Section 1
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Molar mass of a gas
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Cards (244)
Section 1
(50 cards)
Molar mass of a gas
dRT / P
Graham's law of effusion
Bronsted-Lowry acid
Proton donor
Lewis acid
Electron pair donor
Endpoint
Indicator changes color
Spectator ions
Ions that do not participate in the reaction
STP Conditions
0 degrees Celsius, 22.4 L
Ideal Gas Law
PV = nRT
Dalton's Atomic Theory
Each element is made up of tiny particles called atoms. The atoms of a given element are identical. Chemical compounds are forms when atoms of different elements combine with each other. Chemical reactions involve reorganization of the atoms (changes in the way they are bound together.)
Strong Acids
HF, HBr, HCl, HClO4, HI, HClO3, HNO3
Oxidizing agent
Causes oxidation (is often reduced)
Chromatography
Separating substances through differences in rates
Rutherford
Gold Foil Experiment, discovered nuclei, atoms have a lot of space
Bronsted-Lowry base
Proton acceptor
Kinetic energy
Energy from motion
Solubility Rules
Chlorates, Acetates, Sulfates, Halogens, Nitrates, Group IA
Lewis base
Electron pair acceptor
Redox reaction
Electrons are transferred
Diffusion
Mixing of gases
Distillation
Depends on differences in volatility
1 standard atmosphere
1 atm, 760 mm Hg, 760 torr, 101,325 Pa
Dilution Formula
M1V1 = M2V2
Boyle's Law
P1V1 = P2V2
Weak Electrolytes
Conduct currents very weakly
Reducing agent
Causes reduction (is often oxidized)
Types of Chemical Reactions
Precipitation reactions, Acid-Base reactions, and Redox reactions
Potential energy
Energy from position or composition
Law of conservation of mass
Mass is neither created nor destroyed
Dalton's law of partial pressures
Ptot = P1 + P2 + P3...
Charles's Law
V1 / T1 = V2 / T2
Root mean square velocity
Average velocity of gas particles
Arrhenius base
Produces OH- in water
Solubility Rules Exceptions
Calcium, Barium, Strontium, Mercury, Silver, Lead (Sulfates) Mercury, Silver, Lead (Halogens)
Effusion
Gas into a vacuum
Millikan
Oil Drop Experiment, determined mass and magnitude of the electron
Equivalence point
Enough titrant added to analyte
Reduction
Gain of electrons (GER)
Mole fraction
n1 / ntot
Strong Electrolytes
Good conductors, easily ionized
Oxidation
Loss of electrons (LEO)
Molarity
moles / L
Strong Bases
All Group IA elements with OH- Ca(OH)2, Sr(OH)2, Ba(OH)2,
Pressure
force / area
Precipitation reaction
An insoluble substance is formed as a result of the reaction
JJ Thomson
Cathode Ray, discovered the electron
Law of conservation of energy
Energy can be converted but never destroyed
Density
mass / volume
Filtration
Separating a solid from a liquid
KMT
Volume of individual particles is negligible Particles are in constant motion Particles exert no forces on each other Collisions of particles with container walls are cause of pressure from gas
Arrhenius acid
Produces H+ (H3O+) in water
Section 2
(50 cards)
Types of electromagnetic radiation (smallest to largest)
gamma, X-rays, UV, visible, IR, micro, radio
First law of thermodynamics
The energy of the universe is constant
Covalent bonding
Electrons are shared by nuclei
Name of a linear shape?
MX2
Hund's rule
Different electrons to different orbitals, same spin
Diffraction
Light is scattered from points or lines
Bond energy
Energy needed to break bond
Frequency
number of cycles per second
Bond angle of a trigonal planar shape?
120
Hybridization of a bent shape?
sp2
Basic wave equation
speed of light = wavelength x frequency
Ionization energy
Energy required to remove a valence electron from an atom
Bond angle of a bent shape?
<120
Number of bonds in a linear shape?
