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Flashcards

Chem Test 1

eliza hamilton-jones Chemistry Inglês 94 flashcards

Flashcards do conjunto (94)

  1. 1SI Base Units (Length, Mass, Time, Temperature and Amount of Substance)Physical Measurement
    Meters (m), Kilograms (kg), Seconds (s), Temperature (K), Moles (mol)
  2. 2Tera (T)10^12
  3. 3Giga (G)10^9
  4. 4Mega (M)10^6
  5. 5Kilo (K)10^3
  6. 6Deci (d)10^-1
  7. 7Milli (m)10^-3
  8. 8Micro (Fancy M)10^-6
  9. 9Nano (n)10^-9
  10. 10Pico (p)10^-12
  11. 11Femto (f)10^-15
  12. 12Atto (a)10^-18
  13. 13Volumem^3
  14. 14Speedm/s
  15. 15Accelerationm/s^2
  16. 16Densitykg/m^3
  17. 17FrequencyHz
  18. 181.5 Gal ----> 2.04 Kg ----> 298 K ----> 8.25 S^-1 ---->English
    Derived
    Base Unit
    Derived
  19. 19Significant DigitsDetermines precision of a measurement
  20. 20Qualitative DescriptionsIdentity or Form of a substance
  21. 21Quantitative DescriptionsAmount of substance
  22. 22AccuracyHow close a measurement is to the true value (average)
  23. 23PrecisionHow close measurements of the same item are to each other.
  24. 24Precision in Single Measurements-Determined by measuring device
    -Smaller scale division on the tool gets, the more precise
  25. 25Counting Sig Figs-Zeroes to the right of a number are significant only if the number has a decimal point
    -Zeroes that precede all of the nonzero digits are not significant
  26. 26Multiplying Sig FigsLeast Precise Number (Fewest Sig Figs)
  27. 27Adding Sig FigsThe number of decimal places
  28. 28Density-Used to identify substances
    -Mass per unit volume
    -Intensive property
  29. 29Kelvin273.15 K (Freezes)
    373.15K (Boils)
  30. 30Pure SubstanceElement or Compound
  31. 31MixtureHeterogenous or Homogenous (Solution)
  32. 32Antimony Tin Gold Tungsten MercurySb
    Sn
    Au
    W
    Hg
  33. 33Ca(No3)21 Ca
    2 N
    6 O
  34. 34Law of Conservation Mass (Principle of Mass Conservation)Matter is neither created nor lost (Antoine Lavoisier, quantitative experiment of the reaction of Phosphorus with Oxygen)
  35. 35Law of Definite Proportions (Law of Constant Proportion)Any given compound is composed of definite proportions by mass of its elements
  36. 36Law of Multiple ProportionsFor any 2 different compounds that are composed of the same elements, for a given mass of 1 of the elements, the ratio of the masses of any other element in the compound is a small whole-number ratio.
  37. 37Daltons Atomic Theory-Matter is made up of very tiny, invincible particles
    -Each atom of a particular element has the same mass but the mass of an atom of one element is different from the mass of an atom of any other element
    -Atoms combine to form molecules
    -Atoms of some pairs of elements can combine with each other in different small whole-number ratios to form different compounds
  38. 38Law of DP- All samples of a pure compound have identical proportions by mass
  39. 39Law of MP-Atoms of the same pairs of elements can combine in different small whole-number ratios
    -If mass of one element is held constant, the ratio of the masses of the element must be a whole-number ratio
  40. 40Electron!!lol
  41. 41J.J ThompsonCathode Ray Tube (different substances emitted into identical cathode ray tubes with a charge-to-mass ratio of -1.76 x 10^8 C/g.
  42. 42Dalton AtomIndivisible sphere
  43. 43Thompson AtomNegative charges suspended in a larger sphere of positive charge
  44. 44Single Electron Charge1.60 x 10^-19 C (Millikan)
  45. 453 types of particlesAlpha (positive), Beta (negative), Gamma (neutral)
  46. 46Plum Pudding Model-Rutherford predicted that alpha particles would pass through atoms
    -Alpha particles are small and charged they travel very rapidly
    (Tested by Rutherford, Gieger, Marsden)
  47. 47More PPM-Positive charge and majority of its mass in nucleus
    -Vast majority of atom is empty
    -Protons (equal in magnitude of E-)
    -Neutral atoms contain the same number of protons and electrons
  48. 48Subatomic ParticlesProton (+1)
    Electron (-1)
    Neutron (0)
  49. 49Atomic NumberZ
  50. 50Protons-The atomic number
    -Determines an elements identity
  51. 51Isotopes-2 atoms with the same number of protons but different number of neutrons are isotopes of the same element
    -Isotopes have the name atomic #, but have different masses bc of the different # of neutrons
  52. 52Mass NumberTotal number of protons and neutrons!!!!
    The Number of neutrons is the difference between the mass # and the atomic #
    (Symbols and names for isotopes include the element name or symbol and the mass #)
  53. 53Ions-Atoms can gain or lose electrons to form charged particles called ions
    -Cation (+)
    -Anion (-)
  54. 54Atomic Masses-Weighted average of the actual masses of all naturally occurring isotopes
