1. Basic Chemistry

2. Matter and Energy
Matter – anything that occupies space and has mass (weight)
Energy – the ability to do work
Chemical- energy stored in bonds
Electrical- energy from movement of particles
Mechanical- directly involved in moving matter
Radiant-travels in waves (heat, light, x-rays)

3. Composition of Matter Elements Fundamental units of matter
96% of the body is made from four elements
Carbon (C)
Oxygen (O)
Hydrogen (H)
Nitrogen (N)
Atoms
Building blocks of elements

4. Atomic Structure Nucleus Protons (p+) Neutrons (n0) Outside of nucleus
Electrons (e-)
Figure 2.1

5. Identifying Elements Atomic number Atomic mass number
Equal to the number of protons that the atoms contain
Atomic mass number
Sum of the protons and neutrons

6. Isotopes and Atomic Weight
Have the same number of protons
Vary in number of neutrons
Figure 2.3

7. Isotopes and Atomic Weight
Close to mass number of most abundant isotope
Atomic weight reflects natural isotope variation

8. Radioactivity
Radioisotope
Heavy isotope
Tends to be unstable
Decomposes to more stable isotope
Radioactivity
Process of spontaneous atomic decay

9. Molecules and Compounds
Molecule – two or more like atoms combined chemically
Compound – two or more different atoms combined chemically

10. Chemical Reactions Atoms are united by chemical bonds
Atoms dissociate from other atoms when chemical bonds are broken

11. Electrons and Bonding
Electrons occupy energy levels called electron shells
Electrons closest to the nucleus are most strongly attracted
Each shell has distinct properties
Number of electrons has an upper limit
Shells closest to nucleus fill first

12. Electrons and Bonding
Bonding involves interactions between electrons in the outer shell (valence shell)
Full valence shells do not form bonds

13. Inert Elements Have complete valence shells and are stable Rule of 8s
Shell 1 has 2 electrons
Shell 2 has 10 electrons
10 = 2 + 8
Shell 3 has 18 electrons
18 =
Figure 2.4a

14. Reactive Elements Valence shells are not full and are unstable
Tend to gain, lose, or share electrons
Allows for bond formation, which produces stable valence
Figure 2.4b

15. Chemical Bonds 3) IONIC BONDS
a) Form when electrons are completely transferred from one atom to another
4)IONS
a) Charged particles
i)Anions are negative
ii) Cations are positive
iii)Either donate or accept electrons

16. Chemical Bonds
5) COVALENT BONDS a) Atoms become stable through shared electrons b) Single covalent bonds share one electron c) Double covalent bonds share two electrons
Figure 2.6c

17. Examples of Covalent Bonds
Figure 2.6a–b

18. Polarity- unequal sharing of e-
8) OCCURS IN COVALENTLY BONDED MOLECULES
a) Some are non-polar
i)Electrically neutral
as a molecule
b) Some are polar
i) Have a positive
and negative side
Figure 2.7

19. Chemical Bonds
9) HYDROGEN BONDS a) Weak chemical bonds b) Hydrogen is attracted to negative portion of polar molecule c) Provides attraction between molecules d) Important for i) properties of H2O ii)3-D structure of proteins iii) holding DNA strands together

20. Patterns of Chemical Reactions
11)SYNTHESIS REACTION (A+B AB) a) Atoms or molecules combine b) Energy is absorbed for bond formation 12) DECOMPOSITION REACTION (ABA+B) a) Molecule is broken down b) Chemical energy is released

21. 13)Synthesis and Decomposition Reactions
Figure 2.9a–b

22. Patterns of Chemical Reactions
14) EXCHANGE REACTION (AB+CAC+B) a) Involves both synthesis and decomposition reactions b) Switch is made between molecule parts and different molecules are made
Figure 2.9c

