1. Do Now What is an atom? Why do we have a periodic table? What information can we find in a periodic table?

2. Chapter 6 Biochemistry

3. Objectives To define an atom. To determine the make-up of an atom. To list different elements that can be found on Earth. To explain what type of information can be gathered from the periodic table.

4. Brain-Based Learning Proton Electron Neutron Name __________________

5. Atoms Building blocks of matter Contain 3 parts –Protons: positively charged, contain mass –Neutrons: no charge, contain mass –Electrons: negatively charged, insignificant mass + -

6. Atoms make up Elements a pure substance that can’t be broken down into other substances by physical or chemical means. Made up of only 1 type of atom Contain a unique name and symbol.

7. Periodic Table of Elements Periods: horizontal rows Groups: vertical columns –elements in the same group have similar chemical and physical properties. **Organized based on the # of protons in the nucleus of an atom.**

8. Periodic Table Information Atomic number- tells us the # of protons (and electrons) Symbol- unique for each element. Atomic Mass- # of protons and neutrons C 6 12.02

9. Practice Problems N 7 9.01 4 Ne 20 C 12.02 Complete the missing information and include the number of protons, neutrons, and electrons.

10. Neutron Partners… List the number of protons, neutrons, and electrons for the following… –Mg –Ca –Fe –Cl

11. Drawing an atom… Things to remember! –Proton # = Electron # –Protons and Neutrons are in the nucleus and add up to the atomic mass. –Electrons are arranged in energy levels 1 st energy level holds 2 electrons 2 nd energy level holds 8 3 rd energy level holds 8 Etc.

12. Lets Draw Oxygen! What is the atomic number of oxygen?

13. Do Now Answer the following based on the picture to the right… –Name of Element –# of Protons –# of Neutrons –# of Electrons K 19 39.10

14. Objectives Draw an atom. Define isotopes. Identify different types of common compounds. Compare and contrast the two types of bonds.

15. Get with your Electron Partner! 1.Draw atoms for the following elements. Neon Boron Lithium Oxygen

16. What is wrong with this picture? Carbon -atomic symbol “C” -atomic # 6 -atomic mass 12.02

17. Isotopes Isotopes contain the same # of protons as the element, but a different number of neutrons. –Ex: Carbon-14 Contains 6 protons (still carbon) Also contains 8 neutrons, instead of 6 **What else will be different other than the number of protons and neutrons?**

18. Radioactive Isotopes Changing the # of neutrons changes the stability of the atom, causes decay in the nucleus or causes it to break apart. –Ex: Carbon-14 is used in carbon-dating. We can tell how old something is by how much carbon is left.

19. What happens if there are different number of ______ than a normal atom? Protons and Neutrons? More protons than electrons? More electrons than protons?

20. Neutral Atoms Atoms need to have the right number of electrons around them (neutral) Ions- charged atom or groups of atoms Ions can lose or gain electrons to be neutral Na - Cl +

21. How many electrons does each of the following want to be “neutral”. Oxygen Carbon Hydrogen Nitrogen

22. Neutron Partners! List the number of protons, electrons, and neutrons in each ion –O- –Na+ –N 3- Are any of these atoms neutral?

23. Do Now Identify the element and then state if it is a normal atom, an isotope, or an ion.

24. Objectives Identify compounds. Determine what information can be gotten from a chemical formula. Compare and contrast ionic bonding vs. covalent bonding. Explain what “Vanderwalls interactions” are.

25. Compounds A pure substance formed when 2 or more elements combine. –Always formed using a specific ratio Ex: 2 molecules of Hydrogen + 1 molecule of Oxygen will give us water (H 2 O) –Chemically and physically different from the elements that make them up. –Must be broken down CHEMICALLY, not physically

26. Chemical Formulas The number before the formula states how many molecules Ex. 4 H 2 O = 4 water molecules The subscript number states how many of that type of atom Ex. H 2 O = 2 hydrogen atoms

27. Let’s try some examples (neutron partners) For the following examples list the total number of atoms for each element and how many of each molecule. 1.C 6 H 12 O 6 2.3CH 4 3.5CO 2 4.3O 3 5.4HCl

28. Do Now Take out your homework from last night! Determine the # of molecules, # of atoms for each element, and then the total number of atoms for the following compounds… –6H 2 O 4 –3CO 2 –NaCl2

29. Objectives Understand how elements are held together. Explain the components of a reaction.

30. How do compounds stay together? Bonds! –2 most common types 1.Covalent- atoms share electrons 2.Ionic- atoms gain or lose electrons to bond

31. Covalent Bonding Molecule: compound held together by covalent bonds. Carbon (C) – form 4 bonds (another 4 e) Hydrogen (H) – form one bond (1 e) Nitrogen (N) – form 3 bonds (3 e) Oxygen (O) – form 2 bonds (2 e) H 2 O H H O

32. Ionic Bonding

33. Ionic Bond Some atoms tend to donate or accept electrons more easily than other atoms. –Ex. Metals (D) and Non Metals (A)

34. Review! How many protons, neutrons, and electrons are in O 2- ? An acid releases ____ ions in solution and a base releases ____ ions in solution. Using the formula 3C 6 H 12 O 6, how many atoms of oxygen are present?

35. Quiz on the info up till now!

36. On the quiz… Parts of an atom –Protons, neutrons, electrons Drawing- neutral atoms, ions, isotopes Compounds- what are they? Bonds –Covalent and Ionic, what are they? –How many bonds can elements make (according to their valence electrons) Chemical formulas –Determine molecule #, atom #, total atom #

37. Do Now What happens during a chemical reaction? What are the components of a chemical reaction. Write an example of a chemical reaction we have worked with in one of our labs.

