-
What are the diatomic elements?
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Molarity=
M= moles / liters
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PH scale
- Acidic solutions PH < 7
- Neutral solutions PH = 7
- Basic solutions PH >7
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Caloric Values
- Carbohydrate = 4
- Fat = 9
- Protein = 4
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Combined gas law
(P1V1)/(N1T1)= (P2V2)/(N2T2)
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1Atm
- 760 mmHg
- 760 torr
- 14.7 lb / in2101325 pa (pascales)
- 101.325 KPa
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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.
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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.
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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.
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Suspension
- Types of particles: very large particles that may be visible.
- Settling: particles settle rapidly.
- Seperation: Particles can be seperated by filters.
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Alkalosis
Respiratory Alkalosis: CO2 down PH up ( over 7.45)
Metabolic Alkalosis: H+ down PH up
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Esthers
- End in "yl"
- Look Like: -O-
- ie: CH3-O-CH3 (dimethyl ether)
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Ether
- R - O - R
- Note: R stands for any number of C chain.
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Formic Acid
Methenoic Acid; found in ant bites, bee stings
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Acitic Acid
Ethanoic Acid; found in Viniger for salads
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Chiral Carbon
Mirror imiges but can not be super imposed
- Cl
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- H-C-F
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- Br
- (4 different functional groups)
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Benedicts Test
- Aldehyde with an adjacent
- -OH (hydroxl group)
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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.
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Boiling points for Alcohols
- Lowest => highest
- Alkane
- Ether
- Aldehyde
- Ketone
- Alcohol
- Carboxylic Acid (highest)
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-
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Carboxylic Acid
- O
- ||
- R-C-O-H
- Functional group: alcohol
- (has an OH)
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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
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Amine
NH 2
- Alkaloids are bad for you; nicotine, Caffeine, Morphene.
- Has "N"
- Basic
- (likes to take H to become positive Ion)
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Amide
- O
- ||
- C-N
- Are barbituates, low doses= pain killers, high doses = sleep inducers, Are Habit Forming
Also double bond to "O"
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Dehydration of an alcohol
- H+Alcohol------->Alkene+H2O
- (Heat)
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Not Superimposable
Chirality occures when stereoisomers have mirror imiges that cannot be placed on top of each other.
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Carboxyl group
A carbon-oxygen double bond.
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Amine classification
- 1 degree: CH3-NH2
2 degree: CH3-NH-CH3 3 degree: CH3-N-CH3| - CH3
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Primary Alcohol oxidized
- OH O O
- | || ||
- CH3-CH ==> C-H => C-O-H
- Aldehyde carb acid
[aldehyde] then [carboxylic acid]
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Secoundary Alcohol oxidized
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Tirtiary alcohol oxidized
Not able to oxidized
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Alkenes
Roses, lemons, oranges, lavender
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-
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Alkanes
Single bonds C-C
- Structeral Formulas
- H H
- | |
- H-C-C-H
- | |
- H H
- OR
- CH3-CH3
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Alkene
- Double bonds
- C=C
- OR
- H H
- | |
- H-C=C-H
- OR
- CH2=CH2
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Alkynes
Triple bond between Carbons
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Alcohols classification
Have -OH bonded to C
ie: CH3-CH2-OH
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Ether classification
Has O bonded to 2 C'S
- Condensed formula:
- CH3-O-CH3
- H H
- | |
- H-C-O-C-H
- | |
- H H
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Metric prefixes
- Tera. 1•1012Giga. 1•109Mega. 1•106Kilo. 1•103=1000
- ----- 1
- Deci. 1•10-1=0.1
- Centi. 1•10-2=0.01
- Milli. 1•10-3=0.001
- Micro. 1•10-6Nano. 1•10-9Pico. 1•10-12
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Prefixes for covalent compounds
- 1. Mono
- 2. Di
- 3. Tri
- 4. Tetra
- 5. Penta
- 6. Hexa
- 7. Hepta
- 8. Octa
- 9. Nona
- 10. Deca
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Partial Pressures of Oxygen
- Gas = O2,
- Oxygenated Blood = 100, Deoxygenated Blood = 40, Tissue = 0 < 30 (30 or less)
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Partial Pressure of Carbon dioxide
- Gas = CO2Oxygenated Bloob = 40
- Deoxygenated Blood = 46
- Tissue = 50 < (50 or greater)
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Oxidation
- Loss of e-Loss of Hydrogen
- Gain of Oxygen
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Reduction
- Gain of e-Gain of Hydrogen
- Loss of Oxygen
-
Strong Electrolyte
- Dissociate: Completly
- Contents of Solution: Ions only
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Week Electrolyte
- Dissociate: Partally
- Contents of Solution: Mostly molecules and a few ions
-
None Electrolytes
- Dissociate: none
- Contents in solution: molecules only
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STP
Standard, Temperature, Pressure
1 Mole = 22.4 L
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Enantiomer
Is a srerioisomer that is a mirror image of another molecule, that can not be superimposed.
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Respiritory Acidosis
- CO2 Up
- PH Down
- Note: Standard Ph is 7.35
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Metabolic Acidoses
- H Up
- PH Down
- (Inhale)
- Note: Standard Ph is 7.35
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Dimer
- Carboxylic acids form dimers
- 2 carboxylic acids combine to each other
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Organic
- Low BP
- Low MP
- High Flammability
- Covalent bonds
- Not Soluable in H2O
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Inorganic
- High BP
- High MP
- Low Flammability
- Ionic Bonds
- Soluable in H2O
-
Ionic Bonds
- Metal + non-metal
- Strongest
- H
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Covalent Bonds
- 2 non-metaloids
- (can then go to polar or none polar)
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Polar Bonds
- (Always from covalent)
- Form either Hydrogen or diepole diepole
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Hydrogen bonds
With F, O, N,
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Non-polar
- Disperson forces
- *Landon Landon (weakest forces)
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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.
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Diepole-diepole attractions
Attractive forces between oppositely charged ends of polar molecules.
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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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