2
Dual nature of light
Light acts as a wave and as particulate matter
Lattice energy
Change in energy when separated gas ions form an ionic solid Equation: LE = k(Q1Q2 / r) k is proportionality constant, Q is charge of ions, r is shortest distance between centers of ions
Dipolar or dipole moment
Has center of positive and center of negative charge
Photoelectric effect
Effect occurring when electrons are emitted from the surface of a metal when light strikes it
Number of bonds in a trigonal planar shape?
3
Hess's Law Rules
If a reaction is reversed, the sign of delta H is reversed delta H is proportional to the quantities of reactions and products
Hybridization of a linear shape?
sp
Name of a trigonal planar shape?
MX3
Energy of a photon equation
Planck's constant x speed of light / frequency
Ionization energy trend
Increases across a period (electron shielding not complete), decreases down a group (more electron shielding)
Types of electromagnetic radiation (largest to smallest)
radio, micro, IR, visible, UV, X-rays, gamma
Pauli exclusion principle
Electrons with the same spin cannot occupy the same space
Wavelength
distance between two peaks or troughs in a wave
de Broglie's equation
Wavelength of a particle
Endothermic
Energy into the system
Heat
Transfer of energy with temperature
Hybridization of a trigonal planar shape?
sp2
Internal energy (delta E)
delta E = q + w
Resonance
More than one valid Lewis structure
Heisenberg Uncertainty Principle
We cannot know both the position and momentum of an electron (the more we know one, the less we know the other)
Electron affinity
Energy change associated with the addition of an electron to a gaseous atom
Localized electron model
Molecule is composed of atoms bound together by sharing pairs of electrons
Heat capacity
heat absorbed / increase in temperature
Exothermic
Energy out of the system
Work
Force acting over a distance
Localized electron model parts
Lewis diagram, VSEPR model (geometry), type of atomic orbitals
Enthalpy (delta H)
delta H = delta E + P(delta V)
Atomic radius trend
Decreases across a period (more effective nuclear charge), increases down a group (more electron shielding)
Calorimetry equation
q = mCAT
Change in enthalpy for reaction
sum of heat of formations of products - sum of heat of formations of reactions
Bond angle of a linear shape?
180
Standard enthalpy of formation
change in enthalpy with formation of one mole of compound from its elements
Coulomb's law
Energy of interaction between a pair of ions
Aufbau principle
Progressively add electrons to each sub level
Lone pairs
Pairs of electrons localized
Electronegativity
Ability of an atom in a molecule to attract shared electrons to itself
Section 3
(50 cards)
Number of bonds in an octahedron?
6
Number of nonbonding pair in a square planar shape?
2
Hybridization of a tetrahedral shape?
sp3
Hybridization of a square pyramidal shape?
sp3d2
Number of nonbonding pairs in a trigonal pyramidal shape?
1
Bond angle of an octahedron?
90
Bond angle of a V shape?
<109.5
Hybridization of a T-shape?
sp3d
Bond angle of a square pyramidal shape?
<90
Ionic bond
Transfer of electrons
Bond angle of a see-saw shape?
<120, <90
Bond angle of a square planar shape?
90
Number of nonbonding pairs in a bent shape?
1
Number of bonds in a square planar shape?
4
Hybridization of a linear (2) shape?
sp3d
Number of nonbonding pairs in a V shape?
2
Number of a bonds in a V shape?
2
Hybridization of a V shape?
sp3
Number of nonbonding pairs in a T-shape?
2
Nonpolar covalent bond
Equal sharing of electrons
Bond angle of a linear (2) shape?
180
Number of nonbonding pairs in a linear (2) shape?
3
Name of a tetrahedral shape?
MX4
Hybridization of an octahedron?
sp3d2
Number of bonds in a trigonal bipyramidal shape?
5
Number of bonds in a tetrahedral shape?
4
Number of nonbonding pairs in a square pyramidal shape?
1
Number of bonds in a linear (2) shape?
2
Number of nonbonding pairs in a see-saw shape?
1
Name of an octahedron?
