• Quiz  1

  1.  Explain the difference between accuracy and precision.
  2. Name the SI units used in Chemistry and tell me why we use them.

  3. Convert 100l to dl.

  4. Convert 0.0123mg to kg.

  5. What is 0.000123 and 109809.00 in scientific notation?

  6. Explain what Kelvin is and convert 15.7 °C to Kevlin.

  7. How much Carbon is in 7.86 Mols?

  8. Why do we use the scientific method?

  9. Create your own Hypothesis and experiment and results. Make a graph of your results.

  10. Why do we use significant figures? How many significant figures are in: 9.866, 0.098652 and 9520? Round these numbers off to three significant figures.

  • Quiz 2 

  1. What is a molecule? Give me an example of one.

  2. Where do we find protons? What is their charge? What is their mass?

  3. Electrons are to be found in?

  4. Give me two (or more) physical properties of water.

  5. When a molecule changes chemically – what happens to its physical properties?

  6. When you remove a neutron from an atom – what do you get?

  7. When Milk turned into plastic – what happened to the Casein molecule?

  8. Explain to me what intensive properties are? Give me examples.

  9. Explain to me what extensive properties are? Give me examples.

  10. Draw me a picture of what an atom with six electrons looks like.

  • Quiz 3

  1. What did Dalton find about the atom?

  2. What did Thomson find about the atom?

  3. What experiment did Thomson do? And how does this show us his results?

  4. What did Rutherford say about the atom?

  5. What experiment did Rutherford do? And how does this show us his results?

  6. What did Bohr say about the atom?

  7. What did Heisenberg say about the atom?

  8. Give me 5 known facts about the atom that we have today.

  9. How do these scientists inspire us?

  • Quiz 4

  1. The electron exist as both a ….. and …….

  2. What experiment shows this? Explain it in your own words? Hint: Scientists shot electrons through double slits.

  3. Why does the Periodic Table exist?

  4. What does the ATOMIC NUMBER tell us?

  5. What does the element symbol tell us?

  6. What does the ATOMIC MASS NUMBER tell us?

  7. Draw Four elements of your choice and show me these three (Q 4,5,6) on each.

  8. What is ionization energy and why does it increase from left to right of a period?

  9. What is electron affinity and why does it increase from left to right of a period?

  10. What does a group number tell us and Why does atomic radius increase down a group?

  11. Draw me a periodic Table and show me all the trends in it.

  • Quiz 5

  1.  Why was the Periodic table made?

  2. Each elemental block contains three bits of information – what are they?

  3. What is the symbol for Helium, Calcium, Hydrogen, Carbon, Sulfur, Argon, Fluorine, Magnesium and Oxygen?

  4. How many electrons does (neutral) B, Ca, C, Li, Be, Fe, Zn, Cl, P, N and Ti have?

  5. What is the atomic mass of Argon, Neon, He, Na, Potassium, Arsenic and Beryllium? Then tell me how many neutrons (roughly) these elements have.

  6. What are valence electrons?

  7. What do valence electrons do?

  8. What four bits of information does the Periodic Table tell us? (Hint: Groups is 1 of them)

  9. What elements in group 2, 3, 6 and 7 have the smallest radius and why?

  10. Will Fluorine want more electrons then Bromine? Tell me why you give me your answer. 11.) Will Be loose electrons easier then Ca? Tell me why you give me your answer.

  11. Are periods the horizontal or vertical lines in the periodic table?

  12. Is the atomic radius of – Chlorine bigger then Na? Why? – Nitrogen bigger then Boron? Why? – Aluminum smaller then Mg? Why? – P smaller then Silicon? Why?

  13. Is more energy needed to remove an electron from Neon or Oxygen? Why?

  14. Will: – Be want electrons more then F? Why? – Aluminum want electrons less then P? Why? – Nitrogen want electrons less then F? Why?

  15. Is Oxygen more a non-metal then Ir?

  16. What do the different blocks tell us about the orbitals of each element?

  • Quiz 6

  1. Calculate the energy given off by a Hydrogen atom if its electron moves from the N=4 to N=3 energy level.

  2. When light (energy) is absorbed by an atom, something happens. Write and explain what happens. (Hint: six steps).

  3. If the wavelength of light given off by an atom when an electron drops from N = ? energy level to N=? energy level is 1.02 x10^(-7). Calculate the energy given off by this atom.

  4. Give me three reasons why Science does not disprove God.

  5. What are the four phases of matter?

  6. Draw pictures of the solid, liquid and gas phases. Pictures that show us something of what molecules look like when they are in these phases.

  7. How is a covalent molecular solid different to a covalent network solid?

  8. What are the names of the two main groups of solids?

  9. How are these two groups different? Draw a picture of each of these groups – showing me how they are different?

  10. If we zoom into a metal, what will we see? Draw this picture.

  • Quiz 7

  1. Amorphous solids can exist in three different structures. Name and draw all three.

  2. Crystalline solids can exist in three different cube structures. Name and draw all three.

  3. Name one characteristic (property) of all five different kinds of solids we have talked about in class. E.g. Malleability.

  4. Liquids have surface tension. Draw a picture and explain in words how the surface tension of water can hold up a piece of paper.

  5. Liquids have smells and tastes. Why? Draw pictures and explain with words.

  6. Liquids can exist in two different forms. What is the difference between the two.

  7. Liquids can evaporate (boil and go into the gas phase). Explain and draw how this happens.

    This is the phase diagram of Coca Cola. Use it to answer these questions.

