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AP Biology

AP Biology. Biochemistry: Chemistry Basics. Most Common Elements in all life forms. CHNOPS (The most common elements in ALL life forms.) and Trace elements (present in small amounts). Iodine deficiency. Atom

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AP Biology

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  1. AP Biology Biochemistry: Chemistry Basics

  2. Most Common Elements in all life forms CHNOPS (The most common elements in ALL life forms.) and Trace elements (present in small amounts)

  3. Iodine deficiency

  4. Atom • The smallestunit of matter that has chemical properties because of it having all the subatomic parts. • Atoms still maintain their original properties of that element, because the subatomic parts are all present.

  5. Subatomic Particles (Small parts that make up atoms.)(sub means “below” or “lower”) • Proton (These particles carry a positive charge.) (They are located in the nucleus of an atom.) • The number of protons never changes in an element. (This allowed the Periodic Table to be created.) • Neutron (These particles carry NO charge, which is called neutral.)(They are also located in the nucleus of an atom.) • The number of neutrons can change. (Atoms with different numbers of neutrons than the normal amount for that element are called Isotopes.)

  6. Electrons (These particles carry a negative charge.) (They are located in the “Electron cloud”. • The cloud is created because electrons move at the speed of light which creates a blur around the atom.) • The electrons moving, which is called kinetic energy, is why they are associated with energy and batteries. • It is potential energy when they are bonded. The symbol is e-.

  7. Cloud of negative charge (2 electrons) Electrons Nucleus LE 2-4

  8. The number of electronscanchange. (Atoms with different numbers of electrons than the normal amount for that element are called Ions.)

  9. Molecule • Two or more atoms bonded together. (They maybe the same type of atom or they maybe different atoms.)

  10. Molecule: Same element

  11. Molecule: Different elements

  12. Energy (represented by the symbol “E”) • Energy comes primarily from the rapid movement of electrons (e-). • Potential Energy (PE) – Energy of position. (Usually refers to electrons “locked” in a chemical bond.) • Kinetic Energy (KE) – Energy of movement. (Usually refers to electrons that can move freely.)

  13. E levels or e- shells – Where the electrons or E is located within an atom or molecule. • Adding energy to electrons makes them move farther out; losing energy causes them to move inward.

  14. Third energy level (shell) Energy absorbed Energy and Atoms Second energy level (shell) First energy level (shell) Energy lost Atomic nucleus

  15. Valence Shell- Where the outer most electrons are located on an atom. • Valence e- - Refers to the outer most electrons. (These are the most important for chemical bonds and the chemical properties of an element or molecule.) • Valence – Refers to the bonding capacity of an atom. (Depends on the number of valence electrons.)

  16. Valence Electrons

  17. Chemical Bonds (These occur between elements or molecules.) • These are attempts to fill the outer most shell (valence shell) so as to become stable molecules. • Covalent Bonds • This type is the strongest type of chemical bond. • Results from sharing electrons between elements or molecules to fill both outer shells. • They always create a molecule. (The size of the molecule may differ though.) • Two or more atoms together of any kind.

  18. Covalent Bonds

  19. Polarmolecules carry an electrical charge at opposite poles(poles refers to the “ends” of the molecule) and non-polar molecules do not have an electrical charge. • Ex: H2O

  20. – POLAR MOLECULE O H H + + H2O

  21. Electronegativity • Refers to the element’s or molecule’s desire to acquire or release electrons. • Hydrogen atoms (The LEAST electronegative biological element. It wants to RELEASE e-) • Oxygen (The MOST electronegative biological element. It wants to ACQUIRE e-)

  22. Structural Formula is used to show the shape of the molecule. • Molecular Formula are used to tell the elements, and number of atoms of each, that make up a molecule. • A.K.A. Chemical Formula

  23. ISOMERS • MOLECULES WITH THE SAME FORMULA BUT A DIFFERENT ARRANGEMENT OF ATOMS AND DIFFERENT PROPERTIES

  24. (stereoisomers)

  25. Monosaccharides- Structural Isomers

  26. Alpha-glucose------Beta-glucose Geometric isomers-changed the position of the functional groups

  27. Small changes in the position of atoms may dramatically change the chemistry of a molecule. Geometric isomer-changed the position of the functional groups Structural isomers-change the arrangement of the carbon atoms Ex: glucose and fructose

  28. L-Dopa (effective against Parkinson’s disease) D-Dopa (biologically inactive) Figure 4.8 Enantiomers: Are important in the pharmaceutical industry.

  29. Ionic Bonds • These are fairly strong bonds while dry – but are weak in water so they dissolve into ions. • These bonds are created by swapping electrons between elements so that each element can fill it’s outer most shell. • When dissolved in water Ions (charged particles) are created. (Gatorade is a ion loaded drink.) • Cations – possess a positive charge because it has more protons than electrons. • Anions – possess a negative charge because it has more electrons than protons.

  30. Ionic Bonds

  31. THESE LOVE WATER. (Because water is a polar molecule too.)

  32. SALT • Ionic Compounds • A cation bonded to an anion to make a salt when dry. Na+ Cl–

  33. Hydrogen Bonds • Fairly weak bonds. (It is “like” a magnet) (A positive Hydrogen attracted to a negative “Substance”…USUALLY oxygen.) • THESE ARE THE MOSTIMPORTANT BIOLOGICAL BONDS

  34. – + Water (H2O) HYDROGEN BONDS + Hydrogen bond – Ammonia (NH3) + + +

  35. Van der WaalsInteractions • These are temporary bonds. (Usually a fraction of a second.)(Involves enzymes mostly.) • These interactions are “created” when electrons clump on one side of an atom making that side temporarily “negative” and the other side “positive” so that charged particles can attach momentarily and then they unclump, because electrons are moving, and the “interaction” disappears because of loss of the charge.

  36. Van der Waals Interactions e- e- e- e- e- e- e- e- NUCLEUS

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