chapter 2 the chemistry of life. atom i. atom-smallest part of an element
TRANSCRIPT
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Chapter 2The Chemistry of Life
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I. atomatom-smallest part of an element.
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A. Made up of:
1. Nucleus
Protons (+)
Neutrons (neutral)
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a. Protons’ mass = neutron mass
2. Electrons (e-) (-)
a. Move around nucleus b. Move in cloudy pathway called orbitalsorbitals.
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c. Much smaller than a proton or neutrond. Same # as protons
e. (+) charge of nucleus holds the (-) e- in their orbitals.
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B. ElementElement- pure substance that consists entirely of one type of atom.
6
CCarbon12.011
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1. The difference between atoms of different
elements is the # of protons and electrons it has.
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2. IsotopesIsotopes- atoms of the same element that have a different number of neutrons.
a. Radioactive isotopeRadioactive isotope- isotopes that have an unstable nucleus.
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6 electrons6 protons8 neutrons
6 electrons6 protons7 neutrons
6 electrons6 protons6 neutrons
Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14
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i. Used to determine the age of rocks and fossils, treat cancer, kill bacteria, and trace different molecules through organisms.
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II. Chemical bondsChemical bonds-linkbetween atoms
A. Make:
1. CompoundsCompounds-bonding of at least two different elements.
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B. Why do atoms bond to each other?
1. To fill their electron orbitals.
2. MoleculeMolecule-two or more atoms joined together by a covalent bond.
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C. Types of bonds 1. Covalent bondsCovalent bonds-e- are
shared between 2 atoms.
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a.Can be:
i. Single bond
ii. Double bond
iii. Triple bond
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2. Ionic bondsIonic bonds- when e- are lost or gained, then the resulting ions attract.
a. ionion- an atom that has gained or lost e-, therefore acquiring a charge.
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Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na+) Chloride ion (Cl-)
Transferof electron
Protons +11Electrons -11Charge 0
Protons +17Electrons -17Charge 0
Protons +11Electrons -10Charge +1
Protons +17Electrons -18Charge -1
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Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na+) Chloride ion (Cl-)
Transferof electron
Protons +11Electrons -11Charge 0
Protons +17Electrons -17Charge 0
Protons +11Electrons -10Charge +1
Protons +17Electrons -18Charge -1
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3. Van der Waals forcesVan der Waals forces- an attraction between oppositely charged parts of nearby molecules.
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D. Chemical formulas
1. Examples:
a. H2O
b. C6H12O6
c. CH4
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III. WaterA. Properties of water1. PolarPolar- has a slight positive
charge on one end of the molecule, and a slight
negative charge on the other end b/c one atom pulls e- closer than the other.
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a. O pulls harder than H
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2. Forms hydrogen bonds.
a. Because of this water has:
i. CohesionCohesion- attraction between molecules of the same substance.
- causes water’s surface tension.
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b. AdhesionAdhesion- attraction between molecules of different
substances.
- causes capillary action (how water gets from the roots to stem and leaves)
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3. Water is the universal solvent.
a. b/c it’s polar, it pulls apart other molecules (things
dissolve in it easily).
b. SolventSolvent- substance in which the solute dissolves.
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c. SoluteSolute- substance that is dissolved.
d. SolutionSolution- mixture of two or more substances where
each substance is evenly distributed.
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e. Aqueous solutionAqueous solution- when something is dissolved in water.
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IV. pH scale (ranges from 0-14)
A. H20 H+ + OH-
C. basebase- produces OH- ions (>7-14).
B. acidacid- produces H+ ions (0<7).
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D. BufferBuffer- weak acids or bases that react with strong
acids or bases to prevent a sudden change in pH.
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V. Compounds of Life
A. Carbon=most important element in life
1. Why?
a. Can form 4 strong covalent bonds.
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b. Can form long chains or rings.
c. Can form single, double, or triple bonds.
