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| a covalent bond between atoms that have different electronegativity. The shared electrons are pulled closer to the more electronegative atom, making it slightly negative and the other atom slightly positive. Example: Water molecule. |
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| A molecule with an uneven distribution of charges in different regions of the molecule. Example: water. |
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| Hydrogen bonds that hold a substance together, causing this ____ effect. This phenomenon makes the transport of water against gravity in plants possible. |
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| One substance clinging to another. |
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| this is a measure of how difficult it is to stretch or break the surface of a liquid. Water has more of this than most liquids, meaning it doesn't break easily. This is why some animals can walk on water. |
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| This is a measure of heat intensity that represents the average kinetic energy of molecules, regardless of volume. |
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| The amount of heat it takes to raise the temperature of 1 g of water by 1 degree celsius. |
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| The amount of heat required to raise the temperature of 1 kilogram (kg) of water by 1 degree celsius. |
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| An energy unit equal to 0.239 calories. |
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| The amount of heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1 degree celsius. This is different for all elements. Water has an especially high one of these, meaning it resists changing its temperature. |
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| vaporization or evaporation |
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| What happens when molecules are moving fast enough to overcome their attraction to one another and leave the liquid and enter the air as a gas. |
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| The quantity of heat a liquid must absorb for 1 g of it to be converted from a liquid to a gas. |
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| When a liquid evaporates, the surface of the liquid that remains behind cools down, causing this effect ______. The "hottest" molecules are most likely to leave as a gas. |
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| Explain how water freezes and why ice water will float. |
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| As the temperature falls to 0 degrees celsius, water begins to freeze because its molecules are moving too slowly to break hydrogen bonds. The molecules becoem locked into a crystalline lattice, with each water molecule hydrogen-bonded to four partners. This makes them far enough apart to make ice about 10% less dens than liquid water. This is why ice will float on water. |
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| A liquid that is completely homogeneous mixture of two or more substances. |
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| The substance in a solution that is the dissolving agent. So if sugar is added to water, water is the solvent. |
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| The substance in a solution that is being dissolved. So if sugar is added to water, sugar is the solute. |
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| A solution where water is the solvent. |
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| The sphere of water molecules around each dissolved ion in a solution. |
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| Any substance with an affinity for water. Substances can even be this without actually dissolving in water. They can remain suspended in the aqueous liquid of the cell, which is called a colloid. |
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| A stable suspension of fine particles in a liquid. |
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| Any substance that cannot form hydrogen bonds and repels water. They are usually nonionic and nonpolar. |
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| The sum of the masses of all the atoms in a molecule. |
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| This unit of measurement represents the exact number of objects in a molecule: 6.02 x 10^23. One unit of this measurement has exactly the same number of molecules as one unit of measurement of any other substance. |
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| the number of moles of solute per liter of solution. |
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| A single proton of hydrogen with a charge of 1+. |
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| A water molecule that lost a proton and now has a charge of 1-. |
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| A water molecule that has gained a proton and now has a charge of 1+. |
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| A substance that increases the hydrogen ion concentration of a solution. |
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| A substance that reduces the hydrogen ion concentration of a solution. |
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| A substance that allows biological fluids to maintain a relatively constant pH by minimizing changes in the concentrations of H+ and OH-. They do this by accepting hydrogen ions from the solution when they are in excess and donating hydrogen ions to the solution when they have been depleted. |
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| the negative logarithm (base 10) of the hydrogen ion concentration. |
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| CO2 from human pollution dissolves in seawater to form carbonic acid that lowers the ocean's pH. |
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| Acid Precipitation/Acid Rain |
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| Burning fossil fuels creates sulfur oxides and nitrogen oxide which react with water in the air to form strong acids which fall to earth with rain or snow. |
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