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97 Cards in this Set
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Chemistry
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the central science, which deals with all the matter in the universe and the changes it undergoes
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Matter
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anything which has mass and takes up space(volume)
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Solid
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definite shape, and volume and is not easily compressed
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Liquid
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indefinite shape and volume, and not easily compressed
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Gas
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indefinite shape and volume and is easily compressed
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Homogeneous Mixture
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a mixture that is visually the sample throughout the entire sample
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Heterogeneous Mixture
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a mixture that is visually different throughout the sample
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Element
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contains only one type of atom
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Compound
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can be broken down to simpler substances by chemical means
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Physical Change
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can be observed without changing the identity of the substance
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Chemical Change
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the substance identity is different after the change
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Density
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the ratio of the mass of an object to its volume
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Dalton
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1808-Dalton’s Atomic Theory
1.All elements are composed of invisible parts called atoms 2.Atoms of the same element are identical-False because of isotopes 3.Atoms can combine, separate, and rearrange in a Chemical Reaction 4.Atoms combine in simple whole number ratios |
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Proton
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a positively charged subatomic particle found in a nucleolus of an atom
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Electron
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“-” charged subatomic particle outside the nucleus
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Nucleus
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a time dense central portion of an atom, composed of protons and neutrons.
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Atom
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the smallest particle of an element that retains its identity in a chemical reaction
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Atomic Number
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is equal to the number of protons found in the nucleus of the atom
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Mass Number
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is the sum of protons and neutrons in the nucleus of the atom
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Chemistry
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the central science, which deals with all the matter in the universe and the changes it undergoes
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Matter
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anything which has mass and takes up space(volume)
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Solid
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definite shape, and volume and is not easily compressed
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Liquid
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indefinite shape and volume, and not easily compressed
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Gas
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indefinite shape and volume and is easily compressed
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Homogeneous Mixture
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a mixture that is visually the sample throughout the entire sample
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Heterogeneous Mixture
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a mixture that is visually different throughout the sample
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Element
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contains only one type of atom
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Compound
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can be broken down to simpler substances by chemical means
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Physical Change
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can be observed without changing the identity of the substance
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Chemical Change
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the substance identity is different after the change
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literaly chemical change
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Isotopes
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atoms of the same element that have the same atomic number but different atomic masses due to a different number of neutrons
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Electron configuration
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the arrangement of electrons of an atom in its ground state into various orbitals around the nuclei of atoms
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Valence Electrons
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electrons in the highest energy level
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Aufbau Principle
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states that we must occupy the lowest energy level orbital that can receive it
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Hund’s Rule
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states that each orientation of an orbital must be occupied by one electron before electron before a second electron is added to any orbital orientation.
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Pauli Exclusion Principle
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states that no two electrons in any one atom can have the same set of four quantum numbers
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Octet Rule
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atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas, usually eight valence electrons.
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Photon
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a quantum of light; a discrete bundle of electromagnetic energy that interacts with matter similarly to particles
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Nonmetal
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no luster, not malleable, not ductile, not good conductor of heat and electricity
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Metalloid
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semi-metal
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Ion
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charged atom-gained or loss electrons
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Anion
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a negative ion
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Cation
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a positive ion
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Ionization Energy
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the energy required removing an electron from an atom in its gaseous state
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Electronegativity
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an ability of an atom in a bond to attract an electron
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Atomic Radius
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one-half the distance between the nuclei of the two atoms of the same element when the atoms are joined
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↓,←
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Lewis/ Electron Dot Structure
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a notation that depicts valence electrons as dots around the atomic symbol of the element; the symbol represents the inner electrons and atomic nucleus; also called Lewis dot Structure
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Covalent
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sharing of electrons between two atoms
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Diatomic molecule
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a molecule consisting of two atoms
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Polar molecule
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a molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive.
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Non-polar covalent bond
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a covalent bond in which the electrons are shared equally by two atoms.
