1. Chemistry & Carbon The Cellular Basis of Life

2. Atomic Structure  Elements: smallest unit a substance can be broken down into and still have the same chemical properties 1. 92 naturally occurring elements 2. 25 of the 92 are essential to life 3. carbon, nitrogen, hydrogen, & oxygen are important 4. trace elements are required by an organism in very small amounts

3. Atomic Structure Continued  Atom: smallest form of an element, made up of …. 1. proton – positive charge; in nucleus 2. neutron – no charge; in nucleus 3. electron – negative charge; outer energy level (only 2 e-’s can occupy the same orbital)

4. Atomic Structure  Compound: 2 or more elements combined in a fixed ratio  Atomic Number: # of protons  Mass Number: # of protons + # of neutrons  Isotopes: atoms of the same elements with different numbers of neutrons  Ion: negatively charged particle

5. Bonding & Electrons  Atoms want to fill their outer energy level to b/c stable  Electrons have energy  the further from the nucleus, the more energy e- ’s have  As e-’s move to higher energy levels, energy is ADDED to them  As e-’s move back down energy levels, energy is LOST or RELEASED

6. Chemical Bonding Types of Chemical Bonds Ionic Bond Covalent Bond Hydrogen Bond Non-polar Covalent Bond Polar Covalent Bond

7. 1) Ionic Bonds  Definition: attraction of oppositely charged ions;  Lose and gain electrons  Ex. Na+ + Cl-  NaCl  The Na+ gives up one electron & the Cl- gains one electron  Easier to break than covalent bonds

8. 1) Ionic Bonds

9. 2) Covalent Bonds  Definition: two atoms share electrons; strong bond Non-polar Covalent Bond: electrons are shared equally Ex. Hydrocarbon chains

10. 2) Covalent Bonds Continued  Polar Covalent Bonds: electrons are shared unequally due to electronegativity; strong bond Ex. Water

11. 3) Hydrogen Bonds  Definition: when electrons b/w hydrogen and other atoms are shared unequally  Hydrogen has a partial positive charge  Hydrogen is attracted to slightly negatively charged atoms  Advantage: briefly together, respond & separate

12. 4) Van der Waals Interactions  Definition: weak electric forces that attract neutral molecules to one another; Ex - A non-polar molecule with areas that are positively and/or negatively charged These areas allow them to “stick” to another molecule or area of a molecule  Weak force

13. Weak Bonds  Examples of Weak Bonds are: 1. Hydrogen 2. Ionic 3. Van der Waals Forces  Advantage is…. 1. Holds a 3-D molecule in it’s correct shape 2. may form b/w molecules 3. may form b/w regions of a single molecule

14. Strong Bonds  Examples of strong bonds are: 1. Polar covalent 2. Non-polar covalent  Advantage is…. 1. bonds do not easily break 2. these bonds hold together living organisms in adverse situations

15. Carbon & Organic Chemistry  Carbon  6 protons, electrons, & neutrons  What type of bond will it form? Why?  Carbon always wants to have ____ bonds  Other elements  Element# of Bonds Nitrogen Oxygen Hydrogen

16. Types of Isomers  Structural Isomer: differ in structural arrangement of their atoms  Geometric Isomer: differ in spatial or 3-D arrangements  Stereoisomers: mirror images of each other Ex. Thalidomide

17. Structural Isomer

18. Geometric Isomer

19. Stereoisomer

20. Functional Groups & Behavior  Chemical groups attached to the carbon skeleton of a molecule Determine the “behavior”or properties of the molecule Ex – Hydroxyl =‘s polar behavior = will bond with other polar molecules Ex – Methane =‘s nonpolar behavior = will bond with other nonpolar molecules

21. Functional Groups Functional GroupFormula Hydroxyl or Alcohol-OH Carboxyl-COOH Amino-NH 2 Ketone & Aldehyde-CO & -CHO Phosphate-PO 4 Sulfhydryl-SH

22. Monomers Link to Make Polymers

23. How are Polymers Made from Monomers?  Dehydration Synthesis Aka, condensation reactions Links monomers together by removing water H (from one monomer) and OH (from another monomer combine to form water

24. How are Polymers broken back down into monomers?  Hydrolysis Breaking a polymer into many monomers by adding water

25. Dehydration Synthesis & Hydrolysis