Section 1
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Equivalence point
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Mar 1, 2020
Cards (197)
Section 1
(50 cards)
Equivalence point
Enough titrant added to analyte (analyte is what's being studied)
Strong Acids
HF, HBr, HCl, HClO4, HI, HClO3, HNO3
Strong Electrolytes
Good conductors, easily ionized
Solubility Rules Exceptions
Calcium, Barium, Strontium, Mercury, Silver, Lead (Sulfates) Mercury, Silver, Lead (Halogens)
Standard enthalpy of formation
change in enthalpy with formation of one mole of compound from its elements
Filtration
Separating a solid from a liquid
Heat
Transfer of energy with temperature
Kinetic Molecular Theory
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
Chromatography
Separating substances through differences in rates
Rutherford
Gold Foil Experiment, discovered nuclei, atoms have a lot of space
Potential energy
Energy from position or composition
Endpoint
Indicator changes color
Dalton's law of partial pressures
Ptot = P1 + P2 + P3...
Law of conservation of mass
Mass is neither created nor destroyed
Spectator ions
Ions that do not participate in the reaction
Effusion
Gas into a vacuum
Strong Bases
All Group IA elements with OH- Ca(OH)2, Sr(OH)2, Ba(OH)2,
Change in enthalpy for reaction
sum of heat of formations of products - sum of heat of formations of reactions
Heat capacity
heat absorbed / increase in temperature
Arrhenius acid
Produces H+ (H3O+) in water
Law of conservation of energy
Energy can be converted but never destroyed
Enthalpy (∆H)
∆H = ∆E + P(∆V)
Exothermic
Energy out of the system
Internal energy (∆E)
∆E = q + w
Reducing agent
Is oxidized (causes reduction)
Endothermic
Energy into the system
Lewis base
Electron pair acceptor
Arrhenius base
Produces OH- in water
Reduction
Gain of electrons (GER) Reduction is gaining (RIG)
Distillation
Depends on differences in volatility
Bronsted-Lowry base
Proton acceptor
Diffusion
Mixing of gases
Solubility Rules
Chlorates, Acetates, Sulfates, Halogens, Nitrates, Group IA
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.)
1 standard atmosphere
1 atm, 760 mm Hg, 760 torr, 101,325 Pa
Weak Electrolytes
Conduct currents very weakly
STP Conditions
0 degrees Celsius, 22.4 L
Work
Force acting over a distance
Bronsted-Lowry acid
Proton donor
First law of thermodynamics
The energy of the universe is constant
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
Redox reaction
Electrons are transferred
Lewis acid
Electron pair donor
Precipitation reaction
An insoluble substance is formed as a result of the reaction
Oxidation
Loss of electrons (LEO) Oxidation is Losing (OIL)
Kinetic energy
Energy from motion
Types of Chemical Reactions
Precipitation reactions, Acid-Base reactions, and Redox reactions
Oxidizing agent
Is reduced (causes oxidation)
JJ Thomson
Cathode Ray, discovered the electron
Millikan
Oil Drop Experiment, determined mass and magnitude of the electron
Section 2
(50 cards)
Bond angle of a linear shape?
180
Aufbau principle
Progressively add electrons to each sub level
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)
Dual nature of light
Light acts as a wave and as particulate matter
Number of nonbonding pairs in a V shape?
2
Localized electron model parts
Lewis diagram, VSEPR model (geometry), type of atomic orbitals
Number of bonds in a tetrahedral shape?
4
Metallic bond
Delocalized electron
Pauli exclusion principle
Electrons with the same spin cannot occupy the same space
Ionization energy trend
Increases across a period (electron shielding not complete), decreases down a group (more electron shielding)
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
Bond angle of a trigonal planar shape?
120
Energy of a photon equation
Planck's constant x speed of light / frequency
Covalent bonding
Electrons are shared by nuclei
Hybridization of a tetrahedral shape?
sp3
Resonance
More than one valid Lewis structure
Wavelength
distance between two peaks or troughs in a wave
Ionization energy
Energy required to remove a valence electron from an atom
Localized electron model
Molecule is composed of atoms bound together by sharing pairs of electrons
Hybridization of a linear shape?
sp
Hybridization of a bent shape?
sp2
Dipolar or dipole moment
Has center of positive and center of negative charge
Number of bonds in a bent shape?
2
Electron affinity
Energy change associated with the addition of an electron to a gaseous atom
Number of bonds in a trigonal planar shape?