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Intermolecular Forces
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are forces of attraction between molecules
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London Dispersion Forces
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an intermolecular force between two Non Polar molecules
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Dipole-Dipole Factors
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an attractive force between two polar molecules
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Hydrogen Bonding
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a intermolecular force between Hydrogen and a highly electronegative atom. (FONS)
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Resonance
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when a single Lewis Dot cannot explain the observed Bonding
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Metallic Bonding
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the force of attraction that holds metals together; it consists of the attraction of free-floating valence electrons for positively charged metal ions.
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VESPER
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a valance-shell electron-pair repulsion theory; because electron pairs repeal, molecules adjust their shapes so that valence electron pairs are as far apart as possible.
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Hybridization
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the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals.
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Single Replacement
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a chemical equation that does not indicate the relative amounts of reactants and products
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Double Replacement
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a chemical change that involves an exchange of positive ions between two compounds.
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Synthesis
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a chemical change in which two or more substances react to form a single new substance
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Decomposition
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a chemical change in which a single compound is broken down into tow or more simpler products
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Combustion
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a chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light
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Oxidation Number
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a positive or negative number assigned to an atom to indicate its degree of oxidation or reduction; the oxidation number of an uncombined element is zero
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Molar Mass
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a term used to refer to the mass of a mole of any substance
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Percent Composition
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the percent by mass of each element in a compound
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Empirical Formula
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a formula with the lowest whole-number ratio of elements in a compound; the empirical formula of hydrogen peroxide (H2O2 → HO)
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Molecular Formula
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represents the exact number of atoms in a molecule
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Reactant
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a substance present at the start of a reaction
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Product
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a substance produced in a chemical reaction
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Theoretical Yield
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the amount of product that could form during a reaction calculated from a balanced chemical equation; it represents the maximum amount of product that could be formed from a given amount of reactant.
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Percent Yield
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the ration of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
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Ideal Gas Law
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the relationship PV=nRT, which describes the behavior of an ideal gas
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Boyle’s Law
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for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure.
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Charles Law
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the volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant.
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V up T up
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Combined Gas Law
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the law that describes the relationship among the pressure, temperature, and the volume of an enclosed gas.
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Dalton’s Law of Partial Pressure
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at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressure of the component of gas.
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V=constant
T=constant P=sum of partial pressure of gas |
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Kinetic Molecular Theory
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the theory explaining the states of matter, based on the concept that all matter consists of tiny particles that are in constant motion
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Effusion
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the process that occurs when a gas escapes through a tiny hole in its container
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Diffusion
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the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
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Vaporization
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the conversion of a liquid to a gas or a vapor
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Standard temperature and pressure (STP)
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the conditions under which the volume of a gas is usually measured; standard temperature is 0°C, and the standard pressure is 101.3kPA, or 1 atmosphere(atm).
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Phase Diagram
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a graph showing the conditions at which a substance exists as a solid, liquid, or vapor.
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Kinetic Energy
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the energy an object has because of its motion
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Equilibrium
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the relative concentrations of reactants and products of a reaction that has reached equilibrium; indicates whether the reactants or products are favored in the reversible reaction
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Molar Heat of Vaporization (Δhvap)
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the amount of heat absorbed by one mole of a liquid as it vaporizes at a constant temperature.
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Molar Heat of Fusion- (Δhfus)
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the amount of the hat absorbed by one mole of a solid substances as it melts to a liquid a constant temperature
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Molar Heat of Condensation- (ΔHcond)
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the amount of heat released by one mole of a vapor as it condenses to a liquid at a constant temperature
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Enthalpy (H)
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the heat content of a system at constant pressure
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Entropy (S)
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a measure of the disorder of a system; systems tend to go from a state of order (low entropy) to a state of disorder (high entropy)
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Solubility
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the amount of a substance that dissolves in a given quantity of solvent at specified conditions of temperature and pressure to produce a saturated solution
Solute- dissolved particles in a solution |
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Solute
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dissolved particles in a solution
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Solvent
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the dissolving medium in a solution
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Molarity (M)
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the concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 liter of solution
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Molality(m)
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the concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 kilogram (1000g) of solvent.
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Aqueous Solution
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water that contains dissolved substances
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