{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Lecture Outline 2 - Biomolecules Cells Tissues Biomolecules...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
Biomolecules, Cells, & Tissues Biomolecules and Molecular Interactions Silverthorn Ref. Chapter 2 Learning Objectives: 2-1. Define and Characterize the subatomic particles of atoms and apply atomic number, atomic mass, and mole principles 2-2. List chemical elements of living organisms and explain their importance of human biomolecules through their usefulness 2-3. Describe the basic chemical reaction and apply universal laws that influences reactivity 2-4. Recognize and associate biomolecular names to chemical types, chemical formulas and attributable characteristics so that their usefulness in living cells is revealed 2-5. Explain Enzyme function with changes in activation energy and regulatory advantage to the governance of cellular metabolism 2-6. Define an aqueous solution and explain the principle of molarity in comparing solution differences in bodily fluid compartments 2-7. Explain the behavior of the biomolecules in aqueous solutions and how bodily solutions compare Key Terminology Atom, Periodic Table, Atomic Number / Mass, Proton, Neutron, Electron, Isotope, Functional Group, Molecular bonds, Biomolecule, Carbohydrate, Lipid , Protein, Amino acid, DNA, RNA, Polar, Non- Polar, Dipole, Anabolic and Catabolic reactions, Energy, Equilibrium, concentration, solution, molarity, osmolarity, mole, reactant, product, chemical bond, solubility, pH, ion, covalent, hydrophobic, hydrophilic, electronegativity, molecular weight I. Chemistry of the living cell – Metabolic Work A. Atoms and Elements 1. Components, Size and Weight- proton, neutron, electron (atom is stable when e- shell is full) 2. Electronegativity and Reactivity- B. The Essential and Trace Elements- Carbon, Oxygen, Hydrogen C. The basic Chemical Reaction 1. Reactants and Products 2. Universal Laws on Chemical Reactions
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
a. Equilibrium and Entropy b. Potential (body stores energy to be the source of input energy), Kinetic (use of energy to create reaction), and Activation Energy (barrier to getting a reaction started) c. Spontaneous and Catalyzed Reactions- to prohibit random reactions, reactions are catalyzed 3. Work is a measurement of Energy Expenditure 4. Exergonic- lowers free energy (catabolic/destructive); occur randomly bc of low activation energy 5. Endergonic- increase in energy (anabolic/synthetic); do not occur randomly bc of high activation energy D. Chemical Bonds and Molecule Formation 1. Bond type and energy a. Weak Bonds -Van der Waals Forces- proton-electron attraction; Hydrogen attracted due to dipole-- flexibility in molecule makes it more adaptable b. Strong Bonds: Ionic (attraction b/n + and -), Covalent (sharing of e-) 2. Molecule Characterization a. Mass and Complexity- molecular weight; simple or compound? b. Polarity- equal sharing of e- = nonpolar (not soluble) unequal sharing of e- = polar (soluble) c. Solubility- ability to dissolve in a solvent; fat soluble (nonpolar) v. water soluble (polar) d. Organic and Inorganic (ionic)- Organic compounds stay together (cannot overcome activation energy) II. Biomolecules- carbohydrate, lipid, protein, nucleic acid A. Carbohydrate
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}