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79 Cards in this Set
- Front
- Back
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Actual yield
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the amount of product actually obtained in a reaction
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Accuracy
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the closeness of a measurement to the true value of the quantity that is measured
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Anion
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An ion with a net negative charge
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Bronsted acid
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A substance capable of donating a proton
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Bronsted base
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A substance capable of accepting a proton
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Buffer Solution
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A solution that has the ability to resist small changes in pH upon the addition of small amounts of either acid or base
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Catalyst
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A substance that increases the rate of a chemical reaction without itself being consumed
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Cation
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An ion with a net positive charge
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Chemical reaction
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Processes in which one or more substances are converted into other substances. (Also called chemical changes)
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Chemical Kinetics
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The area of chemistry concerned with the speeds, or rates, at which chemical reactions occur
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Compound
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A substance composed of atoms of two or more elements chemically united in fixed proportions
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Covalent Bond
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A bond in which two two electrons are shared by two atoms
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Density
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The mass of a substance divided by its volume
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Diffusion
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The gradual mixing of one substance with another due to random molecular motion
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Dilution
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A procedure for preparing a less concentrated solution from a more concentrated solution
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Electrolyte
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A substance that, when dissolved in water, results in a solution that can conduct electricity
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Electronegativity
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The ability of an atom to attract electrons toward itself in a chemical bond
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Element
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A substance that cannot be separated into simpler substances by chemical means
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Endothermic processes
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Processes that absorb heat from the surroundings
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Energy
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The capacity to do work or to produce change
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Enzyme
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A biological catalyst
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Equilibrium
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A state in which there are no observable changes as time goes by.
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Excess reagents
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One or more reactants present in quantities greater that those needed to react with quantity of the limiting reagent
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Exothermic Processes
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Processes that give off heat to the surroundings
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First Law of Thermodynamics
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Energy can be converted from one form to another, but cannot be created nor destroyed
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Full Ionic equation
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A reaction equation which shows all soluble compounds in their ionic forms
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Heat
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The transfer of thermal energy between two bodies that are at different temperatures
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Hess's Law
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When reactants are converted to products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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Hydrogen bond
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A special type of dipole-dipole interaction between molecules containing hydrogen bonded to an electronegative element. Particularly F, O, and N.
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Inorganic Compounds
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Compounds other than organic compounds.
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Ion
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A charged species.
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Ionic Compound
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A chemical compound composed of cations, and anions combined so that the total positive and negative charges are equal.
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Ionic Bond
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The electrostatic force that holds ions together in an ionic compound
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Ionization energy
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The minimum energy required to remove an electron from an isolated atom in its ground state
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Isotopes
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Atoms having the same number of protons but different numbers of neutrons
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Joule
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Unit of energy given by newtons- meters
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Kinetic Energy
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Energy available because of the motion of an object
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Le Chatelier's Principle
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If an external stress is applied to a system at equilibrium, the system will adjust itself in such a way as to partially offset the stress
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Limiting reagent
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The reactant used up first in a reaction
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Macroscopic properties
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Properties that can be measured directly
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Metals
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Elements that are good conductors of heat and electricity and have the tendency to form positive ions in ionic compounds
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Mixture
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A combination of two or more substances in which the substances retain their identity
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Molar Mass
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The mass of one mole of atoms, molecules, or other particles
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Molarity
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The number of moles of solute in one liter of solution
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Mole
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A collection of Avogadro's number of objects
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Molecular Compound
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A compound consisting of atoms that are covalently bonded
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Molecular equation
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A reaction which shows the complete chemical formulas of all reactants and products
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Molecule
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A neutral aggregate of two or more atoms held together by covalent bonds
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Net Ionic Equation
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A reaction equation in which all spectator ions are removed leaving only the ions and molecules directly involved in the reaction
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Nonelectrolyte
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A substance that, when dissolved in water, gives a solution that is not electrically conducting
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Nonmetals
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Elements that are usually poor conductors of heat and electricity, and have the tendency to gain electrons and form negative ions
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Nonpolar bond
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A covalent bond in which the electrons are equally shared by two atoms, so there are no positive and negative ends
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Nonpolar molecule
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A molecule that does not possess a dipole moment
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Octet rule
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An atom other than hydrogen tends to form bonds until it is surrounded by eight valence electrons
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Organic Chemistry
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The branch of chemistry that deals with carbon compounds
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Oxidation number
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The number of charges an atom would have if electrons were transferred completely in the direction of the atoms with the higher electronegativity
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Oxidation Reaction
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The half-reaction that involves the loss of electrons
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Oxidizing agent
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A substance that can accept electrons from another substance or increase the oxidation number in another substance
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Percent yield
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The ratio of actual yield to theoretical yield, multiplied by 100
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pH
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The negative logarithm of the hydrogen ion concentration
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Photon
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A particle of light
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Physical property
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Any property of a substance that can be observed without transforming the substance into some other substance
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Polar Bond
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A covalent bond in which the bonding electrons are more strongly attracted by one of the bonding atoms creating partial positive and negative ends
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Polar molecule
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A molecule that possesses a dipole moment
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Potential energy
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Energy available by virtue of an object's position
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Precipitate
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An insoluble solid that separates from the solution
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Precision
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The closeness of agreement of two or more measurements of the same quantity
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Pressure
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Force applied per unit area
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Redox reaction
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A reaction in which there is either a transfer of electrons or a change in the ox. numbers of the substances taking part in the reaction
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Reduction reaction
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The half reaction that involves the gain of electrons
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Salt
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An ionic compound made up of a cation and an anion
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Saturated solution
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At a given temperature the solution that results when the maximum amount of a substance dissolves in a solvent
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Significant Figures
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The number of meaningful digits in a measure quantity
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Solubility
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The maximum amount of solute that can be dissolved in a given quantity of solvent at a specific temperature
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Specific Heat
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The amount of energy required to raise the temperature of one gram of the substance by one degree celcius
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Spectator Ions
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Ions that are not involved in the overall reaction
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Thermochemistry
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The study of heat changes in chemical reactions
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Thermodynamics
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The scientific study of the interconversion of heat and other forms of energy
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Titration
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The addition of a know solution to an unknown solution until the reaction between the two is complete
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