Chemistry Review – Second Semester

 

  1. Draw a periodic table and show where the following groups are by color coding them.
    1. Noble gases – yellow
    2. Halogens – green
    3. Alkali metals – blue
    4. Transition metals – orange
    5. Metalloids – red
  2. Make a dot diagram for the following atoms.
    1. Sodium
    2. Magnesium
    3. Carbon
    4. Oxygen
    5. Neon
  3. What is the atomic number for calcium?
    1. What does this number tell you about a calcium atom?
    2. Combine this number with the atomic mass of calcium and determine how many neutrons are in a calcium atom.
  4. Find the number of protons, neutrons, and electrons in the following atoms.
    1. Chlorine
    2. Gold
    3. Carbon
  5. For the given elements, determine which of the elements in the list behind them they will react with.
    1. Sodium reacts with? – barium, strontium, oxygen, fluorine
    2. Iodine reacts with? – sulfur, bismuth, argon, lithium
    3. Carbon reacts with? – potassium, selenium, krypton, silver
  6. In order to form a stable molecule, how many bonds would each of the following atoms like to form?
    1. Aluminum
    2. Silicon
    3. Bromine
  7.  Balance these equations.
    1. SiO2  +  C  à  SiC  +  CO
    2. CH4  +  O2  à  CO2  +  H2O
    3. NH3  +  O2  à  NO  +  H2O
  8. When you performed the different forms of copper lab, you started with a shiny piece of copper wire and you ended up with a blue-green solution. What happened to the copper atoms during this lab?
  9. Calculate the percent composition of each of the following molecules.
    1. H2O                 % H = _______           % O = _________
    2. Ca(OH)2          % Ca = _______         % O = _________       % H = ______
  10. Calculate the molar mass of the following compounds.
    1. Al(NO3)3
    2. AuO
  11. How many moles are in the following quantities?
    1. 36 grams of water
    2. 6.02 x 1024 atoms of silver
  12. When you built your spectroscope, what was the purpose of having the two razor blades and placing them very close together?
  13. When you did the Qualitative Analysis Lab, why did you only need a couple of drops of each chemical when you were testing the substances?
  14. Name the three parts of the Kinetic Theory. Diagram a balloon and show how each part would affect the balloon.
  15. When you tested reactions in the calorimeter, why did you use the calorimeter; what purpose did it serve?
  16. When you mixed two chemicals in the calorimeter, the temperature on the thermometer went up. Is this reaction exothermic or endothermic?
  17. Decide if these reactions are endothermic or exothermic.
    1. Ice melting
    2. Paper burning
    3. Grass growing
  18. Which is a warmer temperature, 100º Celsius or 150º Fahrenheit?
  19. Why is the Kelvin temperature scale so much different from the other two (Celsius and Fahrenheit)?
  20. If I say that aluminum has a higher heat capacity than iron, what does that mean? How could I apply this knowledge to making cooking pans?
  21. Why is water a good substance to use as a fluid in a calorimeter?
  22. When you performed the fruit cell electrochemistry lab, what was the salt bridge in the system and what was its purpose?
  23. What is the definition of electric current? What units of measure is current measured in?