  8. Image result for phase diagram for coke
  9. 8. If a can of Coca Cola is in an environment where the pressure is 1×10^(6) Pa  and temperature is 400 K. What phase will it be in?

  10. 9. If this can of Coca Cola in question 8 dropped in temperature to 100 K, What phase would it then be in? Draw a picture and write in words what will happen to the molecules of Coca Cola when it drops from 400 K to 100 K.

  • Quiz 8 

  1. Explain why molality is better to calculate than Molarity? Draw a picture to show me your answer.

  2. Sungyong wants to make a solution of molality 2 moles/kg. If Mr W gives him NaCl salt and 550 ml of water. How much NaCl should he use to make the solution? The density of water is 1 g/ml.

  3. Heeun mixes 3 moles of salt A into a beaker and adds 5 kg of solvent. What is the molality?

  4. Liquid B has a molar mass of 253.8 g/mol. It was used in class and is a dark liquid. If 2 g of the liquid is placed into 500 ml of water. What is the Molarity? Liquid B has a density of 4.93 g/ml.

    Bonus marks: What is liquid B? Hint: the molecule contains only 2 atoms.

  5. Hanyong mixes water into 2 moles of KI salt until the solution is 150 ml. What is the Molarity of his solution?

  6. Mr Lee asks you to give him a 23.5 % mass concentration solution of NaCl salt but you only have a 25 ml bottle. How will you do this? Give me all your calculations.

  • Quiz 9 

  1. Name one reason why Science and Christianity are NOT at war with each other.

  2. Write (use a picture if you want) why this reason (in question 1) is a good reason.

  3. Name the three different types of bonding we have been talking about in class and show me how they are different. Use words and pictures.

  4. Read this, “Bond length and the attractive/repulsive forces between two atoms are NOT related.” Write down why this is wrong.

  5. If Minu mixes two molecules and this reaction happens:

     C2H3Cl + Br2 —-> C2H3Br2Cl

    (The shapes of these molecules will be drawn on the board during the quiz)

    What is the TOTAL change of energy (heat) if the bond energies are these:

    C=C 614 KJ/MOL

    Br-Br 193 KJ/MOL

    C-Br 276 KJ/MOL

    C-C 347 KJ/MOL

    – Is this exothermic or endothermic?

  6. Draw these molecules in LEWIS dot form. Then, for each of them, replace the bonds with a line (or stick). Make sure you show me the electrons that do not bond. We call them, “lone pairs.”

    – Br2

    – C2H3Cl

    – NH3

    – SO2

  7. Draw the three dimensional shapes for these molecules. Write the name of the TYPE of shape each molecule is:

    – BeF2

    – NH3

    – H2O

    – PCl5

    – CH4

    – BBr3

    – O3

    • Quiz 10 

  1. We have been building up all year for something – what is it? It is the, “heart” of chemistry?

  2. Why are chemical indicators important? (20 words)

  3. If you did not know what molecule was in a beaker (call it molecule A). Write down, step by step in a logical way, how you could find out the empirical (proper) formula for the molecule called A.

  4. Here is a common chemical reaction:

  5. NH3  +  O2        NO  +  H2O

    – Write in all the CORRECT signs and symbols.

    – Write down, using arrows to show me what you are writing about, what each sign and symbol means.

    – Balance this equation and explain what the coefficients in the balanced equation mean.

    – Name ALL molecules in this reaction.

    – Draw the 3D drawings of EACH molecule.


  1. What does a mole conversion fraction do in stoichiometry? Give me one example to explain yourself.

  2. If you have 10 g of NaCl – how would you calculate the number of moles? Do the calculation to show your thinking.

  3. C6H12O6 = C2H5OH + CO2

    – If 3.60 g of C6H12O6 decomposes and makes CO2 gas, what will the theoretical mass in grams of CO2 be?

    – How many molecules of C6H12O6 are there at the start of the decomposition? (before any decomposes)

    – If the theoretical mass of the CO2 gas is at 100 K with a volume of 2.15 L. What will the pressure in Pa (Pascal’s) be?

  4. 75.0 g of Mg and 75.0 g of Cl2 are placed in a beaker and they react like this:

    Mg + Cl2 = MgCl2

    – Which substance is the limiting reagent?

    – How many grams of the excess reactant remain?

    – What is theoretical yield in grams of MgCl2?

    – If 72.0 g of product are actually formed – what is the percentage yield of MgCl2?

  5. If Na2S2O3 + AgBr = NaBr + Na3[Ag(S2O3)2]

– How many moles of Na2S2O3 are needed to react completely with 42.7 g of AgBr

– How many molecules of AgBr are there in 42.7 g of AgBr?

– What is the mass of NaBr that will be produced from 42.7 g of AgBr?


  • Pop Quiz  

  1. When copper ions replace silver ions in 10L of 0.1M silver nitrate, AgNO3. How many grams of silver will be produced? Hint, CU(NO3)2 is one product.

  2. When 1.00 g of zinc metal is placed in 25ml of a 0.250M lead nitrate solution, Pb(NO3)2, crystals of lead form. The other product is zinc nitrate, Zn(NO3)2. Which reactant is the limiting reactant and which is the excess reactant? How many grams of lead will form? How many grams of the excess reactant is left over, unreacted?

  3. At equilibrium the concentrations of these three gases are: [HI] = 0.0175M; [H2] = 0.0045M and [I2] = 0.00125M. What is the value of the equilibrium constant?

    HI = H2 + I2