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| thermal energy that is transferred from an object at higher temperature to one at lower temperature. |
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| a measurement of thermal energy present in an object or substance, reflecting how much the constituent molecules are moving. |
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| the kinetic energy of molecular motion |
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| the energy of motion. Compare with potential energy. |
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| energy stored in matter as a result of its position or molecular arrangement. Compare with kinetic energy. |
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| the energy of motion. Compare with potential energy. |
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| energy stored in matter as a result of its position or molecular arrangement. Compare with kinetic energy. |
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| the capacity to do work or to supply heat. May be stored (potential energy) or available in the form of motion (kinetic energy) |
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| referring to a chemical reaction that releases heat. Compare with endothermic. |
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| referring to a chemical reaction that absorbs heat. Compare with exothermic. |
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| a dynamic but stable state of a reversible chemical reaction in which the forward reaction and reverse reactions proceed at the same rate, so that the concentrations of the reactants and products remain constant. |
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| any of the final materials formed in a chemical reaction. |
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| any of the starting materials in a chemical reaction. |
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| (adj. homeostatic) the array of relatively stable chemical and physical conditions in an animal's cells, tissues, and organs. May be achieved by the body's passably matching the conditions of a stable external environment (conformational homeostasis) or by active physiological process (regulatory homeostasis) triggered by variations in the external or internal environment. |
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| a substance that, in solution, acts to minimize changes in the pH of that solution when aid or base is added. |
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| a measure of the concentration of protons in a solution and thus of acidity or alkalinity. Defined as the negative or the base- 10 logarithm of the proton concentration: pH= -log[H+]. |
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| any compound that a quires protons or gives up electrons during a chemical reaction or accepts hydrogen ions when dissolved in water. |
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| any compound that gives up protons or accepts electrons during a chemical reaction or that releases hydrogen ions when dissolved in water. |
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| (OH-) an oxygen atom and a hydrogen atom joined by a singe covalent bond and carrying a negative charge: formed by dissociation of water |
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| (H+) a single proton with a charge of 1+: typically, one that is dissolved in solution or that is being transferred from one atom to another in a chemical reaction |
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| the energy required to vaporize 1 gram of a liquid into a gas |
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| the amount of energy required t raise the temperature of 1 gram of a substance by 1 degree C; a measure of the capacity of a substance to absorb energy. |
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| the cohesive force that causes molecules at the surface of a liquid to stick together, thereby resisting deformation of the liquid's surface and minimizing its surface area. |
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| the tendency of certain dissimilar molecules to cling together due to attractive forces. compare with cohesion. |
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| the tendency of certain like molecules (e.g. water molecules) to cling together due to attractive forces. Compare with adhesion. |
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| not interacting readily with water. Hydrophobic compounds are typically non polar compounds that lack charged or electronegative atoms and often contain many C-C and C-H bonds. Compare with hydrophilic |
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| interacting readily with water. hydrophilic compounds are typically polar compounds containing charged electronegative atoms. com are with hydrophobic. |
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| a weak interaction between two molecules or different parts of the same molecule resulting from the attraction between a hydrogen atom with a partial positive charge and another atom (usually O or N) with a partial negative charge. |
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| any substance that is dissolved in a liquid. |
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| any liquid in which one or more solids or gases can dissolve |
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| a common unit of solute concentration equal to the number of moles of a dissolved solute in 1 liter of solution. |
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| a liquid containing one or more dissolved solids or gases in a homogeneous mixture |
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| the sum of the mass numbers of all of the atoms in a molecule; roughly, the total number of protons and neutrons in the molecule. |
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| the amount of a substance that contains 6.022 X 10^23 of its elemental entities (e.g. atoms, ions, or molecules). This number of molecules of a compound will have a mass equal to the molecular weight of that compound expressed in grams. |
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| any process in which one compound or element is combined with others or is broken down; involves the making and/or breaking of chemical bonds. |
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| a representation of a molecule where atoms are shown as balls-- color-coded and scaled to indicate that atom's identify-- attached to each other in the correct geometry. |
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| a representation of a molecule where atoms are shown as balls--colored and scaled to indicate the atom's identity-- and covalent bonds are shown as rods or sticks connecting the balls in the correct geometry |
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| a two-dimensional notation in which the chemical symbols for the constituent atoms are joined by straight lines representing single (-) double (=) and triple covalent bonds. |
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| a notation that indicates only the numbers and types of atoms in a molecule, such as H2O for the water molecule. |
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| a negatively charged ion. |
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| an atom or a molecule that has lost or gained electrons and thus carries an electric charge, either positive or negative, respectively. |
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| a chemical bond that is formed when an electron is completely transferred from one atom to another so that the atoms remain associated due to their opposite electric charges. |
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| a covalent bond in which electrons are shared unequally between atoms differing in electronegativity, resulting in the more electronegative atom having a partial negative charge and the other atom, a partial positive charge. |
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| a covalent bond in which electrons are equally shared between the two atoms of the same or similar electronegativity. |
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| a measure of the ability of an atom to attract electrons toward itself from an atom to which it is bonded. |
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| a combination of two or more atoms held together by covalent bonds |
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| a type of chemical bond in which two atoms share one or more pairs of electrons. |
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| an attractive force binding two atoms together. covalent bonds, ionic bonds, and hydrogen bonds are types of chemical bonds. |
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| the number of unpaired electrons in the outermost electron shell of an atom; determines how many covalent bonds the atom can form. |
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| an attractive force binding two atoms together. covalent bonds, ionic bonds, and hydrogen bonds are types of chemical bonds. |
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| the number of unpaired electrons in the outermost electron shell of an atom; determines how many covalent bonds the atom can form. |
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| an electron in the outermost electron shell, the valence shell, of an atom. Valence electrons tend to be involved in chemical bonding. |
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| a group of orbitals of electrons with similar energies. electron shells are arranged in roughly concentric layers around the nucleus of an atom, with electrons in outer shells having more energy than those in inner shells. Electrons in the outermost shell, the valence shell, often are involved in chemical bonding. |
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| the spherical region around an atomic nucleus in which an electron is present most of that time |
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| a unit of mass equal to 1/12 the mass of one carbon-12 atom;about the mass of 1 proton or 1 neutron. |
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| any of several forms of an element that have the same number of protons bud differ in the number of neutrons |
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| a total number of protons and neutrons in an atom |
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| the number of protons in the nucleus of an atom, giving the atom its identity as a particular chemical element. |
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| a substance, consisting of atoms with a specific number of protons, that cannot be separated into or broken down to any other substance. Elements preserve their identity in chemical reactions. |
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| the theory that simple chemical compounds in the ancient atmosphere and ocean combined via spontaneous chemical reactions to form larger, more complex substances, eventually leading to the origin of life and the start of biological evolution |
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