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Atoms and Bonds: Understanding the Building Blocks of Matter

Explore the fundamental properties of atoms, including subatomic particles and isotopes. Discover how atoms form bonds and make up the stuff that everything is made of.

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Atoms and Bonds: Understanding the Building Blocks of Matter

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  1. Atoms and Bonds What is “stuff” made of?

  2. Atoms and Bonds I. Atoms A. Matter     1. Elements are different forms of matter which have different chemical and physical properties, and can not be broken down further by chemical reactions. 2. The smallest unit of an element that retains the properties of that element is an atom. 3. Atoms are composed of protons and neutrons in the nucleus, orbited by electrons: Proton: in nucleus; mass = 1, charge = +1 - Defines Element Neutron: in nucleus; mass = 1, charge = 0 Electron: orbits nucleus; mass ~ 0, charge = -1

  3. Atoms and Bonds I. Atoms A. Matter B. Properties of Atoms 1. Subatomic Particles Proton: in nucleus; mass = 1, charge = +1 - Defines Element Neutron: in nucleus; mass = 1, charge = 0 Electron: orbits nucleus; mass ~ 0, charge = -1 Orbit at quantum distances (shells) Shells 1, 2, and 3 have 1, 4, and 4 orbits (2 electrons each) Shells hold 2, 8, 8 electrons = distance related to energy

  4. Neon (Bohr model)

  5. Atoms and Bonds I. Atoms A. Matter B. Properties of Atoms 1. Subatomic Particles 2. Mass = protons + neutrons 8 O 15.99

  6. Atoms and Bonds I. Atoms A. Matter B. Properties of Atoms 1. Subatomic Particles 2. Mass = protons + neutrons 3. Charge = (# protons) - (# electrons)... If charge = 0, then you have an ...ION

  7. Atoms and Bonds I. Atoms A. Matter B. Properties of Atoms 4. Isotopes -

  8. Atoms and Bonds I. Atoms A. Matter B. Properties of Atoms 4. Isotopes - 'extra' neutrons... heavier Some are stable Some are not... they 'decay' - lose the neutron These 'radioisotopes' emit energy (radiation)

  9. Atoms and Bonds I. Atoms A. Matter B. Properties of Atoms 4. Isotopes - 'extra' neutrons... heavier Some are stable Some are not... they 'decay' - lose the neutron These 'radioisotopes' emit energy (radiation) This process is not affected by environmental conditions and is constant; so if we know the amount of parent and daughter isotope, and we know the decay rate, we can calculate the time it has taken for this much daughter isotope to be produced.

  10. Atoms and Bonds I. Atoms A. Matter B. Properties of Atoms 4. Isotopes - 'extra' neutrons... heavier Gamma decay -   neutron emits energy as a photon - no change in neutron number, mass, or element. Alpha decay - loss of an alpha particle  (2 protons and 2 neutrons) from the nucleus.  This changes the mass and element. (Uranium with 92 protons decays to Thorium with 90 protons) Beta decay - a neutron changes to a proton, and an electron is emitted. This changes only the element (determined by the number of protons.), but not the mass. (C14 decays, neutron changes to proton, and N14 is produced)

  11. - K40-Ar40  suppose 1/2 of total is Ar40 = 1.3by                 (Now, you may be thinking, "be real"! How can we measure something that is this slow?)

  12. - K40-Ar40  suppose 1/2 of total is Ar40 = 1.3by                 (Now, you may be thinking, "be real"! How can we measure something that is this slow?) - Well, 40 grams of Potassium (K) contains: 6.0 x 1023 atoms

  13. - K40-Ar40  suppose 1/2 of total is Ar40 = 1.3by                 (Now, you may be thinking, "be real"! How can we measure something that is this slow?) - Well, 40 grams of Potassium (K) contains: 6.0 x 1023 atoms - So, For 1/2 of them to change, that would be: 3.0 x 1023 atoms in 1.3 billion years (1.3 x 109)

  14. - K40-Ar40  suppose 1/2 of total is Ar40 = 1.3by                 (Now, you may be thinking, "be real"! How can we measure something that is this slow?) - Well, 40 grams of Potassium (K) contains: 6.0 x 1023 atoms - So, For 1/2 of them to change, that would be: 3.0 x 1023 atoms in 1.3 billion years (1.3 x 109) - So, divide 3.0 x 1023  by 1.3 x 109 = 2.3 X 1014 atoms/year.