23. 15) Biochemistry: Essentials for Life
16) ORGANIC COMPOUNDS
a) Contain carbon
b) Most are covalently bonded
c) Example: C6H12O6 (glucose)
17) INORGANIC COMPOUNDS
a) Lack carbon
b) Tend to be simpler compounds
c) Example: H2O (water)

24. 18) Important Inorganic Compounds
19) WATER a) Most abundant inorganic compounds b) Vital properties i) High heat capacity ii) Polarity/solvent properties iii) Chemical reactivity iv) Cushioning

25. 20) Important Inorganic Compounds
21) SALTS a) Ionic compounds b) Dissociate into ions in water c) Vital to many body functions d) Include electrolytes which conduct electrical currents

26. Important Inorganic Compounds
22) ACIDS a) Can release detectable hydrogen ions 23) BASES a) Proton acceptors 24) NEUTRALIZATION REACTION a) Acids and bases react to form water and a salt

27. 25) pH
26) MEASURES RELATIVE CONCENTRATION OF HYDROGEN IONS [H+] a) pH 7 = neutral b) pH below 7 = acidic c) pH above 7 = basic d)Buffers: chemicals that can regulate pH change
Figure 2.11

28. 27)Important Organic Compounds
28) CARBOHYDRATES a) Contain carbon, hydrogen, and oxygen b) Include sugars and starches c) Classified according to size i) Mono/saccharides – simple sugars ii) Di/saccharides – two simple sugars joined by dehydration synthesis iii) Poly/saccharides – long branching chains of linked simple sugars

29. Carbohydrates
Figure 2.12a–b

30. Carbohydrates
Figure 2.12c

31. Important Organic Compounds
29) LIPIDS a) Contain carbon, hydrogen, and oxygen i) Carbon and hydrogen outnumber oxygen b) Insoluble in water- do not dissolve i) Oil in salad dressing c) Hydrophobic- water hating

32. Lipids
30) COMMON LIPIDS IN THE HUMAN BODY a) Neutral fats (triglycerides) i) Found in fat deposits ii) Composed of fatty acids and glycerol iii) Source of stored energy

33. Common Lipids in the human body (continued)
b) Phospholipids i) Form cell membranes

34. Common Lipids in the human body (continued)
c) Steroids i) Include cholesterol, bile salts, vitamin D, and some hormones
Figure 2.14a–b

35. Cholesterol a) The basis for all steroids made in the body
Figure 2.14c

36. Important Organic Compounds
32) PROTEINS a) Made of amino acids i) Contain carbon, oxygen, hydrogen, nitrogen, and sometimes sulfur 33) ACCOUNT FOR OVER HALF OF THE BODY’S ORGANIC MATTER a) Provides for construction materials for body tissues b) Plays a vital role in cell function c) ACT AS ENZYMES, HORMONES, AND ANTIBODIES

37. Proteins are made of Amino Acids
20 different amino acids
Vary by R group- gives chemical character

38. Proteins have different 3-D structures
Based on sequence of amino acids
Levels-
Primary- sequence
Secondary- twist or pleats
Tertiary- folding together
Quarternary-subunits associate

39. 34) Enzymes
a) Act as biological catalysts b) Increase the rate of chemical reactions
Figure 2.17

40. Important Organic Compounds
35) Nucleic Acids a) Provide blueprint of life b) Nucleotide bases i) A = Adenine ii) G = Guanine iii) C = Cytosine iv) T = Thymine v) U = Uracil c) Make DNA and RNA

41. Nucleic Acids
36) Deoxyribonucleic acid (DNA) a) Organized by complimentary bases to form double helix b) Replicates before cell division c) Provides instructions for every protein in the body
Figure 2.18c

42. Important Organic Compounds
37) Adenosine triphosphate (ATP) a) Chemical energy used by all cells b) Energy is released by breaking high energy phosphate bond c) ATP is replenished by oxidation of food fuels

43. Adenosine Triphosphate (ATP)
Figure 2.19a

44. 38) How ATP Drives Cellular Work
Figure 2.20