 | Term | Definition |
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ΔT |
ΔQ is proportional to this |
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Temperature |
The average amount of kinetic energy of particles in the substance |
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Temperature |
A function of the heat content of a body |
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Electronic |
The type of energy that is chemical potential energy |
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Vibrational |
Solid, liquid & gas kinetic energy |
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Rotational |
Liquid & gas kinetic energy |
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Translational |
Gas kinetic energy |
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ΔU=ΔQ-w |
Equation for change in internal energy |
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w=PΔV |
Equation for work done |
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Temperature |
Dictates direction in which any energy will flow |
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Heat |
Sum of movement of molecules (vibration, rotation, translation) |
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Heat |
This is transferred due to difference in temperature |
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Internal Energy |
Total amount of energy stored in heat and chemical potential energy (vibrational, rotational, translational and electronic) |
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Internal Energy |
This shows change in heat or ability to work (only gas, change volume of gas at constant pressure) |
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Work |
Force overcoming or resisting another force |
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Work |
This is shown when mass has traveled a distance in a 3-D plane |
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Zeroth Law |
This states that heat (energy) moves from hot to cold objects |
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Maxwell-Boltzmann distribution |
At the point where heat no longer flows between bodies, the distribution of kinetic energy in all particles of the system follows one of these: |
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Heat Death of the Universe |
The phenomenon where the universe reaches thermal equilibrium |
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Heat capacity |
The capacity to take heat without rise in temperature |
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Specific heat capacity |
The quantity of heat required to raise 1 K in 1 gram of a substance |
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ΔQ=mcΔT |
Equation for heat change involving specific heat |
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4.1868 |
Liquid water's specific heat capacity [with J/(Kg)] |
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calorie |
Another name for 4.184 J/(Kg) |
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Total heat content |
The total sum of all kinetic energies in a sample |
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Internal Energy |
Potential energy combined with kinetic energy |
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Enthalpy |
The combined sum of all energy in any sample of matter |
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ΔH=ΔU+w |
Equation for change in enthalpy |
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ΔQ |
At constant pressure ΔH (R.T.P) is equal to this |
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First law |
The law which states that energy can neither be destroyed nor created |
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0 |
Total sum of ΔH in the universe |
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Conduction |
1st way heat can travel (alphabetically) |
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Convection |
2nd way heat can travel (alphabetically) |
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Radiation |
3rd way heat can travel (alphabetically) |
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Amount |
1st state of matter (alphabetically) |
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Pressure |
2nd state of matter (alphabetically) |
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Temperature |
3rd state of matter (alphabetically) |
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Volume |
4th state of matter (alphabetically) |
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Enthalpy |
An example of a state function |
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Entropy |
Measure of disorder (chaos) in a system |
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Entropy |
The probability distribution within matter |
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Second law |
The law which states that energy will always spontaneously flow in a direction in which entropy increases |
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Third law |
The law which states that the entropy of a perfect crystal at absolute zero is zero |
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Increases |
Entropy increases as the number of partices in a system... |
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Increases |
Entropy increases as the temperature of a reacting system... |
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Phase |
Entropy increases as the substance changes this |
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Fixed energy |
Energy which cannot perform work |
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Free energy |
Energy available to do work |
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ΔG=ΔH-TΔS |
The change in Gibbs Free energy (assume constant temperature) |
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Feasible |
A reaction with negative ΔG is |
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Collision theory |
This theorizes that energy is required to break chemical bonds (+ΔH, endothermic) and energy is released when bonds are formed (-ΔH, exothermic) |
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Activation energy |
The energy required to initiate reactions under kinetic control |
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Electrodes |
Two of these (made of different substances) are required to make a reacting cell |
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Physical contact |
The reactants of a battery cell cannot have this with each other |
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solution |
Half-cells contain one of this of the metal used as the electrode |
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salt bridge |
porous barrier |
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Anode |
This electrode shrinks |
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Cathode |
This electrode grows |
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Galvanic cell |
