2013 mrs redican – Flashcards
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What cannot be broken down or decomposed? |
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elements |
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What can be decomposed? |
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compounds |
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SOLIDS |
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rigid, geometric, network lattice definite shape and definite volume particles vibrate in fixed position closely packed particles strong intermolecular forces small distance between particles |
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LIQUIDS |
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definite volume , no definite shape has surface tension and viscosity particles can flow past one another |
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GASES |
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spreads to fill the entire container no definite shape no definite volume random, constant , straight-line motion weak intermolecular forces |
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INTERMOLECULAR FORCES |
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forces between molecules solids have strong forces, and gases have weak forces |
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what is AVERAGE KINETIC ENERGY? |
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energy of particle motion TEMPERATURE |
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when does potential energy change? |
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changes during a phase change energy of how the particles are spread out |
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what are SUBSTANCES? |
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elements and compounds only one type of particle |
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MIXTURES |
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a combinations of elements and/or compounds |
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PRESSURE-VOLUME OF GASES |
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[image] |
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KINETIC MOLECULAR THEORY OF GASES |
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* gases move in constant random straight line motion * gases do not lose or gain energy when they collide -- they have elastic collisions *gas particles have a volume that is insignificant compared to the volume of the total gas * average kinetic energy is temperature * gas particles have no significant forces between them |
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IDEAL GASES |
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high temperature -- move very fast low pressure -- very far apart |
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MELTING |
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solid -liquid equilibrium (s)-->(l) |
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VOLUME -TEMPERATURE OF GASES |
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[image] |
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FREEZING |
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solid-liquid equilibrium (l)-->(s) |
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BOILING /EVAPORATION VAPORIZATION |
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liquid-gas equilibrium (l)-->(g) |
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CONDENSATION |
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liquid-gas equilibrium (g) --> (l) |
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SUBLIMATION |
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(s) --> (g) like dry ice |
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DEPOSITION |
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(g) --> (s) like frost on your windows |
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PHASE CHANGES |
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temperature does NOT change kinetic energy does not change potential energy changes |
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TEMPERATURE CHANGES |
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kinetic energy changes |
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1 MOLE |
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6 x 10^23 particles |
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MOLAR MASS |
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gram formula mass (add up the pieces using mass from the Periodic Table) |
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SYNTHESIS |
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A3 + 2B --> AB2 coming together to make one product |
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DECOMPOSITION |
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1 reactant breaking down into more than one product AB ---> A + B |
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SINGLE REPLACEMENT |
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1 element and 1 compound replacing part of each other A + BC --> B + AC |
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DOUBLE REPLACEMENT |
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compound 1 + compound 2 replacing part of each other ex. PbCl + K(NO3) --> KCl + Pb(NO3) |
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COMBUSTION |
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CH + O2 ---> CO2 + H20 |
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PHYSICAL CHANGES |
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boiling, melting, freezing, condensation, evaporation, solidifcation,sublimation, deposition |
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5 types of CHEMICAL REACTIONS |
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synthesis, decomposition, single replacement, double replacement, combustion |
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ATOM |
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the simplest unit of an element |
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Which subatomic particles have mass? |
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protons and neutrons a mass of 1 amu each |
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Which subatomic particle has almost no mass and is very small? |
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electrons |
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According to the wave mechanical model of the atom, where are electrons located? |
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orbitals , regions of high probability of finding an e- |
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VALENCE ELECTRONS |
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electrons in the outermost shell (the last number in the e- configuration) |
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ISOTOPES |
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same protons and atomic number and symbol different mass number and different numbers of NEUTRONS |
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How do we calculate atomic mass? ( THIS IS NOT MASS NUMBER!!) |
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mass multiply by abundance (in decimal percent , to the left, to the left like Beyonce :) The abundance decimal point gets moved NOT the mass. C-12 mass 12.01 abundance 98.7% (12x0.987) + ... |
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ORBITALS |
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the most likely region to find an electron (areas of high probability) |
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QUANTUM LEAP |
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1) e- absorb energy 2) go to a higher level "excited state" (unstable) 3) go to a lower level 4) release a photon of light (bright line atomic spectra) |
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MASS NUMBER |
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number of protons + number of neutrons (added up) |
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ATOMIC NUMBER |
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number of protons can be found on the periodic table |
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ATOM ELECTRICALLY NETURAL |
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because # of protons = # of electrons |
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EXCITED STATE |
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electron jumped up to a higher energy shell |
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BRIGHT LINE ATOMIC SPECTRA |
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unique "fingerprint" that can identify an element produced when electron goes to a lower energy level and releases photon of light |
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ALPHA |
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positive and has the most mass weakest power |
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GAMMA |
