1. PowerPoint ® Lecture Slide Presentation by Patty Bostwick-Taylor, Florence-Darlington Technical College Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings PART A 2 Basic Chemistry

2. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Balance of Life  A human body is a highly organized, ever changing collection of chemicals.  These chemicals must maintain a certain concentration or BALANCE in order for the human organism to survive

3. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Balance of Life  Example of this balance is IRON (Fe)  Blood has 4 iron atoms in each blood cell to help carry oxygen (O2)  If to little iron (Fe) in blood than cells can’t carry O2  Appears pale, fatigue, short of breath, rapid pulse

4. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Balance of Life Conversely – Too much Iron (Fe) leads to Hemochromatosis – to much iron in blood.  Iron gets stored in organs: heart, liver, pancreas destroying them over time. Disease Symptoms - joint pain, fatigue, weight loss, increased skin pigmentation. Maintaining a Chemical Balance is important for human function

5. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Introduction to Chemistry  Chemistry is the branch of science that considers the composition (what things are made up of) of matter and how this composition changes.  Understanding chemistry is essential for understanding how the body funtions

6. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Matter and Energy  Matter—anything that occupies space and has mass (weight)  Includes – all solids, liquids and gases  Energy—the ability to do work  Chemical  Electrical  Mechanical  Radiant  Potential

7. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Composition of Matter  Elements—fundamental units of matter  Living organisms require 20 different elements  96% of the body is made from four elements  Carbon (C)  Oxygen (O)  Hydrogen (H)  Nitrogen (N) Element's are composed of Atoms – the smallest unit of an element

8. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Atoms  Atoms of a single element may be similar to each other but vary between elements.  Vary in:  Size  Weight  How the attract to each other - Chemical Bond (some atoms can combine with atoms like themselves but others can not)

9. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Atomic Structure  Nucleus  Protons (p + )  Neutrons (n 0 )  Outside of nucleus  Electrons (e - ) Figure 2.1

10. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Atom Structure Since the protons in the nucleus are positively charged the and the electrons are negatively charged – when the same number of electrons match the number of protons – make a neutral charged atom

11. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Atomic Structure of Smallest Atoms Figure 2.2

12. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Identifying Elements  Atomic number—equal to the number of protons that the atom contains  Atomic Weight—sum of the protons and neutrons  IE:  Hydrogen has one proton = Atomic Weight =1  Lithium has 4 protons and 3 neutrons atomic weight = 7

13. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Isotopes and Atomic Weight  Isotopes  Have the same number of protons and electrons  Vary in number of neutrons Figure 2.3

14. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Isotopes and Atomic Weight  Atomic weight  The number of protons plus number of neutrons  Atomic weight reflects natural isotope variation

15. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Radioactivity  Radioisotope – unstable nucleus  Heavy isotope  Tends to be unstable  Decomposes to more stable isotope  Radioactivity—process of spontaneous atomic decay

16. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Molecules and Compounds  Molecule—two or more like atoms combined chemically  Compound—two or more different atoms combined chemically Figure 2.4

17. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Chemical Reactions  Atoms are united by chemical bonds  Atoms dissociate from other atoms when chemical bonds are broken

18. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Electrons and Bonding  Electrons occupy energy levels called electron shells  Electrons closest to the nucleus are most strongly attracted  Each shell has distinct properties  The number of electrons has an upper limit  Shells closest to the nucleus fill first

19. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Electrons and Bonding  Bonding involves interactions between electrons in the outer shell (valence shell)  Full valence shells do not form bonds

20. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Inert Elements  Atoms are stable (inert) when the outermost shell is complete  How to fill the atom’s shells  Shell 1 can hold a maximum of 2 electrons  Shell 2 can hold a maximum of 8 electrons  Shell 3 can hold a maximum of 18 electrons

21. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Inert Elements  Atoms will gain, lose, or share electrons to complete their outermost orbitals and reach a stable state  Rule of eights  Atoms are considered stable when their outermost orbital has 8 electrons  The exception to this rule of eights is Shell 1, which can only hold 2 electrons

22. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Inert Elements – valance shell is complete Figure 2.5a

23. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.5b Reactive Elements  Valence shells are not full and are unstable  Tend to gain, lose, or share electrons  Allow for bond formation, which produces stable valence

24. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Chemical Bonds  Ionic bonds  Form when electrons are completely transferred from one atom to another  Ions  Charged particles  Anions are negative  Cations are positive  Either donate or accept electrons

25. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Ionic Bonds Figure 2.6 +– Sodium atom (Na) (11p + ; 12n 0 ; 11e – ) Chlorine atom (Cl) (17p + ; 18n 0 ; 17e – ) Sodium ion (Na + )Chloride ion (Cl – ) Sodium chloride (NaCl) ClNaCl Na

26. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Ionic Bonds Figure 2.6, step 1 Sodium atom (Na) (11p + ; 12n 0 ; 11e – ) Chlorine atom (Cl) (17p + ; 18n 0 ; 17e – ) Cl Na

27. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Ionic Bonds Figure 2.6, step 2 Sodium atom (Na) (11p + ; 12n 0 ; 11e – ) Chlorine atom (Cl) (17p + ; 18n 0 ; 17e – ) Cl Na

28. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Ionic Bonds Figure 2.6, step 3 +– Sodium atom (Na) (11p + ; 12n 0 ; 11e – ) Chlorine atom (Cl) (17p + ; 18n 0 ; 17e – ) Sodium ion (Na + )Chloride ion (Cl – ) Sodium chloride (NaCl) ClNaCl Na

29. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Covalent Bonds PLAY Chemical Bonds  Covalent bonds  Atoms become stable through shared electrons  Single covalent bonds share one pair of electrons  Double covalent bonds share two pairs of electrons

30. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Examples of Covalent Bonds Figure 2.7a

31. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Examples of Covalent Bonds Figure 2.7b

32. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Examples of Covalent Bonds Figure 2.7c

33. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Polarity  Covalently bonded molecules  Some are non-polar  Electrically neutral as a molecule  Some are polar  Have a positive and negative side Figure 2.8

34. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Chemical Bonds  Hydrogen bonds  Weak chemical bonds  Hydrogen is attracted to the negative portion of polar molecule  Provides attraction between molecules

35. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Hydrogen Bonds Figure 2.9

36. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Patterns of Chemical Reactions  Synthesis reaction (A + B  AB)  Atoms or molecules combine  Energy is absorbed for bond formation  Decomposition reaction (AB  A + B)  Molecule is broken down  Chemical energy is released Disaccharides PLAY

37. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Synthesis and Decomposition Reactions Figure 2.10a

38. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Synthesis and Decomposition Reactions Figure 2.10b

39. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Patterns of Chemical Reactions  Exchange reaction (AB + C  AC + B)  Involves both synthesis and decomposition reactions  Switch is made between molecule parts and different molecules are made

40. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Patterns of Chemical Reactions Figure 2.10c

41. PowerPoint ® Lecture Slide Presentation by Patty Bostwick-Taylor, Florence-Darlington Technical College Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings PART A 2 Basic Chemistry

42. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Molecules and Compounds  Molecule – two or more same type of atoms bond together  Gases like hydrogen, oxygen, nitrogen common  Compound – Atoms of different molecules bond together  ie: two atoms of hydrogen bond with atom of oxygen = H2O  A molecule of a compound ALWAYS contains same kind and number of atoms – otherwise it changes – H2O2 = hydrogen peroxide

43. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Molecular Formula Molecular Formula represents the numbers and types of atoms in a molecule.  Displays the element symbol & # of atoms for each element.  ie: Water H2O = each water molecule has 2 atoms of hydrogen and one atom of oxygen  Sugar (glucose) – C6-H12-06 = 6 carbon atoms, 12 hydrogen atoms and 6 oxygen atoms

44. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Chemical Reactions #1 - Synthesis Chemical reactions either FORM or BREAK bonds between atoms, ions or molecules. Synthesis - When two or more atoms (reactants) bond to form a new more complex structure.  ie: H2 O2 synthesis H2O and gives off a single O molecule  A + B AB  Synthesis is important in growth and repair

45. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Chemical Reactions # 2 - Decomposition Decomposition – when bonds within a molecule break into simpler atoms  ie: AB A + B  Important in the breakdown of food for energy

46. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Chemical Reaction # 3 Exchange Reaction  Exchange Reaction – parts of two different types of molecules change position.  ie: AB + CD AD + CB  Example of this type is when acid reacts with a base Reversible Reactions – some reactions can go either way  (opposite arrows)

47. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Independent - Class work  Complete packet questions 1 – 12.

48. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Biochemistry: Essentials for Life  Organic compounds  Contain carbon and hydrogen  Most are covalently bonded  Example: C 6 H 12 O 6 (glucose)  Inorganic compounds  Lack carbon  Tend to be simpler compounds  Example: H 2 O (water)

49. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Inorganic Compounds  Water  Most abundant inorganic compound in living organism makes up 2/3 of the weight.  Vital properties  High heat capacity  Polarity/solvent properties – many substances dissolve in water – when smaller, chemicals have greater chance or reacting with each other  Chemical reactivity  Cushioning

50. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Inorganic Compounds  Salts  Easily dissociate into ions in the presence of water  Vital to many body functions  Include electrolytes which conduct electrical currents  Smaller ions are important to body function ie:  Transport substances in and out of cell  Muscle contraction  Nerve impulse conduction

51. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Inorganic Compounds  Acids  Release hydrogen ions (H + )  Are proton donors  Bases  Release hydroxyl ions (OH – )  Are proton acceptors  Neutralization reaction  Acids and bases react to form water and a salt

52. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.12 pH  Measures relative concentration of hydrogen ions  pH 7 = neutral  pH below 7 = acidic  pH above 7 = basic  Buffers—chemicals that can regulate pH change

53. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Organic Compounds  Carbohydrates  Contain carbon, hydrogen, and oxygen  Include sugars and starches  Classified according to size  Monosaccharaides—simple sugars  Disaccharides—two simple sugars joined by dehydration synthesis  Polysaccharides—long-branching chains of linked simple sugars

54. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Carbohydrates Figure 2.13a–b Disaccharides PLAY

55. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Carbohydrates Polysaccharides PLAY Figure 2.13c

56. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Organic Compounds  Lipids  Contain carbon, hydrogen, and oxygen  Carbon and hydrogen outnumber oxygen  Insoluble in water

57. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Lipids PLAY Lipids  Common lipids in the human body  Neutral fats (triglycerides)  Found in fat deposits  Composed of fatty acids and glycerol  Source of stored energy  Insulation  Protection

58. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Lipids  Common lipids in the human body (continued)  Phospholipids  Form cell membranes  Steroids  Include cholesterol, bile salts, vitamin D, and some hormones

59. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Organic Compounds  Proteins  Made of amino acids  Contain carbon, oxygen, hydrogen, nitrogen, and sometimes sulfur Figure 2.16

60. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Proteins  Account for over half of the body’s organic matter  Provide for construction materials for body tissues  Play a vital role in cell function  Act as enzymes, hormones, and antibodies

61. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Proteins  Amino acid structure  Contain an amine group (NH 2 )  Contain an acid group (COOH)  Vary only by R groups

62. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.17a Proteins  Fibrous proteins  Also known as structural proteins  Appear in body structures  Examples include collagen and keratin  Stable

63. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.17b Proteins  Globular proteins  Also known as functional proteins  Function as antibodies or enzymes  Can be denatured – broken apart

64. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Independent Study – Class Work  Work Packet Questions: # 13 - 17

65. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.18a Enzymes  Act as biological catalysts  Increase the rate of chemical reactions

66. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Organic Compounds  Nucleic Acids  Provide blueprint of life  Nucleotide bases  A = Adenine  G = Guanine  C = Cytosine  T = Thymine  U = Uracil  Make DNA and RNA Figure 2.19a

67. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Nucleic Acids  Deoxyribonucleic acid (DNA)  Organized by complimentary bases to form double helix  Replicates before cell division  Provides instructions for every protein in the body Figure 2.19c

68. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Organic Compounds  Adenosine triphosphate (ATP)  Chemical energy used by all cells  Energy is released by breaking high energy phosphate bond  ATP is replenished by oxidation of food fuels

69. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Adenosine Triphosphate (ATP) Figure 2.20a

70. Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Independent Work – Complete Work Book Packet  Questions: #18 - 26