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Chem stone 2
Polyatomic Ions, Vocab for ch. 1-11, 20
| Question | Answer |
|---|---|
| Accuracy | The closeness of a measurement to the true value of the quantity that is being measured |
| Anion | An ion with a negative net charge |
| Cation | An ion with a positive net charge |
| Chemical Formula | An expression showing the chemical composition of a compound in terms f the symbols for the atoms of the elements involved |
| Chemical Properties | Any property of a substance that cannot be without converting the substance into some other substance |
| Chemistry | The science that studies the properties of substances and how substances react with one another |
| Compounds | Substances composed of two or more elements chemically united in fixed proportions |
| Empirical Formula | An expression using chemical symbols to show the types of elements in a substance and the simplest ratios of the different kinds of atoms |
| Energy | The capacity to do work or produce change |
| Extensive Property | A property that depends on how much matter is being considered |
| Hypothesis | A tentative explaination for a set of observations |
| Intensive Property | A property that does not depend on how much matter is being considered |
| Law | A concise verbal or mathematical statement of a relationship between phenomena that is always the same under the same conditions |
| Law of Conservation of Energy | The total quantity of energy in the universe is constant |
| Law of Conservation of Mass | Matter can be neither created nor destroyed |
| Limiting Reagent | The reactant used up first in a reaction |
| Matter | Anything that occupies space and possesses mass |
| Mole | The amount of substance that contains as many entities (atoms, molecules, or other particles) as there are exactly atoms in exactly 12 grams of the carbon-12 isotope |
| Molecular Formula | An expression showing the exact number of atoms of each element in a molecule |
| Molecule | An aggregate of at least two atoms helt together by special forces |
| I - | Iodide |
| Fl - | Fluoride |
| Br - | Bromide |
| MoO4 2- | Molybdate |
| MnO4 - | Permangante |
| WO4 - | Tungstate |
| Se 2- | Selenide |
| ClO4 - | Perchlorate |
| ClO3 - | Chlorate |
| ClO2 - | Chlorite |
| ClO - | Hypochlorite |
| Cl - | Chloride |
| CrO4 2- | Chromate |
| Cr2O7 2- | Dichrimate |
| CO3 2- | Carbonate |
| HCO3 - | Bicarbonate |
| C2H3O2 - | Acetate |
| C2O4 2- | Oxalate |
| CN - | Cyanide |
| SCN - | Thiocynate |
| O2 2- | Peroxide |
| O 2- | Oxide |
| OH - | Hydroxide |
| H - | Hydride |
| NO2 - | Nitrite |
| NO3 - | Nitrate |
| N 3- | Nitride |
| NH2 - | Amide |
| PO4 3- | Phosphate |
| HPO4 2- | Hydrogen Phosphate |
| H2PO4 - | Dihydrogen Phosphate |
| HSO3 - | Bisulfite |
| SO4 2- | Sulfate |
| SO3 2- | Sulfite |
| S2O3 2- | Thiosulfate |
| S4O6 2- | Tetrathionate |
| S 2- | Sulfide |
| HSO4 - | Bisulfate |
| Area of High Electron Density | Area of an atom or ion at which either a lone pair, single, double, or triple bond is located. |
| Atomic Mass | The mass of an atom in atomic mass units. |
| Atomic Number (Z) | The number of protons in the nucleus of an atom. |
| Atomic Radius | One-half the distance between the nuclei in two adjacent atoms of the same element in a metal. For elements that exist as diatomic units (e.g. oxygen), the atomic radius is one-half the distance between the nuclei of two atoms in a particular molecule. |
| Aufbau Principle | As protons are added one by one to the nucleus to build up the elements, electrons similarly are added to the atomic orbitals. |
| Coordinate Covalent Bond | A bond in which the pair of electrons is supplied by one of the two bonded atoms. |
| Covalent Bond | A bond in which two electrons are shared by two atoms. |
| Covalent Compounds | Compounds containing only covalent bonds. |
| Dipole-dipole Forces | Forces that act between polar molecules. |
| Dipole Moment | The product of charge and distance between the charges in a molecule. |
| Electron Affinity | The negative of the energy change that takes place when an electron is accepted by an atom (or an ion) in the gaseous state. |
| Electronegativity | The ability of an atom to attract electrons toward itself in a chemical bond. |
| Formal Charge | The electrical charge difference between the number of valence electrons in an isolated atom and the number of electrons assigned to that atom in a Lewis structure. |
| Hund's Rule | The most stable arrangement of electrons in atomic subshells is the one with the greatest number of parallel spins. |
| Hybrid Orbitals | Atomic orbitals obtained when two or more nonequivalent orbitals of the same atom combine before covalent bond formation. |
| Aldehydes | Compounds with a carbonyl functional group and the general formula RCH0,in which R is an H atom, an alkyl, or an aromatic hydrocarbon group. |
| Alcohol | An organic compound containing the hydroxyl group (- OH) |
| Alkanes | Hydrocarbons having the general formula CnH2n+2, in which n=1, 2... |
| Alkenes | Hydrocarbons containing one or more carbon-carbon double bonds. They hace the general formula CnH2n, in which n=2, 3,... |
| Alkynes | Hydrocarbons that contain one or more carbon-carbon triple bands. They have the general formula CnH2n-2, in whcih n=2, 3,... |
| Amines | Organic bases that have the functional group (-NR2), in which R may be H, an alkyl group, or an aromatic hydrocarbon group. |
| Aromatic hydrocarbon | A hydrocarbon that contains one or more benzene rings. |
| Bronsted base | A substance capable of accepting a proton in a reaction. |
| Carboxylic acids | Acids that contain the carboxyl group (-COOH). |
| Chelating agent | A substance that forms complex ions with metal ions in solution. |
| Chiral | Compounds or ions that are not superimposable with their mirror images. |
| Combination reaction | A reaction in which two or more substances combine to form a single product. |
| Concentration of a solution | The amount of solute present in a given quantity of solution. |
| Coordination number | In coordination compounds, it is defined as the number of donor atoms surrounding the central metal atom in a complex. |
| Decomposition reaction | The breakdown of a compound into two or more components. |