  15. - K40-Ar40  suppose 1/2 of total is Ar40 = 1.3by                 (Now, you may be thinking, "be real"! How can we measure something that is this slow?) - Well, 40 grams of Potassium (K) contains: 6.0 x 1023 atoms - So, For 1/2 of them to change, that would be: 3.0 x 1023 atoms in 1.3 billion years (1.3 x 109) - So, divide 3.0 x 1023  by 1.3 x 109 = 2.3 X 1014 atoms/year. - Divide 2.3 x 1014 by 3.65 x 102 days per year = 0.62 x 1012 /day

  16. - K40-Ar40  suppose 1/2 of total is Ar40 = 1.3by                 (Now, you may be thinking, "be real"! How can we measure something that is this slow?) - Well, 40 grams of Potassium (K) contains: 6.0 x 1023 atoms - So, For 1/2 of them to change, that would be: 3.0 x 1023 atoms in 1.3 billion years (1.3 x 109) - So, divide 3.0 x 1023  by 1.3 x 109 = 2.3 X 1014 atoms/year. - Divide 2.3 x 1014 by 3.65 x 102 days per year = 0.62 x 1012 /day - Divide 6.2 x 1011 by 24*60*60 = 8.64 x 104) =

  17. - K40-Ar40  suppose 1/2 of total is Ar40 = 1.3by                 (Now, you may be thinking, "be real"! How can we measure something that is this slow?) - Well, 40 grams of Potassium (K) contains: 6.0 x 1023 atoms - So, For 1/2 of them to change, that would be: 3.0 x 1023 atoms in 1.3 billion years (1.3 x 109) - So, divide 3.0 x 1023  by 1.3 x 109 = 2.3 X 1014 atoms/year. - Divide 2.3 x 1014 by 3.65 x 102 days per year = 0.62 x 1012 /day - Divide 6.2 x 1011 by 24*60*60 = 8.64 x 104) = 0.7 x 107 = 7 x 106 = 7 million atoms changing from Potassium to Argon every second!!!                  This radiation is detectible and measureable...and when it has been measured over the last 100 years, it is always the same.  So, not only is there theoretical justification for expecting a constant decay rate, tests have confirmed this expectation.

  18. Atoms and Bonds I. Atoms II. Bonds A. Molecules

  19. Atoms and Bonds I. Atoms II. Bonds A. Molecules   1. atoms chemically react with one another and form molecules - the atoms are "bound" to one another by chemical bonds - interactions among electrons or charged particles.

  20. Atoms and Bonds I. Atoms II. Bonds A. Molecules     1. atoms chemically react with one another and form molecules - the atoms are "bound" to one another by chemical bonds - interactions among electrons or charged particles.    2. Bonds form because atoms attain a more stable energy state if their outermost shell is full. It can do this by loosing, gaining, or sharing electrons.  This is often called the 'octet rule' because the 2nd and 3rd shells can contain 8 electrons.

  21. Atoms and Bonds I. Atoms II. Bonds A. Molecules B. Covalent Bonds - atoms are shared

  22. Atoms and Bonds I. Atoms II. Bonds A. Molecules B. Covalent Bonds - atoms are shared C. Ionic Bond - transfer of electron and attraction between ions Na Cl

  23. Atoms and Bonds I. Atoms II. Bonds A. Molecules B. Covalent Bonds - atoms are shared C. Ionic Bond - transfer of electron and attraction between ions D. Hydrogen Bonds - weak attraction between partially charged hydrogen atom in one molecule and a negative region of another molecule

  24. D. Hydrogen Bonds - weak attraction between partially charged hydrogen atom in one molecule and a negative region of another molecule

  25. D. Hydrogen Bonds - weak attraction between partially charged hydrogen atom in one molecule and a negative region of another molecule

  26. D. Hydrogen Bonds - weak attraction between partially charged hydrogen atom in one molecule and a negative region of another molecule

