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| Anything that takes up space and has mass. |
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| Any substance that cannot be broken down into another substance by chemical reactions. |
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| A substance consisting of two or more different elements combined in a fixed ratio. |
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| An element indispensable for life, but required in extremely minute amounts. |
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| The smallest unit of matter that still retains the properties of an element. |
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| A subatomic particle having no electrical charge (electrically neutral), with a mass of about 1.7X10-24 g, found in the nucleus of an atom |
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| A subatomic particle with a single positive electrical charge, with a mass of about 1.7X10-24g found in the nucleus of an atom. |
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| A subatomic particle with a single negative charge and a mass about 1/2,000 that of a neutron or proton. One or more move around the nucleus of an atom. |
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| An atom's dense central core, containing protons and neutrons. |
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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 number of protons in the nucleus of an atom, unique for each element and designated by a subscript to the left of the elemental symbol. |
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| The sum of the number of protons and neurons in an atom's nucleus. |
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| The total mass of an atom, which is the mass in grams of 1 mole of the atom. |
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| One of several atomic forms of an element, each with the same number of protons but a different number of neutrons, thu differing in atomic mass. |
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| An isotope that is unstable; the nucleus decays spontaneously, giving of detectable particles and energy. |
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| The capacity to cause change, especially to do work. |
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| The energy that matter possesses as a result of its location or spatial arrangement. |
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| An energy level of electrons at a characteristic average distance from the nucleus of an atom. |
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| An electron in the outermost electron shell. |
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| The outermost energy shell of an atom, containing the valence electrons involved in the chemical reactions of that atom. |
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| The three-dimensional space where the electron in found 90% of the time. |
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| An attraction between two atoms, resulting from a sharing of outer-shell electrons or the presence of opposite charges on the atoms. The bonded atoms gain complete outer electron shells. |
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| A type of strong chemical bond in which two atoms share one or more pairs of valence electrons. |
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| A single covalent bond; the sharing of a pair of valence electrons by two atoms. |
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| A type of molecular notation in which the constituent atoms are joined by lines representing covalent bonds. |
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| A type of molecular notation representing the quantity of constituent atoms, but not the nature of the bonds that join them. |
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| A double covalent bond; the sharing of two pairs of valence electrons by two atoms. |
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| The bonding capacity of a given atom; usually the number of unpaired electrons required to complete the atom's outermost (valence) shell. |
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| The attraction of a given atom for the electrons of a covalent bond. |
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| A type of covalent bond in which electrons are shared equally between two atoms of similar electronegativity. |
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| A covalent bond between atoms that differ in electronegativity. The shared electrons are pulled closer to the more electronegative atom, making it slightly negative and the other atom slightly positive. |
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| An atom or group of atoms that has gained or lost one or more electrons, thus acquiring a charge. |
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| A positively charged ion. |
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| A negatively charged ion. |
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| A chemical bond resulting from the attraction between oppositely charged ions. |
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| A compound resulting from the formation of an ionic bond. |
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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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| Van der Waals Interactions |
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Definition
| Weak attractions between molecules or parts of molecules that result from localized charge fluctuations. |
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| The making and breaking of chemical bonds, leading to changes in the composition of matter. |
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| A starting material in a chemical reaction. |
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| A material resulting from a chemical reaction. |
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| In a chemical reaction, the state in which the rate of the forward reaction equals the rate of the reverse reaction, so that the relative concentrations of the reactants and products do not change with time. |
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| A molecule (such as water) with opposite charges on different ends of the molecule. |
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| The binding together of like molecules, often by hydrogen bonds. |
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| The attraction between different kinds of molecules. |
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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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| The energy associated with the relative motion of objects. Moving matter can perform work by imparting motion to other matter. |
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| The total amount of kinetic energy due to the random motions 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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| A measure of the intensity of heat in degrees, reflecting the average kinetic energy of the molecules. |
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| A temperature scale equal to 5/9(F-32) that measures the freezing point of water at 0 degrees and the boiling point at 100 degrees. |
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| The amount of energy required to raise one gram of water one degree Celsius. |
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| Calorie (with a capital C) |
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| used to indicate the energy content of food (is a kilocalorie) |
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| A unit of energy; 1 J=.239 cal; 1 cal=4.184 J. |
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| The amount of heat that must be absorbed or lost for 1 gram of a substance to change its temperature by 1 degree. |
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| The quantity of heat a liquid must absorbed for 1 gram of it to be converted from the liquid to the gaseous state. |
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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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| A liquid that is homogeneous mixture of two or more substances. |
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| The dissolving agent of a solution. Water is the most versatile solution known. |
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| A substance that is dissolved in a solution. |
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| A solution in which water is the solvent. |
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| The sphere of water molecules around a dissolved ion. |
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| Having an affinity for water. |
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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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| Having an aversion to water; tending to coalesce and form droplets in water. |
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| The sum of the masses of all the atoms in a molecule; sometimes called molecular weight. |
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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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| A common measure of solute concentration, referring to the number of moles of solute per liter of solution. |
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| A single proton with a charge of 1+. The dissociation of a water molecule (H(sub)2(/sub)O) leads to the generation of a hydroxide ion (OH(sup)-(/sup)) and a hydrogen ion (H(sup)+(/sup)). |
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Definition
| A water molecule that has lost a proton; OH(sup)-(/sup). |
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| A water molecule that has an extra proton bound to it; H(sub)2(/sub)O(sup)+(/sup)/ |
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