Chemistry and BiochemistryChemistry Why chemistry? Physiology all boils down to chemical reactions Matter and energy Matter Mass States: solid, liquid, gaseous Energy Kinetic Potential: stored, not yet being used, can be used Chemical: energy stored in form of chemical bonds Electrical: energy produced by movement of charged particles Mechanical Radiant/electromagnetic Composition of matter = elements (simplest components of matter) Substances that cannot be broken down into simpler substances Major elements: make up bulk of human of human body- Oxygen, carbon, hydrogen, nitrogen Lesser elements: lesser in abundance, no importance - Calcium, potassium, phosphorous, sodium, chlorine, iron Trace elements: exist in minute amounts in body mass Composition of matter = atoms Proton: have mass and electrical charge (+) Neutron: have mass and no electrical charge (neutral) Electron: have tiny mass and electrical charge (-) Nucleus = protons + neutrons- In the center- Have an anatomic cloud- Atoms are electrically neutral Always have equal number of electrons and neutrons They want to be stable Identifying elements Atomic number = number of protons Mass number Isotopes: alternate forms of atoms that differ in number of neutrons Radioisotopes: have large unstable nuclei - EX)-- Half-life: amount of times it takes for half of radioactive isotopes to decay Atomic weight: reflects average mass Combinations of matter Molecules: put two or more atoms together by chemical bonds But more than one of the same, you have molecule of element Ex) O2 Compounds: put two different atoms together Ex) H2O (H+ and O- and H+) Mixtures: mixing substances without chemical bonds Solutions Colloids Suspensions Solvent: substance that exists in greater quantity Solute: substance that exists in lesser quantity Chemical Bonds Come together by the interaction of electrons Electron shells: organized around the nucleus Can have up to 7 electron shells Can hold max number of electrons Valence shell: most outside shell- Determine chemical properties and kinds of atoms it can make 1st=2, 2nd=8, 3rd=18, 4th=32, 5th=50- 2(n)^2 n=number of electron shell- ex) 2(1)^2 2(1) 2 Rule of 8: stable with 8 or if number it is allowed - Ex) 3rd is stable with 8 or 18- Except the 1st one is only stable with 2 Covalent bonds: electrons shared between interacting atoms, between shells Electrons shared- Single (pairs), double (2 pairs), triple (3 pairs of electrons) bonds- Ex) oxygen atom + oxygen atom = molecule of oxygen gas (O2) or O=O (structural formed shoed double bonds)- Reacting atoms = resulting molecules- Polar vs. Non-polar - One has partial (-) and one has partial (+) H+ --- O- --- H+ polar covalent O=C=O nonpolar covalent Ionic Bonds Electrons transferred- Cations (+) and anions (-)- Ex) sodium ion (Na+) and chloride ion (Cl-) = sodium chloride (NaCl) Opposites attract Hydrogen bonds By itself weak, but together strong Bonds between different ends of polar molecules negative O is attracted to positive H Chemical Reactions Chemical bonds are made, broken, or rearranged Chemical equations Reactants Products Number of atoms - Reactants product Ex) H + H H2 (hydrogen has) Ex) 4H + C CH4 (methane gas) Synthesis (combination) reactions: chemical bonds are formed Smaller particles are bonded together to form larger, more complex molecules Anabolic A + B AB Ex) dehydration (condensation) reaction - AH + BOH H2O + AB- Get principle product (AB) and product of H2O Require energy… traps energy Decomposition reactions: chemical bonds being broken down Bonds are broken in larger molecules, resulting in smaller, less complex molecules Catabolic: energy released AB A + B Ex) Hydrolysis- AB + H2O AH + BOH Exchange (displacement) reactions: chemical bonds being broken and made Both synthesis and decomposition AB + C AC + B Oxidation-reduction (redox) reactions Electrons exchange LEO says GER Often involves gain/loss of hydrogen atoms Energy flow Exergonic: energy is released Endergonic: energy is being required/put in Reversibility Equilibrium: forward = reverse Some will spontaneously reverse Rate Temperature (increase = increase chemical reactions) Concentration (increase = increase chemical reactions) Particle size (decrease = increase chemical reactions) Catalysts (presence of this increase chemical reactions)- Ex) enzymes Biochemistry Organic compounds (can share metabolic pathways, all have C, O, H) Carbohydrates, proteins, lipids, nucleic acids All are made up of sub groups called monomers Bio molecules are formed from their monomers/units by dehydration synthesis and broken down to monomers by hydrolysis reactions Monomer dimer polymer Functional groups Carboxyl (-COOH) Amino (-NH2) Hydroxyl (-OH) Phosphate (-PO4) Carbohydrates Cellular fuel Monosaccharides (combine through dehydration synthesis)- Monomers- Glucose, fructose, galactose (glucose + fructose = sucrose) Disaccharides- Polymers Polysaccharides- Polymers Lipids (fats and oils) Membrane that surrounds the cell and is in cell- Doesn’t dissolve in H2O, but dissolve in some other lipids Hydrophobic Cell membranes, hormones, etc Triglycerides- Neutral fats, fatty acids (saturated vs. unsaturated… 1+ double bond)- Glycerol + 3 fatty acid chains triglyceride (neutral fat) + 3 H2O molecules Phospholipids - Polar head, non-polar tail- Phosphorous containing group (polar head=hydrophilic) + glycerol backbone + 2 fatty acid chains (non-polar tail=hydrophobic) Steroids Eicosanoids Proteins Most abundant, very diverse Support, movement (contractile), buffering, catalysts, etc Polymers of amino acids Amine group + acid group + central carbocation (can be bother weak acids and bases)- Ex) amino acids (50 attached, polypeptide chain, 8____, 12___)- R group (central carbocation) determines function Amino acid structures- Glycine, aspartic acid, lysine, cysteine Structural levels: attached by peptide bonds - Primary: chain of amino acids- Secondary: helix or pleated sheet- Tertiary:
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