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Test 2 chem
Ch 2,5,6&7. Chemistry an introduction Timberlake
| Question | Answer |
|---|---|
| Activation Energy | The energy needed upon collision to break apart the bonds of the reacting molecules |
| Avagadro's Number | The number of items in a mole equal to 6.02 x 10^23 |
| Balanced equation | Final form of a chemical equation that shows the same number of atoms of each element in the reactants and products |
| Catalyst | A substance that increases the rate of reaction by lowering the activation energy |
| Chemical Change | The formation of a new substance with a different composition and different properties than the initial change |
| Chemical Equation | A shorthand way to represent a chemical reaction using chemical formulas to indicate the reactants, products and coefficient to show reacting ratios |
| Chemical Reaction | The process by which a chemical change takes place |
| Coefficients | Whole number placed in front of the formulas to balance the number of atoms or moles of atoms of each element on both sides of an equation |
| Combination Reaction | A reaction in which reactants combine to form a single product |
| Decomposition Reaction | A reaction in which a single reactant splits into two or more simpler substances |
| Double Replacement Reaction | A reaction in which parts of two different reactants exchange place |
| Endothermic Reaction | A reaction that requires heat; the energy of the product is higher than the energy of the reactants |
| Exothermic Reaction | A reaction that releases heat; the energy of the products is lower than the energy of the reactants |
| Formula Unit | The group of ions represented by the formula of an ionic compound |
| Molar Mass | The mass, in grams, of 1 mole of an element equal numerically to the atomic mass. The molar mass of a compound is equal to the sum of the masses of the elements multiplied by their subscripts of the formula |
| Mole | A group of atoms, molecules, or formula units that contain 6.02 x 10^23 of these items |
| Mole-Mole Factor | A conversion factor that relates the number of moles of two compounds derived from the coefficients in an equation |
| Oxidation | The loss of electrons of a substance. Biological oxidation may involve the addition of oxygen or the loss of hydrogen |
| Oxidation-Reduction Reaction | A reaction in which the oxidation of one reactant is always accompanied by the reduction of another reactant |
| Physical Change | A change in which the physical appearance of a substance changes but the chemical composition stays the same |
| Products | The substances formed as a result of a chemical reaction |
| Reactants | The initial substances that undergo change in a chemical reaction |
| Reduction | The gain of electrons by a substance. Biological reduction may involve the loss of oxygen or gain of hydrogen |
| Single Replacement Reaction | A reaction in which an element replaces a different element in a compound. |
| Atmosphere (atm) | the pressure exerted by a column of mercury 760 mm high |
| Atmospheric Pressure | the pressure exerted by the atmosphere |
| Avogadro's Law | Volume of gas directly related to number of moles |
| Boyle's Law | pressure of gas is inversely related to the volume |
| Charles's Law | volume of gas directly related to change in K temperature |
| Combined gas law | A relationship that combines several gas laws relating pressure, volume and temperature when the amount of gas does not change: P1V1/T1 = P2V2/T2 |
| Dalton's Law | Total pressure exerted=sum of pressures of gases in container |
| Direct Relationship | A relationship in which two properties increase or decrease together |
| Gay-Lussac's Law | Pressure of gas changes directly with change in temperature |
| Inverse relationship | A relationship in which two properties change in opposite directions |
| Kinetic molecular theory of gases | A model used to explain the behavior of gases |
| Molar Volume | A volume of 22.4L occupied by 1 mole of a gas at STP conditions of 0ￂﾰ C (273K) and 1 atm |
| Partial Pressure | The pressure exerted by a single gas in a gas mixture |
| Pressure | The force exerted by gas particles that hit the walls of a container |
| STP | Standard conditions of 0ￂﾰC (273 K) temperature and 1 atm pressure used for the comparison of gases |
| Boiling | the formation of bubbles of gas throughout the liquid |
| Boiling Point | The temperature at which a liquid changes to gas (boils) and gas changes to liquid (condenses) |
| Caloric Value | The kilocalories obtained per gram of food types: carbohydrate, fat and protein |
| Calorie (cal) | The amount of heat energy that raises the temperature of 1 g of water exactly 1 ￂﾰC |
| Change of state | The transformation of one state of mater into another; ex: liquid to solid |
| Condensation | The change of state from a gas to a liquid |
| Cooling Curve | A diagram that illustrates temperature changes and changes of state for a substance as heat is removed |
| Energy | The ability to do work |
| Evaporation | The formation of a gas (vapor) by the escape of higher energy molecules from the surface of a liquid |
| Freezing | The change of state from a liquid to a solid |
| Freezing point (fp) | The temperature at which a liquid changes to a solid (freezes), a solid changes to a liquid (melts) |
| Gas | A state of matter characterized by no definite shape of volume, particles in a gas move rapidly |
| Heat | The energy associated with the motion of particles in a substance |
| Heat of Fusion | The energy required to melt exactly 1 g of a substance at its melting point, for water: 80 cals are needed to melt 1 g of ice, 80 cal are released when 1 g of water freezes |
| Heat of Vaporization | The energy require to vaporize 1 g of substance at its boiling point. For water, 540 calories are needed to vaporize exactly 1 g of liquid; 1 g of steam gives of 540 cal when it condenses |
| Heating Curve | A diagram that shows the temperature changes and changes of state of a substance as it is heated |
