Chem 4, College of the Desert, general.txt

  1. What are the diatomic elements?

    • Br, H, O, N, F, Cl, I
  2. Molarity=
    M= moles / liters
  3. PH scale
    • Acidic solutions PH < 7
    • Neutral solutions PH = 7
    • Basic solutions PH >7
  4. Caloric Values
    • Carbohydrate = 4
    • Fat = 9
    • Protein = 4
  5. Combined gas law
    (P1V1)/(N1T1)= (P2V2)/(N2T2)
  6. 1Atm
    • 760 mmHg
    • 760 torr
    • 14.7 lb / in2
    • 101325 pa (pascales)
    • 101.325 KPa
  7. Solubility
    Def: Amount of solute that can dissolve in a given amount of solvent.

    • NaCl does not change with high temp.
    • NaPO4 decreases with high temp < 40
    • Saturated: a solution contains all of the solute that can dissolve (greater then solubility).
    • Unsaturated: when a solute readily dissolves in a solvant.
  8. Solutions
    • Types of particles: Small particles, Ion, atoms, and small molecules.
    • Settling: partivles do not settle.
    • Seperation: particles cannot be seperated by filters or semipermeable membranes.
  9. Colloid
    • Type of Particle: larger molecules or groups of molecules or Ions.
    • Settling: Particles do not settle.
    • Seperation: particles can be seperated by semipermeable membranes but not by filters.
  10. Suspension
    • Types of particles: very large particles that may be visible.
    • Settling: particles settle rapidly.
    • Seperation: Particles can be seperated by filters.
  11. Alkalosis
    Respiratory Alkalosis: CO2 down PH up ( over 7.45)

    Metabolic Alkalosis: H+ down PH up
  12. Esthers
    • End in "yl"
    • Look Like: -O-
    • ie: CH3-O-CH3 (dimethyl ether)
  13. Ether
    • R - O - R
    • Note: R stands for any number of C chain.
  14. Formic Acid
    Methenoic Acid; found in ant bites, bee stings
  15. Acitic Acid
    Ethanoic Acid; found in Viniger for salads
  16. Chiral Carbon
    Mirror imiges but can not be super imposed

    • Cl
    • |
    • H-C-F
    • |
    • Br
    • (4 different functional groups)
  17. Benedicts Test
    • Aldehyde with an adjacent
    • -OH (hydroxl group)
  18. Alcohol
    • 1-4 are all soluable
    • "Aldehyde, Ketone, and carboxylic acids, alcohols are soluable in H2O so long as C is 1-4 &
    • 5 and 6 C for benzoic are slightly soluable.
  19. Boiling points for Alcohols
    • Lowest => highest
    • Alkane
    • Ether
    • Aldehyde
    • Ketone
    • Alcohol
    • Carboxylic Acid (highest)
  20. Thiol
    • End in Thiol
    • -SH

    • H H
    • | |
    • H-C-C-S-H
    • | |
    • H H
  21. Aldehyde
    • Ending "al"
    • O
    • ||
    • C-H
  22. Ketone
    • Ending "one"
    • O
    • ||
    • R-C-R
  23. Carboxylic Acid
    • O
    • ||
    • R-C-O-H
    • Functional group: alcohol
    • (has an OH)
  24. Ester
    • O
    • ||
    • R-C-O-R
    • Carboxylic acid + alcohol -> ester + water
    • ie: O
    • ||
    • CH3-C-O-H+ H-O-CH3-->
    • O
    • ||
    • H2O + CH3-C-O-CH3
    • (water+methyl ethanoate)
    • ie: perfume, flowers, fruit
  25. Amine
    NH2

    • Alkaloids are bad for you; nicotine, Caffeine, Morphene.
    • Has "N"
    • Basic
    • (likes to take H to become positive Ion)
  26. Amide
    • O
    • ||
    • C-N
    • Are barbituates, low doses= pain killers, high doses = sleep inducers, Are Habit Forming

    Also double bond to "O"
  27. Dehydration of an alcohol
    • H+
    • Alcohol------->Alkene+H2O
    • (Heat)
  28. Not Superimposable
    Chirality occures when stereoisomers have mirror imiges that cannot be placed on top of each other.
  29. Carboxyl group
    A carbon-oxygen double bond.
  30. Amine classification
    • 1 degree: CH3-NH2
    • 2 degree: CH3-NH-CH3
    • 3 degree: CH3-N-CH3
    • |
    • CH3
  31. Primary Alcohol oxidized
    • OH O O
    • | || ||
    • CH3-CH ==> C-H => C-O-H
    • Aldehyde carb acid

