Final – Chemistry Answers – Flashcards
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| Binary Compounds |
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| a chemical compound composed of only two elements |
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| Diatomic Gases |
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| elements that are present in the gaseous state as molecules composed of two atoms (O2, N2, Cl2, H2, F2, I2, Br2) |
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| Polyatomic Ions |
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| a charged ion composed of two or more atoms covalently bonded |
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| Oxidation Number |
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| a number assigned to an element in chemical combination that represents the number of electrons lost |
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| Hydrate |
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| a compound, typically a crystalline one, in which water molecules are chemically bonded to another compound or an element (a solid with water in it) |
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| Anhydrous |
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| containing no water |
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| Mole Mass |
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| a number equal to the sum of the atomic masses of the atoms in a molecule |
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| Molecules |
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| a group of atoms bonded together, representing the smallest fundamental unit of a chemical compound that can take part in a chemical reaction |
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| Empirical Formulas |
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| a formula giving the proportions of the elements present in a compound but not the actual numbers or arrangement of atoms |
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| Conservation of Mass |
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| a principle stating that mass cannot be created or destroyed |
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| Chemical Equations (States) |
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| aq - dissolved in water l - liquid s - solid g - gas |
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| Reactants |
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| a substance that takes part in and undergoes change during a reaction |
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| Product |
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| a substance that is formed as the result of a chemical reaction |
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| Catalyst |
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| a substance that increases the rate of a chemical reaction without itself undergoing any permanent chemical change |
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| Endothermic |
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| energy taken in, feels cold to the touch |
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| Exothermic |
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| energy given off, feels warm to the touch |
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| Coefficients |
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| a number placed in front of a molecule in a chemical equation representing the number of atoms needed |
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| Subscripts |
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| a number placed after an atom in a molecule in a chemical equation stating the number of atoms needed to stabalize the charge |
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| Test for Hydrogen |
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| light a splint of wood stick it in gas if you hear a pop then there is hydrogen |
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| Test for Oxygen |
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| light a splint of wood blow it out stick it in gas if relights then there is oxygen |
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| Limiting Reactant |
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| the reactant that is used up; once it is all used, the reaction stops |
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| Excess Reactant |
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| the reactant that is not used up |
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| Absolue 0 |
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| the temperature at which there is no molecular motion |
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| Air Pressure |
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| caused by the number of collisions of gas molecules -standard pressure = 1 atmosphere = 760mmHg = 760torr = 101.3 Kpa |
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| Altitude |
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| air pressure decreases with altitude |
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| Barometer |
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| measures air pressure |
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| Temperature |
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| measure of average kinetic energy of particles |
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| Changes of State (6) |
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| Melting Sublimation Vaporization Freezing Deposition Condensation |
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| Melting |
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| solid to liquid (endothermic) |
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| Sublimation |
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| solid to gas (endothermic) |
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| Vaporization |
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| liquid to gas (endothermic) |
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| Freezing |
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| liquid to solid (exothermic) |
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| Deposition |
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| gas to solid (exothermic) |
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| Condensation |
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| gas to liquid (exothermic) |
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| Volatile |
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| becomes gas easliy |
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| Boyles Law |
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| when pressure goes up, volume goes down, inversly related (P1V1=P2V2) |
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| Charles' Law |
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| when temp goes up volume goes up, directly related (V1/T1=V2/T2) |
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| Ideal Gas Law |
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| PV=nRT n = # moles R = ideal gas law constant |
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| Combustion of a Hydrocarbon |
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| the combustion of any hydrocarbon always produces the same products: CO2 and H2O (carbon dioxide and water) |
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| Melting Point |
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| of water is 0*C |
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| Freezing Point |
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| of water is 0*C (melting point = freezing point) |
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| Boiling Point |
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| of water is 100*C |
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| Precipitate |
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| when a solid settles out of a solution (the solid is the precipitate) |
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| Precent Yield |
