Chemistry Exam Thursday at 8:00 (3rd period class)
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| 789484864 | Emperical Formula | smallest whole number ratio between elements in a compound. This is the accepted value for ionic compounds | 0 | |
| 789484865 | Molecular Formula | whole number multiple of empirical formula | 1 | |
| 789484866 | percent composition | relative amount of each element in a compound | 2 | |
| 789484867 | Combustion reaction | Hydrocarbons react with oxygen to produce CO2 and H2O | 3 | |
| 789484868 | Decomposition Reaction | a single compound undergoes a reaction that produces 2 or more simpler substances | 4 | |
| 789484869 | Double Replacement reaction | 2 ionic compounds react by exchanging cations for new compounds | 5 | |
| 789484870 | Single Replacement reaction | an element replaces a similar element in a compound | 6 | |
| 789484871 | Synthesis Reaction | 2 substances combine to form 1 new compound | 7 | |
| 789484872 | Active metal compound+ Less active metal | Active metal + less active metal compound------> | 8 | |
| 789484873 | Salt + H2 | Metal + Acid----> | 9 | |
| 789484874 | Halogen compound + halogen | Halogen + halogen compound-----> | 10 | |
| 789484875 | Metallic Hydroxide + H2 | Metal + H2O-----> | 11 | |
| 789484876 | BX + AY | AX + BY-----> | 12 | |
| 789484877 | element + element | Binary Compound decomposes into ---- | 13 | |
| 789484878 | metallic Oxide + CO2 | metallic Carbonate decomposes into ---- | 14 | |
| 789484879 | metallic chloride + O2 | Metallic Chlorate decomposes into ---- | 15 | |
| 789484880 | Metallic Oxide + H2O | Metallic Hydroxide and H2O decomposes into---- | 16 | |
| 789484881 | KOH, NaOH | ________ and ____________ will never decompose when heated | 17 | |
| 789484882 | Nonmetallic oxide + h2O | Acid decomposes into---- | 18 | |
| 789484883 | Compound | Element + Element----> | 19 | |
| 789484884 | CO2 + H2O | Hydrocarbons + H2O ----> | 20 | |
| 789484885 | actual yield | amount of product produced when a reaction takes place | 21 | |
| 789484886 | theoretical yield | the maximum amount of product that should be formed in a reaction | 22 | |
| 789484887 | Actual yield divided by theoretical yield , times 100. | Percent Yield | 23 | |
| 789484888 | stoichiometry | the calculation of quantities in chemical reactions | 24 | |
| 789484889 | Absolute Zero | the temperature at which the movement of all particles theoretically ceases | 25 | |
| 794868600 | 0k or -273 C | What is the temperature of absolute zero? | 26 | |
| 794868601 | Allotrope | 2 or more different forms of the same element in the same physical state | 27 | |
| 794868602 | Amorphous Solids | solids composed of particles that have no set pattern and lack an ordered internal structure | 28 | |
| 794868603 | Barometer | device used to measure atmospheric pressure | 29 | |
| 794868604 | Boiling Point | temperature at which the vapor pressure of a liquid equals the external pressure on the surface of the liquid | 30 | |
| 794868605 | Melting Point | the temperature of which solid changes to liquid, heat has to be added | 31 | |
| 794868606 | Crystal | a substance arranged in an ordered repeating 3d pattern called a crystal lattice | 32 | |
| 794868607 | dynamic equilibrium | an equilibrium condition in which the rate of evaporation equals the rate of condensation | 33 | |
| 794868608 | elastic collision | Kinetic energy is transferred from one particle to another but the total kinetic energy is constant | 34 | |
| 794868609 | evaporation | vaporization on the surface of a non boiling liquid | 35 | |
| 794868610 | fluids | ... | 36 | |
| 794868611 | intermolecular forces | hold liquid particles together and reduce the space between particles. therefore, liquids are more dense than gases | 37 | |
| 794868612 | Kinetic Energy (Ek) | energy of motion | 38 | |