    [aldehyde] then [carboxylic acid]
  32. Secoundary Alcohol oxidized
    • OH
    • ||
    • CH3-CH-CH3=>ketone
  33. Tirtiary alcohol oxidized
    Not able to oxidized
  34. Alkenes
    Roses, lemons, oranges, lavender
  35. Esthers
    Flowers, Fruit
  36. Diatomic
    • Br2
    • H2
    • O2
    • N2
    • F2
    • Cl2
    • I2
  37. Alkanes
    Single bonds C-C

    • Structeral Formulas
    • H H
    • | |
    • H-C-C-H
    • | |
    • H H
    • OR
    • CH3-CH3
  38. Alkene
    • Double bonds
    • C=C
    • OR
    • H H
    • | |
    • H-C=C-H
    • OR
    • CH2=CH2
  39. Alkynes
    Triple bond between Carbons
  40. Alcohols classification
    Have -OH bonded to C

    ie: CH3-CH2-OH
  41. Ether classification
    Has O bonded to 2 C'S

    • Condensed formula:
    • CH3-O-CH3
    • H H
    • | |
    • H-C-O-C-H
    • | |
    • H H
  42. Metric prefixes
    • Tera. 1•1012
    • Giga. 1•109
    • Mega. 1•106
    • Kilo. 1•103=1000
    • ----- 1
    • Deci. 1•10-1=0.1
    • Centi. 1•10-2=0.01
    • Milli. 1•10-3=0.001
    • Micro. 1•10-6
    • Nano. 1•10-9
    • Pico. 1•10-12
  43. Prefixes for covalent compounds
    • 1. Mono
    • 2. Di
    • 3. Tri
    • 4. Tetra
    • 5. Penta
    • 6. Hexa
    • 7. Hepta
    • 8. Octa
    • 9. Nona
    • 10. Deca
  44. Partial Pressures of Oxygen
    • Gas = O2,
    • Oxygenated Blood = 100, Deoxygenated Blood = 40, Tissue = 0 < 30 (30 or less)
  45. Partial Pressure of Carbon dioxide
    • Gas = CO2
    • Oxygenated Bloob = 40
    • Deoxygenated Blood = 46
    • Tissue = 50 < (50 or greater)
  46. Oxidation
    • Loss of e-
    • Loss of Hydrogen
    • Gain of Oxygen
  47. Reduction
    • Gain of e-
    • Gain of Hydrogen
    • Loss of Oxygen
  48. Strong Electrolyte
    • Dissociate: Completly
    • Contents of Solution: Ions only
  49. Week Electrolyte
    • Dissociate: Partally
    • Contents of Solution: Mostly molecules and a few ions
  50. None Electrolytes
    • Dissociate: none
    • Contents in solution: molecules only
  51. STP
    Standard, Temperature, Pressure

    1 Mole = 22.4 L
  52. Enantiomer
    Is a srerioisomer that is a mirror image of another molecule, that can not be superimposed.
  53. Respiritory Acidosis
    • CO2 Up
    • PH Down
    • Note: Standard Ph is 7.35
  54. Metabolic Acidoses
    • H Up
    • PH Down
    • (Inhale)
    • Note: Standard Ph is 7.35
  55. Dimer
    • Carboxylic acids form dimers
    • 2 carboxylic acids combine to each other
  56. Organic
    • Low BP
    • Low MP
    • High Flammability
    • Covalent bonds
    • Not Soluable in H2O
  57. Inorganic
    • High BP
    • High MP
    • Low Flammability
    • Ionic Bonds
    • Soluable in H2O
  58. Ionic Bonds
    • Metal + non-metal
    • Strongest
    • H
  59. Covalent Bonds
    • 2 non-metaloids
    • (can then go to polar or none polar)
  60. Polar Bonds
    • (Always from covalent)
    • Form either Hydrogen or diepole diepole
  61. Hydrogen bonds
    With F, O, N,
  62. Non-polar
    • Disperson forces
    • *Landon Landon (weakest forces)
  63. Diepole
    The seperation of positive and negitive charges in a polar bond indicated by an arrow that is drawn from the more positive atom to the more negative atom.
  64. Diepole-diepole attractions
    Attractive forces between oppositely charged ends of polar molecules.
  65. Methanal
    Formaldehyde
  66. Ethanol
    Acetalaldehyde
  67. Propanal
    Propionaldehyde
  68. Butanal
    Butyraldehyde
  69. Boiling Points
    Chapter 12
    Butane, Ethyl methyl ether, propanal, propanone, 1-propanol, carboxylic acid

    • Family
    • Alkane, ether, aldehyde, ketone, alcohol, carboxylic acid
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Chem 4, College of the Desert, general.txt
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