MX6
Number of bonds in a square pyramidal shape?
5
Hybridization of a see-saw shape?
sp3d
Number of bonds in a T-shape?
3
Polar covalent bond
Unequal sharing of electrons
Bond angle of a tetrahedral shape?
109.5
Name of a square pyramidal shape?
MX5
Number of bonds in a see-saw shape?
4
Metallic bond
Delocalized electron
Name of a square planar shape?
MX4
Number of bonds in a trigonal pyramidal shape?
3
Hybridization of a trigonal bipyramidal shape?
sp3d
Bond angles of a trigonal bipyramidal shape?
120, 90
Hybridization of a trigonal pyramidal shape?
sp3
Name of a trigonal bipyramidal shape?
MX5
Bond angle of a trigonal pyramidal shape?
<109.5
Name of a trigonal pyramidal shape?asily ionized
MX3
Number of bonds in a bent shape?
2
Hybridization of a square planar shape?
sp3d2
Name of a V shape?
M2X
Bond angle of a T-shape?
<90
Section 4
(50 cards)
Positive delta H
Energy absorbed
Critical pressure
Pressure required to produce liquefaction at the critical temperature
Temperature and rate
Higher temperature increases rate
First order slope
Slope = -k
Critical point
Critical temperature and critical point
Rate law
Rate depends on concentration
Vapor pressure
Pressure of vapor at equilibrium
Interstitial alloy
Small atoms in holes
Heat of solution
Enthalpy change formation of a solution, sum of enthalpy values from each step
Tyndall effect
Scattering of light by particles
Colloid
Suspension of particles
Pressure and solubility
Increases solubility of a gas
Positive deviation from Raoult's law
Less IMFs, more molecules escape, higher vapor pressure
Initial rate
Instantaneous rate after reaction begins
First order plot
ln[A] vs. t
Pi bond
Bond between the p orbitals
Zeroth order slope
Slope = -k
Zeroth order plot
[A] vs. t
Zeroth order half life
t1/2 = [A]0 / 2k
Coagulation
Destruction of colloid by heating or adding electrolyte
Crystalline solids
Components organized in a lattice
Sublimation
Solid directly to gas
Vapor pressure formula (Hg column)
Patmosphere = Pvapor +Pmercury column
Sigma bond
Bond between the s orbitals
Temperature and vapor pressure?
Vapor pressure increases significantly with temperature
Amorphous solids
Components frozen in place with no arrangement
Zeroth order rate law
Rate = k
Raoult's Law
Nonvolatile solute simply dilutes the solvent
Henry's Law
Amount of gas dissolved proportional to pressure of gas above solution
First order rate law
Rate = k[A]
Negative deviation from Raoult's law
More IMFs, lower vapor pressure
First order integrated rate law
ln[A] = - kt + ln[A]0
Hydrogen bond
Special type of dipole, hydrogen with N, F, or O atom
Negative delta H
Energy released
Substitutional alloy
Metal atoms replaced by metal atoms of same size
Phase diagram
Representation of phases of a substance
London dispersion forces
Between non polar molecules
Temperature and solubility
Increases solubility of solid, decreases solubility of gases
Heat of fusion
Enthalpy change which occurs at the melting point when a solid melts
Critical temperature
Temperature above which vapor cannot be liquefied no matter the pressure
Colligative properties
Freezing point depression, boiling point elevation, osmotic pressure
IMFs and vapor pressure?
High IMFs --> low vapor pressure, Low IMFs --> high vapor pressure
Electronegativity differences
Nonpolar covalent (0-0.4), polar covalent (0.4-1.67), ionic (above 1.67)
Reaction rate
Change of concentration over time (Rate = delta [A] / delta t)
Alloy
Contains a mixture of elements and has metallic properties
Surface area and rate
More surface area increases rate
Zeroth order integrated rate law
[A] = -kt + [A]0
Triple point
Where all three states exist
Integrated rate law
Concentrations depends on time
Catalyst
Increases rate of reaction but not consumed
Section 5
(44 cards)