| Displacement reaction | A reaction in which an atom or an ion in a compound is replaced by an atom of another element. |
| Donor atom | The atom of a ligand that is bonded directly to the metal atom. |
| Electrolyte | A substance that, when dissolved in water, results in a solution that can conduct electricity. |
| End point | Occurs in a titration when the indicator changes color. |
| Enantiomers | Compounds and their nonsuperimposable mirror images. |
| Equivalenve point | The point at which an acid is completely reacted with or neutralized by a base. |
| Esters | Compounds that have the ceneral formula RCOOR', in which R can be H or an alkyl group or an aromatic hydrocarbon and R' is an alkyl group or an aromatic hydrocarbon. |
| Ether | An organic compound containint the R-O-R' linkage, in which R and R' are alkyl and/or aromatic hydrocarbons. |
| Geometric isomers | Compounds with the same type and number of atoms and the same chemical bonds but different spatial arrangements; such isomers cannot be interconverted without breaking a chemical bond. |
| Hydrocarbons | Compounds made up of only carbon and hydrogen. |
| Ionic equation | An equation that shows dissolved ionic compounds in terms of their free ions. |
| Ketones | Compounds with a carbonyl functional group and the general formula RR'CO, in which R and R' are alkyl and/or aromati c hydrocarbon groups. |
| Lewis acid | A substance that can accept a pair of electrons. |
| Lewis base | A substance that can donate a pair of electrons. |
| Ligand | A molecule or an ion that is bonded to the metal ion in a complex ion. |
| Metathesis reaction | A reaction that involves the exchange or parts between compounds. |
| Molarity | The number of moles of solute in one liter of solution. |
| Molecular equations | Equations in which the formulas of the compounds are written as though all species existed as molecules or whole units. |
| Net ionic equation | An equation that includes only the ionic species that actually take part in the reaction. |
| Spectator ions | Ions that are not involved in the overall reaction. |
| Nonelectrolytes | A substance that, when dissolved in water, gives a solution that is not electrically conducting. |
| Oxidation number | The number of charges an atom would have in a molecule if electrons were transferred completely in the direction indicated by the difference in electronegativity. |
| pH | The negative logarithm of the hydrogen ion concentration in a aqueous solution. |
| Polymer | A molecular compound distinguished by a high molar mass and made up of many repeating units. |
| Racemic mixture | An equimolar mixture of two enantioners. |
| Redox reaction | A reaction in which there is either a transfer of electrons or a change in the oxidation numbers of the substances taking part in the reaction. |
| Resonance | The use of two or more Lewis structures to represent a particular molecule. |
| Saturated hydrocarbon | Hydrocarbons that contain only single covalent bonds. |
| Solute | The substance present in the smaller amount in a solution. |
| Solvent | The substance present in larger amount in a solution. |
| Structural isomers | Molecules that have the same molecular formula but different structures. |
| Titration | The gradual addition of a solution of accurately known concentration to another solution of unknown concentration until the chemical reaction between the two solutions is complete. |
| Unsaturated hydrocarbons | A solution that contains less solute than it has the capacity to dissolve. |
| Heat | The thermal energy that can be transferred from an object at one temperature to an object at another temperature. |
| Energy | The capacity to do work or cause change. |
| Internal energy | The sum pf potential and kinetic energy of a system; the internal energy of a chemical system depends on 1) the number of particles, 2) the type of particles, and 3) the temperature. |
| Kinetic energy | Energy due to the motion of an object. |
| Potential energy | Energy stored in an object because of the relative positions or orientations of its components. |
| Endothermic | Any reaction or process that results in an addition of heat to the system; indicated by +q. |
| Exothermic | Any reaction or process that results in a loss of heat from the system; indicated by -q. |
| Thermodynamics | the science of heat (energy) transfer. |
| Thermal equilibrium | The system and the surroundings are equal in temperature; heat transfer occurs until thermal equilibrium is established. |
| System | The object under study; generally the reactants. |
| Surroundings | Everything outside the system. |
| Law of Conservation of Energy | Energy is conserved. q surroundings = -q system |
| Heat capacity (C) | The amount of heat required to raise the temperature of a given quantity of substance by one degree Celcius. |
| Specific heat capacity | calculated as [heat lost of gained by substance, J] / [mass, g] x [T change, K] |
| First law of thermodynamics | The change in energy is equal to the heat transferred plus the work done by the system. |
| Melting | The phase change from a solid to a liquid. |
| Freezing | The phase change from a liquid to a solid. |
| Deposition | The process in which vapor molecules are converted directly to the solid phase. |
| Sublimation | The process in which molecules go directly from the solid phase into the vapor phase. |
| Evaporation | The phase change from a liquid to a gas. |
| Condensation | The phase change from a gas to a liquid. |
| State function | The properties of a system that depend only on the state of the system. |
| Standard state temperature | 298.15 K |
| Standard state pressure | 1.0000 atm |
| Standard states matter | Any solid is a pure solid; any liquid is a pure liquid; and gas is at 1.00 atm of pressure. |
| Enthalpy | A thermodynamic quantity used to describe heat changes taking place at constant pressure. |
| Hess's law | When reactants are converted to products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps. |
| Thermochemical equation | An equation that shows both the mass and enthalpy relations. |
| Enthalpy of formation | The enthalpy for the reaction in which one mole of a substance is formed from its constituent elements. |
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