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BIO101 HUMAN A&P
BIO101 AP Chapter 2 ECPI
| Define Chemistry | Studies composition, properties, interaction of matter |
| Define Biochemistry | Studies physiological process and disease |
| Define Matter | Anything that takes space and has weight |
| Define Mass | Amount of matter present |
| Define Weight | Heaviness due to gravitation pull on mass |
| What is matter made up of? | Atoms |
| What are the states of matter? | Solid, Liquid, and Gas |
| Describe Atoms | Smallest unit of ordinary matter Forms chemical elements Vary in size and ways they interact with other atoms Made up of subatomic substances Isotopes and radioactive isotopes |
| What are the subatomic substances? | Electrons, Protons, and Neurons |
| What are the chemical basis of life? | Elements # of protons in the nucleus determines what element an atom will be Atomic weight= pro + neu |
| Describe Molecules | 2 or more atoms chemically bond together (H2 or O3) |
| Describe Compounds | 2 or more different molecules bond together (NaCl. H2O, CO2) |
| Describe Molecule Formulas | Depict the elements present and the # of each atom present in the molecule |
| When do atoms bond? | Chemical bonds form when atoms combine with other atoms |
| What regions do electrons occupy? | Electron Shells |
| How many electrons do the 1st shell hold? | 2 Electrons |
| How many electrons do the 2nd shell hold? | 8 Electrons |
| How many electrons do the 3rd shell hold? | 8 Electrons |
| What do the electrons in the outermost shell determine? | Whether the atom will react with others |
| What are the types of Chemical Bonds? | Ionic, Covalent, and Hydrogen Bonds |
| Describe Ionic bonds | (Opposites attract) One atom gives up an electron to another atom The attraction between a cation and an anion |
| Describe Covalent bonds | Atoms share electrons Polar and nonpolar covalent bonds |
| Describe Hydrogen bonds | Helps hold water molecules together A weak bond (creates surface tension) |
| Describe a Cation | An electron Donor Loses an electron Becomes more positive |
| Describe an Anion | Electron Acceptor Gains an electron Becomes more negative |
| Describe an Ion | Electrolyes Electrically charged particles # of electrons does NOT equal the # of protons |
| Describe Covalent Bonds | Sharing of electrons Much stronger and have more energy than ionic bonds |
| Describe Polarity | Polar Covalent Bonds and Non-polar Covalent Bonds |
| Describe Polar Covalent Bonds | Unequal sharing of electrons (water and salt) |
| Describe Non-Polar Covalent Bonds | Equal sharing of electrons |
| Describe Hydrogen Bonds | Weak attraction of slightly positive end of one polar molecule to slightly negative end of a nearby polar molecules Form between adjacent water molecules Weakest type of bond Causes surface tension |
| When do chemical reactions occur? | When chemical bonds form or break between atoms, ions, or molecules |
| What are Reactants? | The starting materials of a chemical reaction (atoms, ions, or molecules) |
| What are Products? | Substances formed at the end of a chemical reaction |
| 4 types of Chemical Reactions | Synthesis, Decomposition, Exchange, Reversible |
| Describe Synthesis | More complex chemical structures is formed (A+B -> AB) |
| Describe Decomposition | Broken down bonds that form a simpler structure (AB -> A+B) |
| Describe Exchange | Bonds that are broken and form new bonds (AB + CD -> AD + CB) |
| Describe Reversible | Products that change back to the reactants (A+B <-> AB) |
| Define Electrolyes | Substances that release ions in water |
| Define Acids | Electrolytes that dissociate to release hydrogen ions in water |
| Define Bases | Susbstances that release ions that can combine with hydrogen ions |
| Define Salts | Electrolytes formed by the reaction between an acid and a base |
| Define pH | A meaure of the concentration of hydrogen ions in a solution |
| What is the level of Neutral pH? | 7.0 |
| What is the normal pH balance of human blood? | 7.35-7.45 |
| Describe Acidic | pH lower than 7.0 High H+ concentration Low OH- concentration Sour taste |
| Describe Basic | pH higher than 7.0 Lower H+ concentration Higher OH- concentration Bitter taste |
| When does Acidemia occur? | When blood pH drops to 7.0-7.3 |
| What does Acidosis do to people? | Disorientation |
| When does Acidosis occur? | Excessive vomitting of alkaline intestinal contents, diabetes, and lung disease |
| When does Alkalemia occur? | When blood pH rises to 7.5-7.8 |
| What does Alkalosis do to people? | Dizziness |
| When does Alkalosis occur? | High altitude breathing and vomitting of acidic stomach contents |
| What do Homeostatic mechanisms help? | Help regulate pH |
