Term
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Definition
| the zero point on the kelvin temperature scale, equivalent to -273.15C |
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Term
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Definition
| a quantity used by general agreement of the scientific community |
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Term
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Definition
| the closeness of a measurement to the true value of what is being measured |
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Term
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Definition
| a compound that produces hydgrogen ions in solution |
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Term
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Definition
| a list of elements in order of decreasing activity |
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Term
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Definition
| the amount of product that forms whe a reaction is carried out in the labratory |
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Term
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Definition
| one of two or more differnet molecular forms of an element in the same physical state |
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Term
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Definition
| a misture composed of two or more elements, at least one of which is a metal |
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Term
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Definition
| the hight of a wave's crest |
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Term
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Definition
| any atom or group of atoms with a negative charge |
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Term
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Definition
| water that contains dissolved substances |
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Term
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Definition
| the pattern formed whn light passes through a prism or diffraction grating to separate it into the different frequencies of light it contains |
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Term
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Definition
| the weighted average of the masses of the isotopes of an element |
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Term
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Definition
| a unit of mass equal to one-twelfth the mass of carbon-12 atom |
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Term
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Definition
| the number of protons in the nucleus of an atom of an element |
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Term
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Definition
| a mathematical expression describing the probability of finding an electron at various locations |
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Term
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Definition
| one-half the distance between the nuclei of two atoms of the same element when the atoms are joined |
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Term
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Definition
| the rule that electrons occupy the orbitals of lowest energy first |
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Term
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Definition
| the number representative particles contained in one mole of a substance |
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Term
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Definition
| a chemical equation in which mass is conserved |
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Term
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Definition
| a compound that produces hydroxide ions in solution |
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Term
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Definition
| a compound composed of two elements |
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Term
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Definition
| the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent |
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Term
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Definition
| a molecular orbital that can be occupied by two electrons of covalent bond |
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Term
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Definition
| for a given mass of gas at constant temp, the volume of the gas varies inversely with pressure |
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Term
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Definition
| the chaotic movement of colloidal particles, caused by collision with particles of the solvent in which they are dispersed |
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Term
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Definition
| the quantity of heat needed to raise the temperature of 1 g fo pure water |
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Term
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Definition
| an insulated device used to measure the absorption or release of heat in chemical or physical processes |
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Term
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Definition
| the precise measurement of heat flow out of a system for chemical and physical processes |
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Term
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Definition
| a substance that increases the rate of reaction by lowering the activation-energy barrier |
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Term
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Definition
| a stream of electrons produced at the negative electrode of a tube containing a gas at low pressure |
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Term
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Definition
| any atom or group of atoms with a positve charge |
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Term
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Definition
| 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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Term
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Definition
| an expression representing a chemical reaction |
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Term
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Definition
| an expression that indicates the number and type of atoms present in the smallest representative unit of substance |
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Term
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Definition
| a small whole number that appears in front of a formula in a balanced chemical equation |
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Term
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Definition
| a property of a solution that depends only upon the number of solute particles, and not upon their identities |
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Term
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Definition
| the law that describes the relationship among the pressure, temperature, and volume of an enclosed gas |
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Term
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Definition
| 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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Term
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Definition
| an equation that shows dissolved ionic compounds as dissociated free ions |
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Term
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Definition
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Term
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Definition
| a measure of how much the volume of matter decreases under pressure |
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Term
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Definition
| a solution containing a large amount of solute |
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Term
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Definition
| a measurement of the amount of solute that is dissolved in a given quantity of solvent |
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Term
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Definition
| a ratio of equivalent measurements used to convert a quantity from one unit to another |
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Term
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Definition
| a covalent bond in which one atom contributes both bonding electrons |
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Term
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Definition
| the number of ions of oppisite charge that surround each ion in a crystal |
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Term
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Definition
| a bond formed by the sharing of electrons between atoms |
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Term
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Definition
| a chemical change in which a single compound is broken down into two or more simpler products |
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Term
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Definition
| a molecule consisting of two atoms |
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Term
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Definition
| the tendancy of molecules to move toward areas of lower concentration until the concentration is uniform throughout |
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Term
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Definition
| a solution that contains a small amount of solute |
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Term
