Transcript Chemistry 1
Chemistry For Life • Matter - occupies space and has mass • Elements - C,H,O,N,S,Fe,Ca,Na,Cl,K; make up matter and can’t be decomposed by ordinary chemical means • Atoms • Protons • Neutrons • Electrons location weight charge • Protons - nucleus • Neutrons - nucleus • Electrons - orbit 1 1 0 + none - • Atomic number - number of protons • Atomic weight - protons + neutrons • Ions - cations (+ ions that have lost an electron), anions (- ions that have gained an electron) • Isotope - same atomic number, different atomic weight - thus the number of neutrons differs • Radioisotopes - break down and emit radiation that may be of clinical value Covalent - sharing of a pair of electrons Ionic - giving and taking electrons • Hydrogen - weak attraction between the positive part of one polar molecule and the negative part of another polar molecule; provides stability to large molecules Atomic Combinations • Molecules - stable combination of 2 or more elements • Polar - electrons are unequally shared • Nonpolar - electrons are equally shared • Compounds - stable combination of 2 or more different kind of elements • Synthesis - anabolism - building molecules • Decomposition - catabolism - breaking molecules down • Exchange - buffers • Reversible - goes in both directions depending on the conditions • Oxy-Redox - leo the lion goes ger Factors Influencing Reactions • Temperature - rises increase speed of reactions to a point and vice versa • Concentration - same as temp. • Particle size - smaller ones act faster • Catalysts - speed up reactions • Kinetic energy (being used) and potential energy (being stored) • Chemical - in bonds • Mechanical - muscles moving body • Radiant - heat or light • Electrical - flow of electrons in nerve impulses Inorganic Compounds • Lack carbons bonded to hydrogens • Water - 60-80% of our weight • Acids - release H ions when dissociating in water; tastes sour • Bases - release OH ions when dissociating in water; tastes bitter • pH - a measure of how acidic or basic a substance is. It runs from 0, which is most acidic, to 14, which is most basic. 7 is neutral. • Buffers - maintain the pH of a particular region by forming weaker acids or bases • Salts - dissociates into cations and anions, which are not H or OH ions, when in water Organic Compounds • Compounds containing carbon bonded to hydrogen and oxygen • C, H, O • Monosaccharides • Glucose - blood sugar • Fructose - the sweetest sugar • Ribose - part of RNA • Disaccharides • Lactose - milk sugar • • • • • • Sucrose - table sugar Maltose - in beer Polysaccharides Starch - our most abundant dietary carbohydrate Glycogen - our stored carbohydrate in our muscle and our liver Cellulose - a fiber that keeps us regular • C, H, O • Fats and oils - glycerol + 3 fatty acids, a triglyceride; SFA, MUFA, PUFA • Eicosanoids such as prostaglandins which influence the cells that produce them • Phospholipids - build cell membranes • Sterols - cholesterol, sex hormones • Vitamins - A, D, E, K • C, H, O, N • Amino acids - amino, carboxyl, hydrogen and radical around a C; they bind by peptide bonds to make polypeptides • Enzymes are all proteins – they catalyze reactions and often require coenzymes (vitamins or minerals); work like a lock and key Other Organic Compounds • Nucleic acids - DNA, RNA ATP Structure • ATP - the energy compound • Cyclic AMP involved in hormone and neurotransmitter action