Section 1
Preview this deck
Bronsted-Lowry acid
Front
| 5 | 0 | ||
| 4 | 0 | ||
| 3 | 0 | ||
| 2 | 0 | ||
| 1 | 0 |
Active users
0
All-time users
1
Favorites
0
Last updated
6 years ago
Date created
Mar 1, 2020
Cards (244)
Section 1
(50 cards)
Bronsted-Lowry acid
Proton donor
Lewis acid
Electron pair donor
Dalton's law of partial pressures
Ptot = P1 + P2 + P3...
STP Conditions
0 degrees Celsius, 22.4 L
Strong Acids
HF, HBr, HCl, HClO4, HI, HClO3, HNO3
Arrhenius base
Produces OH- in water
JJ Thomson
Cathode Ray, discovered the electron
Reduction
Gain of electrons (GER)
Solubility Rules Exceptions
Calcium, Barium, Strontium, Mercury, Silver, Lead (Sulfates) Mercury, Silver, Lead (Halogens)
Law of conservation of mass
Mass is neither created nor destroyed
Distillation
Depends on differences in volatility
Ideal Gas Law
PV = nRT
Mole fraction
n1 / ntot
Oxidation
Loss of electrons (LEO)
Root mean square velocity
Average velocity of gas particles
Types of Chemical Reactions
Precipitation reactions, Acid-Base reactions, and Redox reactions
Molar mass of a gas
dRT / P
Potential energy
Energy from position or composition
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.)
Equivalence point
Enough titrant added to analyte
Millikan
Oil Drop Experiment, determined mass and magnitude of the electron
Kinetic energy
Energy from motion
Diffusion
Mixing of gases
Dilution Formula
M1V1 = M2V2
Arrhenius acid
Produces H+ (H3O+) in water
Bronsted-Lowry base
Proton acceptor
Charles's Law
V1 / T1 = V2 / T2
1 standard atmosphere
1 atm, 760 mm Hg, 760 torr, 101,325 Pa
Molarity
moles / L
Effusion
Gas into a vacuum
Strong Bases
All Group IA elements with OH- Ca(OH)2, Sr(OH)2, Ba(OH)2,
Precipitation reaction
An insoluble substance is formed as a result of the reaction
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
Reducing agent
Causes reduction (is often oxidized)
Lewis base
Electron pair acceptor
Filtration
Separating a solid from a liquid
Redox reaction
Electrons are transferred
Oxidizing agent
Causes oxidation (is often reduced)
Chromatography
Separating substances through differences in rates
Boyle's Law
P1V1 = P2V2
Solubility Rules
Chlorates, Acetates, Sulfates, Halogens, Nitrates, Group IA
Endpoint
Indicator changes color
Strong Electrolytes
Good conductors, easily ionized
Rutherford
Gold Foil Experiment, discovered nuclei, atoms have a lot of space
Graham's law of effusion
Density
mass / volume
Weak Electrolytes
Conduct currents very weakly
Spectator ions
Ions that do not participate in the reaction
Pressure
force / area
Law of conservation of energy
Energy can be converted but never destroyed
Section 2
(50 cards)
Hund's rule
Different electrons to different orbitals, same spin
Basic wave equation
speed of light = wavelength x frequency
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
Wavelength
distance between two peaks or troughs in a wave
Photoelectric effect
Effect occurring when electrons are emitted from the surface of a metal when light strikes it
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
Ionization energy
Energy required to remove a valence electron from an atom
Ionization energy trend
Increases across a period (electron shielding not complete), decreases down a group (more electron shielding)
Name of a linear shape?
MX2
Electron affinity
Energy change associated with the addition of an electron to a gaseous atom
Dipolar or dipole moment
Has center of positive and center of negative charge
Atomic radius trend
Decreases across a period (more effective nuclear charge), increases down a group (more electron shielding)
Bond angle of a bent shape?
<120
Number of bonds in a trigonal planar shape?
3
Heat
Transfer of energy with temperature
Lone pairs
Pairs of electrons localized
First law of thermodynamics
The energy of the universe is constant
Enthalpy (delta H)
delta H = delta E + P(delta V)
Types of electromagnetic radiation (largest to smallest)
radio, micro, IR, visible, UV, X-rays, gamma
de Broglie's equation
Wavelength of a particle
Dual nature of light
Light acts as a wave and as particulate matter
Bond angle of a linear shape?
180
Bond energy
Energy needed to break bond
Localized electron model
Molecule is composed of atoms bound together by sharing pairs of electrons
Energy of a photon equation
Planck's constant x speed of light / frequency
Internal energy (delta E)
delta E = q + w
Aufbau principle
Progressively add electrons to each sub level
Heat capacity
heat absorbed / increase in temperature
Name of a trigonal planar shape?
MX3
Electronegativity
Ability of an atom in a molecule to attract shared electrons to itself
Diffraction
Light is scattered from points or lines
Calorimetry equation
q = mCAT
Work
Force acting over a distance
Hybridization of a trigonal planar shape?
sp2
Bond angle of a trigonal planar shape?
120
Exothermic
Energy out of the system
Frequency
number of cycles per second
Resonance
More than one valid Lewis structure
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
Covalent bonding
Electrons are shared by nuclei
Hybridization of a linear shape?
sp
Endothermic
Energy into the system
Hybridization of a bent shape?
sp2
Number of bonds in a linear shape?
