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| A substance that increases the hydrogen ion concentration of a solution. |
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| Rain, snow, or fog that is more acidic than pH 5.2. |
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| The attraction between different kinds of molecules. |
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| A solution in which water is the solvent. |
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| A substance that reduces the hydrogen ion concentration of a solution. |
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| A substance that consists of acid and base forms in a solution and that minimizes changes in pH when extraneous acids or bases are added to the solution. |
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| The amount of heat energy required to raise the temperature of 1 g of water by 1°C; also the amount of heat energy that 1 g of water releases when it cools by 1°C. The Calorie (with a capital C), usually used to indicate the energy content of food, is a kilocalorie. |
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| A temperature scale (°C) equal to 5/9(°F – 32) that measures the freezing point of water at 0°C and the boiling point of water at 100°C. |
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| The binding together of like molecules, often by hydrogen bonds. |
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| A mixture made up of a liquid and particles that (because of their large size) remain suspended rather than dissolved in that liquid. |
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| A measure of mass for atoms and subatomic particles; the same as the atomic mass unit, or amu. |
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| The attraction of a given atom for the electrons of a covalent bond. |
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| New properties that arise with each step upward in the hierarchy of life, owing to the arrangement and interactions of parts as complexity increases. |
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| The process by which a liquid changes to a gas. |
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| The process in which the surface of an object becomes cooler during evaporation, owing to a change of the molecules with the greatest kinetic energy from the liquid to the gaseous state. |
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| The total amount of kinetic energy due to the random motion of atoms or molecules in a body of matter; also called thermal energy. Heat is energy in its most random form. |
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| The quantity of heat a liquid must absorb for 1 g of it to be converted from the liquid to the gaseous state. |
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| The sphere of water molecules around a dissolved ion. |
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| A type of weak chemical bond that is formed when the slightly positive hydrogen atom of a polar covalent bond in one molecule is attracted to the slightly negative atom of a polar covalent bond in another molecule. |
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| A single proton with a charge of 1+. The dissociation of a water molecule (H2O) leads to the generation of a hydroxide ion (OH–) and a hydrogen ion (H+). |
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| A water molecule that has an extra proton bound to it; H3O+. |
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| Having an affinity for water. |
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| Having an aversion to water; tending to coalesce and form droplets in water. |
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| A water molecule that has lost a proton; OH–. |
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| A unit of energy: 1 J = 0.239 cal; 1 cal = 4.184 J. |
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| A thousand calories; the amount of heat energy required to raise the temperature of 1 kg of water by 1°C. |
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| The energy associated with the relative motion of objects. Moving matter can perform work by imparting motion to other matter. |
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| A common measure of solute concentration, referring to the number of moles of solute per liter of solution. |
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| The number of grams of a substance that equals its molecular weight in daltons and contains Avogadro’s number of molecules. |
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| The sum of the masses of all the atoms in a molecule; sometimes called molecular weight. |
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| A measure of hydrogen ion concentration equal to –log [H+] and ranging in value from 0 to 14. |
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| A molecule (such as water) with opposite charges on different ends of the molecule. |
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| A substance that is dissolved in a solution. |
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| A liquid that is a homogeneous mixture of two or more substances. |
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| The dissolving agent of a solution. Water is the most versatile solvent known. |
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| The amount of heat that must be absorbed or lost for 1 g of a substance to change its temperature by 1°C. |
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| One of several compounds that have the same molecular formula but differ in the covalent arrangements of their atoms. |
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| A measure of how difficult it is to stretch or break the surface of a liquid. Water has a high surface tension because of the hydrogen bonding of surface molecules. |
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| A measure of the intensity of heat in degrees, reflecting the average kinetic energy of the molecules. |
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