Post on 01-Jan-2016
Chapter 2The Chemistry of Life
I. atomatom-smallest part of an element.
A. Made up of:
1. Nucleus
Protons (+)
Neutrons (neutral)
a. Protons’ mass = neutron mass
2. Electrons (e-) (-)
a. Move around nucleus b. Move in cloudy pathway called orbitalsorbitals.
c. Much smaller than a proton or neutrond. Same # as protons
e. (+) charge of nucleus holds the (-) e- in their orbitals.
B. ElementElement- pure substance that consists entirely of one type of atom.
6
CCarbon12.011
1. The difference between atoms of different
elements is the # of protons and electrons it has.
2. IsotopesIsotopes- atoms of the same element that have a different number of neutrons.
a. Radioactive isotopeRadioactive isotope- isotopes that have an unstable nucleus.
6 electrons6 protons8 neutrons
6 electrons6 protons7 neutrons
6 electrons6 protons6 neutrons
Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14
i. Used to determine the age of rocks and fossils, treat cancer, kill bacteria, and trace different molecules through organisms.
II. Chemical bondsChemical bonds-linkbetween atoms
A. Make:
1. CompoundsCompounds-bonding of at least two different elements.
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.
C. Types of bonds 1. Covalent bondsCovalent bonds-e- are
shared between 2 atoms.
a.Can be:
i. Single bond
ii. Double bond
iii. Triple bond
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.
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
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
3. Van der Waals forcesVan der Waals forces- an attraction between oppositely charged parts of nearby molecules.
D. Chemical formulas
1. Examples:
a. H2O
b. C6H12O6
c. CH4
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.
a. O pulls harder than H
2. Forms hydrogen bonds.
a. Because of this water has:
i. CohesionCohesion- attraction between molecules of the same substance.
- causes water’s surface tension.
http://www.worldstarhiphop.com/videos/video.php?v=wshh7jcpeM1fE63Eqwx2
b. AdhesionAdhesion- attraction between molecules of different
substances.
- causes capillary action (how water gets from the roots to stem and leaves)
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.
c. SoluteSolute- substance that is dissolved.
d. SolutionSolution- mixture of two or more substances where
each substance is evenly distributed.
e. Aqueous solutionAqueous solution- when something is dissolved in water.
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).
D. BufferBuffer- weak acids or bases that react with strong
acids or bases to prevent a sudden change in pH.
V. Compounds of Life
A. Carbon=most important element in life
1. Why?
a. Can form 4 strong covalent bonds.
b. Can form long chains or rings.
c. Can form single, double, or triple bonds.
Methane Acetylene Butadiene Benzene Isooctane
2. Organic compoundOrganic compound-any compound that contains carbon.
3. Inorganic compoundsInorganic compounds- any compound that
does not contain carbon.
VI. Macromolecules
1. MonomerMonomer- small molecule that makes up polymers.
2. PolymerPolymer- large molecules made of smaller molecules (monomers).
3. MacromoleculeMacromolecule- large polymers.
A. Four major classes of macromolecules (Carbohydrates, Lipids, Proteins, Nucleic Acids)
a. Living things use them as their main
source of energy.
1. CarbohydratesCarbohydrates- made of carbon, hydrogen,and oxygen.
b. Include sugars (monomers) and starches (polymers)
c. Simple sugars (glucose & fructose) = C6H12O6
i. Simple sugars are also called monosaccharidesmonosaccharides.
d. Organisms store simple sugars by linking them into polymers.
i. These polymers are called polysaccharidespolysaccharides.
ii. In plants = starch iii. In animals = glycogen
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.
c. Lipids are made of glycerol and fatty acids (monomers).
b. Two kinds of fats:
i. Saturated fatSaturated fat- fatty acids have the max # of H’s
ii. Unsaturated fatsUnsaturated fats- fatty acids don’t have maximum # of H’s.
3. Nucleic acidsNucleic acids- polymers assembled from individual monomers called nucleotides.
a. Nucleic acids store and transmit heredity or genetic information.
b. Two kinds of nucleic acids:
i. DNA (Deoxyribonucleic acid)
ii. RNA (Ribonucleic acid)
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
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.
General structure Alanine Serine
Amino group
Carboxyl group
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).
e. polypeptidepolypeptide- (another name for protein) several amino acids bound togetherf. The instructions for
arranging a protein are in the DNA.
1 2
34
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.
iv. Control the rate of chemical reactions and regulate cell processes.
V. Chemical ReactionChemical Reaction- process that changes one set of chemicals into another set.
A. Your body uses chemical reactions everyday.
C. ex: CO2 + H20 H2CO3
ReactantsReactants ProductsProducts
B. Chemical reactions always involve breaking bonds
and making new bonds.
D. Energy is released when chemical bonds are broken; energy is stored when chemical bonds are made.
E. Activation energyActivation energy- energy that’s needed to get a
reaction started.
1. CatalystCatalyst- molecule that speeds up a chemical reaction.
Energy-Absorbing Reaction Energy-Releasing Reaction
Products
Products
Activation energy
Activation energy
Reactants
Reactants
2. EnzymeEnzyme- protein catalyst in living things.
a. An enzyme lowers the amount of activation energy it takes to start a reaction.
Glucose
Substrates
ATP
Substratesbind toenzyme
Substratesare convertedinto products
Enzyme-substratecomplex
Enzyme(hexokinase)
ADPProducts
Glucose-6-phosphate
Productsare released Active site
b. Factors that can affect how an enzyme works:
i. Temperature
ii. pH