Semester 1 Exam review:

Use the following electron configuration to answer the questions 1-9:

1s22s22p63s23p63d104s24p3

  1. How many energy rings does the atom contain?
  2. What element is represented?
  3. How many electrons does the atom contain?
  4. What is the atomic number?
  5. How many valence electrons does the element contain?
  6. How many more electrons are needed for an octet?
  7. Write the orbital notation for the element.
  8. The element is found in what group?
  9. The element is found in what period?
  10. How can you determine the number of energy rings an atom has by looking at the periodic table?
  11. What is the maximum number of electrons that can be in the third energy level?
  12. What is the maximum number of electrons that can be in the second energy level?
  13. What is the maximum number of electrons that can be in the first energy level?
  14. What is the maximum number of electrons that can be in the fourth energy level?
  15. Which elements on the periodic table are classified as metalloids?
  16. What are valence electrons?
  17. What is the octet rule?
  18. Why is the period number of an element important?
  19. What is the Aufbau principle?
  20. What is the Pauli Exclusion Principle?
  21. What is Hund’s rule?
  22. Write the electron configuration for the element chromium.
  23. Write the electron configuration for the element Iodine.
  24. What is an ion?
  25. What is a physical property? What is a chemical property?
  26. What is a physical change? What is a chemical change?
  27. Give an example of a physical property for water.
  28. Give an example of a physical change for water.
  29. Give an example of a chemical property for iron.
  30. Give an example of a chemical change for iron.
  31. Discuss the following properties: volume, compressibility, density, conductivity, malleablility, reactivity, freezing, melting, and boiling
  32. Know the difference between homogeneous and heterogeneous mixtures and how they could be separated using filtration, distillation, chromatography, or evaporation.
  33. What are the subatomic particles found in an atom, their individual mass and their individual charges?
  34. Does an atom have a charge? Why or why not?
  35. Does the nucleus of an atom have a charge? Why or why not? If yes, what is the charge?
  36. What was Rutherford’s experiment and what was discovered/learned?
  37. What was Thompson’s experiment and what was discovered/learned?
  38. Explain Bohr’s model.
  39. What is the modern atomic theory. How it differs from Dalton’s atomic theory.
  40. What is the electromagnetic spectrum?
  41. What is the equation for calculating the energy of a wave?
  42. Calculate the energy of a gamma ray photon whose frequency is 5.02 x 1020 Hz.
  43. What is Plank’s constant?
  44. What is the unit for energy?
  45. What is the unit for frequency and define frequency?
  46. What is the unit for Plank’s constant?
  47. What is the unit for wavelength and define wavelength?
  48. What is the unit for speed?
  49. What is the equation for calculating speed of a wave?
  50. A helium-neon laser emits light with a wavelength of 633 nm. What is the frequency of this light?
  51. An FM radio station broadcasts at a frequency of 98.5 MHz. what is the wavelength of the station’s broadcast signal?
  52. What are the 4 states of matter? Describe the molecular motion, the volume, and the shape of each state. Know how the kinetic molecular theory is related to energy phase transitions.
  53. What is the atomic theory?
  54. What is a nuclear reaction/change?
  55. Elements found in group I form what type of ions? Group 2? Groups 3-12? group 13? group 14? group 15? group 16? group 17? and group 18?
  56. Why do atoms bond?
  57. What is an ionic bond?
  58. What is a covalent bond?
  59. Write the orbital notation for selenium and Cr?
  60. Characterize each of the following as absorption or emission: an electron moves from E2 to E1; an electron moves from E1 to E3 and an electron moves from E6 to E3.
  61. In the question above which energy-level change above emits or absorbs the highest energy? The lowest energy?
  62. State what sublevels are would be found in the first 4 energy levels and their location on the periodic table.
  63. Know that spectral lines are the result of transitions between energy spacing levels and be able to calculate energy (E=hv)
  64. What type of bond would form between two elements with a 2.2 difference in electronegativity?
  65. What type of bond would form between two elements with a .2 difference in electronegativity?
  66. Explain the difference between a polar covalent bond and nonpolar covalent bond.
  67. How does lattice energy affect the force of attraction in a bond?
  68. Be able to predict the type of bond that would form between two elements.
  69. Be able to name ionic compounds when given a formula.
  70. Be able to write ionic formulas when given the compound name.
  71. Be able to name covalent compounds when given a formula.
  72. Be able to write formulas when given the covalent compound name.
  73. Explain how temperature affects each state of matter.
  74. What are isotopes?
  75. Describe the parts to an atom: protons, neutrons, and electrons.
  76. Know how to calculate atomic mass unit.
  77. Know where the metals, metalloids, and nonmetals are located on the periodic table.
  78. Review Lewis structures, hydrogen bonds and Van der Waals forces
  79. What is the charge of the nucleus?
  80. Review the steps of the scientific method (know the meaning of the steps) Review your scale.
  81. What is a mass number and what is it used for
  82. What is atomic number and what is it used for
  83. How many grams are in 5.80 moles of calcium?
  84. How many moles are in 2.87 grams of aluminum?
  85. What is amu and when is it used?
  86. How are electrons held outside the nucleus?
  87. Know how models are used by scientist
  88. What is the principle quantum number and angular momentum number
  89. What is molecular composition and give an example
  90. Define temperature