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Definition
| a technique of problem-solving that uses the units that are part of a measurement to help solve the problem |
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Term
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Definition
| a molecule that has two poles, or regions with opposite charges |
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Term
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Definition
| attractions between molecules caused by the electron motion on one molecule affectin g the electron motion on the other trhough electrical forces |
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Term
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Definition
| a process used to separate dissolved solids from a liquid, which is biled to produce a vapor that is then condencsed into a liquid |
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Term
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Definition
| a bond in which two atoms share two pairs of electrons |
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Term
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Definition
| a chemical change that involves an exchange of positive ions between tow compuonds |
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Term
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Definition
| the process that occurs when a gas escapes through a tiny hole in its container |
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Term
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Definition
| a compound that conducts an electric current when it is in a an aqueous solution or in the molten state |
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Term
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Definition
| the arrangement of electrons of an atom in its ground state into various orbitals around the nuclei of atoms |
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Term
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Definition
| a notation that depicts valence electrons as dots areound the atomic symbol of the element |
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Term
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Definition
| the ability of an atom to attract electrons when the atom is in a compound |
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Term
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Definition
| a formula with the lowest whole number ratio of elements in a compound |
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Term
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Definition
| a process that absorbs heat from the surroundings |
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Term
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Definition
| the specific energies an electron in an atom or other system can have |
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Term
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Definition
| the heat content of a system at constant pressure |
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Term
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Definition
| the difference between the accepted value and the experimental value |
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Term
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Definition
| a reactant present in a quantity that is more than sufficent to react with a limiting reactant |
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Term
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Definition
| a process that releases heat to its surroundings |
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Term
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Definition
| a quantitative value measured during an experiment |
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Term
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Definition
| a property that depends on the amount of matter in a sample |
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Term
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Definition
| a process that separates a solid from the liquid in a heterogeneous mixture |
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Term
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Definition
| the lowest whole number ratio of ions in an ionic compound |
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Term
| freezing point depression |
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Definition
| the difference in temperature between the freezing point of a solution and the freeaing point of the pure solvent |
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Term
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Definition
| the number of wave cycles that pass a given point per unit of time |
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Term
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Definition
| the pressure of a gas is directly proportional to the kelvin temperature if the volume is constant |
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Term
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Definition
| the lowest possible energy of an electron described by quantum mechanics |
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Term
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Definition
| energy that transfers from one object to another because of a temperature diffeence between teh objects |
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Term
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Definition
| it is impossible to know exactly both the velocity and the positio of a particle at the same time |
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Term
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Definition
| electrons occpy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible |
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Term
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Definition
| a compound that has a specific number of water molecules bound to each formula unit |
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Term
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Definition
| the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals |
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Term
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Definition
| attractive forces in which a hydrogen covalentlybonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom |
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Term
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Definition
| a property that depends on the type of matter in a sample, not the amount of matter |
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Term
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Definition
| a property that depends on the type of matter in a sample, not the amount of matter |
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Term
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Definition
| an atom or group of atoms that has a positive or negative charge |
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Term
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Definition
| the electrostatic attraction that binds oppositely charged ions together |
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Term
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Definition
| the energy required to remove an electron from an atom in its gaseous state |
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Term
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Definition
| atoms of the same element that hve the same atomic number but different atomic masses due to a different number of nuetrons |
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Term
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Definition
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Term
| law of conservation of energy |
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Definition
| in any chemical or physical process, energy is neither created nor destroyed |
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Term
| law of definite proportions |
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Definition
| in samples of any chemical compound,the masses of elements are always in the same proportion |
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Term
| law of conservation of mass |
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Definition
| in any physical change or chemical reaction, mass is conserved |
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Term
| law of multiple proportions |
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Definition
| whenever two elements form more than one compound |
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Term
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Definition
| any reactant that is used up first in a chemical reaction |
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Term
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Definition
| the total number of the amount of matter that an object contains |
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Term
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Definition
| the temperature at which a substance changes from a solid to a liquid |
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Term
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Definition
| the force of attractino that holds metals together |
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Term
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Definition
| the concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 kilogram of solvent |
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Term
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Definition
| a term used to refer to the massof a mole of any substance |
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Term
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Definition
| the volume occupied by 1 mole of a gas at standard temperature and pressure |
