1. Chapter 2 The Chemistry of life Objectives What three subatomic particles make up atoms? How are all of the isotopes of an element similar? Calculate the number of subatomic particles in an atom from the atomic number and mass number of that atom. Homework – S. R. 2-1 loose leaf Do Now!! "...protons give an atom its identity, electrons its personality." — Bill Bryson (A Short History of Nearly Everything)Bill BrysonA Short History of Nearly Everything What do you think he is saying???

3. Do Now/Quiz Label Each Structure 1._________ 1.Electron 2.___________ 2. Proton 3.__________ 3. Neutron

4. The Chemistry of Life Cell (skin cell) basic building block of living organisms (life) Atom basic building block of matter

5. subatomic particlesThe parts that make up an atom are called subatomic particles. –Protons (p+) positively charged particle –Neutron (n) neutral particle (uncharged) –Electrons (e-) negatively charged particle nucleusNeutrons and Protons are located in the nucleus of an atom. Electrons orbit around the nucleus

6. Where can we find a list of all the different types of atoms? The Periodic Table of Elements? How do elements and atoms fit together? An element is made of only one type of atom.

7. How do atoms of different elements differ from one another? (How does a helium atom differ from a carbon atom?) They contain different numbers of –Protons And most of the time –Electrons –Neutrons Carbon Atomic Number = 6 Mass Number = 12

8. The Periodic Table and Atoms Atomic Number – Gives us the number of electron and protons in an atom. Atom Mass –Tells us the atomic mass of an atom of that element

9. How do we know how many neutrons there are in an atom? 1 proton = 1 atomic mass unit 1 neutron = 1 atomic mass unit 1 electron = nothing –Electrons are 1/1840 the size of a proton or neutron. –They do not factor into the atomic mass of an element

10. Draw Your Own Atoms Hydrogen, Carbon, Nitrogen, Oxygen

11. Question 1 Create this table and fill in the blanks. ElementAtomic # Atomic Mass ProtonsElectonsNeutrons Ar1839.948 amu He22 O15.999 amu 8

12. Isotopes An atom is determined by the number of protons. –If the number of protons change you have an atom of a different element The chemical properties of an atom are determined by the number of electrons. –If the number of electrons change the chemical properties of that atom will change, but it will still be the same element. However, the number of neutrons in the atom of an element can be change and still have the same element. Isotopes - Atoms of the same element with different numbers of neutrons

14. Today you will learn about: Objectives How are isotopes of an element similar? Compare and contrast ionic, covalent, and hydrogen bonds. Homework - None Do Now!! Draw the Bohr Model for Na.

15. Isotopes Because they have the same number of electrons, all isotopes of an element have the same chemical properties.

16. Radioactive Isotopes Radioactive decay – the break down of the nucleus of an atom Radioactive Isotopes –Isotopes where the nucleus is unstable and breaks down at a constant rate over time –Radioactive isotopes can be useful is a variety of ways

17. SubstanceSubstance –That which has mass and occupies space; matter. –A substance is pure meaning: A material of a particular kind or constitution. Chemical CompoundA Chemical Compound is a substance formed by the chemical combination of two or more elements is definite proportion. –Molecule –Molecule – A compound bound together by covalent bonds. –Ionic Compound – A compound bound together by ionic bonds. Chemical Compounds

18. The Octet Rule The octet rule says that atoms tend to gain, lose or share electrons so as to have eight electrons in their outer electron shell. –It is a very useful rule but you should also know that there are many bonding situations where it does not apply. Very simply, when atoms bond together they want to have 8 electrons in their outer shell.

19. Sodium As a pure substance sodium is a soft metal which can be easily cut. Its atomic number is 11.

20. When sodium is added to water it reacts violently.

21. Chlorine As a pure substance chlorine is a poisonous gas. Its atomic number is 17.

22. What do we get if we combine Na and Cl.

23. Homework Objectives –Compare and contrast ionic bonds and covalent bonds. –Describe a hydrogen bond. –Describe the emergent properties of water 2-1 and 2-2 handouts will be collected tomorrow Quiz tomorrow –Atoms, subatomic particles –Atomic number, Atomic Mass –Isotopes –Ionic, covalent bonds Using H+ and OH-, describe an acid, a base, and a neutral solution.

