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| A property of materials that is related to the ease with which they flow. It is a qualitative observation but can be made quantitative |
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| The shape, size, flexibility, forces of attraction, etc. of the molecules determine |
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| How easily (or not easily) the liquid flows |
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| Force times distance divided by area times velocity |
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| The viscosity usually ________ with an ________ in temperature for liquids and soft solids |
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| The viscosity of gases usually _______ with ________ temperature |
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| If the volume of a mixture is equal to the sum of the volumes of the components mixed, it is said that the volumes are ______ for this mixture |
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| A form of thermal energy that flows spontaneously from an area of high temperature to an area of low temperature. |
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| Two objects that start out at different temperatures will reach _______ when brought into contact with one another because heat flows from the object with the higher temperature to the object with lower temperature |
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| Heat flow into a substance causes the temperature of that substance to rise unless a phase change (solid to liquid, etc) is occurring. The amount of heat required to raise one gram of a substance one degree C. |
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| The amount of heat required to raise the temperature of one gram of water by one degree C |
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| The amount of heat required to raise the temperature of one pound of water by one degree Fahrenheit |
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| The space inside a sealed, insulated container. No heat (or matter) goes into or out of the container |
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| Systems that allow energy to go into and out of them but no matter to go into or out of them |
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| Systems that allow both energy and matter to transfer into and out of them |
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| Gas molecules occupy negligible volume compared to the empty space between the molecules and the intermolecular forces of attraction and repulsion are insignificant. If molecules of liquid water move fast enough, they could break free from the attraction of other liquid water molecules and a gas molecule will form, as long as the temperature remains fixed, regardless of if the water is at its boiling point |
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| Force per unit area or the total force applied divided by the total surface area over which that force is applied |
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| The pressure required to support a column of mercury to a height of 760.0 mm |
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| P is the pressure exerted by the sample of gas measure in atmospheres, V is the volume of the sample in liters, T is the temperature in Kelvin, and n is the number of moles in the sample |
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| Maintaining constant temperature amount of moles in a sealed piston, the volume of the sample can be systematically varied. As pressure increases, volume decreases |
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| As Pressure increases, Temperature increases at constant volume and moles |
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| As Volume increases, Temperature increases at constant pressure and moles |
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| The sum of the partial pressures of the component gases in the mixture |
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| Dalton's law of partial pressures |
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| The sum of the partial volumes of the individual gases that would occupy at the same pressure and temperature |
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| The heat of vaporization of a liquid generally _______ as the temperature of vaporization _______ |
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| The amount of heat required to evaporate a certain amount of water |
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Definition
| Heat of vaporization of water |
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| The temperature at which its vapor pressure is equal to the pressure exerted on the liquid |
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Definition
| Boiling point of a liquid |
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| The temperature at which its vapor pressure is equal to 760 mm Hg |
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Definition
| Normal Boiling point of a liquid |
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Term
| Liquids can be heated to a temperature above their boiling point and yet no boiling occurs |
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| Arises from conflict between attractive energy (enthalpy) and tendency toward disorder (entropy) |
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| Solids at room temperature, but do not exist as discrete molecules |
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| Formed by the reaction of non-metals with non-metals |
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| Exist as discrete molecules. Can exist as solids, liquids, or gases at room temperature (NO, SO3, CH4, PCl3) |
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Definition
| Molecular covalent compounds |
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| Do not exist discrete molecules. All the atoms are bound together to make a giant molecules. Always solids at room temperature. (SiC and SiO2) |
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| Network covalent compounds |
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| Metals do not react with other metals to form compounds. They form mixtures with each other |
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| Forces between the atoms in the molecule |
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| Forces between different molecules |
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| The force of attraction between two oppositely charged ions is ________ than the attraction between two neutral molecules |
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| In order to convert an ionic compound into a liquid, the very strong forces between the positive and negative ions must be partially overcome and the ions much be able to move while being attracted strongly to each other. Heating adds ________ to the particles in the solid |
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| In a covalent solid, the molecules are held in a geometric pattern by intermolecular attractions between the molecules |
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| For covalent compounds, the amount of energy needed to partially overcome the intermolecular attractions is significantly ______ on the average than is needed fro ionic compounds |
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| One must find the temperature at which a solid and the liquid phases exist together in equilibrium |
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| When both solid and liquid are present, the temperature ______ when heat is removed and some liquid freezes until all the liquid is frozen |
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| Sometimes a liquid will cool below its freezing point without freezing |
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| If two objects are at two different temperatures and then come into contact with one another, they will reach equilibrium temperature because the heat from the object will flow to the object with lower temperature until they have the same temperature |
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Definition
| Zeroth Law of Thermodynamics |
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| A liter of gas A contains the same number of molecules of A as the number of molecules of B in a liter of gas B provided the temperature and pressure are the same for the liter of a and the liter of B |
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| If a container is kept at a constant temperature and a vacuum is in the container at atmospheric pressure. Liquid water is introduced into the bottom of the container and the pressure will increase until a value is reached which remains unchanged |
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