 Subatomic particles  Nucleus Proton Neutron Quarks  Electrons Outside the nucleus Different distances (levels, clouds) Move randomly  Size

 Atomic number  # of protons  Mass #  # of protons + # of neutrons  Atomic mass

 Carbon  Atomic # # of protons # of electrons  Mass # # of protons + # of neutrons  Most common form of carbon  Carbon – 14  14 = mass #  # of protons  # of electrons  # of neutrons  Isotope : same # of protons, but different # of neutrons from most common form

 Boron – 11  # of protons  # of electrons  # of neutrons  Isotope?  Boron – 10  # of protons  # of electrons  # of neutrons  Isotope?

 Determine the number of protons, neutrons and electrons in each of the following  Fluorine-20  Helium-4  Which of those compounds is an isotope?

 Makes up a lot of living things  Many useful/helpful properties  Polarity  Lopped side appearance  One side slightly positive  Creates solutions  Because of charge can dissolve Other polar and ionic (fully charged) 2 or 3 types of compounds Examples  Can break apart other substances Creates suspensions Examples es/Newsletters/39/Water_related_activities.htm

 Can hold lots of heat  Takes more energy to heat up  Releases energy back more slowly  Examples  Is more dense as a liquid

 Very strong between molecules  Each water can have 4 H- bonds  Causes  Cohesion  Adhesion  Capillary action  Surface tension Surface tension ter_strider.htm transpiration/

 Water breaks down to H + and OH -  pH = how much H +  pH of 7 means H + and OH - are equal  Acids  pH lower than 7  Lower # = stronger  Examples  Bases  pH higher than 7  Higher # = stronger  Examples  Buffers  Help with homeostasis

 Define:  Cohesion  Adhesion  pH  Describe 4 reasons why water is a versatile molecule that is important to living beings  Stomach acid has a pH of 2 and ocean water has a pH of 8  Which one is acidic?  Which one is closer to being neutral?

 Atom  Molecule  Atoms are generally neutral  Ions  Atom with a charge  Sodium 11 protons + 11 electrons = neutral Gains or loses electrons 11 protons + 10 electrons = +1 Caffeine

 Make molecules  An attraction, not a physical thing  Hydrogen  Ionic  Involves ions  Gaining/losing electrons  Very strong  Covalent  Sharing electrons  Not as strong  More common

 C, H, N, O, P, S  Organic  Contains C and H  Covalent bonds  Usually large molecules  In living things  Inorganic  No C (unless simple, like CO or CO 2 )  Examples – water, O 2, N 2

 Definition  Polymer  Made of monomers  Each bond created releases water  Breaking a bond releases water

 Basics  1C:2H:1O  Main source of energy  Structural  Monosaccharides  Simple sugar  Glucose  Galactose  Fructose  Disaccharides  2 sugars  Sucrose = glucose + fructose  Lactose = glucose + galactose

 Polysaccharides  Starch  Storage in plants  Glucose units  Glycogen  Storage in animals Released from liver  Glucose units  Cellulose  Glucose units  Structure in plants Wood

 Fill in the chart with the missing vocabulary terms  Define:  Ions  Chemical bond  Macromolecule  Polymer  Give examples of monosaccharides, disaccharides, and polysaccharides Carbohydrates Composed on one subunit Composed of 2 subunits Composed of more than 2 subunits

 Fats, waxes, oils, steroids, hormones  Insoluble in water  Glycerol + fatty acid(s)  Functions  Cell structure  More efficient energy storage (9 vs. 4 calories)  Communication  Steroids  Ring of carbons  Hormones  Cholesterol

 Saturated  All single carbon bonds  Solid  Examples  Unsaturated  Carbon to carbon double bond(s)  Liquid  Examples  Good vs. bad

 Name what each is made of and a use for each:  Carbohydrate  Lipid  What is the difference between a saturated and unsaturated fat?

 Contain C, H, N, O  Made of amino acids  Very specific order or amino acids  Complex 3d shape  Chain of amino acids = polypeptide chain  Folds and crumples  May have multiple subunits  Function  Structural  Nutrient storage  Transportation  Identification of cells (defense)  Enzymes macromolecules/proteins.php

 Change shape easily  Denature  Caused by changes in  Temperature  pH  Salt concentration  Molecules present  May permanently disable the protein or cause it to malfunction  Frying an egg

 Atoms don’t change  Atoms rearranged  Chemical bonds broken and formed  Usually requires energy - activation energy  Getting energy slows down the reaction

 Proteins  Catalyst  Not changed  Lowers activation energy  Speeds up reaction  Lock and key  Substrate  Active site  Will not work if denatured  Used in most biological processes

 Proteins are complex. Describe how they form their complex structure.  In a chemical reaction, what exactly happens to the atoms?  What are 4 functions of a protein?  What does it mean to denature a protein and what cause to happen to that protein?  How are enzymes helpful to living organisms?

 Contains C, H, N, O, P  Made from nucleotides  5-carbon sugar  Phosphate group  Nitrogenous base (5 different)  Purpose – genetic information  DNA, RNA

 Outermost electrons  Participate in bonds  Fill levels in a pattern  2 in first  8 in second  18 in third  Lewis structure  Shows just valence electrons

 Macromolecules  Polymer  Monomer  Carbohydrate  Polysaccharide  Disaccharide  Monosaccharide  Lipid  Glycerol and fatty acid  Saturated  Unsaturated  Protein  Enzyme  Catalyst  Amino acid  Denature  pH  Acid  Base  Neutral  Nucleic acid  Nucleotide  Chemical bond  Hydrogen  Ionic  Covalent  Chemical reaction  Activation energy  Valence electrons  Atom  Molecule  Proton, neutron, electron  Ion  Isotope  Water  Cohesion  Adhesion  Surface tension  Capillary action  Polarity  Solution