2
Localized electron model parts
Lewis diagram, VSEPR model (geometry), type of atomic orbitals
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)
Types of electromagnetic radiation (smallest to largest)
gamma, X-rays, UV, visible, IR, micro, radio
Pauli exclusion principle
Electrons with the same spin cannot occupy the same space
Change in enthalpy for reaction
sum of heat of formations of products - sum of heat of formations of reactions
Section 3
(50 cards)
Hybridization of a trigonal bipyramidal shape?
sp3d
Metallic bond
Delocalized electron
Number of bonds in an octahedron?
6
Number of bonds in a trigonal bipyramidal shape?
5
Number of bonds in a T-shape?
3
Number of nonbonding pairs in a V shape?
2
Hybridization of a trigonal pyramidal shape?
sp3
Number of nonbonding pairs in a T-shape?
2
Number of nonbonding pairs in a bent shape?
1
Number of a bonds in a V shape?
2
Polar covalent bond
Unequal sharing of electrons
Name of a trigonal pyramidal shape?asily ionized
MX3
Number of bonds in a linear (2) shape?
2
Bond angle of a trigonal pyramidal shape?
<109.5
Name of a square pyramidal shape?
MX5
Hybridization of a square planar shape?
sp3d2
Number of nonbonding pairs in a square pyramidal shape?
1
Bond angle of a V shape?
<109.5
Number of nonbonding pair in a square planar shape?
2
Nonpolar covalent bond
Equal sharing of electrons
Number of bonds in a bent shape?
2
Ionic bond
Transfer of electrons
Name of an octahedron?
MX6
Number of bonds in a trigonal pyramidal shape?
3
Number of nonbonding pairs in a trigonal pyramidal shape?
1
Hybridization of a see-saw shape?
sp3d
Hybridization of a tetrahedral shape?
sp3
Number of bonds in a square planar shape?
4
Number of nonbonding pairs in a see-saw shape?
1
Bond angle of a square pyramidal shape?
<90
Bond angles of a trigonal bipyramidal shape?
120, 90
Bond angle of a square planar shape?
90
Name of a trigonal bipyramidal shape?
MX5
Number of bonds in a square pyramidal shape?
5
Hybridization of a V shape?
sp3
Hybridization of an octahedron?
sp3d2
Bond angle of a tetrahedral shape?
109.5
Number of nonbonding pairs in a linear (2) shape?
3
Bond angle of an octahedron?
90
Name of a tetrahedral shape?
MX4
Hybridization of a linear (2) shape?
sp3d
Hybridization of a T-shape?
sp3d
Hybridization of a square pyramidal shape?
sp3d2
Bond angle of a T-shape?
<90
Number of bonds in a see-saw shape?
4
Number of bonds in a tetrahedral shape?
4
Name of a square planar shape?
MX4
Bond angle of a see-saw shape?
<120, <90
Bond angle of a linear (2) shape?
180
Name of a V shape?
M2X
Section 4
(50 cards)
Vapor pressure
Pressure of vapor at equilibrium
Temperature and solubility
Increases solubility of solid, decreases solubility of gases
Heat of solution
Enthalpy change formation of a solution, sum of enthalpy values from each step
Alloy
Contains a mixture of elements and has metallic properties
Phase diagram
Representation of phases of a substance
Electronegativity differences
Nonpolar covalent (0-0.4), polar covalent (0.4-1.67), ionic (above 1.67)
Tyndall effect
Scattering of light by particles
Coagulation
Destruction of colloid by heating or adding electrolyte
Amorphous solids
Components frozen in place with no arrangement
London dispersion forces
Between non polar molecules
Rate law
Rate depends on concentration
Temperature and rate
Higher temperature increases rate
Positive deviation from Raoult's law
Less IMFs, more molecules escape, higher vapor pressure
Interstitial alloy
Small atoms in holes
Raoult's Law
Nonvolatile solute simply dilutes the solvent
Critical pressure
Pressure required to produce liquefaction at the critical temperature
Pi bond
Bond between the p orbitals
Temperature and vapor pressure?
Vapor pressure increases significantly with temperature
Zeroth order integrated rate law
[A] = -kt + [A]0
Pressure and solubility
Increases solubility of a gas
Zeroth order half life
t1/2 = [A]0 / 2k
Hydrogen bond
Special type of dipole, hydrogen with N, F, or O atom
Catalyst
Increases rate of reaction but not consumed
Integrated rate law
Concentrations depends on time
Sublimation
Solid directly to gas
Reaction rate
Change of concentration over time (Rate = delta [A] / delta t)
Positive delta H
Energy absorbed
First order integrated rate law
ln[A] = - kt + ln[A]0
Sigma bond
Bond between the s orbitals
Critical temperature
Temperature above which vapor cannot be liquefied no matter the pressure
Negative delta H
Energy released
Negative deviation from Raoult's law
More IMFs, lower vapor pressure
First order plot
ln[A] vs. t
Heat of fusion
Enthalpy change which occurs at the melting point when a solid melts
Henry's Law
Amount of gas dissolved proportional to pressure of gas above solution
Triple point
Where all three states exist
Colloid
Suspension of particles
Critical point
Critical temperature and critical point
Zeroth order slope
Slope = -k
Surface area and rate
More surface area increases rate
IMFs and vapor pressure?
High IMFs --> low vapor pressure, Low IMFs --> high vapor pressure
Colligative properties
Freezing point depression, boiling point elevation, osmotic pressure
Zeroth order plot
[A] vs. t
First order slope
Slope = -k
Crystalline solids
Components organized in a lattice
Initial rate
Instantaneous rate after reaction begins
First order rate law
Rate = k[A]
Substitutional alloy
Metal atoms replaced by metal atoms of same size
Zeroth order rate law
Rate = k
Vapor pressure formula (Hg column)
Patmosphere = Pvapor +Pmercury column
Section 5
(44 cards)