24. Ionic Bonds A bond between atoms when electrons are transferred.

25. Covalent Bonds A bond between atoms when electrons are shared. Types of covalent bonds: -single bond -double bond -triple bond

26. WATER (H 2 O)

27. Electronegativity and Polarity Electronegativity – the affinity (want) for electrons. A water molecule is polar because there is an uneven distribution of electrons between the oxygen and hydrogen atoms.

28. TIMEOUT from WATER

29. Van Der Waals Forces Forces of attraction between molecules. Not nearly as strong as ionic or covalent bonds. Molecule – smallest unit of most covalently bound compounds.

30. Hydrogen Bonds A type of Van Der Waals force. Not as strong as Ionic or covalent bonds

31. Cohesion The attraction between molecules of the same substance

32. Adhesion The attraction between molecules of different substances.

33. Capillary Action Combination of adhesion and cohesion

34. Why does polarity and hydrogen bonding makes water so special? 1.Less dense as a solid 2.Universal Solvent 3.High Specific Heat

35. #1 ICE Floats ICE FLOATS Water is one of the only substances that expands when is freezes. Almost all other substance constricts when temperature drops. This occurs because of the polarity of the molecule. Ice is less dense than water.

36. #2 - Water is the “UNIVERSAL SOLVENT” Water has the ability to dissolve a vast amount of different substances. Mixture – material composes of 2 or more elements (or compounds) which can be physically separated. –Two types of mixtures are Solutions – mixture where all components are evenly distributed (salt water) Suspensions – mixture of water that contains nondissolved materials (pond water)

37. Solutions Solute – the substance that is dissolved. Solvent – the substance that dissolves the solute.

38. Acids, Bases, and the pH Scale Quiz pushed back until Thursday (Maybe Friday) Objectives: –Compare and contrast acids and bases. –Describe what the pH scale measures.

39. Water (Acids and Bases) What makes up water? HO H (hydrogen) + O (oxygen) What is the chemical formula for water? H2OH2OH2OH2O What is the chemical equation for forming water? 2HOH 2 O 2H + O  H 2 O

40. Do you think water can do this? H 2 O2HO H 2 O  2H + O Yes, but its more likely to do this: H 2 O  H + + OH - In pure water, about 1 water molecule in 550 million will react to form hydrogen ions and hydroxide ions

41. The pH Scale measurement system used to indicate the concentration of hydrogen ions (H+) in solution; ranges from 0 to 14

42. Acids Acidic solutions contain higher concentrations of H+ ions than pure water and have pH values below 7.

43. Bases Basic, or alkaline, solutions contain lower concentrations of H+ ions than pure water and have pH values above 7.

44. Acid and Base Buffers Cells in our body like to keep their pH between 6.5 and 7.5 on the pH scale. A buffer helps to do just that! Buffer - weak acid or base that can react with strong acids or bases to help prevent sharp, sudden changes in pH

47. Macromolecules Objectives Organic Chemistry Macromolecules –Carbohydrates –Lipids –Proteins –Nucleic Acids Homework Complete Handout Due Wednesday Do Now –You have 15 minutes to gather your notes on: Carbohydrates Lipids Proteins Nucleic Acids

48. Macromolecules Carbohydrates Lipids Proteins Nucleic Acids

49. Organic Chemistry The study of carbon compounds. Is Carbon that important to devote an entire branch of chemistry to it? YES Carbon atoms 1.Four valence electrons 2.Four covalent bonds 3.Carbon can bond with many elements 4.hydrogen, oxygen, phosphorus, sulfur, and nitrogen. Even more important, carbon can bond with itself.