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most penetrating power pure energy no mass , no charge |
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FISSION |
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nuclear power U + n --> Ba + Kr + 3 n + energy to split apart |
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FUSION |
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H + H --> He + energy to combine |
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NATURAL TRANSMUTATION |
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one element decaying and becoming a new element X --> |
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ARTIFICIAL TRANSMUTATION |
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one element and a particle becoming a new element X + beta/gamma/alpha ---> |
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USES OF RADIOISOTOPES |
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I-131 thyroid treatment Co-60 cancer C-14 date organic material U-238 date rocks |
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PROS and CONS NUCLEAR POWER |
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pros + cheap, clean, less pollution cons - radioactive waste, possible breakdown and radiation leaks/sickness |
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HALF_LIFE |
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the time it takes for a sample size to decay with only half remaining half-life is a steady, constant rate |
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AVOGADRO'S LAW |
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gases at the same temp and pressure, will have equal volume and equal number of molecules |
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MOLAR RATIOS |
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Given a balanced equation, if the problem goes from moles to moles - --use molar ratios to solve |
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CONSERVATION OF MASS |
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mass and charge are both conserved Given a balanced equation if a problem is about grams and grams - - use conservation of mass to add/subtract to find the answer |
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VALENCE ELECTRONS |
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electrons in the outermost shell the last number in an electron configuration |
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SIMILAR ELEMENTS |
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have same number of valence e- same group |
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ACROSS A PERIOD |
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radii get smaller (positive nucleus pulls e- inward) IE increases EN increases less metallic character |
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DOWN A GROUP |
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atomic radii get larger, more e- shells IE decreases EN decreases metallic character increases |
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METALS |
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lose e- malleable luster/shiny solid (except mercury) ductile good conductors b/c of free mobile e- (sea of e-) hi density *they become totally different when they react to become ionic want to lose e |
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NONMETALS |
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dull brittle solids or gases (except Br) poor conductors (no free mobile e-) want to gain e- , high EN |
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IONIC BOND |
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metals with nonmetals transfer of e- high melt point dissolve /soluble in water conducts in water (electrolyte) |
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COVALENT BOND |
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nonmetal with nonmetal shares e- low melt point |
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POLAR covalent |
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shares unevenly EN difference high asymmetrical soluble in water |
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NONPOLAR covalent |
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shares evenly EN difference low or zero symmetrical insoluble in water poor conductor |
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LEWIS DOT DIAGRAMS |
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dot represent valence e- if more than one atom present, show how the electrons are transferred (if ionic) or shared (if covalent) |
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ENTHALPY |
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heat energy |
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ENDOTHERMIC |
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heat is absorbed A + heat --> B + C feels cool , because the rxn absorbs energy from the surroundings heat of reaction is + Table I |
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EXOTHERMIC |
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heat is released A --> B + C + heat feels warm, because the rxn releases energy to the surroundings heat of reaction is - Table I |
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ENTROPY |
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disorder of a system solid is least , gases are the most the more molecules the more disorder |
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Nature and SPONTANEOUS RXNS |
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greater disorder , more entropy usually also exothermic, but not always |
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COLLISION THEORY |
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there must be collisions for molecules to react there must me sufficient energy to react there must be more stability in the products formed |
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REACTION RATE |
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if the reaction rate increases, the time it takes is less |
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TEMPERATURE AND RXN RATE |
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higher temp, more kinetic energy, more collisions, faster rxn |
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CONCENTRATION AND RXN RATE |
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more particles per volume, more collisions, faster rxn |
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SURFACE AREA AND RXN RATE |
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crushing/powder, grinding makes more surface area for more possible collisions, faster rxn |
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REACTIVITY OF ELEMENTS |
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Table J, higher is more reactive |
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CATALYST |
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creates an alternate pathway with a lower activation energy ( faster) |
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HEAT OF REACTION |
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H products - H reactants |
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ACTIVATION ENERGY |
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the minimum energy required for the rxn to occur |
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ACID |
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H+ donor H..., usually sour reacts with metals pH below 7 |
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BASE |
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H+ acceptor ...OH, usually bitter slippery pH above 7 |
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NEUTRALIZATION |
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Acid + Base ---> ionic salt and HOH |
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MOLARITY |
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moles of solute / liter of solution |
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pH |
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goes by factors of 10 |
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pH goes from 6 to 4 |
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increase H+ by 10*10 = 100 times more acidic |
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pH goes from 11 to 8 |
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decrease in H+ 10^3 = 1000 less basic (going closer to neutral) 1/1000 of H+ |
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LEO |
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lose electrons oxidation oxidation # goes up e- are on the product side oxidized reducing agent |
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GER |
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gain e- reduction e- are on the reactant side oxidation # goes down reduced oxidizing agent |
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flow of e- |
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always anode to cathode |
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AN OX RED CAT |
