Chemistry Final Review – Flashcards
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| Scientific Method |
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| 1. Make Observations 2. Hypothesize 3. Test Hypothesis/Experiment 4. Develop Theories |
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| Theory |
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| a statement not scientifically proven, studied over a long period of time |
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| Law |
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| proven through mathematics and science |
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| Mass |
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| tells how much matter is in an object, never varies |
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| Volume |
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| a measure of the space occupied by an object |
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| Extensive Properties |
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| amount of matter |
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| Intensive Properties |
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| type of matter |
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| Solid |
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| vibrates in place, still, close together, can't be compressed, definite shape and volume |
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| Liquid |
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| particles moving past each other, no set place, in motion, no definite shape, definite volume |
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| Gas |
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| a form of matter that takes both the shape and volume of its container, move wildly, bounce of one another, very separated |
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| Heterogeneous |
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| composition different, not alike throughout |
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| Homogeneous |
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| composition same, alike throughout |
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| Separation of Magnetism |
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| separations of different elements with magnets, physical change |
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| Separation of Solubility |
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| dissolving ability to separate elements, physical change |
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| Separation of Phase Change |
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| changing one element's phase, change from solid to liquid or liquid to gas of one element only, physical change |
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| Rusting |
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| Rusting one element in order to separate |
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| Burning |
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| Burning one element in order to separate |
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| Rotting |
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| Rotting of one element in order to separate |
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| How many Significant Figures: 104,000 |
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| three, zero's act as place holders |
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| How many Significant Figures: 104,000. |
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| six, all significant before decimal point |
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| How many Significant Figures: 104,000.0090 |
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| ten, after decimal all numbers significant |
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| How many Significant Figures: 0.00090 |
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| 2, must be a number before decimal point in order for zero's to be significant |
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| How many Significant Figures: 0.0009010 |
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| four, all zero's before nin are not significant |
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| SI Unit Kg |
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| Kilograms, mass |
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| SI Unit sec |
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| Seconds, time |
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| SI Unit m |
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| Meter, distance |
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| SI Unit N |
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| Newtons, force |
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| SI Units J |
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| Joules, energy |
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| SI Cal |
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| Calorie, energy, Cal = 1 food cal |
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| SI cal |
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| Calorie, energy, 1000 cal = 1 Cal |
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| SI Unit Pa, Kpa, ATM, mmHg |
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| Pascal, Kilopascal, Atmosphere, units of Pressure |
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| Kilo |
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| 1000 |
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| Milli |
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| + 1,000,000 |
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| Micro |
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| - 1,000,000 |
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| Centi |
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| - 100 |
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| 1000 m = |
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| 1m3 |
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| 1000 mL = |
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| 1 L |
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| Distillation |
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| separates mixutures with boiling, different elements boil at different temperatures, one boils the other does not, separates |
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| (O2 + 2H2 = ...) Mixture + Electrical Spark = |
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| (2H20) Compound |
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| Law of Conservation of Matter |
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| matter can't be created/destroyed, change one form to another, Lavoisier |
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| Democritus |
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| Atmos, believed atoms were indivisible and indestructible |
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| Dalton's Atomic Theory |
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| 1. all elements composed of atoms 2. atoms the atoms of same element are identical 3. atoms of different elements can physically mix together or combine into compounds 4. chemical reactions occur when atoms are separated joined or rearranged |
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| Scientific Notation: 0.00059 |
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| 5.9 x 10^-4, move decimal to the right, negative exponent |
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| Scientific Notation: 59000.0 |
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| 5.9 x 10^4, move decimal point to the left, positive exponent |
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| D = m/v |
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| Density = mass/volume |
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| D = m/v + change in heat = |
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| d = m/V (volume bigger, density smaller) |
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| JJ Thompson |
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| Cathode Ray Tube, discovered electrons, atom with only electrons scattered, 1/1840 of an amu |
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| Proton (H+) |
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| mass of 1 amu |
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| Neutron (n) |
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| mass of 1 AMU |
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| Rutherford |
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| Gold Foil Experiment, discovered the nucleus |
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| Mass # |
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| # protons (H+) + # neutrons (n) |
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| Isotopes |
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| Atoms of same elements with different mass |
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| SI Unit of Temp |
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| K = C + 273 |
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| Aufbau |
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| lowest energy level to highest |
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| Pauli Exclusion Principle |
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| no more than 2 per orbital, opposite signs |
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| Hund's Rule |
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| electrons occupy orbitals of the same energy in a way that makes the # of electrons w/ the same spin direction as large as possible |
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| Bohr proposed... |
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| an electron is found only in specific circular paths, or orbits, around the nucleus |
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| Quantum |
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| the amount of energy required to move an electron from one energy level to another |
