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2–1 The Nature of Matter A. Atoms B. Elements and Isotopes 1. Isotopes 2. Radioactive Isotopes C. Chemical Compounds D.

Section Outline. Section 2-1. 2–1 The Nature of Matter A. Atoms B. Elements and Isotopes 1. Isotopes 2. Radioactive Isotopes C. Chemical Compounds D. Chemical Bonds 1. Ionic Bonds 2. Covalent Bonds 3. Van der Waals Forces. Go to Section:. ATOMS Questions 1-4. Basic unit of matter

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2–1 The Nature of Matter A. Atoms B. Elements and Isotopes 1. Isotopes 2. Radioactive Isotopes C. Chemical Compounds D.

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  1. Section Outline Section 2-1 • 2–1 The Nature of Matter A. Atoms B. Elements and Isotopes 1. Isotopes 2. Radioactive Isotopes C. Chemical Compounds D. Chemical Bonds 1. Ionic Bonds 2. Covalent Bonds 3. Van der Waals Forces Go to Section:

  2. ATOMS Questions 1-4 • Basic unit of matter • Comes from word atomos, meaning “unable to be cut” further • Consist of subatomic particles

  3. ATOMS Questions 1-4 • Atoms are neutral because same number of positive particle (protons) as negative particles (electrons)

  4. Elements and Isotopes Questions 5-9 • Elements – Pure substance that consists of only one type of atom. • Those things listed on the periodic table of elements Helium Water

  5. ELEMENTS Questions 5-9

  6. An Element in the Periodic Table Section 2-1 Elements and Isotopes Questions 5-9 6 C Atomic Number – Number of protons (number of electrons) Carbon 12.011 Average atomic mass – Average of all isotopes Go to Section:

  7. Elements and Isotopes Questions 5-9 • Isotopes • Atom that differs in number of neutrons they contain • Identified by their various mass numbers • Electron number determines chemical property and isotopes of the same element still have same number of electrons

  8. Figure 2-2 Isotopes of Carbon Section 2-1 10% of carbon has mass of 14 Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 7 neutrons 6 electrons 6 protons 8 neutrons Radioactivity – lose neutrons 90% of all carbon Has mass of 12 Go to Section:

  9. ELEMENTS and ISOTOPES • How are radioactive isotopes useful? • Used to date material based on the given rate at which isotope decays. • Carbon dating

  10. Half Life – Amount of time it takes for half of C14 to decay

  11. ..\..\..\..\Desktop\United Streaming Videos\Radiometric_Dating.asf • ..\..\..\..\Desktop\United Streaming Videos\Radioactivity__Half_life__Dating.asf

  12. ELEMENTS and ISOTOPES • Decaying isotopes – decay at a constant and predictable rate!!! 100 50 25 12.5 Same amount of time to lose half

  13. Chemical Compounds 10-11 • Chemical Compound • Substance formed by chemical combination (chemically bonded) of two or more elements • Examples: Salt (NaCl), Water (H20), Glucose (C6H12O6) Two hydrogen atoms for every one oxygen Chemical Formula indicates that one sodium atom for every one chlorine atom

  14. Chemical Bonds 12-18 • Chemical Bonds • Form to make each atom “happy” = full outer electron shell (8 or 2) • hold atoms in a compounds together • two types Covalent Bond Electrons are shared between atoms so that both have full outer shell One or more electrons are transferred from one atom to another so that each can have full outer shell Ionic Bond

  15. Chemical Bonds 12-18 • Ionic Bonding • When electrons are transferred between atoms one atom will become positive (if it loses an electron) the other will become negative (if it gains and electron). • These are called Ions – atoms that have positive or negative charge • Oppositely charged particles are attracted to each other • The attraction results in an ionic bond

  16. Figure 2-3 Ionic Bonding Section 2-1 Chemical Bonds 12-18 Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na+) Chloride ion (Cl-) Transfer of electron Protons +11 Electrons -11 Charge 0 Protons +17 Electrons -17 Charge 0 Protons +11 Electrons -10 Charge +1 Protons +17 Electrons -18 Charge -1 Go to Section:

  17. Figure 2-3 Ionic Bonding Section 2-1 Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na+) Chloride ion (Cl-) Transfer of electron Protons +11 Electrons -11 Charge 0 Protons +17 Electrons -17 Charge 0 Protons +11 Electrons -10 Charge +1 Protons +17 Electrons -18 Charge -1 Go to Section:

  18. Chemical Bonds 12-18 Ionic Bonding Clip • ..\..\..\..\Desktop\United Streaming Videos\ionic bonding.asf

  19. Chemical Bonds 12-18 • Covalent Bonds • electrons are shared between atoms so that each is stable (full outer shell) • results in a Molecule

  20. Chemical Bonds 12-18 Carbon atom = 4 electrons in outer shell Carbon wants 8 Hydrogen atom = 1 atom in outer shell hydrogen wants two