| Describe Inorganic Compounds | Molecules that do not contain a carbon AND a hydrogen atom Dissolve in water and dissociate, forming ions, and are electrolytes Carbon Dioxide, O2, H2O, and inorganic acids, bases, and salts |
| Describe Organic Compounds | Molecules that contain carbon AND hydrogen Found in living things Depending on the type, they will dissolve in water or organic liquids Water-soluble organic compounds do not release ions, and are non electrolytes |
| 4 main groups of Organic Compounds | Carbohydrates, Proteins, Lipids and Nucleic Acids |
| 4 Inorganic Substances | Water, O2, CO2, and Inorganic Salts |
| 4 Organic Substances | Carbohydrates, Lipids, Protein, and Nucleic Acids |
| Describe Carbohydrates | Contain carbon, hydrogen and oxygen (1:2:1 ratio) Water soluble Main source of cellular energy Made by plants (photosynthesis) |
| What are the size classification of Carbohydrates? | Monosaccharides, Disaccharides, Polysaccharides |
| Describe Monosaccharides | Single sugars 3-7 Carbon Atoms Glucose, Fructose, and Galatose Readily Absorbed |
| Describe Disaccharides | Double sugars 2 simple sugars condensed by dehydration synthesis Sucrose, Maltose, Lactose Need to be broken down |
| Describe Polysaccharides | Complex carbs Many monosaccharides condensed by dehydration synthesis Glycogen, Starch, cellulose (fiber) Need to be broken down |
| Describe Synthesis (Anabolism) | Formation of a chemical bond by removing water |
| Define Anabolism | Building up, requires energy |
| Describe Synthesis Reaction | Opposite of decomposition |
| Describe Hydrolysis (Catabolism) | Breaking things down Releases energy Decomposition Reaction |
| Describe Lipids (fats) | Hydrophobic molecules (fats, oils, waxes) Includes fatty acids, fats, steroids, phospholipids |
| Describe Fatty Acids | Long chains of hydrocarbons and a carboxyl group Saturated (no double bonds) Unsaturated (contains at least 1 carbon-carbon double bond) |
| Describe Fats | 1 glycerol molecule and 3 fatty acid chains Most abundant lipid Used for cellular energy Contains more energy per gram than carbohydrates Supplies and stores energy Insulates and protects |
| Describe Steroids | 4 connected rings of carbon Component of cell membranes Used to synthesize adrenal and sex hormones Cholesterol is the main steroid in the body Cholesterol (LDL, HDL, VLDL) |
| Describe Hormones | Estrogen, Testosterone, Corticosterioids, Calcitroil |
| Describe Bile Salts | Made in the liver and stored in the bladder Emulsifies fat |
| Describe Phosholipids | Similar to triglycerides (a glycerol head, 2 fatty acid tails and a phosphate group) Makes up cell membrane (both hydrophilic and hydrophobic) |
| Describe Proteins | Most diverse, abundant, and essential organic compounds Used as structual materials, energy source, hormones, receptors, enzymes, and antibodies Composed of 20 amino acids Basic building blocks of proteins Bound to each other by peptide bonds |
| Protein Functions | Structual support (collagen) Movement of cells and materials (transport) Buffering system to regulate pH Hormones to coordinate and control cellular functions (signaling) Form antibodies to defend the body against pathogens |
| Protein Functions Cont. | Energy Regulates the formation and breakdwon of substances in the cell via enzymes |
| Describe Enzymes | Specialized protein molecules Helps control chemical reactions Provides energy for cellular functions Organic catalysts Highly specific in their actions |
| 3 Levels of Protein Structures | Primary, Secondary, and Tertiary |
| Describe Primary Structure | Amino Acid sequence Linear Nonfunctiona protein |
| Describe Secondary Structure | Helix Formed by hydrogen bondingd between nonadjacent amino acids Alpha or Beta Nonfunctional protein |
| Describe Tertiary Structure | Polypeptide chains Unique conformation which determines function |
| Describe Denaturation | Change in secondary or tertiary structure of a protein Caused by heat, pH changes, radiation, and chemicals Sometimes reversible |
| Describe Nucleic Acid | Carry genetic material (DNA and RNA) Encode amino acid sequences of proteins Made up of subunits called Nucleotides |
| Describe DNA | Double chain of nucleotides A-T G-C |
| Describe RNA | Single chain of nucleotides A-U G-C |
| Describe Nucleotides | Building blocks of DNA and RNA Has 3 parts |
| What are the 3 parts of Nucleotides | Sugar Phosphate group Organic/Nitrogenous Base (A,G,T, C, or U) |
| Describe DNA | Double strand of nucleic acids (double helix) Stores genetics Macromolecules reside in the nucleus Direct replication, transcription and translation Controls enzyme production Controls metabolism |
| Describe RNA | Single strand Interacts with DNA to conduct protein synthesis Controls transcription |
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