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anode is where oxidation occurs cathode is where reduction occurs |
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voltaic cell vs electrolytic |
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voltaic requires a salt bridge that lets ions flow voltaic, no battery , so it is spontaneous voltaic : chemical energy converted to electrical electrolytic requires a battery, not spontaneous electrolytic : electrical energy converts to chemical energy |
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solute vs solvent |
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solute gets dissolved solvent does the dissolving |
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HETEROGENEOUS MIXTURES |
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different particles not evenly spread out |
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HOMOGENEOUS MIXTURES |
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Solutions if in water, aqueous |
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SEPARATE BY SIZE LIKE HETEROGENEOUS MIXTURES |
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filtration (like sand and water) |
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SEPARATE INKS DYES, COLORS |
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chromatography |
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SEPARATE BY BOILING POINT |
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distillation like crude oil (fractional distillation) |
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SEPARATE BY EVAPORATION |
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dissolved solids in water/liquids like salt water |
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ADDING MORE PARTICLES MAKE THE |
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freezing point go down boiling point go up vapor pressure go down osmotic pressure go up |
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SUPERSATURATED, SATURATED, UNSATURATED |
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supersaturated= above the accepted value, saturated = equal to the accepted value unsaturated = less than the accepted value |
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PRECIPITATE |
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Solid in solution, occurs when something is insoluble |
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What has a fixed ratio or proportion? |
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compounds |
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If a substance has a high boiling point what kind of intermolecular forces does it have? Conversely, low boiling point? |
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strong or high Low boiling point means lower intermolecular forces |
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Which two subatomic particles have the same quantity of charge but opposite signs? |
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proton +1, and electron -1 |
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Which subatomic particle holds the nucleus together? |
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neutrons |
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Which subatomic particle is equal to the atomic number? |
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protons only |
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Which two subatomic particles have the same quantity of charge but opposite signs? |
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proton +1, and electron -1 |
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Which subatomic particle holds the nucleus together? |
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neutrons |
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Which subatomic particle is equal to the atomic number? |
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protons only |
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Which subatomic particle has no charge? |
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neutron |
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Which subatomic particle has a charge of -1? |
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electron |
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What does NOT change during excited state? |
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nucleus |
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How do we calculate atomic mass of isotopes? |
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take the weighted average of all the naturally occurring isotopes |
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Mass into lots of energy |
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nuclear power |
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chemical energy into electrical |
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voltaic cell |
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electrical energy into chemical energy |
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electrolytic cell |
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How do the boiling points of water and a solution compare? |
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the solution will have a higher boiling point and lower freezing point (boiling pt elevation and freezing pt depression) |
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How are C graphite and C diamond different? |
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different structures so different properties |
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How are allotropes different? |
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different structures and different properties |
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What makes something organic? |
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Carbon |
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What elements are in a hydrocarbon? |
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H and C only |
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What is a saturated molecule? |
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all single bonds = alkanes |
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What is an unsaturated molecule? |
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contains at least 1 multiple bond (double or triple) |
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-COO- |
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ketone |
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-COOH |
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organic acid |
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What reaction produces polymers? |
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polymerization |
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What reaction produces esters? |
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esterification |
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What reaction produces alcohol? |
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fermentation |
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CH4 + Cl2 ==> CH3Cl + HCl |
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substitution |
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What are esters made from? |
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alcohol + organic acid |
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What element can make long chains, rings and networks? |
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carbon |
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How many electrons are shared in a triple bond? |
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6 e- or 3 pairs of e- |
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What is equilibrium? |
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when forward and reverse reaction rates are equal and the concentration of the reactants and the products remains constant |
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What is Le Chatelier's Principle? |
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that a system in equilibrium , when disturbed, will shift and return to equilibrium |
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What type of bonding gives water an unusually high boiling point? |
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hydrogen bonding |
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What are the 3 types of hydrogen bonds? |
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H-N H-O H-F because of high EN |
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A system in equilibrium, when pressure is increased will shift towards ________ |
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the side with less moles of gas |
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A system in equilibrium, when pressure is decreased will shift towards ________ |
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the side with more moles of gas |