Chemistry Semester II Final Review

Atomic & Nuclear Theory

  1. Describe how each of the following scientists changed the theory of the atom.
  2. Dalton:
  3. Rutherford:
  4. Bohr:
  5. Explain what nuclear forces are.
  6. Determine the stable ion for each of the following elements:

  1. Al:
  2. O:
  3. Na:

  1. Determine the correct full electron configuration for each of the following atoms or ions:

  1. Mg:______
  2. Si:
  3. N3-:______
  4. Na+:______

  1. Describe each of the following types of nuclear decay and the effects of the particle that is emitted can have on people.
  2. Alpha Decay:
  3. Beta Decay:
  4. Gamma Decay:
  5. Finish each of the following reactions:


Periodic Table & Trends

  1. Define each of the following terms:
  2. Atomic Number:
  3. Atomic Mass:
  4. Average Atomic Mass:
  5. Isotope:
  6. Ion:
  7. Ionization Energy:
  8. Atomic Radius/Size:
  9. Electronegativity:
  10. Name and describe the properties of each of the following groups in the Periodic Table:
  11. Group 1 & 2:
  12. Groups 3-12:
  13. Group 17:
  14. Group 18:
  15. Describe how each property changes as you move across and down the Periodic Table.

  1. Atomic Radius/Size:______
  2. Ionization Energy:______
  3. Electronegativity:______

Molecular Theory

  1. Define each of the following:
  2. Covalent Bond:
  3. Ionic Bond:
  4. Metallic Bond:
  5. Octet Rule:
  6. Draw the Lewis Structure for each of the molecules below:

  1. OF2
  2. NO3
  3. NH3
  4. SF6

  1. Calculate the molecular mass of each of the following molecules:

  1. MgCl2
  2. NH3
  3. NaOH
  4. Al2(SO4)3

  1. Convert the following:

  1. 4.5 grams MgCl2 to moles
  2. 2.6 moles NaOH to grams
  3. 2.9 grams OF2 to molecules
  4. 4.9 x 1027 atoms Al to moles

Reactions & Stoichiometry

  1. Balance the following equations:
  2. ___ Mg(s) + ___ HCl(aq)  ___ H2 (g) + ___ MgCl2 (aq)
  3. ___ Al(s) + ___ CuSO4 (aq)  ___ Al2(SO4)3 (aq) + ___ Cu(s)
  4. ___ Fe(s) + ___ O2 (g)  ___ Fe2O3 (s)
  5. Based on the equation below, complete the calculations.

4 Fe(s) + 3 O2 (g)  2 Fe2O3 (s)

  1. How many moles of Fe2O3 can be produced if 2.8 moles of Fe are used?
  2. Calculate the amount of Fe in grams needed to produce 52.9 grams of Fe2O3.

Thermochemistry

  1. Describe or explain the following terms:
  2. Temperature Scales: Celsius, Kelvin
  3. Endothermic:
  4. Exothermic:
  5. Specific Heat:
  6. Enthalpy:
  7. Entropy:
  8. Free Energy:
  9. Heat of Fusion:
  10. Heat of Vaporization:
  11. Phase Changes
  12. Which phase changes are exothermic?
  13. Which phase changes are endothermic?
  14. Calculate the heat required for each of the following situations:
  15. A 5.2 gram sample of iron is heated from 0oC to 50oC. (Specific heat is 0.449 J/gK)
  16. A 55.6 gram sample of iron is cooled from 150K to 125K. (Specific heat is 0.215 J/gK)
  17. Boiling 320 grams of water at 100oC. (Specific heat is 4.186 J/gK)

Acids & Bases

  1. What is the difference between weak acids or bases and strong acids or bases?
  2. If a strong acid and base are mixed together, what are the products?
  3. Calculate the pH:
  4. 2.63 x 10-3 M HCl
  5. 8.36 x 10-9 M HNO3

Solutions

  1. Define the following:
  2. Solution
  3. Solvent
  4. Solute
  5. Complete the following calculations:
  6. Determine the molarity if 2.25 moles of NaCl is mixed into 8.5 L of solution.
  7. Determine how much NH3 is in 4.2 L of a 2.8 M solution.

Equilibrium

  1. Describe the following
  2. Le Chatelier’s Principle
  3. Equilibrium
  4. Determine the direction the following reactions will move towards (reactants or products):
  5. Heat is added to an endothermic reaction (heat is on the left).
  6. 2H2 (g) + O2 (g)  2H2O (l); pressure is added
  7. List at least 4 things that can be done to a reaction to increase the rate of the reaction.

Organic Chemistry

  1. Define the following
  2. Organic Molecule
  3. Polymer
  4. Proteins
  5. Carbohydrates