  27. Atoms and Bonds I. Atoms II. Bonds III. Biologically Important Molecules A. Water

  28. Atoms and Bonds I. Atoms II. Bonds III. Biologically Important Molecules A. Water 1. Structure

  29. Atoms and Bonds I. Atoms II. Bonds III. Biologically Important Molecules A. Water 1. Structure 2. Properties

  30. 2. Properties - liquid at most Earth temperatures - medium for life

  31. 2. Properties - liquid at most Earth temperatures - medium for life - universal solvent - dissolves polar and ionic compounds

  32. 2. Properties - liquid at most Earth temperatures - medium for life - universal solvent - dissolves polar and ionic compounds - cohesive/adhesive - bonds to itself and other charged matter

  33. 2. Properties - liquid at most Earth temperatures - medium for life - universal solvent - dissolves polar and ionic compounds - cohesive/adhesive - bonds to itself and other charged matter - high specific heat - takes large energy change to change temp/state

  34. 2. Properties - liquid at most Earth temperatures - medium for life - universal solvent - dissolves polar and ionic compounds - cohesive/adhesive - bonds to itself and other charged matter - high specific heat - takes large energy change to change temp/state - max, density is a 4C... so ice floats

  35. 2. Properties - liquid at most Earth temperatures - medium for life - universal solvent - dissolves polar and ionic compounds - cohesive/adhesive - bonds to itself and other charged matter - high specific heat - takes large energy change to change temp/state - max, density is a 4C... so ice floats - dissociates into ions .... 1 x 10-7 molecules in pure water (pH = 7)

  36. Atoms and Bonds I. Atoms II. Bonds III. Biologically Important Molecules A. Water B. Carbohydrates

  37. Atoms and Bonds I. Atoms II. Bonds III. Biologically Important Molecules A. Water B. Carbohydrates 1. Structure - monomer = monosaccharide (simple sugar)

  38. Atoms and Bonds I. Atoms II. Bonds III. Biologically Important Molecules A. Water B. Carbohydrates 1. Structure - monomer = monosaccharide (simple sugar) CnH2nOn glucose, galactose, fructose are hexose sugars

  39. 1. Structure - monomer = monosaccharide (simple sugar) CnH2nOn glucose, galactose, fructose are hexose sugars ribose, ribulose, deoxyribose are pentose sugars

  40. 1. Structure - monomer = monosaccharide (simple sugar) CnH2nOn glucose, galactose, fructose are hexose sugars ribose, ribulose, deoxyribose are pentose sugars - monomers are linked together into polymers using dehydration synthesis - a removal of a water molecule (dehydration) and the synthesis of a bond. This requires energy and is catalyzed by enzymes in living systems.

  41. 1. Structure - monomer = monosaccharide (simple sugar) CnH2nOn glucose, galactose, fructose are hexose sugars ribose, ribulose, deoxyribose are pentose sugars - monomers are linked together into polymers using dehydration synthesis - a removal of a water molecule (dehydration) and the synthesis of a bond. This requires energy and is catalyzed by enzymes in living systems. - polymer = polysaccaharide disaccharide - 2 - sucrose (glucose and fructose) poly's: starch, glycogen, chitin, cellulose

  42. Atoms and Bonds I. Atoms II. Bonds III. Biologically Important Molecules A. Water B. Carbohydrates C. Proteins

  43. C. Proteins 1. Structure monomer = amino acid

  44. C. Proteins 1. Structure monomer = amino acid

  45. C. Proteins 1. Structure monomer = amino acid polymer = polypeptide - chain 100-300 amino acids long linked together by dehydration synthesis reactions

  46. C. Proteins 1. Structure monomer = amino acid polymer = polypeptide - chain 100-300 amino acids long linked together by dehydration synthesis reactions VARIABLE... 20 "letters" can make a very diverse "language" of words...

  47. C. Proteins 1. Structure 2. Functions a. energy storage... but since they probably do other things, these are metabolized last... b. structure - after water, animals are mostly protein collagen, elastin, actin, myosin, etc... c. metabolic - enzymes d. transport - in the cell membrane - hemoglobin and other transport proteins e. immunity: antibodies are proteins

  48. Atoms and Bonds I. Atoms II. Bonds III. Biologically Important Molecules A. Water B. Carbohydrates C. Proteins D. Lipids

  49. D. Lipids 1. Structure monomer = fatty acid

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