids
• Inorganic - usually "support" life - no specific
  ratio of CH
• Water (H2O), Carbon Dioxide (CO2)

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CHEMICAL BONDS

• Chemical bonds hold the atoms in a molecule
  together.
• There are 2 types of chemical bonds IONIC and
  COVALENT

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IONIC BONDS

• Occur when 1 or more electrons are TRANSFERRED
  from one atom to another.
• When an atom loses an electron it is a POSITIVE
  charge.
• When an atom gains an electron it is a NEGATIVE
  charge
• IONS Charged particles formed when electrons are
  lost or gained
• Example Na

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COVALENT BONDS

• Occur when electrons are SHARED by atoms.
• In general, the more chemical bonds a molecule
  has the more energy it contains

SHARING IS CARING!
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FORMULA

• The chemical symbols and numbers that compose a
  compound ("recipe")
• Structural Formula Line drawings of the
  compound that shows the elements in proportion
  and how they are bonded
• Molecular Formula the ACTUAL formula for a
  compound

C2H6O
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Organic Compounds Found in Living
ThingsBiochemistry Basics
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ORGANIC COMPOUNDS
LIPIDS
PROTEINS
NUCLEIC ACIDS
CARBOHYDRATES
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CARBOHYDRATES

• Why are carbohydrates important?
• Living things use carbohydrates as a key source
  of ENERGY!
• Plants use carbohydrates for structure
  (CELLULOSE)
• include sugars and complex carbohydrates
  (starches)
• contain the elements carbon, hydrogen, and oxygen
  in a 121 ratio

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Monosaccharides (simple sugars)

• all have the formula C6 H12 O6
• all have a single ring structure
• (glucose is an example)

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Disaccharides (double sugars)

• Sucrose (table sugar) is an example

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Polysaccharides

• Formed of three or more simple sugar units
• Glycogen - animal starch stored in liver
  muscles
• Cellulose - indigestible in humans - forms cell
  walls
• Starches - used as energy storage

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How are complex carbohydrates formed and broken
down?
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Dehydration Synthesis

• Combining simple molecules to form a more complex
  one with the removal of water
• ex. monosaccharide monosaccharide ----gt
  disaccharide water
• (C6H12O6 C6H12O6 ----gt C12H22O11 H2O
• Polysaccharides are formed from repeated
  dehydration syntheses of water
• They are the stored extra sugars known as starch

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Hydrolysis

• Addition of WATER to a compound to SPLIT it into
  smaller subunits
• ex. disaccharide H2O ---gt monosaccharide
  monosaccharide
• C12 H22 O11 H2 O ---gt C6 H12 O6 C6 H12 O6

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Lipids (Fats)

• Why are lipids important?
• Chiefly function in energy storage, protection,
  and insulation
• Contain carbon, hydrogen, and oxygen but the HO
  is not in a 21 ratio
• Tend to be large molecules that are insoluble
  in water

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Lipids

• Lipids are formed from the union of one glycerol
  molecule and 3 fatty acids
• 3 fatty acids glycerol ----gt (lipid)
• Lipids along with proteins are key components of
  cell membranes

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PROTEINS

• contain the elements carbon, hydrogen, oxygen,
  and nitrogen
• composed of MANY amino acid subunits
• The basic amino acid form has a carboxyl group on
  one end, a methyl group that only has one
  hydrogen in the middle, and a amino group on the
  other end.
• Attached to the methyl group is a R group.

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R-Groups vary producing different amino
acids 20 amino acids exist in living things
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Why are Proteins important?

• Growth and repair
• Energy
• Carrying out chemical reactions(enzymes)

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Polypeptide (protein)

• composed of three or more amino acids linked by
  synthesis reactions
• Examples of proteins include insulin, hemoglobin,
  and enzymes.
• There are an extremely large number of
  different proteins.
• The bases for variability include differences in
  the number, kinds and sequences of amino acids in
  the proteins

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NUCLEIC ACIDS

• in all cells
• composed of NUCLEOTIDES
• store transmit heredity/genetic information
• Nucleotides consist of 3 parts
• 1. 5-Carbon Sugar
• 2. Phosphate Group
• 3. Nitrogenous Base

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DNA (deoxyribonucleic acid)

• contains the genetic code of instructions that
  direct a cell's behavior through the synthesis of
  proteins
• found in the chromosomes of the nucleus

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RNA (ribonucleic acid)

• directs cellular protein synthesis
• found in ribosomes nucleoli