Methane Acetylene Butadiene Benzene Isooctane
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2. Organic compoundOrganic compound-any compound that contains carbon.
3. Inorganic compoundsInorganic compounds- any compound that
does not contain carbon.
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VI. Macromolecules
1. MonomerMonomer- small molecule that makes up polymers.
2. PolymerPolymer- large molecules made of smaller molecules (monomers).
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3. MacromoleculeMacromolecule- large polymers.
A. Four major classes of macromolecules (Carbohydrates, Lipids, Proteins, Nucleic Acids)
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a. Living things use them as their main
source of energy.
1. CarbohydratesCarbohydrates- made of carbon, hydrogen,and oxygen.
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b. Include sugars (monomers) and starches (polymers)
c. Simple sugars (glucose & fructose) = C6H12O6
i. Simple sugars are also called monosaccharidesmonosaccharides.
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d. Organisms store simple sugars by linking them into polymers.
i. These polymers are called polysaccharidespolysaccharides.
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ii. In plants = starch iii. In animals = glycogen
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2. LipidsLipids- are made mostly of carbon and hydrogen and includes waxes, fats, & oils.
a. Lipids are used to store energy.
b. Lipids are an important part of biological membranes.
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c. Lipids are made of glycerol and fatty acids (monomers).
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b. Two kinds of fats:
i. Saturated fatSaturated fat- fatty acids have the max # of H’s
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ii. Unsaturated fatsUnsaturated fats- fatty acids don’t have maximum # of H’s.
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3. Nucleic acidsNucleic acids- polymers assembled from individual monomers called nucleotides.
a. Nucleic acids store and transmit heredity or genetic information.
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b. Two kinds of nucleic acids:
i. DNA (Deoxyribonucleic acid)
ii. RNA (Ribonucleic acid)
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b. Each nucleotide (monomer of nucleic acids) is made up of:
i. 5-carbon sugar (Ribose in RNA and Deoxyribose in DNA)
ii. Phosphate group
iii. Nitrogenous base
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3. ProteinsProteins- polymers of molecules of amino acids.
a. There are 20 different amino acids.
b. Each amino acid has an amino group (NH2) and a carboxyl group (COOH) at the end.
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General structure Alanine Serine
Amino group
Carboxyl group
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c. Each also has an “R” group that is different for every amino acid.
d. When two amino acids bond, the COOH bonds to
the NH2 to form a peptide bond and water (H2O).
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e. polypeptidepolypeptide- (another name for protein) several amino acids bound togetherf. The instructions for
arranging a protein are in the DNA.
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1 2
34
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g. Proteins have many functions including:
i. Providing structure (making muscle, bone, etc.)
ii. Transport substances in and out of the cell.
iii. Fight off diseases.
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iv. Control the rate of chemical reactions and regulate cell processes.
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V. Chemical ReactionChemical Reaction- process that changes one set of chemicals into another set.
A. Your body uses chemical reactions everyday.
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C. ex: CO2 + H20 H2CO3
ReactantsReactants ProductsProducts
B. Chemical reactions always involve breaking bonds
and making new bonds.
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D. Energy is released when chemical bonds are broken; energy is stored when chemical bonds are made.
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E. Activation energyActivation energy- energy that’s needed to get a
reaction started.
1. CatalystCatalyst- molecule that speeds up a chemical reaction.
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Energy-Absorbing Reaction Energy-Releasing Reaction
Products
Products
Activation energy
Activation energy
Reactants
Reactants
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2. EnzymeEnzyme- protein catalyst in living things.
a. An enzyme lowers the amount of activation energy it takes to start a reaction.
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Glucose
Substrates
ATP
Substratesbind toenzyme
Substratesare convertedinto products
Enzyme-substratecomplex
Enzyme(hexokinase)
ADPProducts
Glucose-6-phosphate
Productsare released Active site
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b. Factors that can affect how an enzyme works:
i. Temperature
ii. pH