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74 Cards in this Set
- Front
- Back
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0.000001 M_ =
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0.001 k_
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0.001 k_ =
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1 _
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1_ =
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100 c_
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100 c_=
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1000 m_
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1000 m_ =
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1000000 M*_
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2.54 cm=
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1 in.
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1 kg =
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2.2 lbs
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1 atm. =
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760 mm Hg
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Celsius from Fahrenheit
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5/9(F-32)
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From Celsius to Kelvins
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C+ 273= K
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Melting
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changing from solid to liquid
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Vaporization
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changing from liquid to gas
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Condensation
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changing from gas to liquid
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Freezing
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changing from liquid to solid
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Sublimination
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changing from solid to gas; ie: dry ice
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Deposition
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changing from gas to solid; ie: snow
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Charge of a proton and electron
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+/- 1.602 x 10 to the -19
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1 calorie of energy =
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4.184 Joules
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amplitude (A)=
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how much the wave varies from the baseline
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wavelength (lambda)=
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1 full wave
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frequency (nu)=
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number of waves per second
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To find wavelength
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wavelength = speed of light constant/ frequency
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To find frequency
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frequency = constant/ wavelength
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Electron Configuration
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1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10 4f14
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Electronegativity
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ability to attract electrons in chemical bond
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NH4+
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ammonium
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OH-
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hydroxide
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ClO-
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hypochlorite
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NO3-
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nitrate
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HCO3-
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bicarbonate
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C2H3O2-
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acetate
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SO4 2-
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sulfate
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CO3 2-
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carbonate
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PO4 3-
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phosphate
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HBr
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hydrobromic acid
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HCl
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hydrochloric acid
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H2CO3
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carbonic acid
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Mole=
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6.02 x10 to the 23
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a mole of water=
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18 mL
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Finding Calorimetry
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HH2O= m(ass of water) x c(specific heat) x (final temp.- initial temp.)
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Boyle's Law
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a sample of a gas at a constant temp. will have pressure and volume that are inversely proportional; P1V1= P2V2
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Charles's Law
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a sample of gas at a constant pressure the temp and volume are directly proportional; T1V2=T2V1
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Avagadro
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if we have equal volumes of gases at the same temp and same pressure they will have an equal number of particles; P1T1= P2T2
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Ideal Gas Law
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describes behavior of gases in terms of units; P(ressure)V(olume)=nR(constant)T(emp)
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Condensation
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process of losing energy so gases return to liquid state
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Molarity
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M= mole of solute/ L of solution
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Molality
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m= number of moles of solute/ kg of solvent
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Molefractions
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mf= moles of one component/ total moles of solution
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Solvation
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solvent particles surround solute particles
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Solubility
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ability to dissolve
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Boiling Point Elevation
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Change in boiling temp = Kb(constant of solvent) x molality (mole/kg)
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Freezing Point Depression
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change in freezing temp = Kf(constant) x molality (mole/kg)
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To find equilibrium
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Keq = [C]c[D]d/ [A]a[B]b
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Reaction Quotient
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if Q > Keq: shift to the left to make more reactions
if Q < Keq: shift to the right to make more products if Q = Keq: equilibrium |
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Amphoteric
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ability of water to be either an acid or a base
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Acid
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less than 7 on pH scale
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Base
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more than 7 on pH scale
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How to find pH
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pH= -log[H+]
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How to find [H+] or [H3O+]
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10 to the -pH
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How to find [OH-]
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[OH-][H+]= 10 to the -14
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Ka=
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[H+]
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Kb=
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[OH-]
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pOH=
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14-pH
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Reaction rate=
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change in concentration/ change in time
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Rate of reactions
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rate= k(constant)[A]x[B]y
x,y- relative number of moles A,B- reactants that effect reaction rate |
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exothermic, + entropy
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always spontaneous
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exothermic, - entropy
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spontaneous at low temps.
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endothermic, + entropy
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spontaneous at high temps.
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endothermic, - entropy
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never spontaneous
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Endothermic
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absorbs heat; ie: melting ice
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Exothermic
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gives off heat; combustion
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Density
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mass/volume
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What are the generally soluble in water rules?
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1. Alkali metals (IA) and ammonium ions
2. acetate ion 3. nitrate ion 4. halide ions (except AgX, Hg2X2, and PbX2) 5. sulfate ion (except SrSO4, BaSO4, and PbSo4) |
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Rules of insoluble in water
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6. carbonate ion (except when matched with IA or NH4+)
7. chromate ion (except rule 1) 8. phosphate ion (rule 1) 9. sulfide ion (except CaS, SrS, BaS and rule 1) 10. hydroxide ion (except Ca(OH)2, Sr(OH)2, Ba(OH)2, and rule 1) |