Another name for a Voltaic cell (a spontaneous cell with -ΔG) |
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Electrolytic cell |
A type of cell in which an external power source overcomes the natural tendency of the electron flow |
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Decoherence |
The phenomenon that the possibilities of quantum mechanics collapses into one state |
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Blackbody radiation |
The phenomenon that all objects at the same temperature glow at the same color |
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E=hv |
The equation of the relationship between energy and the frequency of light |
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Harmonic oscillator |
All waves begin with this |
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Photoelectric effect |
The phenomenon in which electrons are emitted from matter after they are absorbed |
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C |
The symbol for wavelength multiplied by frequency |
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Particle-wave duality |
The phenomenon that light can be reflected and refracted, but that it also can be blocked and it has momentum (no mass) |
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Energy levels |
Bohr's atomic model stated that electrons inhabited these specific regions |
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Lyman series |
Ultraviolet emission lines for hydrogen |
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Balmer series |
Visible light emission lines for hydrogen |
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Paschen series |
Near-Infrared emission lines for hydrogen |
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Brackett series |
1 of 2 Intermediate Infrared emission lines for hydrogen (alphabetically) |
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Pfund series |
2 of 2 Intermediate Infrared emission lines for hydrogen (alphabetically) |
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Wavelength |
Planck's constant, divided by the product of mass and frequency |
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Heisenberg's uncertainty principle |
The idea that during an experient the act of observation affects the results of experimentation |
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101.325 kPa |
Sea-level atmospheric pressure |
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n |
symbol for principal quantum number (main energy level electron inhabits) |
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l |
Symbol for angular momentum quantum number |
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n-1 |
The possible values of l (angular momentum quantum number) ranges from 0 to ... |
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ml |
Symbol for magnetic quantum number (don't worry about subscript) |
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l |
Possible values for the magnetic quantum number ranges from a negative to a positive of this value |
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ms |
Symbol for spin quantum number (don't worry about subscript) |
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n |
The number of sublevels in an orbital |
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n^2 |
The number of orbitals per main energy level |
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2n^2 |
The number of electrons per main energy level |
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orbital |
The region of space that surround the nucleus where the electron is most likely found |
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node |
A region of space where the wave amplitude is always zero |
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Aufbau principle |
This states that electrons will always fill the orbitals from bottom to top with respect to energy |
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Pauli Exclusion principle |
This states that no two fermions (electrons) can share the same set of quantum numbers |
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Hunds Rule |
This states that in any orbital, we fill all of the positive spin interger particles into the sub-orbitals before any spin negatives |
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Period |
A row in a periodic table |
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Group |
A column in a periodic table |
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periodic function |
The physical and chemical characteristics of elements have this relationship with their atomic number |
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periodicity |
A repeating pattern that is at regular intervals |
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8, 8, 18, 18, 32, 32 |
These are the periodic numbers in order |
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Transition Metals |
Groups 3-12 |
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Alkali Metals |
Group 1 |
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Alkaline Earth Metals |
Group 2 |
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Halogens |
Group 17 |
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Noble Gases |
Group 18 |
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Coinage Metals |
Group 11 |
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Other Metals & Other Non-metals |
group 13-16 |
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Semi-conductors |
The four nonmetals and the two metals along the metal-nonmetal dividing line (Boron, silicon, Germanium, Arsenic, Antimony, Tellurium) |
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Rare Earths |
Lanthanoids and Actinoids (Up to Uranium) |
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Trans-uranic |
Elements with atomic number higher than 92 are such |
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Stoichiometry |
The relative proportions in which elements form compounds, or in which substances react |
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The law of definite proportions |
"The proportions of elements by mass in a compound are always the same, no matter how the compound is made" |
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The law of Multiple Proportions |
“When two elements A & B combine to form more than one compound, then the masses of B that combine with a fixed mass of A are in a simple ratio to one another” |
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The law of Equivalent Proportions |
"When two elements A & B each form a compound with a third element C, then a compound of A & B will contain A & B in the relative proportions in which they react with C." |
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The same |
At the same temperature and pressure, the number of particles in the same volume of two different gases are... |