| 794868613 | Pascal | SI unit of pressure, which means a newton per meter squared | 39 | |
| 794868614 | phase diagram | graph that shows the relation between temperature, pressure, and state | 40 | |
| 794868615 | pressure | the force per unit area of a substance | 41 | |
| 794868616 | STP | standard temperatures and pressures | 42 | |
| 794868617 | 0C or 273K | What is standard Temperature? | 43 | |
| 794868618 | 101.3kPa, 760mmHg, and 1atm | What is standard Pressure? | 44 | |
| 794868619 | sublimation | the conversion of a solid to a gas of vapor without passing through the liquid state | 45 | |
| 794868620 | Vapor Pressure | force due to the gas above a liquid | 46 | |
| 794868621 | (little c) calorie | the quantity of heat needed to change the temperature of 1 gram of WATER 1C | 47 | |
| 794868622 | calorimeter | insulated container used to help measure heat absorbed or released by a substance | 48 | |
| 794868623 | endothermic | Heat is absorbed (+) | 49 | |
| 794868624 | exothermic | heat is released (-) | 50 | |
| 794868625 | Enthalpy (H) | heat content of a system at constant pressure | 51 | |
| 794868626 | Heat of combustion | the heat released during a chemical reaction in which one mole of a substance is completely burned | 52 | |
| 794868627 | Heat of reaction | the heat absorbed or released during a chemical reaction; equivalent to h, the change in enthalpy | 53 | |
| 794868628 | Hess's law of heat summation | in going from a particular set of reactions to a particular set of products, the enthalpy changes in the same whether the reaction takes place in one step or in a series of steps | 54 | |
| 794868629 | summation | ... | 55 | |
| 794868630 | joule | the SI unit for energy, equal to one (little c) calorie | 56 | |
| 794868631 | Heat of vaporization | the amount of heat needed to change a unit mass of a substance from a liquid to a vapor at its boiling point | 57 | |
| 794868632 | Heat of fusion | the amount of heat needed to change a unit mass of a substance from solid to liquid at its melting point | 58 | |
| 794868633 | heat of solution | ... | 59 | |
| 794868634 | Specific Heat Capacity | quantity of heat needed to change the temperature of 1 gram of A SUBSTANCE 1C | 60 | |
| 794868635 | Standard Heat of Formation | the change in enthalpy for a reaction in which one mole of a compound is formed from its constituent elements | 61 | |
| 794868636 | Thermochemical Equation | an equation that includes the heat change in a reaction | 62 | |
| 794868637 | Thermochemistry | the study of heat changes in chemical reactions | 63 | |
| 794868638 | Avagadro's Hypoghesis | equal volumes of gasses at the same temperature and pressure contain an equal number of particles | 64 | |
| 794974598 | Boyle's Law | For a given mass of a gas, the volume varies indirectly with the pressure if the temperature is constant | 65 | |
| 794974599 | Charle's Law | the volume of a fixed mass of a gas is directly proportional to the Kelvin Temperature if Pressure is constant | 66 | |
| 794974600 | Combined Gas Law | If P, V, or T is not constant, use this law | 67 | |
| 794974601 | Compressibility | the measure of how much the volume decreases under pressure | 68 | |
| 794974602 | Dalton's Law of partial pressures | at constant V and T, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each component gas | 69 | |
| 794974603 | diffusion | the tendency of particles to spread throughout a given volume | 70 | |
| 794974604 | Gay-Lussac's Law | the pressure of a fixed mass of a gas varies directly with the kelvin temperature if volume is constant | 71 | |
| 794974605 | Graham's Law of Effusion | the rate of effusion of a gas is indirectly proportional to the square root of its molar mass | 72 | |
| 794974606 | R, 8.31L kPa Mole K | what is the ideal gas constant?, and what is its #? | 73 | |
| 794974607 | Ideal Gas Law | describes the behavior of an ideal gas, PV=nRT | 74 | |
