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 |