50. Macromolecules Are “giant molecules” formed from thousands or hundreds of thousands of smaller molecules Monomers (links) are the smaller units which are joined together to form Polymers (bike chain) The four main groups of macromolecules (organic compounds) are: Carbohydrates Lipids Nucleic Acids Proteins Polymerization Polymerization When small molecules, called monomers, join together, they form polymers, or large molecules.

51. Carbohydrate Contains C, H, and O usually in a ratio of 1:2:1 Living things use carbohydrates as their main source of energy. Plants, fungus, and some animals use carbohydrates for structural purposes. Monosaccharides(monomer):Monosaccharides(monomer): glucose [C 6 H 12 O 6 ], fructose, ribose, deoxyribose DisaccharidesDisaccharides: sucrose, lactose- a carb formed by the covalent bonding of 2 or more Monosaccharides Polysaccharides(Polymer):Polysaccharides(Polymer): starch, cellulose - large macromolecule formed from monosaccharides includes starches, cellulose and glycogen.

52. Monosaccharides

53. Disaccharide Polysaccharide

54. Cellulose

55. Homework Website (macromolecules continued) 1. Key Concept Name four groups of organic compounds found in living things. 2. Key Concept Describe at least one function of carbohydrates and lipids. 3. What properties of carbon explain carbon’s ability to form many different macromolecules?

56. Chitin

57. Dehydration Synthesis and Hydrolysis Dehydration Synthesis Joining the sugars (monomers) to form a disaccharide

59. Fat Comprised of: Glycerol Heads Fatty Acid Tails Lipids can be used to store energy. Some lipids are important parts of biological membranes and waterproof coverings. Two key types (triglycerides, phospholipids) Saturated Fat – completely saturated with hydrogen no double bonds unsaturated fat – contains one double bond polyunsaturated fat – contains more than one double bond Fatty Acid Tails are - Hydrophobic Glycerol Heads (backbone) are - Hydrophylic

60. Dehydration Synthesis of Lipid

62. Lipids Saturated fat – full of hydrogen, no double bonds Unsaturated fat – one double bond Polyunsaturated fat – more than one double bond

63. Protein Monomer – Amino Acids. There are just over 20 different amino acids. Polymer – Protein (polypeptide) Some proteins control the rate of reactions and regulate cell processes. Some are used to form bones and muscles. Others transport substances into or out of cells or help to fight disease.

64. Macromolecules Objectives Dehydration Synthesis Macromolecules –Proteins –Nucleic Acids Homework Quiz on Friday Do Now –Name the monomer and polymer of carbohydrates. –Name a couple key polysaccharides. –What are the two key structures of a lipid? –What is a saturated fatty acid? …unsaturated?

65. Dehydration Synthesis and Hydrolysis Dehydration Synthesis Joining the sugars (monomers) to form a disaccharide

66. Dehydration Synthesis

67. Quiz tomorrow!! Multiple Choice Label the following with one or more or the following: monomer, polymer, monosaccharide, disaccharide, polysaccharide, simple sugar, starch 1. Exoskeleton 2. Cell Wall 3. sugar for coffee

69. There are 20 Amino Acids

70. Protein Structure Primary Structure– straight protein chain Secondary Structure – beta – pleated sheet or Alpha - helix Tertiary Structure – Protein starts to wrap and fold around itself Quaternary Structure – Protein starts to fold and wrap around other proteins

71. Nucleic Acids Monomer - Nucleotides Polymer - DNA or RNA Nucleic Acids store and transmit hereditary/genetic information Each nucleotide contains a 5-C sugar as either ribose or deoxyribose phosphate group (PO 4 - ) and a Nitrogenous base (either: Adenine, Cytosine, Guanine, Thymine, or Uracil (only in RNA) DNA uses the sugar Deoxyribose RNA uses the sugar Ribose

75. Homework Read textbook pgs. 40-48 Handout on 2-1

76. Homework Read textbook pgs 44-48 Study Guide 2-2

77. Homework SG 2-4 all of SG chapter 2 should be complete Test chapter 2 coming up Friday???