L to J vocab – Flashcards
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| absolute zero |
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| the zero point on the kelvin temperature scale, equivalent to -273.15C |
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| accepted value |
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| a quantity used by general agreement of the scientific community |
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| accuracy |
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| the closeness of a measurement to the true value of what is being measured |
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| acid |
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| a compound that produces hydgrogen ions in solution |
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| activity series |
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| a list of elements in order of decreasing activity |
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| actual yield |
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| the amount of product that forms whe a reaction is carried out in the labratory |
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| allotrope |
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| one of two or more differnet molecular forms of an element in the same physical state |
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| alloy |
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| a misture composed of two or more elements, at least one of which is a metal |
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| amplitude |
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| the hight of a wave's crest |
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| anion |
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| any atom or group of atoms with a negative charge |
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| aqueous solution |
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| water that contains dissolved substances |
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| atomic emission spectrum |
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| 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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| atomic mass |
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| the weighted average of the masses of the isotopes of an element |
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| atomic mass unit |
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| a unit of mass equal to one-twelfth the mass of carbon-12 atom |
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| atomic number |
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| the number of protons in the nucleus of an atom of an element |
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| atomic orbital |
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| a mathematical expression describing the probability of finding an electron at various locations |
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| atomic radius |
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| one-half the distance between the nuclei of two atoms of the same element when the atoms are joined |
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| aufbau principle |
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| the rule that electrons occupy the orbitals of lowest energy first |
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| avagadro's number |
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| the number representative particles contained in one mole of a substance |
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| balanced equation |
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| a chemical equation in which mass is conserved |
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| base |
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| a compound that produces hydroxide ions in solution |
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| binary compound |
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| a compound composed of two elements |
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| bioling point elevation |
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| the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent |
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| bonding orbital |
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| a molecular orbital that can be occupied by two electrons of covalent bond |
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| boyle's law |
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| for a given mass of gas at constant temp, the volume of the gas varies inversely with pressure |
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| brownian motion |
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| the chaotic movement of colloidal particles, caused by collision with particles of the solvent in which they are dispersed |
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| calorie |
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| the quantity of heat needed to raise the temperature of 1 g fo pure water |
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| calorimeter |
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| an insulated device used to measure the absorption or release of heat in chemical or physical processes |
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| calorimetry |
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| the precise measurement of heat flow out of a system for chemical and physical processes |
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| catalyst |
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| a substance that increases the rate of reaction by lowering the activation-energy barrier |
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| cathode ray |
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| a stream of electrons produced at the negative electrode of a tube containing a gas at low pressure |
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| cation |
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| any atom or group of atoms with a positve charge |
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| charle's 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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| chemical equation |
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| an expression representing a chemical reaction |
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| chemical formula |
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| an expression that indicates the number and type of atoms present in the smallest representative unit of substance |
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| coefficients |
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| a small whole number that appears in front of a formula in a balanced chemical equation |
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| colligative properties |
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| a property of a solution that depends only upon the number of solute particles, and not upon their identities |
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| combined gas law |
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| the law that describes the relationship among the pressure, temperature, and volume of an enclosed gas |
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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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| complete ionic equation |
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| an equation that shows dissolved ionic compounds as dissociated free ions |
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| composition |
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| compressibility |
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| a measure of how much the volume of matter decreases under pressure |
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| concentrated solution |
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| a solution containing a large amount of solute |
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| concentration |
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| a measurement of the amount of solute that is dissolved in a given quantity of solvent |
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| conversion factor |
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| a ratio of equivalent measurements used to convert a quantity from one unit to another |
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| coordinate covalent bond |
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| a covalent bond in which one atom contributes both bonding electrons |
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| coordination number |
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| the number of ions of oppisite charge that surround each ion in a crystal |
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| covalent bond |
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| a bond formed by the sharing of electrons between atoms |
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| decomposition |
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| a chemical change in which a single compound is broken down into two or more simpler products |
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| diatomic molecule |
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| a molecule consisting of two atoms |
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| diffusion |
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| the tendancy of molecules to move toward areas of lower concentration until the concentration is uniform throughout |
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| dilute solution |
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| a solution that contains a small amount of solute |
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| dimensional analysis |
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| a technique of problem-solving that uses the units that are part of a measurement to help solve the problem |
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| dipole |
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| a molecule that has two poles, or regions with opposite charges |
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| dispersion force |
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| 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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| distillation |
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| 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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| double covalent bond |
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| a bond in which two atoms share two pairs of electrons |
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| double displacement |
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| a chemical change that involves an exchange of positive ions between tow compuonds |
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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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| electrolyte |
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| a compound that conducts an electric current when it is in a an aqueous solution or in the molten state |
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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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| electron dot diagram |
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| a notation that depicts valence electrons as dots areound the atomic symbol of the element |
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| electronegativity |
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| the ability of an atom to attract electrons when the atom is 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 |
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| endothermic process |
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| a process that absorbs heat from the surroundings |
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| energy levels |
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| the specific energies an electron in an atom or other system can have |
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| enthalpy |
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| the heat content of a system at constant pressure |
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| error |
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| the difference between the accepted value and the experimental value |
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| excess reactant |
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| a reactant present in a quantity that is more than sufficent to react with a limiting reactant |
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| exothermic process |
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| a process that releases heat to its surroundings |
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| experimental value |
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| a quantitative value measured during an experiment |
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| extensive property |
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| a property that depends on the amount of matter in a sample |
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| filtration |
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| a process that separates a solid from the liquid in a heterogeneous mixture |
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| formula unit |
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| the lowest whole number ratio of ions in an ionic compound |
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| freezing point depression |
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| the difference in temperature between the freezing point of a solution and the freeaing point of the pure solvent |
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| frequency |
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| the number of wave cycles that pass a given point per unit of time |
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| Gay-Lussac's Law |