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Term
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Definition
| the concentration of solute in a solution expressed as the numberof moles of solute dissolved in 1 liter of solution |
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Term
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Definition
| the amount of a substance that contains 6.o2x1023 representative particles of that substance |
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Term
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Definition
| a neutral group of atoms joined together by covalent bonds |
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Term
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Definition
| a single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons |
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Term
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Definition
| an equation for a reaction in solution showing only those particles that are directly involved in the chemical change |
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Term
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Definition
| a covalent bond in which the electrons are shared equally by two atoms |
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Term
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Definition
| 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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Term
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Definition
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Term
| Paulie exclusion principle |
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Definition
| an atomic orbital may describe at most two electrons, each with opposite spin direction |
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Term
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Definition
| the percent by mass of each element in a compound |
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Term
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Definition
| the percent that a measured value differs from the accepted value |
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Term
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Definition
| the ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage |
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Term
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Definition
| when the elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties |
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Term
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Definition
| any part of a sample with uniform composition and properties |
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Term
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Definition
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Term
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Definition
| a covalent bond in which the bonding elctrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded axis |
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Term
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Definition
| a covalent bond between atomsin which the electrons are shared unequally |
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Term
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Definition
| a molecule in which one side of the molcule is slightly negative and the opposite side is slightly positive |
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Term
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Definition
| a tightly bound group of atoms that behaves as unit and has a positive or negative change |
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Term
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Definition
| a solid that forms and settles out of a liquid mixture |
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Term
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Definition
| a substance produced in a chemical reaction |
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Term
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Definition
| the amount of energy needed to move an electron from one energy level to another |
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Term
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Definition
| the modern description, primarily mathematical, of the behavior of electrons in atoms |
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Term
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Definition
| a substance present at the start of a reaction |
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Term
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Definition
| the smallest unit into which a substance can be broken down without a change in composition, usually atoms, molecules, or ions |
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Term
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Definition
| a solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure |
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Term
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Definition
| a bond formed when two atomic orbitals combine for form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei |
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Term
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Definition
| all the digits that can be known precisely in a measurement, plus a last estimated digit |
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Term
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Definition
| a bond formed when two atoms share a pair of electrons |
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Term
| single displacement reaction |
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Definition
| a chemical change in which one element replaces a second element in a compound |
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Term
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Definition
| a chemical equation that does not indicate the relative amounts of reactants and products |
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Term
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Definition
| 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 |
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Term
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Definition
| dissolved particles in a solution |
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Term
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Definition
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Term
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Definition
| the dissolving medium in a solution |
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Term
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Definition
| the amount of heat needed to increase the temperature of 1 g of a substance 1 C |
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Term
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Definition
| an ion that is not directly involved in a chemical reaction |
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Term
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Definition
| wavelengths of visible light that are separated when a beam of light passes through a prism |
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Term
| standard temperature and pressure |
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Definition
| the conditions under which the volume of a gas is usually measured |
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Term
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Definition
| that portion of chemistry dealing with numerical relationships in chemical reactions |
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Term
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Definition
| a chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion |
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Term
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Definition
| a solution that contains more solute than it can theoretically hold at a given temperature |
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Term
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Definition
| an inward force that tends to minimize the surface area of a liquid |
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Term
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Definition
| the amount of product that could form during a reaction calculated from a balanced chemical equation |
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Term
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Definition
| a covalent bond in which three pairs of electrons are shared by two atoms |
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Term
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Definition
| scattering of light by particles in a colloid or suspension, which causes a beam of light to become visible |
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Term
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Definition
| a solution that contains less solute than a saturated solution at a given temperature and pressure |
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Term
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Definition
| an electron in the highest occupied energy level of an atom |
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Term
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Definition
| the two weakest intermolecular attractions--dispersion interactions and dipole forces |
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Term
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Definition
| describes the gaseous state of a substance that is generally a liquid or solid at room temperature |
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Term
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Definition
| a measure of the force exerted by a gas above a liquid in a sealed container |
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