3
Bond energy
Energy needed to break bond
Coulomb's law
Energy of interaction between a pair of ions
Number of a bonds in a V shape?
2
Number of bonds in a linear shape?
2
Hybridization of a V shape?
sp3
Number of bonds in a trigonal pyramidal shape?
3
Bond angle of a tetrahedral shape?
109.5
Number of nonbonding pairs in a trigonal pyramidal shape?
1
Electronegativity
Ability of an atom in a molecule to attract shared electrons to itself
Bond angle of a trigonal pyramidal shape?
<109.5
Basic wave equation
speed of light = wavelength x frequency
Frequency
number of cycles per second
Lone pairs
Pairs of electrons localized
Bond angle of a bent shape?
<120
Diffraction
Light is scattered from points or lines
Types of electromagnetic radiation (largest to smallest)
radio, micro, IR, visible, UV, X-rays, gamma
Types of electromagnetic radiation (smallest to largest)
gamma, X-rays, UV, visible, IR, micro, radio
de Broglie's equation
Wavelength of a particle
Atomic radius trend
Decreases across a period (more effective nuclear charge), increases down a group (more electron shielding)
Photoelectric effect
Effect occurring when electrons are emitted from the surface of a metal when light strikes it
Hund's rule
Different electrons to different orbitals, same spin
Bond angle of a V shape?
<109.5
Hybridization of a trigonal planar shape?
sp2
Hybridization of a trigonal pyramidal shape?
sp3
Number of nonbonding pairs in a bent shape?
1
Section 3
(50 cards)
Triple point
Where all three states exist
Amorphous solids
Components frozen in place with no arrangement
Alloy
Contains a mixture of elements and has metallic properties
Negative ∆H
Energy released
Negative deviation from Raoult's law
More IMFs, lower vapor pressure
Ionic bond
Transfer of electrons
Nonpolar covalent bond
Equal sharing of electrons
Zeroth order half life
t1/2 = [A]0 / 2k
Zeroth order integrated rate law
[A] = -kt + [A]0
Interstitial alloy
Small atoms in holes
Pi bond
Bond between the p orbitals
Temperature and rate
Higher temperature increases rate
Temperature and solubility
Increases solubility of solid, decreases solubility of gases
Pressure and solubility
Increases solubility of a gas
First order rate law
Rate = k[A]
Henry's Law
Amount of gas dissolved proportional to pressure of gas above solution
Zeroth order rate law
Rate = k
Sigma bond
Bond between the s orbitals
Vapor pressure
Pressure of vapor at equilibrium
Electronegativity differences
Nonpolar covalent (0-0.4), polar covalent (0.4-1.67), ionic (above 1.67)
Colloid
Suspension of particles
Positive deviation from Raoult's law
Less IMFs, more molecules escape, higher vapor pressure
Heat of solution
Enthalpy change formation of a solution, sum of enthalpy values from each step
Hydrogen bond
Special type of dipole, hydrogen with N, F, or O atom
Coagulation
Destruction of colloid by heating or adding electrolyte
Positive ∆H
Energy absorbed
London dispersion forces
Between non polar molecules
Temperature and vapor pressure?
Vapor pressure increases significantly with temperature
Zeroth order slope
Slope = -k
Raoult's Law
Nonvolatile solute simply dilutes the solvent
Catalyst
Increases rate of reaction but not consumed
Initial rate
Instantaneous rate after reaction begins
Tyndall effect
Scattering of light by particles
Critical temperature
Temperature above which vapor cannot be liquefied no matter the pressure
Polar covalent bond
Unequal sharing of electrons
Crystalline solids
Components organized in a lattice
Substitutional alloy
Metal atoms replaced by metal atoms of same size
Zeroth order plot
[A] vs. t
Reaction rate
Change of concentration over time (Rate = delta [A] / delta t)
Heat of fusion
Enthalpy change which occurs at the melting point when a solid melts
Surface area and rate
More surface area increases rate
Sublimation
Solid directly to gas
Phase diagram
Representation of phases of a substance
Critical point
Critical temperature and critical point
Vapor pressure formula (Hg column)
Patmosphere = Pvapor +Pmercury column
Colligative properties
Freezing point depression, boiling point elevation, osmotic pressure
Rate law
Rate depends on concentration
Critical pressure
Pressure required to produce liquefaction at the critical temperature
Integrated rate law
Concentrations depends on time
IMFs and vapor pressure?
High IMFs --> low vapor pressure, Low IMFs --> high vapor pressure
Section 4
(47 cards)