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| the pressure of a gas is directly proportional to the kelvin temperature if the volume is constant |
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| ground state |
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| the lowest possible energy of an electron described by quantum mechanics |
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| heat |
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| energy that transfers from one object to another because of a temperature diffeence between teh objects |
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| heisenberg uncertainty |
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| it is impossible to know exactly both the velocity and the positio of a particle at the same time |
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| Hund's Rule |
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| 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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| hydrate |
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| a compound that has a specific number of water molecules bound to each formula unit |
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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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| hydrogen bonds |
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| 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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| intensive property |
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| a property that depends on the type of matter in a sample, not the amount of matter |
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| intensive property |
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| a property that depends on the type of matter in a sample, not the amount of matter |
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| ion |
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| an atom or group of atoms that has a positive or negative charge |
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| ionic bond |
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| the electrostatic attraction that binds oppositely charged ions together |
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| ionization energy |
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| the energy required to remove an electron from an atom in its gaseous state |
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| isotope |
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| 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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| joule |
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| the SI unit of energy |
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| law of conservation of energy |
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| in any chemical or physical process, energy is neither created nor destroyed |
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| law of definite proportions |
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| in samples of any chemical compound,the masses of elements are always in the same proportion |
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| law of conservation of mass |
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| in any physical change or chemical reaction, mass is conserved |
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| law of multiple proportions |
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| whenever two elements form more than one compound |
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| limiting reactant |
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| any reactant that is used up first in a chemical reaction |
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| mass number |
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| the total number of the amount of matter that an object contains |
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| melting point |
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| the temperature at which a substance changes from a solid to a liquid |
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| metallic bond |
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| the force of attractino that holds metals together |
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| molality |
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| 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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| molar mass |
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| a term used to refer to the massof a mole of any substance |
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| molar volume |
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| the volume occupied by 1 mole of a gas at standard temperature and pressure |
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| molarity |
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| the concentration of solute in a solution expressed as the numberof moles of solute dissolved in 1 liter of solution |
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| mole |
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| the amount of a substance that contains 6.o2x1023 representative particles of that substance |
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| molecule |
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| a neutral group of atoms joined together by covalent bonds |
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| monatomic ion |
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| 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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| net ionic equation |
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| an equation for a reaction in solution showing only those particles that are directly involved in the chemical change |
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| nonpolar covalent bond |
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| a covalent bond in which the electrons are shared equally by two atoms |
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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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| pascal |
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| the SI unit of pressure |
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| Paulie exclusion principle |
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| an atomic orbital may describe at most two electrons, each with opposite spin direction |
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| percent composition |
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| the percent by mass of each element in a compound |
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| percent error |
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| the percent that a measured value differs from the accepted value |
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| percent yeild |
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| the ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage |
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| periodic law |
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| 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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| phase |
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| any part of a sample with uniform composition and properties |
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| photon |
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| a quantum of light |
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| pi bond |
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| 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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| polar bond |
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| a covalent bond between atomsin which the electrons are shared unequally |
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| polar molecule |
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| a molecule in which one side of the molcule is slightly negative and the opposite side is slightly positive |
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| polyatomic ion |
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| a tightly bound group of atoms that behaves as unit and has a positive or negative change |
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| precipitate |
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| a solid that forms and settles out of a liquid mixture |
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| product |
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| a substance produced in a chemical reaction |
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| quantum |
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| the amount of energy needed to move an electron from one energy level to another |
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| quantum mechanical model |
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| the modern description, primarily mathematical, of the behavior of electrons in atoms |
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| reactant |
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| a substance present at the start of a reaction |
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| representative particle |
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| 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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| saturated solution |
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| a solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure |
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| sigma bond |
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| 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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| significant digits |
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| all the digits that can be known precisely in a measurement, plus a last estimated digit |
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| single covalent bond |
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| a bond formed when two atoms share a pair of electrons |
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| single displacement reaction |
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| a chemical change in which one element replaces a second element in a compound |
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| skeletal equation |
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| a chemical equation that does not indicate the relative amounts of reactants and products |
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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 |
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| solute |
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| dissolved particles in a solution |
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| solution |
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| a homogeneous mixture |
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| solvent |
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| the dissolving medium in a solution |
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| specific heat |
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| the amount of heat needed to increase the temperature of 1 g of a substance 1 C |
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| spectator ion |
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| an ion that is not directly involved in a chemical reaction |
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| spectrum |
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| wavelengths of visible light that are separated when a beam of light passes through a prism |
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| standard temperature and pressure |
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| the conditions under which the volume of a gas is usually measured |
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| stoichiometry |
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| that portion of chemistry dealing with numerical relationships in chemical reactions |
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| structural formula |
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| a chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion |
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| supersaturated solution |
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| a solution that contains more solute than it can theoretically hold at a given temperature |
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| surface tension |
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| an inward force that tends to minimize the surface area of a liquid |
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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 |
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| triple covalent bond |
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| a covalent bond in which three pairs of electrons are shared by two atoms |
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| Tyndall effect |
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| scattering of light by particles in a colloid or suspension, which causes a beam of light to become visible |
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| unsaturated solution |
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| a solution that contains less solute than a saturated solution at a given temperature and pressure |
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| valence electron |
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| an electron in the highest occupied energy level of an atom |
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| van der waals force |
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| the two weakest intermolecular attractions--dispersion interactions and dipole forces |
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| vapor |
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| describes the gaseous state of a substance that is generally a liquid or solid at room temperature |
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| vapor pressure |
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| a measure of the force exerted by a gas above a liquid in a sealed container |