  21. Chemical Bonds 12-18 Notice: by sharing electrons carbon has 8 electrons and hydrogen has 2 = Happy!

  22. Covalent Bonding Clip • ..\..\..\..\Desktop\United Streaming Videos\covalent bond.asf

  23. Assignment for Wednesday • Complete Concept Map 2-1 • Complete Guided Reading 2-3 Questions 1-12

  24. Matter differ in the number of made of basic unit are same type of made of particles called of one type make neutrons that breakdown different forms radioactive chemically combine to make used for held together by transfer one type is one type is share atom isotopes elements protons electrons dating compounds bonds ionic covalent 2-1 Concept Map

  25. Section Outline Section 2-3 • 2–3 Carbon Compounds A. The Chemistry of Carbon B. Macromolecules C. Carbohydrates D. Lipids E. Nucleic Acids F. Proteins Go to Section:

  26. Section 2-3 Carbon Compounds • The Chemistry of Carbon 1-2 • Carbon can bond to carbon atoms giving it the ability to form extremely long chains • This is done by forming covalent bonds with each other

  27. Section 2-3 Carbon Compounds • The Chemistry of Carbon 1-2 • Carbon has four valence electrons (outer shell electrons) • Reminder: it wants 8

  28. Section 2-3 Carbon Compounds H H H H H H C – C – C – C – C – C – H H H H H H H H Each line represent a pair of “shared” electrons “Carbon Chain”

  29. Figure 2-11 Carbon Compounds Section 2-3 Methane Acetylene Butadiene Benzene Isooctane Go to Section:

  30. Section 2-3 Carbon Compounds • Macromolecules 3-6 • large molecules • Macro = large • Micro = small • formed by a process called Polymerization

  31. Section 2-3 Carbon Compounds • Macromolecules 3-6 • Polymers = many monomers joined together • mono = one • poly = many

  32. Section 2-3 Carbon Compounds • Macromolecules 3-6 • Four organic compounds formed through this idea of polymerization • Carbohydrates (sugars – simple and complex) • Lipids • Nucleic Acids • Proteins

  33. Section 2-3 Carbon Compounds • Carbohydrates 7-12 • Carbon + water = carbohydrate • carbon, hydrogen, and oxygen • chemical formula ratio C H2O

  34. Section 2-3 Carbon Compounds • Carbohydrates 7-12 • Monomers = Monosaccharide • ENERGY source • Glucose (blood sugar), fructose, galactose • Simple sugars – “sweet” • Upon digestion they don’t have to be broken down • Associated with “sugar highs” – sugar is available immediately • All have chemical formula C6H12O6

  35. Section 2-3 Carbon Compounds • Carbohydrates 7-12 • Disaccharide = two mono’s put together • Table sugar = sucrose • Milk sugar = lactose • relatively small • Sweet – would enter bloodstream quite quickly Two monosaccharide molecules put together

  36. Section 2-3 Carbon Compounds • Carbohydrates 7-12 • Polysaccharide = “many” monosaccharide molecules bonded together • Large macromolecules • Can be 1000’s of glucose molecules long Starch = polysaccharide Glucose = monosaccharide

  37. Section 2-3 Carbon Compounds • Carbohydrates 7-12 • Glycogen (animal starch) • Polysaccharide in animals that stores excess sugar. • Stored in liver and muscles • Released and broken down when glucose (mono) is low. • Excess monosaccharides will be converted

  38. Section 2-3 Carbon Compounds • Carbohydrates 7-12 • Cellulose (fiber) • Polysaccharide in plants that forms cell walls • Very rigid giving plants structure • Can’t be digested by humans but great in our diet.

  39. Organic Molecules one type aka carbohydrates sugar three types include disaccharides monosaccharides polysaccharides two make also known as many make example is starch in plants in animals glucose glycogen cellulose

  40. Carbohydrates Lipids Nucleic acids Proteins Sugars and starches Fats and oils Nucleotides Amino Acids Carbon, hydrogen, oxygen Carbon, hydrogen, oxygen Carbon, hydrogen,oxygen, nitrogen, Carbon,hydrogen, oxygen, nitrogen, phosphorus Concept Map Section 2-3 Carbon Compounds include that consist of that consist of that consist of that consist of which contain which contain which contain which contain Go to Section:

  41. Figure 2-13 A Starch Section 2-3 Starch Glucose Go to Section:

  42. Figure 2-16 Amino Acids Section 2-3 Amino group Carboxyl group General structure Alanine Serine Go to Section:

  43. Figure 2-16 Amino Acids Section 2-3 Amino group Carboxyl group General structure Alanine Serine Go to Section:

  44. Figure 2-16 Amino Acids Section 2-3 Amino group Carboxyl group General structure Alanine Serine Go to Section:

  45. Figure 2-17 A Protein Section 2-3 Amino acids Go to Section:

  46. Organic Molecules One type One type Proteins Nucleic Acids stores Made of monomer Made of monomer Genetic info Amino acids nucleotides have many includes functions deoxyribose phosphate Nitrogen base are one of the following guanine cytosine thymine adenine

  47. LIPIDS 13-17 • Composed of mostly Carbon and Hydrogen • Fats, oils, and waxes • Used for • cell membranes • Store energy (9 calories per gram vs. 4 calories for carbs)

  48. LIPIDS 13-17 • Nutritional sources of lipids • Saturated – Solid at room temp • Butter, animal lipids • Unsaturated – Liquid at room temp • Oil, plant lipids

  49. Review • Carbohydrate

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