Chemistry Exam

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Chemistry Exam
2014-06-02 19:42:49
Chemistry Exam
Chemistry Exam
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  1. What are physical properties of an object
    Color and odor, melting and boiling points, and malleability and hardness are considered physical properties of a substance.
  2. What is absolute zero in C
    -273.15 is the temperature of absolute zero measured in C.
  3. What is 987 mg in grams
    987 milligrams is expressed as .987g.
  4. Density of object having a mass of 8g and volume of 25cm
    The density is .32g/cm^3.
  5. Dalton's atomic theory
    The principles of Dalton’s atomic theory are: 1.)all elements are composed of tiny indivisible particles called atoms, 2.)atoms of the same element are identical, the atoms of any one element are different from those of any other element, 3.) atoms of different elements can physically mix together or can chemically combine in a simple whole- number ratio to form compounds, and 4.) chemical reactions occur when atoms are separated, joined, or rearranged. Atoms of one element, however, are never changed into atoms of another element as a result of a chemical reaction.
  6. What scientists discovered subatomic particles
    Thompson discovered the electron in 1897. Goldstein discovered the proton in 1886. Chadwick discovered the neutron in 1932.
  7. Difference between a substance and mixture
    In a substance, the atoms are chemically combined, while not in a mixture, Substance has fixed composition. Mixture has varying
  8. What must be done to be certain a chemical change took place
    Check the composition of the new matter.
  9. What is true of chemical reactions
    The total mass of the reactants equals the total mass of the products.
  10. electron config of potassium
    1s^2 2s^2 2p^6 3s^2 3p^6 4s^1
  11. What is the energy of a photon having a frequency of 4x10^7 hz
    3x10^-26 J is the approximate energy of a photon having a frequency of 4x10^7.
  12. If the position is known then
    The velocity can also not be known.
  13. The periodic table is arrange in order of increasing
    atomic number
  14. What are the representative elements
    Al, Mg, and Li contains only representative elements.
  15. The study of the composition of matter
    Chemistry studies the composition and structure of matter.
  16. What measurement is the most precise
    2, 2.5,and 3 are the most precise measurements.
  17. What are isotopes
    8438M, 8638M, 8738M are isotopes of the same element.
  18. what causes water to have a bent shape
    According to the VSEPR theory, the repulsion between electron pairs causes molecular shapes to adjust so that the valence-electron pairs stay as far as possible.
  19. What causes hydrogen bonding
    Hydrogen bonding is caused by the bonding of a covalently bonded hydrogen atom with an unshared electron pair.
  20. Name of H2SO3
    The name for H2SO4 is Sulfurous acid.
  21. formula for sulfur hexafloride
    The correct formula for sulfur hexafluoride is SF6.
  22. number of mols in 432 Ba
    The number of moles in 432g of Ba(NO3) is 1.65.
  23. Number of mols in 500 l of He
    The number of moles in 500L of He gas is 22.
  24. Electronegativity in the periodic table?
    Electronegativity values decrease from top to bottom per group.
  25. Electrons that occupy the highest energy level
    The name given to electrons of the highest occupied energy level is valence electrons,
  26. the octet rules states
    The octet rule states that atoms tend to have eight electrons in its valence shells.
  27. An ionic compound is called a
    A compound held together by ionic bonds is called a salt.
  28. Formula for sodium nitride
    Na3N is the formula unit for sodium nitrate.
  29. formula for aluminum oxide
    Al2O3 is the formula unit for aluminum oxide.
  30. formula for sodium sulfate
    NaSO4 is the formula unit for sodium sulfate.
  31. formula for potassium sulfide
    K2S is the formula unit for potassium sulfate.
  32. what is the basis of a metallic bond
    The basis for a metallic bond is the attraction of metal ions to mobile electrons.
  33. A molecule with a single covalent bond
    A molecule with a single covalent bond is Cl2.
  34. what is the empirical formula
    The empirical formula is C2H7N.
  35. According to kinetic theory collision between gases are
    According to kinetic theory, collisions between molecules in a gas are perfectly elastic.
  36. Standard conditions of gases
    Standard conditions when working with gases are defined as 0K and 101.3 kPa.
  37. the smallest group of particles that remain in crystals
    The smallest group of crystals that retains the shape of the crystal is called an unit cell.
