Chem Final

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Chem Final
2011-12-06 15:29:44
Chem 101 Final

Exams 2,3,4, and 5
Show Answers:

  1. Which of the following elements has an atomic number of 4?
    A) Be
  2. Which of the following elements has only 12 protons?
    C) Mg
  3. What is the atomic symbol for silver?
    C) Ag
  4. Nonmetals are located where on the periodic table?
    A) right side
  5. Group 1A elements are also called:
    B) alkali metals.
  6. Group 7A elements are also called:
    B) halogens
  7. Mg is a member of which family?
    D) alkaline earth metals
  8. Xe is a member of which family?
    D) noble gases
  9. Ions are formed when atoms
    A) gain or lose electrons.
  10. When an atom gains an electron, the resulting particle is called
    A) an anion
  11. What is the charge on the barium ion?
    C) 2+
  12. How many protons and electrons are present in O2-?
    C) 8 protons and 10 electrons
  13. How many electrons would be in a -2 charged anion of sulfur?
    A) 18
  14. Isotopes are:
    B) atoms of the same element that have different number of neutrons.
  15. An atom of a carbon-14 isotope would contain
    B) 6 protons, 8 neutrons and 6 electrons
  16. An atom that has the same number of neutrons as 138/56 Ba is:
    D) 136/54 Xe
  17. When elements combine to form compounds,
    A) their properties change completely.
  18. How many carbon atoms are in the formula
    D) 3
  19. Which formula shows the proper use of parentheses?
    A) Ca(NO3)2
  20. How many of each type of atom are there in the formula (NH4)2HPO4?
    D) N = 2, H = 9, P = 1, O = 4
  21. Carbon is considered which of the following?
    D) atomic element
  22. Fouorine is considered which of the following?
    D) molecular element
  23. What is the formula for an ionic compound made of magnesium and sulfur?
    D) MgS
  24. The ionic compound that forms between potassium and oxygen is
    A) K2O
  25. What is the name of Ca(NO3)2
    C) calcium nitrate
  26. Which formula shown is incorrect for the name given?
    C) lithium sulfate: LiSO4
  27. The charge of a vanadium ion in the compound V2O5 is:
    C) 5+
  28. What is the name of the molecular compound SO3?
    B) sulfur trioxide
  29. What is correct name of the compound whose formula is BF3?
    C) boron trifluoride
  30. What is the formula mass for potassium nitrate?
    C) 101.10 amu
  31. What is the correct value for Avogadro's Number?
    C) 6.022 x 1023
  32. How many atoms are in 5.8 moles of He?
    D) 3.49 x 1024
  33. How many atoms are in 1.50 moles of fluorine gas?
    C) 1.81 x 1024
  34. One mole of boron has a mass of ______g.
    C) 10.811
  35. One mole of oxygen gas has a mass of _____g.
    C) 32.0
  36. What is the mass in grams of 5.40 moles of lithium?
    D) 37.5
  37. How many moles of iron are contained in 1.75 kg of iron?
    C) 31.3
  38. How many hydrogen atoms are in 35.0 grams of hydrogen gas?
    D) 1.05 x 1025
  39. What is the mass of 1.56 x 1021 atoms of magnesium in grams?
    B) 0.0630
  40. The mass of one mole of carbon dioxide is _______g.
    A) 44.01
  41. What is the mass in grams of 1 mole of P2O5?
    A) 141.96 g
  42. Which of the following has the lowest number of atoms?
    C) (NH4)2Cr2O7
  43. The molecular weight of Ca3(PO4)2 is _______.
    D) 246
  44. If 3.011 x 1023 molecule have a mass of 20.04 grams, what is the molar mass of this substance?
    C) 10.02 g/mol
  45. One mole of amonium nitrate contains:
    D) 2 moles of nitrogen.
  46. What is the mass percent of chloride in hydrochloric acid?
    D) 97.2
  47. The empirical formula of a compound:
    C) indicates the simplest ratio of atoms in the compound.
  48. Which of the following is already in its empirical forrmula?
    B) C5H12O2
  49. The chemical formula CH2O can be classified as:
    B) empirical, possibly molecular.
  50. What would the empirical formula be for the molecular compuond C6H9O4?
    E) none of the above
  51. A reaction which forms a gaseous product is an example of a _________.
    D) gas evolution reaction
  52. A reaction which forms a solid product is an example of a ________.
    D) precipitation reaction
  53. When the equation, __N2 + __H2 ---> __NH3 is balanced, the coefficient of hydrogen is:
    D) 3
  54. What are the coeffecients for the following reaction when it is properly balanced?
    __HCl + __Mg ----> __MgCl2 + __H2
    C) 2, 1, 1, 1
  55. What are the coefficients for the following reacation when it is properly balanced?
    __nitrogen monoxide + __carbon monoxide --> __nitrogen + __carbon dioxide
    A) 2, 2, 1, 2
  56. An aqueous solution is:
    B) water with another compound dissolved in it.
  57. Which of the following compounds is INSOLUBLE?
    B) magnesium phosphate
  58. Which of the following compounds is SOLUBLE?