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| In the Bohr Model, the higher the energy levels... |
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| the closer they are together |
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| C = ?V |
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| Speed = Wavelength x Frequency |
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| High frequency = |
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| small wavelength |
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| Low frequency = |
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| long wavelength |
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| Metals |
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| shiny, solid, malleable & ductile, dense, conduct heat and electricity |
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| Non Metals |
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| dull, poor conductors, brittle |
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| Covalent Bonds |
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| bond formed by the sharing of electrons between atoms |
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| Covalent Bonds need ... |
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| Octets (8) |
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| Ionic Bond |
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| Non Metal + Metal |
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| Metallic Bond |
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| Metal + Metal |
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| Covalent Bond |
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| Nonmetal + Nonmetal |
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| Electronegativity |
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| the ability of an atom to attract electrons when the atom is in a compound |
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| Electronegativity Chart |
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| Covalent = 0 - 0.4 Mod Polar = 0.4 - 1.0 Very Polar = 1.0 - 2.0 Polar = + 2.0 |
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| Linear |
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| O = C = O CO2 |
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| Triangular Planar |
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| BH3 H | B / H H |
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| Pyramidal |
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| NH3 H-N-H | H |
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| Bent |
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| H2O O / H H |
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| Tetrahedron |
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| CH4 H | H-C-H | H |
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| Diatomic Gases |
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| H2, N2, O2, F2, Cl2, Br2, I2 |
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| Hydrogen Bonds |
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| attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom |
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| Van der Waals Forces |
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| 2 weakest attractions between molecules, consist of dipole interactions and dispersion forces |
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| Dipole interactions |
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| occur when polar molecules are attracted to one another |
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| Dispersion Forces |
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| the weakest of all molecular interactions, caused by the motion of electrons |
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| -IDE |
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| Less Oxygen, (P) |
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| -ITE |
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| Moderate Oxygen (PO3) |
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| -ATE |
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| Most Oxygen (PO4) |
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| Monotomic Ion |
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| A monatomic ion is simply an ion consisting of one element like: Na+ or Au+3, or Zn+2, or Al+3 |
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| Polyatomic Ion |
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| A polyatomic ion is something consisting of more than one element like: SO4-2, or NO3-, or NH4+, or NCS- |
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| Ca^+3 PO4^-3 |
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| Ca3 (PO4)2 |
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| Cation |
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| any atom or group of atoms with a positive charge |
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| Anions |
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| any atom or group of atoms with a negative charge |
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| Product |
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| a substance produced in a chemical reaction |
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| s |
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| solid |
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| l |
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| liquid |
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| g |
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| grams |
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| aq |
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| aqueous |
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| yield |
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| result |
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| catalyst |
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| a substance that increases the rate of reaction by lowering the activation-energy barrier |
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| Reactant |
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| a substance present at the start of a reaction |
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| Excess Reagent |
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| a reagent present in s quantity that is more than sufficient to react with a limiting reagent; any reactant that remains after the limiting reagent is used up in a chemical reaction |
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| Skeletal Equation |
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| unbalanced equation |
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| Balanced |
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| equal on left side and right |
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| Decomposition |
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| equation A+B=AB |
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| Synthesis/Direct Combo |
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| equation AB - A + B |
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| Single Replacement |
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| equation A + BC - AC + B |
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| Mg + CuSO4 -- MgSO4 + Cu |
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| Mg is higher on the activity series than Cu, reaction will take place |
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| 2Na + CuSO4 - MgSO4 + Cu |
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4 g CuSO4 x 1 mol/159g CuSO4 x 2 mol Na/1 mol CuSO4 x 23 g Na/1 mol Na = ____ g Na |
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| Stoichiometry |
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| that portion of chemistry dealing with nimerical relationships in chemical reactions |
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| Find Limiting Reagent |
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| 1. amount of an element in the equation 2. multiply x 1 mol of the same element/mass of that element ex) CuSO4 - Cu = 63 S = 32 Ox4 = 64 ---- 159 g 3. multiply by coefficient of the other element/coefficient of original element 4. multiply by mass of the other element/1 mol of the other element 5. multiply all top factors and then divide by bottom 6. find result - more than original amount? not the limiting reagent. less than original amount? it IS the limiting reagent. |
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| Solute |
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| Substance that is dissolved in a solution |
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| Solution |
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| a homogeneous mixture of two or more substances. |
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| Solvent |
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| The component of a solution that is present in the greatest amount. Ex) Saltwater, salt is solvent |
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| M = mol/L |
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| Molarity = moles of solute/liters of solution |
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| Molarity Equation |
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| 1. mass of element/volume of element ex) 465 gNa/50 mL Na 2. multiply by 1 mol/mass of element 3. multiply amount mL in 1L(1000 mL)/1L 4. multiply top factors and divide by bottom 5. find answer |
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| % Yield |
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| Actual Yield/Theoretical Yield x 100 |
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| Theoretical Yield |
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| Same procedure as limiting reagent, new element |
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| How many grams of KOH are required to make 250.0 mL of a 6.0 M solution of KOH? |
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| 250 mL x 1 L/1000mL x 6.0 mol KOH/1L x 56.1 g KOH/1 mol KOH = 84 g KOH |