| 794974608 | partial pressure | the pressure exerted by each gas in a gaseous mixture | 75 | |
| 794974609 | Aufbau Principle | electrons enter orbitals of lowest energy first | 76 | |
| 794974610 | electron configuration | electrons are shown as superscripts on sublevel and energy level that electron occupies | 77 | |
| 794974611 | energy levels | described by the Principle Quantum number, the period an element is located in tells the highest occupied ____________. | 78 | |
| 794974612 | Hund's Rule | when electrons occupy orbitals of equal energy, 1 electron enters each orbital until all the orbitals contain 1 electron, then the electrons can be paired | 79 | |
| 794974613 | orbitals | described by the 3rd quantum number. This is a region or pair of electrons. | 80 | |
| 794974614 | Pauli Exclusion Principle | no 2 electrons in an atom can have the same set of 4 quantum numbers | 81 | |
| 794974615 | planetary model | electrons orbit the nucleus in concentric circular paths like planets orbit the sun. | 82 | |
| 794974616 | Niels Bohr | who came up with the planetary model? | 83 | |
| 794974617 | quantum mechanical model | also called the modern atomic model. describes the energy and location of electrons in atoms | 84 | |
| 794974618 | Schrodinger | Who invented the quantum mechanical model | 85 | |
| 794974619 | quantum numbers | numbers to describe the location and energy of electrons in atoms | 86 | |
| 794974620 | sublevels | described by the 2nd quantum number, also a division of an energy level | 87 | |
| 794974621 | atomic radius | 1/2 the distance between 2 nuclei in a molecule | 88 | |
| 795021999 | electronegativity | tendency for atoms to attract electrons to themselves when they are combined with other elements | 89 | |
| 795022000 | inner transition elements | lanthanides and actinides. 4f and 5f. outer s full and electrons added to 4f and 5f sublevels | 90 | |
| 795022001 | ionization energy | energy required to remove an electron from and atom | 91 | |
| 795022002 | noble gasses | group 18 with outer s and p sublevels filled except He. Inert because they have 8 electrons in the outer shell (unreactive) | 92 | |
| 795022003 | Know all trends from chapter 14 in notes | Know all trends from chapter 14 in notes | 93 | |
| 795022004 | representative elements | groups 1 and 2, 13-17. have s and p sublevels partially filled | 94 | |
| 795022005 | alkali | group 1 | 95 | |
| 795022006 | alkaline earth metals | group 2 | 96 | |
| 795022007 | Chalcogens | group 16 | 97 | |
| 795022008 | Halogens | group 17 | 98 | |
| 795022009 | transition elements | outer s sublevels full and electrons added to inner d | 99 | |
| 795022010 | concentration | a measure of the amount of solute that is dissolved in a given quantity of solvent, usually expressed mol/L | 100 | |
| 795022011 | dilute | a solution that contains a small amount of solute | 101 | |
| 795022012 | concentrated | a solution that contains a large amount of solute | 102 | |
| 795022013 | molarity | the concentration of solute in a solution expressed as the number of moles of a solute dissolved in 1 kilogram of solvent | 103 | |
| 795022014 | Properties of Acids | 1) sour taste 2) contain Hydrogen 3) acids react with bases to give a salt and Water 4) acids are electrolytes- aquias solution conducts electricity 5) change blue litmus to red | 104 | |
| 795022015 | Properties of Bases | 1)have bitter taste 2)dilute aquias solutions of bases feel slippery to the skin 30 change color from red litmus to blue 4) contain OH and react with acids in neutralization reaction 5) bases are electrolytes | 105 | |
| 795022016 | OH gives you the pOH, the ph+poh = 14. -log(-OH)=poh | OH gives you the pOH, the ph+poh = 14. -log(-OH)=poh | 106 | |
| 795022017 | acid | ph>7 | 107 | |
| 795022018 | neutral | ph=7 | 108 | |
| 795022019 | base | ph<7 | 109 |