| Joule (J) | The SI unit of heat energy. 4.184 J = 1 cal |
| Kilocalorie (kcal) | An amount of energy equal to 1000 calories |
| Kinetic Energy | The energy of moving particles |
| Liquid | A state of matter that takes the shape of its container but has a definite volume |
| Matter | Anything that has mass and occupies space |
| Melting | The change of state from a solid to a liquid |
| Melting Point (mp) | The temperature at which a solid becomes a liquid (melts). It is the same temperature as the freezing point |
| Potential Energy | An inactive type of energy that is stored for future use |
| Solid | A state of matter that has its own shape and volume |
| Specific Heat | A quantity of heat that changes the temperature of exactly 1 g of a substance by exactly 1 ￂﾰC |
| Sublimation | The change of state in which a solid is transformed directly into a gas without forming a liquid first |
| Work | An activity that requires energy |
| Colloid | A mixture having particles that are moderately large. Colloids pass through filters but cannot pass through semi permeable membranes |
| Concentration | A measure of the amount of solute that is dissolved in a specified amount of solution |
| Crenation | The shriveling of a cell because of water's leaving the cell when the cell is placed in a hypertonic solution |
| Dialysis | A process in which water and small solute particles pass through a semi permeable membrane |
| Dilution | A process by which water (solvent) is added to a solution to increase the volume and decrease (dilute) the concentration of the solute |
| Electrolyte | A substance that produces ions when dissolved in water; its solution conducts electricity |
| Equivalent (Eq) | The amount of a positive or negative ion that supplies 1 mole of electrical charge |
| Hemodialysis | A mechanical cleaning of the blood by an artificial kidney using the principle of dialysis |
| Hemolysis | A swelling and bursting of red blood cells in a hypotonic solution because of an increase in fluid volume |
| Henry's Law | The solubility of a gas in a liquid is directly related to the pressure of that gas above the liquid |
| Hydration | The process of surrounding dissolved ions with water molecules |
| Hydrogen Bond | The attraction between a partially positive hydrogen atom in one molecule and a highly electronegative atom such as oxygen in another molecule |
| Hypertonic Solution | A solution that has a higher particle concentration and higher osmotic pressure than the cell of the body |
| Hypotonic Solution | A solution that has a lower particle concentration and lower osmotic pressure than the cells of the body |
| Isotonic Solution | A solution that has the same particle concentration and osmotic pressure as tat of the cells of the body |
| Mass percent | The gram of solute in exactly 100 mL of solution |
| Mass/Volume Percent | The gram of solute in exactly 100 mL of solution |
| Molarity (M) | The number of moles of solute in exactly 1 L of solution |
| Nonelectrolyte | A substance that dissolves in water as molecules; its solution will not conduct an electrical current |
| Osmosis | The flow of a solvent, usually water, through a semipermeable membrane into a solution of higher solute concentration |
| Osmotic Pressure | The pressure that prevents the flow of water into the more concentrated solution |
| Physiological Solution | A solution that is isotonic with and exerts the same osmotic pressure as normal body fluids |
| Saturated Solution | A solution containing the maximum amount of solute that can dissolve at a given temperature. Any addition solute will remain undissolved in the container |
| Semipermable Membrane | A membrane that permits the passage of certain substances while blocking or retaining others |
| Solubility | The maximum amount of solute that can dissolve in exactly 100g of solvent, usually water, at a given temperature |
| Solute | The component in a solution that is present in the smaller quantity |
| Solution | A homogeneous mixture in which the solute is made up of small particles (ions or molecules) that can pass through filters and semipermable membranes |
| Solvent | The substance in which the solute dissolves; usually the component present in greatest amount |
| Strong electrolyte | A polar of ionic compound that ionizes completely when it dissolves in water. Its solution is a good conductor of electricity |
| Suspension | A mixture in which the solute particles are large enough and heavy enough to settle out and be retained by both filters and semipermable membranes |
| Unsaturated Solution | A solution that contains less solute than can be dissolved |
| Volume Percent | A percent concentration that relates the volume of the solute in exactly 100 mL of solution |
| Weak electrolyte | A substance that produces only a few ions along with many molecules when it dissolves in water. Its solution is a weak conductor of electricity. |
| F/N 1 cal = | 1.184 J |
| F/N 1 kJ = | 1000 J |
| F/N 1 kcal = | 1000 cal |
| F/N kcal / gram food: Carb | 4 kcal/1g |
| F/N kcal/gram food: Fat (lipid) | 9 kcal/1g |
| F/N kcal/gram food: Protein | 4 kcal/1g |
| F/N Heat of Fusion for water | 80 cal/1g |
| F/N Heat of Vaporization for water: | 540 cal/1g |
| F/N 1 atm = | 760 mmHg = 760 torr |
| F/N Boyles | P1V1=P2V2 |
| F/N Charles | V1/T1=V2/T2 |
| F/N Gay-Lussacs | P1/T1=P2/T2 |
| F/N Avogadro | V1/n1=V2/n2 |
| F/N Dalton | Pt=P1+P2.... |
| F/N Combined Gas Law | P1V1/T1 = P2V2/T2 |
| F/N STP | 0 c or 273K, 1atm or 760 mmHg, 1 mole = 22.4L |
| F/N Mass percent | Concentration: g solute/(g solute + g solvent) x100 |
| F/N Amount of solvent/100g: g solute/100g solution | |
| F/N Volume Percent | mL solute/mL solution |
| F/N Molarity | mole solute/L solution |
| F/N Dilution: Percent Concentration | C1V1=C2V2 |
| F/N Dilution: Molarity | M1V1=M2V2 |
| F/N Physiological Solution | 5% glucose or .9% NaCl |
| F/N Specific Heat Equation | = mass x change in temperature x specific heat (1C or 4.184J for water) |
Created by:
kallenpoole
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