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| find the amount of product theoretically possible by using the given amount of limiting reactant and stoichiometry divide the amount of product actually produced in the chemical reaction by the amount of product theoretically possible Multiply by 100 to make a percent (ideally close to 100) |
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| Molecular Mass |
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| the mass of a molecule |
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| Diffusion |
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| gas spreading out |
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| Effusion |
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| gas leaking out of opening |
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| Graham's Law |
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| the mathematical expression of the relationship between mass of particles and rate of diffusion/effusion |
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| Amorphous |
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| random arrangement, melts over a range of temperatures; examples --> glass and wax |
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| Crystalline |
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| geometric patterns, definite melting point; examples --> sale and water |
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| Mole |
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| contains Avogadro's number of atoms |
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| Distilled Water |
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| water that has been purified (chemically pure) |
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| Activation Energy |
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| energy needed to start a reaction (match for the bunsen burner) |
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| Avogadro's Number |
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| 6.02 x 10^23 |
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| Kelvin |
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| standard temperature is 273 Kelvin (0*C) |
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| Polyatomic Ion |
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| used in compounds just like monatomic ions (Mg2 or N --> one atom), use parenthesis around the polyatomic ion only if more than one is needed, most are negative and end in 'ite' or 'ate' |
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| STP |
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| means standard pressure and temperature, which is 1 atmosphere and 273 Kelvin |
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| Standard Molar Volume of Gas |
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| 1 mole of any gas at STP has the same volume as 22.4Liters |
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| Gay-Lussac's Law |
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| when temp goes up pressure goes up (directly related) P1/T1=P2/T2 |
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| Combined Gas Law |
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| P1V1/T1 = P2V2/T2 (always use Kelvin) |
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| Ideal Gas |
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| at 0 Kelvin would have no volume |
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| Stoichiometry |
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| 1st write balanced chemical equation 2nd the given amount, must be converted to moles 3rd use the mole ratio to change given moles into moles of what you are trying to find 4th convert these moles into grams if needed |
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| Molarity |
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| (M) moles solute/ L solution |
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| Molality |
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| (m) moles solute/ kg solvent |
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| Saturated |
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| no more solute may be dissolved in a solvent |
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| Unsaturated |
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| being able to dissolve more solute in a solvent |
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| Supersaturated |
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| a solution that contains a higher than saturation concentration of solute |
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| Ionization |
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| a state of an atom that has had at least one electron removed |
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| Dissociation |
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| when a substance is placed in water, the water molecules pull the other molecules apart |
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| Indicators |
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| a substance that indicates the degree of acidity or basicity of a solution through color change (litmus paper, pH paper) |
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| pH |
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| measure of hydrogen ion concentration |
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| Net Ionic Equation |
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| involves everything in the equation but the spectator ions |
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| Spectator Ions |
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| an ion that exists in the same form on both the reactant and product sides of the equation |
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| Titration |
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| an acid or base solution of known concentration is mixed with and acid or base solution of unknown concentration |
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| Neutralization |
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| reaction between an acid and base which produces a neutral solution (pH 7) |
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| Hydrocarbons |
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| made of hydrogen and carbon ending in 'ane' means only single bonds present prefix tells number of carbons meth, eth, prop, but, pent, hex, hept, oct, non, dec -alkanes are saturated (full of hydrogen) |
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| Benzene Ring |
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| a cyclopentene with 3 double bonds |
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| H2SO4 |
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| sulfuric acid |
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| HCl |
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| hydrochloric acid |
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| NO |
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| nitric acid |
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| AlPO4 |
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| aluminum phosphate |
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| FeSO4 |
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| iron (II) sulfate |
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| BeF2 |
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| beryllium fluoride |
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| Strontium Nitrate |
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| Sr(NO3)4 |
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| Rubidium Sulfide |
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| Rb2S |
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| Cobalt (II) Sulfate |
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| CoSO4 |
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| Carbonic Acid |
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| H2CO3 |
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| Nitrogen (IV) Oxide |
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| NO2 |
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| 5 Types of chemical reactions |
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| synthesis decomposition double displacement single displacement combustion |