  38. How are pressure and temp shown on a phase diagram
    The conditions of pressure and temperature at which two phase exist in equilibrium are indicated on a phase diagram by a line separating the phases
  39. What volume will the gas occupy at 84.6 kpa
    A gas that occupies a volume of 2.4 L at 14.1 kPA will occupy a volume of 14.1 L at 84.6 kPa
  40. What volume does a gas occupy at 70C
    the volume is 36 ml
  41. Balance
    _1_AlCl3 + _3_ NaOH---> _1_Al(OH)3 + _3_ NaCl
  42. Decom of lead
    The equation is PbO2->Pb+O2.
  43. What type of reaction with mg(s)
    mg(s)+2hcl(aq)->mgcl2(aq)+h2(g) is a single replacement reaction.
  44. How many grams of oxygen are prduced when 11.6 g of No2 are formed
    the formula produces 5.00 grams of oxygen.
  45. How many mols of H3PO4 are produced
    .the formula produces one mol of H3PO4.
  46. How many grams of metallic copper can be obtained
    21.2 grams of metallic copper are formed.
  47. what is the particular pressure of O2
    the particular measure of O2 is 6 mols
  48. the bonds between adjacent water molecules are
    bonds between adjacent water molecules are hydrogen bonds.
  49. Size of colliods
    colloids range in size from 1-1000mm.
  50. To increase the solubility of a gas what would have to increase?
    the pressure would be increased to 2.7.
  51. Rest
    51.the molarity is 3.52.the molality is 1.7m53.weak electrolytes are ionic compounds that partially dissociate in water.54.Activation energy is the minimum energy that colliding particles must have in order to react.55.the temperature will absorb the heat when increased from equilibrium.56. In a reaction that makes more than it consumes, the reaction makes more reactants as the pressure increases.57. Entropy is the measure of disorder of a system.58. Acids taste sour, can change the color of an acid-base, and can be strong or weak electrolytes in an aqueous solution.59. Bases taste bitter, will change color of an acid-base, and can be strong or weak electrolytes in aqueous solutions.60. The molality of a solution of water and KCl if the freezing point is -30 is .8.61.The quantity of heat required to change the temperature of 1 g of a substance by 1 degree Celsius is defined as specific heat.62. 2.62 joules of energy are needed to warm 4.37 g of silver by 2.5 degrees Celsius.63. -218 kj/mol is the standard heat of reaction.64. -296.7 kj/mol is the change in enthalpy for sulfur dioxide with oxygen.65. LiOH is the Arrhenius base because it gives off hydroxide ions when dissociated in water.66. A dry cell is a commercial voltaic cell in which the electrolyte is a moist paste; despite their name, the compact, portable batteries used in flashlights are dry cells67. In a hydrogen-oxygen fuel cell, oxygen diffuses through the cathode. Reduction always takes place at the cathode. Oxygen is reduced.68. Carbon has 4 valence electrons.  69. To complete the following equation, a beta particle is required147N+0-1e 146C + 11H70. Uranium-238 can be the most useful in dating objects thought to be millions of years old.71. A reaction in which small nuclei combine to form a heavier nuclei is called nuclear fusion.72.Alkanes are hydrocarbons that contain single bonds73.Lewis acids accept electron pairs to form a covalent bond. 74.H20 can act as an acid and a base.75. H20 is the oxidizing agent76. The Cu electrode is negative.77. In a voltaic cell, electrical energy is produced by spontaneous redox reactions within the cell.78. A description for a solution with a hydroxide-ion concentration of 1*10-4M is acidic. 79. The change in atomic number when an atom emits an alpha particle is -2.80. The change in atomic number when an atom emits a beta particle is that it decreases by 1. 81.The atomic number is unchanged when gamma radiation is emitted.82.A reduction reaction occurs when iron oxide becomes iron.83. Cu=Cu2++2e- is an oxidation reaction.84. In 2Na+SNa2S, the reducing agent is Na.  85. The most important way to classify organic compounds is by their functional groups.86.The fundamental unit of life is the atom.87. The two products of photosynthesis are oxygen and glucose. 88 .Peptide bonds are between carbonyl groups89. To complete the nuclear reaction, an alpha particle is needed. 22286Rn 21884Po + 42He90. To solve the equation, Chromium-56 is needed. 5625Mn5624Cr+0-1e.