38. Objectives To identify reactants and products in a chemical reaction. To compare and contrast exothermic vs. endothermic reactions. Explain how enzymes work

39. 6.2 Chemical Reactions A chemical reaction -atoms or groups of atoms are reorganized into different substances. Chemical Reactions: –Production of heat or light, –Formation of a gas, liquid, or solid

40. Parts of a Reaction Reaction- Molecules breaking or coming together Reactants- What goes in the reaction Products- What comes out of the reaction Ex: Na + + Cl - = NaCl

41. Think – Pair - Share  Glucose and oxygen react to form carbon dioxide and water.  Identify:  Products  Reactants  Is this a chemical equation? Why? + ATP (energy)

42. Energy in Reactions The activation energy - minimum amount of energy needed for reactants to turn into products

43. Types of Reactions Exothermic- released heat energy.  The energy of the product is lower than the energy of the reactants.

44. Types of Reactions Endothermic - absorbed heat energy. –The energy of the products is higher than the energy of the reactants.

45. Think – Pair - Share Determine whether or not the following are Exothermic or Endothermic reactions: (Neutron Partner) 1. Combustion reactions of fuels 2. melting ice cubes 3. Nuclear Bomb 4. a candle flame 5. cooking an egg

46. Review What were the reactants in your liver lab? What were the products? What type of reaction was it? (endothermic or exothermic) Give an example of an endothermic reaction (not the example I gave)

47. What you should know about enzymes! -Specialized proteins that act as “catalyst” ( speeds up a reaction) - Usually end in “ase” -Not consumed in the reaction

48. What do they do?

49. How do they work? A substrate fits in the active site of an enzyme. This forms an enzyme substrate complex. They then break or form bonds. Maltose (substrate) Maltase (Enzyme) HOH Active Site

50. Buffers What happens to enzymes in a strong pH? (think about our lab!) Buffers are mixtures that can react with acids or bases to keep the pH within a particular range. (Remember homeostasis? We want to keep our body fluids at a pH of 6.5-7.5)

51. Chemistry in Biology Do Now

52. Objectives List the 4 macromolecules of life. Identify the 3 different types of carbohydrates. Explain the importance of carbs in the body. Explain why low-carb diets can be harmful.

53. Review What is the purpose of an enzyme? What are the components of a solution? Give an example. What are the 2 properties of water we talked about? What are the 2 types of mixtures? Give an example of each.

54. 6.4 Macromolecules of Life Organic Chemistry - The element carbon is a component of almost all biological molecules. (Inorganic= no carbon)

55. Let’s Review Carbon has _____ electrons in its outermost energy level. One carbon atom can form _____ covalent bonds with other atoms.

56. Molecules Macromolecules - –large molecules formed by joining smaller organic molecules together. Polymers - –molecules made from repeating units of identical (or nearly identical) compounds linked together by covalent bonds.

57. Carbohydrates Monosaccharide- ranging from three to seven (simple sugar) Disaccharide - Two monosaccharides joined together Polysaccharide- many monosaccharides joined together

58. Carbohydrates Ratio of carbon : hydrogen : oxygen of 1:2:1 (CH 2 O)n

59. Identify which molecules are carbohydrates… 1) C 6 H 12 O 6 2) CH 3 3) C 4 H 2 O 2 4) C 24 H 36 O 24

60. Classify the following as mono, di, or poly – saccaride 1. C 6 H 12 O 6 2. 3. C 12 H 24 O 12 4.

61. Get with your proton partner and join another pair of proton partners! Read the article and answer the questions. Whatever you do not finish will be homework. Article & Questions

62. Do Now Take out your carbohydrate article! What are carbs used for? Give an example of a simple carb and a complex carb.

63. Objectives To explain how the body uses fats and proteins. To compare and contrast saturated vs. unsaturated fats. To understand the two types of cholesterol.

64. Lets learn about FAT!! http://www.youtube.com/watch?v=2S1mQ YO0g68http://www.youtube.com/watch?v=2S1mQ YO0g68

65. Lipids Made mostly of C and H Triglyceride –Fat – solid at room temperature –Oil – Liquid at room temperature

66. Saturated vs. Unsaturated Saturated Fats  - –Only Single bonds between the carbons –Solid at room temperature (typically) Unsaturated Fats - –Double bonds between the carbons –Liquid at room temperature (typically)

67. Click me

68. Types of Lipids Saturated fatsUnsaturated fats Structural differences all single bonds (one shared pair of electrons) some double bonds (2 shared pairs of electrons) Phase of mattersolid fatsliquid fats sourcecome from animalscome from vegetables healthLess healthyMore healthy Purpose energy storage and insulation

69. So… people have a problem with…. Hydrogenated Oils Trans fats What are they? Why do they have a problem? TRANS FATS ARTICLE WITH PARTNERS

70. Cholesterol HDLLDL name High density lipoproteins low density lipo proteins function transport cholesterol from the body to the liver for breakdown and disposal transport cholesterol from the liver to the body Health good cholesterolbad cholesterol Purposestrengthens cell membranes

71. Proteins Made of small carbon compounds called amino acids Central Carbon

73. Atoms that make up Amino Acids:  carbon, nitrogen, oxygen, hydrogen, and sometimes sulfur.  Amino acids are connected together through a PEPTIDE BOND.

74. Proteins in the Body structural - –hair, collagen, muscle etc enzymes – –speed up chemical reactions

75. Nucleic Acids complex macromolecules that store and transmit genetic information. Nucleic acids are made of smaller repeating subunits called nucleotides composed of carbon, nitrogen, oxygen, phosphorus, and hydrogen atoms.

76. Think – Pair – Share Let’s Try These

77. Think – Pair - Share Try THESE!