chapter 2 chemistry of life - linn–benton community...
TRANSCRIPT
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Chapter 2
Chemistry of Life
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Objectives:
What you need to know
• Define the terms atom, element,
molecule, and compound
• Describe the structure of an atom
• Compare and contrast ionic and
covalent types of chemical bonding
• Distinguish between organic and
inorganic chemical compounds
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Objectives:
What you need to know
• Discuss the chemical characteristics of
water
• Explain the concept of pH
• Discuss the structure and function of the
following types of organic molecules:
carbohydrate, lipid, protein, and nucleic
acid
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Levels of Chemical Organization
• Atoms
– Nucleus—central core of atom
• Proton—positively charged particle in nucleus
• Neutron—uncharged particle in nucleus
• Atomic number—number of protons in nucleus
• Atomic mass—number of protons and neutrons
combined
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Levels of Chemical Organization
• Atoms
– Energy levels—orbital regions surrounding
atomic nucleus that contain electrons
• Electron—negatively charged particle
• May contain up to 8 electrons in each level
• Energy level increases the farther away it is
from the nucleus
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Levels of Chemical Organization
• Elements, molecules, and compounds
– Element—a pure substance; made up of
only one kind of atom
– Molecule—a group of atoms bound
together in a group
– Compound—substances whose molecules
have more than one kind of atom
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Chemical Bonding
• Chemical bonds form to make atoms
more stable
– Atoms react with one another in ways that
make their outermost energy level full
– Atoms may share electrons or donate or
borrow them to become stable
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Chemical Bonding
• Ionic bonds
– Ions form when an atom gains or loses
electrons in its outer energy level to
become stable
• Positive ion—has lost electrons; indicated by
superscript positive sign(s), as in Na+ or Ca++
• Negative ion—has gained electrons; indicated
by superscript negative sign(s), as in Cl–
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Chemical Bonding
• Ionic bonds
– Ionic bonds form when positive and
negative (oppositely charged) ions attract
each other
– Electrolyte—molecule that dissociates
(breaks apart) in water to form individual
ions; an ionic compound
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Chemical Bonding
• Covalent bonds
– Covalent bonds form when atoms share their outer energy ions to complete the energy level and thus become stable
– Covalent bonds do not ordinarily easily dissociate in water
– Covalent bonding is used to form all of the major organic compounds found in the body
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Chemical Bonding
• Hydrogen bonds
– Hydrogen bonds do not create new
molecules
– Hydrogen bonds weakly bond to
neighboring molecules
– Hydrogen bonds are present in water,
DNA, and proteins
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Inorganic Chemistry
• Organic molecules contain carbon-
carbon covalent bonds and/or carbon-
hydrogen covalent bonds; inorganic
molecules do not
• Organic molecules are generally larger
and more complex than inorganic
molecules
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Inorganic Chemistry
• Water
– Water is an inorganic compound essential
to life
– Water is a solvent (liquid into which solutes
are dissolved), forming aqueous solutions
in the body
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Inorganic Chemistry
– Water is involved in chemical reactions
• Dehydration synthesis—chemical reaction in which water
is removed from small molecules so they can be strung
together to form a larger molecule
• Hydrolysis—chemical reaction in which water is added to
the subunits of a large molecule to break it apart into
smaller molecules
• Chemical reactions always involve energy transfers, as
when energy is used to build ATP molecules
• Chemical equations show how reactants interact to form
products; arrows separate the reactants from the
products
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Inorganic Chemistry
• Acids, bases, and salts
– Water molecules dissociate to form equal amounts of H+ (hydrogen ion) and OH–(hydroxide ion)
– Acid—substance that shifts the H+/OH–balance in favor of H+; opposite of base
– Base—substance that shifts the H+/OH–balance against H+; also known as an alkaline; opposite of acid
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Inorganic Chemistry
• Acids, bases, and salts
– pH—Mathematical expression of relative
H+ concentration in an aqueous solution
• 7 is neutral (neither acid nor base)
• pH values above 7 are basic; pH values below
7 are acidic
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Inorganic Chemistry
• Acids, bases, and salts
– Neutralization occurs when acids and
bases mix and form salts
– Buffers form chemical systems that absorb
excess acids or bases and thus maintain a
relatively stable pH
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Organic Chemistry
• Carbohydrates—sugars and complex carbohydrates
– Contain carbon (C), hydrogen (H), oxygen (O)
– Monosaccharides— basic unit of carbohydrate molecules (e.g., glucose)
– Disaccharide—double sugar made up of two monosaccharide units (e.g., sucrose, lactose)
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Organic Chemistry
• Carbohydrates—sugars and complex
carbohydrates
– Polysaccharide—complex carbohydrate
made up of many monosaccharide units
(e.g., glycogen; stored by the body)
– Function of carbohydrates is to store
energy for later use
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Organic Chemistry
• Lipids—fats and oils
– Triglycerides
• Formed by a glycerol unit and joined to three
fatty acids
• Store energy for later use
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Organic Chemistry
• Lipids—fats and oils
– Phospholipids
• Similar to triglyceride structure, but have
phosphorus-containing units—each with a head
and two tails
• The head attracts water and the double tail
does not, thus forming stable double layers
(bilayers) in water
• Form membranes of cells
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Organic Chemistry
• Lipids—fats and oils
– Cholesterol
• Molecules have a steroid structure made up of
multiple rings
• Cholesterol stabilizes the phospholipid tails in
cellular membranes and is also converted into
steroid hormones by the body
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Organic Chemistry
• Proteins
– Very large molecules made up of amino acids held together in long, folded chains by peptide bonds
– Structural proteins• Form essential structures of the body
• Collagen is a fibrous protein that holds many tissues together
• Keratin forms tough, waterproof fibers in the outer layer of the skin
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Organic Chemistry
• Proteins
– Functional proteins
• Participate in chemical processes of the body
• Examples include hormones, cell membrane
channels and receptors, and enzymes
• Enzymes—chemical catalysts
– Help chemical reactions occur
– Enzyme action sometimes called lock-and-key model
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Organic Chemistry
• Nucleic acids
– Made up of nucleotides
• A phosphate unit
• A sugar (ribose or deoxyribose)
• A nitrogen base (adenine, thymine or uracil,
guanine, cytosine)
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Organic Chemistry
• Nucleic acids
– DNA (deoxyribonucleic acid)
• Used as the cell’s ―master code‖ for assembling
proteins
• Uses deoxyribose as the sugar and A, T (not
U), C, and G as bases
• Forms a double helix shape
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Organic Chemistry
• Nucleic acids
– RNA (ribonucleic acid)
• Used as a temporary ―working copy‖ of a gene
(portion of the DNA code)
• Uses ribose as the sugar and A, U (not T), C,
and G as bases
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Organic Chemistry
• Nucleic acids
– By directing the formation of structural and
functional proteins, nucleic acids ultimately
direct overall body structure and function