2nd Semester Test – Flashcards
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| Monatomic ions |
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| consist of a single atom with a positive or negative charge resulting from the loss or gain of one or more valence Electrons |
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| acid |
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| a compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) when dissolved in water |
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| activity series |
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| lists the metals in order of decreasing reactivity |
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| actual yield |
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| the amount of product that actually forms when when the reaction is carried out in lab |
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| allotropes |
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| two or more different molecular forms of the same element in the same physical state |
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| amorphous solid |
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| lacks an ordered internal structure |
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| atmospheric pressure |
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| results from the collisions of atoms and molecules in air with objects |
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| avogadro's hypothesis |
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| states that equal volumes of gasses at the the same temperature and pressure contain equal numbers of particles |
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| balanced equation |
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| in which each side of the equation has the same number of atoms of each element and mass is conserved |
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| barometer |
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| a device that is used to measure atmospheric pressure |
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| base |
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| an ionic compound that produces hydroxide ions when dissolved in water |
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| binary compound |
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a compound composed of two elements; NaCl and Al2O3 are binary compounds |
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| boiling point (bp) |
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| the temperature at which the vapor pressure of the liquid is just equal to the external pressure on the liquid |
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| catalyst |
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| a substance that speeds up the reaction but is not used up in the reaction |
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| chemical equation |
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| a representation of a chemical reaction; the formulas of the reactants(on the left) are connected by an arrow with the formulas of the products (on the right |
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| coefficents |
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| small whole umbers that are placed in front of the formulas in an equation in order to balance it |
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| combination reaction |
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a chemical change in which two or more substances react to form a single new substance example: 2Mg(s) + 02(g) ------> 2MgO(s) |
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| combustion reaciton |
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| a chemical change in which an element or a compound reacts with oxygen,often producing energy in the form of heat and light |
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| complete ionic equation |
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| an equation that shows dissolved ionic compounds as dissociated free ions |
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| decomposition reaction |
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| a chemical change in which a single compound breaks down into two or more simpler products |
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| double replacement reaction |
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| a chemical change involving exchange of positive ions between two compounds |
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| empirical formula |
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| gives the lowest whole-number ratio of the atoms of the elements in a compound |
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| evaporation |
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| a conversion that occurs at the surface of a liquid that is not boiling |
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| excess reagent |
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| the reactant that is not completely used up in a reaction |
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| gas pressure |
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| results from a force exerted by a gas per unit surface area of an object |
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| glass |
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| a rigid state without crystallizing |
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| kinetic energy |
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| the energy an object has because of its motion |
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| law of definite proportions |
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| states that in samples of any chemical compound, the masses of the elements are always in the same proportions |
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| law of multiple proportions |
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| whenever the same two elements form more than one compound the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers |
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| limiting reagent |
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| the reagent that determines the amount of product that can be formed by a reaction |
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| melting point (mp) |
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| the temperature at which a solid changes into a liquid |
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| molar mass |
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| the mass of a mole of a element |
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| molar volume |
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| 22.4 L is molar volume of a gas |
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| mole |
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| is 6.02 X 10^23 representative particles of that substance and is the SI unit for measuring the amount of the substance |
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| mole ratio |
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| a conversion factor derived from the coefficients of a balanced chemical equation interpreted in terms of a mole |
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| net ionic equation |
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| an equation for a reaction in solution that shows only those particles that are directly involved in the chemical change |
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| normal boiling point |
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| defined as the boiling point of a liquid at pressure of 101.3 kPa |
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| pascal (Pa) |
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| the SI unit of pressure |
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| percent compositon |
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| the percent by mass of each element in the compound |
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| percent yield |
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the ratio of the actual yield to the theoretical yield expressed as a percent
formula: percent yield = actual yield/ theoretical yield X 100 |
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| polyatomic ions |
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composed of more than one atom
a tightly bound group of atoms that behaves as a unit and has a positive or negative charge
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| representative particle |
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| refers to the species present in a substance: usually atoms, molecules or formula units |
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| single replacement reaction |
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| a chemical change in which one element replaces a second element in a compound |
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| skeleton equation |
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| a chemical equation that does not indicate the relative amounts of the reactants and products |
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| spectator ion |
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| an ion that appears on both sides of an equation and is not directly involved int he reaction |
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| standard atmosphere (atm) |
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| the pressure required to support 760 mm of mercury in a mercury barometer at 25 degrees Celcius |
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| standard temp and pressure (STP) |
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temp: 0 degrees Celsius Pressure: 101.3 kPa or 1 atm |
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| stoichiometry |
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| the calculations of quantities in chemical reactions |
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| sublimation |
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| the change of a substance from a solid to a vapor without passing through the liquid state |
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| theoretical yield |
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| the maximum amount of product that could be formed from give amounts of reactant |
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| unit cell |
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| the smallest group of particles within a crystal that retains the geometric shape of the crystal |
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| vacuum |
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| an empty space with no particles and no pressure |
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| vapor pressure |
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| a measure of the force exerted by a gas above a liquid |
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| vaporization |
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| the conversion of a liquid to gas or vapor |