  55. 55Artificial Isotopes and Elements-Do NOT have atomic masses
    -Do not contribute to the atomic mass of an element
  56. 56Periodic Table-Similar chemical properties are grouped together (vertical)
    -Elements are arranged horizontally in order of increasing atomic number
  57. 57Noble GasColorless, odorless, mostly inert (discovered later)
  58. 58Row (------)Period
  59. 59Column (|)Group or Family
  60. 60Transitional ElementsLanthanoids, Actinides
    (3 to 12)
  61. 61Main Group ElementsGroups 1, 2 and 13-18 (common and predictable)
  62. 62MetalsShiny, Malleable, Ductile and Conductors of heat and electricity
  63. 63CompoundsChemical formulas form to combine elemental symbols and numerical subscripts to represent compounds
  64. 64Chemical ForumlaShow a formula unit of a compound (symbol is the element, subscripts tell how many atoms)
    -Indicates the # of each type of atom
    -Only indicates the ratio of the atoms of each type
  65. 65Formula UnitBasic ratio of the atoms in a compound
    (1 Formula unit=1 Molecule (basic ratio ONLY))
  66. 66Molecular CompoundsExist as individual particles made up of bonded atoms (molecules)
    (Contain nonmetal atoms bonded by covalent bonds)
  67. 67Ionic CompoundExist as an extended 3D lattice structure of repeating pattern of atoms (no distinct molecules)
    -Held together by ionic bonds
    -Composed of metal and nonmetal atoms
  68. 68Diatomic MoleculesHydrogen, Nitrogen, Oxygen, Flourine, Chlorine, Bromine, Iodine
  69. 69AllotropeDifferent molecular forms of an element
    (O2 is molecular oxygen, O3 is ozone)
    (Carbon ---> diamond, graphite, nanotubes, fullerenes)
  70. 70Formulas for Ionic Compounds-Single atoms from monoatomic ions
  71. 71Binary Ionic Compounds-Form when metal atoms combine with nonmetal atoms (metal (cations) transfers electrons to nonmetals (anions))
  72. 72Common Monoatomic IonsHELP
  73. 73Binary Ionic Compound Formulas-Electrically Neutral
    -Obtain Charges
    -Find LCM
    -Use subscripts to obtain charges equal to LCM and achieve a charge of 0
  74. 74Polyatomic IonsGroups of 2 or more bonded atoms that have lost of gained electrons, and have an overall net charge. (Most are anions)
    -LOOK
  75. 75AcetateC2H302- or CH3COO-
  76. 76BromateBrO3-
  77. 77CarbonateCO3 2-
  78. 78Writing Formulas with Polyatomic Ions1. Obtain ion charges
    2. Use LCM to balance charges
    -Enclose ion in () and place subscripts outside
  79. 79The MoleCounting very tiny!
    A mole contains Avogadro's # of formula units (6.022 x 10^23 = 1 mol of He)
  80. 80Avogadro's Number6.022 x 10^23
    1 mol
  81. 81Individuals in a compound-Once you know the # of moles of each element, multiply that value by Avogadro's number to determine the # of atoms of each element present. ['[
  82. 82Molar MassAM= the avg. mass of an atom
    Molecular Mass= avg. mass of a molecule
    Formula Mass= avg. mass of a formula unit (any substance)
    Molar mass= the mass of any of the above, using the same numerical value, g/mol
  83. 83Molar Masses of atomsThe atomic mass of each element is the average mass of 1 atom, expressed in amu
    (By definition, there are Na atomic mass units in a gram (equation))
    -The molar mass of an element in g/mol is numerically equal to the elements atomic mass in u
  84. 84Atomic Mass of C is 12.011 uMolar Mass of C is 12.011 g/mol
  85. 85The mass of 1 mole of atomsAtomic mass expressed in grams
  86. 86Molar Masses of CompoundsThe sum of the molar masses of all of the atoms in a formula unit of the compound
  87. 87Empirical Formula-Contains simplest whole number ratio of atoms in the compound
    -The actual chemical formula is either the same as the empirical formula or a whole number multiple of the EF
  88. 88Writing Empirical Formulas1. Convert percent data
    2. Convert mass of each element into moles
    3. Divide moles of all elements by smallest # of moles
    4. If not whole numbers, multiply by factor
    5. Insert # of subscripts
  89. 89Ionic EF-Identified by Ef's
    -Some polyatomic Ions contain even #'s of atoms and cannot be reduced to simplest ratio.
  90. 90Covalent EF-Used to determine molecular formula
    EF: CH20
    MF: C6H12O6
  91. 91Molecular FormulasGives the actual number of atoms of each element in one molecule of a covalent compound
  92. 92Empirical Formula and Molecular FormulaMF is always a multiple of EF
  93. 93Combustion AnalysisUsed to determine EF of a compound containing C, H and O
    (all C ends up as CO2, all H ends up as H2O)
    -The masses of CO2 and H2O are measured and used to determine mass of C and H in the original sample)
  94. 94—

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Chemistry FlashCards sobre Chem Test 1 , criado por eliza hamilton-jones em 25-09-2023.
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