    C) aluminum sulfate
  59. The compoud sodium sulfate is soluble in water. When this compound dissolves in water, which ion isted below would be present in the solution?
    A) SO42-
  60. In writing the chemical equation for a precipitation reaction, what abbreviation of the physical state must appear with one of the products?
    A) (s)
  61. Which compound would not form ions in the complete ionic equation?
    B) PbI2
  62. What is the correct complete ionic equation?
  63. What is the correct net ionic equation?
  64. What is the net ionic equation for the reaction of hydrochloric acid with potassium hydroxide?
    D) H+ + OH- ----> H2O
  65. What type of a reaction occurs when a hydrochloric acid solution is mixed with a sodium bicarbonate solution?
    B) gas evolution
  66. What type of reaction occurs when potassium metal reacts with fluorine gas?
    D) oxidation-reduction
  67. Methane gas (CH4), on complete combustion in air, produces:
    A) 1 and 3 only
  68. What type of reaction is the generic equation
    A + B ---> AB
    A) synthesis/ combination
  69. What type of reaction is the generic equation
    AB + CD ---> AD + CB
    C) double-displacement
  70. How many moles of water are made from complete reaction of 1.4 moles of hydrogen gas?
    C) 1.4
  71. How many grams of water are made from the reaction of 4.0 grams of hydrogen gas?
    A) 36
  72. When 4.50 mol of H2O are formed, the amount of NO formed is
    C) 3.00 mol.
  73. The theoretical yield of a reaction is 75.0 grams of product and the actual yield is 42.0g. What is the percent yield?
    B) 56.0
  74. How many moles of water are neededd to react with 2.2 miles of Li2O?
    D) 2.2
  75. If the theoretical yield of the reaction below corresponds to 99.2 g and the actual yield was 60.9 g, calculate the percent yield.
    B) 61.4
  76. Starting with 156g of Li2O and 33.3 g H2O, decide which reactant is present in limiting quantities.
    B) water
  77. The balanced equation involves the corresponding coefficients _________.
    A) 1:3:2:3
  78. The theoretical number of carbon dioxide moles produced from 3 moles C2H6O is _______.
    A) 6
  79. The theoretical number of moles of water produced from 2 moles of C2H6O is _______.
    A) 6
  80. What is the theoretical mass of carbon dioxide produced from one mole of C2H6O?
    C) 88g
  81. The distance between adjacent wave crests is called
    C) wavelength
  82. The number of cycles of a wave that passes a stationary point in one second is called its
    C) frequency.
  83. Which color of the visible spectrum has the longest wavelength (750 nm) ?
    B) red
  84. How are wavelength and frequency of light related?
    A) Wavelength increases as the frequency decreases.
  85. Which form of electromagnetic radiation has the shortest wavelength?
    A) Gamma Rays
  86. When sunglight is passed through a prism, what is observed?
    C) continuous spectrum
  87. The principal quantum number (n):
    C) specifies the principal shell of the orbital
  88. How many subshells are there in the n = 4 principal shell?
    C) 4
  89. The subshell leter:
    B) specifies the 3-D shape of the orbital.
  90. The n = ____ principal shell is the lowest that may contain a d-subshell.
    D) 3
  91. Which subshell letter corresponds to a 4-leaf clover orbital pattern?
    D) d
  92. The "d" subshell can hold a maximum of ___ electrons.
    B) 10
  93. How many electrons can exist in an orbital?
    D) 2
  94. Which element is represented by the electron configuration 1s2 2s2 2p2?
    B) C
  95. What is the electron configuration for Kr?
  96. How many core electrons are in a chlorine atom?
    D) 10
  97. Which Lewis structure below correctly represents KCl?
    B) K+ [:Cl:]-
  98. Lewis theory predicts that the formula of a compound formed between bromine and aluminum is:
    B) AlBr3
  99. When a nonmetal bonds with a nonmetal
    D) all of the above are true
  100. What is the correct Lewis structure for water?
    A) H-O-H
  101. What is the correct Lewis structure for Br2?
    C) :Br - Br:
  102. The Lewis structure for carbon monoxide is :C three O:
    This structure shows
    B) 2 lone pains and 3 bonding pairs.
  103. Which sequence below represents the proper order of increasing bond strengtrh?
    B) single < double < triple
  104. The correct Lewis structure for BF3 would have exactly:
    C) no double bonds
  105. What is the electron geometry if you have 4 electron groups around the center atom?
    A) tetrahedral
  106. What is the molecular geometry of PH3?
    A) trigonal pyramidal
  107. Which substance listed below is a polar molecule?
    B) Cl2O
  108. Which molecule listed below is a nonpolar molecule?
    All of the compounds
  109. Which compound below will dissolve in water?
    B) NH3