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Graham's Law of Effusion
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Last updated
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Date created
Mar 1, 2020
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Section 1
(50 cards)
Graham's Law of Effusion
Effusion of a gas is INVERSELY proportional to the SQUARE ROOT of the molar mass r₁/r₂ =√M₂/M₁
Alkali metals
Group 1 metals
End point
point at which the titrated solution changes color
Common Weak Base Reaction
H⁺+NH₃→NH₄+
Hund's Rule
within a sublevel, place one e⁻ per orbital before pairing them
Number of Molecules in a Mole
6.022x10^23
Experimental yield
the actual amount of product produced in an experiment
Law of Conservation of Mass
mass reactants = mass products
Standard Temperature and Pressure
0.00°C, 1 atm (273 K)
Titrant
buret solution used in titration
6.63x10⁻³⁴Js
Planck's constant, used to calculate energy w/frequency
Heisenberg Uncertainty Principle
we cannot simultaneously determine an atom's exact path or location
Volume of 1 mole of Gas @STP
22.4L
Kinetic Energy per Molecule Equation
1/2mv²
Transition metals
elements in groups 3-12
Indicator
a weak acid that changes color at or near the equivalence point
Alkaline earth metals
Group 2 metals
Strong Bases
Group 1 and heavier Group 2 bases
Molarity
mol/L, concentration of a solution
lambda
wavelength symbol
Dalton's Law of Partial Pressure Equation
Ptotal=Pa+Pb+Pc....
Strong Acids
HCl, HBr, HI, HNO₃, HClO₄, H₂SO₄
Aufbau Principle
e⁻s fill the lowest energy orbital first, then work their way up
E
=h(frequency)
Reduction agent
the reactant that is being oxidized, brings about reduction
Common Weak Acid Reaction
HF+ OH⁻→H₂O
Strong Acid Strong Base Overall Reaction
H⁺+OH⁻→H₂O
Linear Geometry (2 possibilities)
AX₂, AX₂E₃
Percent Yield Equation
experimental yield/theoretical yieldx100
Percent Error Equation
theoretical yield-experimental yield/theoretical yieldx100
Molality
mol/kg of solvent, used in calculating colligative properties
nu
frequency symbol
Soluble Ions
Group 1, Ammonium, Nitrates, Acetates, Sulfates (+Halides)
3.0x10⁸m/s
speed of light, C
Pressure
force per unit area
Oxidizing agent
the reactant that is being reduced, brings about oxidation
Insoluble Ions
Carbonates, Hydroxides, Oxides, Phosphates, Sulfides
standard solution
a solution used in titrations whose concentration is known
Oxidation
loss of electrons, increase in oxidation #
Pauli Exclusion Principle
each orbital can hold two e⁻s each w/ opposite spins
Reduction
gain of electrons, decrease in oxidation #
Analyte
solution in flask being titrated
Excess reactant
reactant which doesn't get used up completely in a chemical reaction
Theoretical yield
amount of product produced when limiting reactant is used up
Equivalence Point
point where acid completely neutralizes base, moles of H+ = moles of OH-
Density
mass/volume
Mole Fraction
mols A/total mols (also known as XA)
1 atm in mmHg and torr
760 mmHg, 760 torr
C =
=lambda(nu) (aka. wavelength x frequency)
Limiting reactant
reactant that's completely used up in a chemical reaction
Section 2
(50 cards)
Catalyst
lowers activation energy
Colligative Properties (What properties change with addition of solute?)
vapor pressure lowering, boiling point elevation, freezing point depression
Activation Energy
the minimum energy that molecules must possess for collisions to be effective, Ea
Heat of Vaporization
energy required for liquid→gas
Network Covalent solids
- atoms joined by a continuous network of covalent bonds - high melting points - nonconductors of electricity - insoluble in water - Ex: diamond, graphite, quartz (compare to molecular solids)
System
the part of the universe one is focused upon (in thermodynamics)
Hydrogen Bonding
unusually strong dipole forces found when H is bonded to N, O, or F
Trigonal Pyramidal
AX₃E
Bent (2 possibilities)
AX₂E, AX₂E₂
Square Pyramidal
AX₅E
Single Bond (# sigma and/or pi)
1 sigma bond
Octahedral
AX₆
Deposition
gas to solid
T-shape
AX₃E₂
Metallic solids
- metal cations held together by electrons not attached to any particular metal cation - high electrical conductivity - conduct heat - ductile and malleable -insoluble in water -high range of melting and boiling points
Melting Point
point at which solid→liquid occurs
Base
puts OH⁻ into solution = ACCEPTS protons
Molecular Substances
-nonconductors of electricity -insoluble in water -low melting and boiling points (covalent)
Trigonal Planar
AX₃
Triple Bond (# sigma and/or pi)
1 sigma bond, 2 pi bonds
Seesaw
AX₄E
Exothermic
negative enthalpy, heat flows into surroundings, favorable for deltaG
Rate
Kinetics, how fast or slow a reaction occurs, becomes slower as it reaches equilibrium
Dipole-Dipole forces
-electrostatic force between the positive and negative ends of a polar molecule -stronger than London forces, but weaker than H bonding
Endothermic
positive enthalpy, heat flows into system, not favorable for deltaG
Q>K (Favors forward or reverse reaction?)
Reverse rxn (Think products/reactants)
Bond Enthalpy
ΔH when 1 mol of bonds is BROKEN in the gaseous state (+broken, -formed)
LeChatelier's Principle
If a system @equilibrium is stressed, the system will shift so as to reestablish equilibrium
Tetrahedral
AX₄
Trigonal Bipyramidal
AX₅
Supercritical fluid
substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
Double Bond (# sigma and/or pi)
1 sigma bond, 1 pi bond
Sublimation
solid to gas
Square Planar
AX₄E₂
Viscosity
resistance to flow
Conjugate acid
the chemical formed when a base accepts a proton
Condensation
gas to liquid
Heat Capacity
heat required to raise the system 1°C (C in q=mC∆T)
Ionic solid
- atoms joined by strong electrical forces between oppositely charged particles - high melting points - nonconducting as solids - conducting when molten or in solution - often water soluble -crystalline structures
Heat of Fusion
energy required for melting to occur
Melting
solid to liquid
Adhesion
molecules' tendency to stick to the container
Boiling Point
point at which liquid→gas occurs, where atmospheric pressure equals vapor pressure
Freezing
liquid to solid
Vaporization
liquid to gas
Cohesion
molecules' tendency to stick to one another
Q<K (Favors forward or reverse reaction?)
Forward rxn (Think products/reactants)
London dispersion forces
weakest IMFs, found in all molecules
Acid
puts H⁺ into solution = DONATES protons
Surroundings
the rest of the universe (in thermodynamics)
Section 3
(50 cards)