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28 Cards in this Set
- Front
- Back
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Hydrate
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crystals that contain attached water molecules
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Anhydrous
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substances without water
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Electronegativity
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measure of an atomic attraction for electrons when bonded to another atom
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Ionization Energy
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the amount of energy required to remove the most loosely bound electrons from an atom
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Molarity
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the concentration of an solution quantitively, the number of moles of solute dissolved in 1L of solution
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Moles
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quantity of anything that has the same number of particles found in 12 g of carbon-12 (6.02 x 10^23)
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Potential Energy
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stored energy
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Kinetic Energy
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energy in motion
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Temperature
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measure of average kinetic energy
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Empirical Formula
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lowest whole number ratio
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Molecular Formula
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gives you the number of atoms in each element in a formula
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Saturated
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when a solution is dissolved to the maximum possible amount of solute, the rate of dissolving is equal to the rate of crystallization
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Unsaturated
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have not hit their saturation points, contain less solute than they can hold, the rate of dissolving is greater than the rate of crystallization
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Super Saturated
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contain a greater amount of solute than needed to form a saturated solution, the rate of dissolving is less than the rate of crystallization
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Catalyst
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speeds up the rate of reaction by decreasing the activation energy by providing an alternate pathway
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Enthalpy
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tendency in nature to change to a state of lower energy
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Entropy
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state of maximum randomness
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Equilibrium
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occurs when opposite reactions occur at the same rate
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Ionic Bond
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when metals transfer/lose electrons to nonmetals
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Covalent Bond
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sharing of electrons in order to form a stable octet between nonmetals only
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Hydrogen Bond
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forms between hydrogen and oxygen,nitrogen, or fluorine. Hydrogen bonds are very specific and lead to certain molecules having special properties due to these types of bonds
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Fission
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splitting of something into two or more parts
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Fusion
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two or more atomic nuclei colliding at a very high speed and join to form a new type of atomic nucleus
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Artificial Transmutation
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the conversion of one element into another by artificial means. Ex: bombarding with fundamental particles
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Natural Radioactivity
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the activity existing in nature
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Activation Energy
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minimum amount of energy needed for particles to collide and for a chemical reaction to occur
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Heat of Reaction
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difference between the potential energy of the reactants and the products, tells whether the energy was released or absorbed
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Activation Complex
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reactants are in the transition state, halfway between being reactants and forming products
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