Objective 1

1
Objective 1

• Students must explain the properties of Carbon
  that make it the perfect building block for
  natural compounds.

2
Objective 2

• Students should be able describe the role of
  atomic structure and electron transfer and
  sharing as it applies to oxidation and reduction.

3
Objective 3

• Students must be able to describe the unique
  physical properties of water and explain their
  importance to living systems in four different
  ways.

4
Objective 4

• Students must be able to read and explain the
  changes in the pH scale .

5
Objective 5

• Students must be able to identify 6 functional
  groups of importance to biochemistry.

6
Objective 6

• Students must be able to apply the IUPAC rules of
  nomenclature to hydrocarbon compounds.

7
Objective 7

• Students must be able to identify, draw, and
  describe the role of four major classes of
  Biomolecules.

8
Objective 8

• Students must be able to identify at least 5
  different types of proteins in living organisms
  by different functions and state their structural
  significance.

9
Objective 9

• Students must be able to describe three examples
  of hydrolysis and dehydration synthesis. In the
  anabolism and catabolism of biologically
  important polymers .

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The Chemistry of Life

• Life requires about 25 chemicals

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Element

• all one type of atom

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Most Abundant Chemicals in Life

• Carbon
• Oxygen
• Hydrogen
• Nitrogen
• Ca, P, K, S, Na, Cl, Mg gt 4

96
13
Compound

• two or more different elements chemically
  combined

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Molecule

• Smallest portion of a substance that still
  retains the properties of that substance
• Two or more atoms combined by a covalent bond

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Atom

• Smallest particle of matter that exists under
  ordinary means

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Nucleus

• Central portion of an atom containing protons and
  neutrons- it contributes to its mass

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Proton (Atomic Number)

• Positive charged particle in the nucleus

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Neutron

• Neutral particles in the nucleus
• number is found by subtracting the atomic number
  from the atomic mass

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Mass Number(Atomic Mass)

• Number of protonsneutrons
• Protons and neutrons have similar mass of 1
  DALTON each

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Isotope

• Elements that have the same number of protons but
  differ in their number of neutrons. ( C12 and
  C14)
• if C12 has 6 protons ____neutrons
• C14 has ______neutrons?

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Electrons

• Negative charge no mass - outside the nucleus

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Energy and Electrons

• The potential energy of electrons increases as
  their distance from the nucleus increases
• Electrons may shift to different energy levels
  with addition of or loss of energy

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Energy Level

• Describes the approximate location of electrons (
  2/8/8) Lowest level holds 2 the next holds 8
  while higher levels hold up to 18.

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Ion

• Result from the loss or gain of electrons

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Ionic Bond

• Bonds resulting from the attraction of opposite
  ions ex. Na Cl-
• Stronger but less stable

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Covalent Bond

• results from the sharing of electrons

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Polar Covalent Bond

• Electrons are not shared equally

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Carbon is special

• Tetrahedral structure- four valence electrons
  shared
• Covalent bonds - stability

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Carbon is Special

• Variations are possible in carbon molecules that
  provide diversity
• Isomers are possible
• structural- differ in structure same
  chemical formula
• geometric-differ in spatial
  relationship
• enantiomers-mirror images of each
  other

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Physical Properties

• Due to the polar nature of water
• Hydrogen bond- weak attraction between hydrogen
  on adjacent molecules such as water

H H O
H H O
Hydrogen bond
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Water and its importance to Life

• Life evolved in water
• Waters unique properties have made life as we
  know it possible

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Physical Properties

• Heat of vaporization- amount of energy that is
  released or gained when changing state from
  liquid to gas or back

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Physical Properties

• High Specific Heat- the amount of heat absorbed
  or released when water changes temperature by one
  degree C. ( 1 cal. )

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Ice Floats

• As a liquid waters hydrogen bonds continuously
  break and reform
• As a solid four molecules form hydrogen bonds
  creating crystals with open channels and thus
  fewer molecules per area.

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Physical Properties

• Water reaches maximum density at 4 degrees C.
• Water is a universal solvent due to its polar
  nature

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Evaluate the importance of the following and
explain the property of water responsible.

• Cytoplasm is 98 water
• Ice Floats
• Lake effect temperature moderation
• Evaporative Cooling
• Spring-Fall Overturn

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Molarity-moles of solute dissolved in a liter of
water

• Mole amount of substance whose mass in grams
  equals its molecular weigh( formula weight )
• Has 6.02 X 10 23 number of molecules

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Solutions

• Homogeneous-same throughout
• solvent- what you are dissolving into
• solute- what you dissolve

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Suspensions

• Particles settle out over time due to size

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Colloids

• Particles are intermediate in size and do not
  settle out but are not homogeneous like a solution

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solution

SOLUTE




SOLVENT
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Hypertonic
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Hypotonic
. . . . . . .
. . .
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Isotonic
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Acid-Base Definitions

• An acid is a substance that . . .
  dissociates in water to produce hydrogen
  ions

• A base is a substance that . . . dissociates
  in water to produce hydroxide ions

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Classifying Common Materials

• Common Acids 1. Vinegar 2. Milk 3. Lemon
  Juice 4. Toilet bowl cleaner 5. Soda 6.
  Foot Powder

• Common Bases 1. Ammonia 2. Baking Soda 3.
  Washing Soda 4. Detergents 5.
  M.O.M. 6. Lime

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pH scale

• Appropriate pH
• 1
• 2
• 3
• 13
• 12
• 11

• 0.1 M HCl
• 0.01 M HCl
• 0.001 M HCl
• 0.1 M NaOH
• 0.01 M NaOH
• 0.001 M NaOH

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The pH Scale
-

• pH

log
H
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Neutralization
H (From the acid)

OH-- (From the base)
H2O (neutral product)
gt
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The General Reaction

• This can be represented as . . .

Acid Base gt
Water Salt
HA MOH gt
H2O MA
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Buffers

• Resist changes in pH
• Accept H ions from solutions when they are in
  excess
• Donate H ions when they are depleted

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Blood and Pond Water

• Most buffers are weak acids or weak bases.

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H2C03 HCO3- H
acceptor
donor