IB Chemistry HL Summer Assignment

Mrs. Smith’s Class

Topic C: Medicinal Chemistry, Unit 11, End of Organic
Due Date: September 13, 2019
Part I

You will be making a presentation of your choice on an assigned topic (I will give these to you on the
last day of class. You can use the following outlets for your presentation:
- Powerpoint
- Prezi
- Another equivalent program
You will be presenting it to the class and I will be making it available on Canvas for students to have
access to. Please keep that in mind.

Guidelines/Grading:
 Include all important information on the topic. Come up with an interesting way to present the
material. You MAY NOT copy the information from the textbook. That is not going to help
you know the material. (content- 50 points)

 Add links to all information from outside sources (10 points)

 Cite all outside sources at the bottom of the page. (10 points)

 Include pictures to make it more interesting. It should be eye catching and informative. Use
your creativity. (20 points)

 If you have the review topic you need at least one review question for each topic that your
fellow students can answer. NO MULTIPLE CHOICE! Topics are ALL short answer/essay
questions on the IB test. You can also make a powerpoint game or other type of review game.
The review is completely open to whatever you would like to do.

 The review questions may not come from the textbook.

 Presentation of material. (10 points)

Part II

Make sure you review ALL of the SL material. We do not have time to spend going back over
material you have already done. Each unit we will spend 1 day going over the SL material and then
you will have a quiz the following class on that material. YOU WILL NOT HAVE THE
OPPORTUNITY TO DO QUIZ CORRECTIONS ON THESE QUIZZES! They are a one-shot deal.
We will then start the HL material. I know there is a lot of material in SL but just wait until we start
doing HL!
Part III

Answer all of the following questions. It is a review of Topic 1 for both SL and HL- Quantitative
Chemistry. These should be done without a calculator as you will not be able to use one on your IB
exam.

1. How many molecules are present in 27.0 g of distilled water?

A. 2.7 x 1024 B. 1.5
C. 9.0 x 1023 D. 4.5

2. How many moles of carbon dioxide will be formed when 32.0 g of methane, CH 4, burns completely in
oxygen?
A. 1.0 B. 2.0 C. 4.0 D. 8.0

3. How many oxygen atoms are present in 0.5 mole of pentahydrated copper(II) sulfate, CuSO 4.5H2O?
A. 2.5 B. 4.5 C. 3.0 x 1023 D. 2.7 x 1024

4. What is the total number of atoms in 3.0 molecules of propanone, CH 3COCH3?

A. 3 B. 10 C. 1.8 x 1024 D. 1.8 x 1025

5. Which contains the same number of ions as the value of Avogadro’s constant?
A. 0.5 mol KBr B. 0.5 mol CaBr2
C. 1.0 mol CaO D. 1.0 mol K2O

6. Which molecular formulas are possible for a compound which has an empirical formula of C 2H4O?
I. CH3CH2OH
II. CH3CH2CH2COOH
III. CH3CH2COOCH3
A. I and II only B. I and III only
C. II and III only D. I, II and III

7. Which compound has the empirical formula with the largest mass?
A. CH4 B. C2H4 C. C2H6 D. C6H6

8. What is the maximum mass, in grams, of magnesium oxide that can be formed when 4.8 g of
magnesium reacts with oxygen?
A. 4.8 B. 8.0 C. 11.2 D. 12.8

9. Which is a correct statement about the molecular formula of a compound?

A. It shows which functional groups are present in the molecule.
B. It shows how all the atoms are bonded in a molecule.
C. It is the simplest ratio of the atoms of different elements in the molecule.
D. It is an integral multiple of the empirical formula.

10. 98 g of a pure hydrocarbon contains 84 g of carbon. Which statements are correct?

I. The compound has an empirical formula of CH 2.
II. The compound has a molecular formula of C 7H14.
III. Not enough information has been given to deduce the molecular formula.
A. I and II only B. I and III only
C. II and III only D. I, II and III

11. When the equation for the combustion of 1 mole of propane is balanced what is the coefficient for
oxygen, O2(g)?
C3H8(g) + __ O2(g) → __ CO2(g) + __ H2O(l)

A. 5 B. 7 C. 10 D. 14

12. What is the maximum amount of methanol, in mol, that could be formed when 4 mol of carbon dioxide
and 6 mol of hydrogen gas are placed in a container and react according to the equation below?
CO2(g) + 3H2(g) → CH3OH(l) + H2O(l)

A. 1 B. 2 C. 3 D. 4

13. When the equation for the complete combustion of two mol of propyne, C 3H4, is balanced what is the
sum of all the coefficients?
2C3H4(g) + __ O2(g) → __ CO2(g) + __ H2O(l)

A. 16 B. 18 C. 20 D. 22

14. 1 mol of any gas occupies 24 dm3 at room temperature and pressure.
When 32 g of methane burn completely in oxygen at room temperature and pressure what volume of
carbon dioxide, in dm3, will be formed?
A. 16 B. 24 C. 32 D. 48

15. Ethane burns in oxygen according to the equation below. What volume of oxygen, in dm 3, reacts with
0.8 dm3 of ethane?
2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l)

A. 0.8 B. 1.6 C. 2.8 D. 5.6

16. Which solution contains the most amount of sodium hydroxide?

A. 10.0 cm3 of 0.700 mol dm-3 NaOH
B. 20.0 cm3 of 0.600 mol dm-3 NaOH
C. 30.0 cm3 of 0.500 mol dm-3 NaOH
D. 40.0 cm3 of 0.400 mol dm-3 NaOH

17. What will be the concentration, in mol dm-3, of the resulting solution when 200 cm 3
of 0.200 mol dm-3 hydrochloric acid, HCl(aq) are mixed with 300 cm 3 of 0.100 mol dm-3
HCl(aq)?
A. 0.140 B. 0.300 C. 0.070 D. 0.150

18. What volume, in cm3, of 0.200 mol dm-3 sodium hydroxide solution, NaOH(aq), is
required to neutralise exactly 25.0 cm 3 of 0.100 mol dm-3 sulfuric acid solution,
H2SO4(aq)?
A. 12.5 B. 25.0 C. 50.0 D. 100

19. What would be the empirical formula of a hypothetical compound that contains 60% by mass of
element A (Ar = 10 ) and 40% by mass of element B (Ar = 20)?
A. A3B2 B. AB3 C. AB2 D. A3B

20. When calcium carbonate is heated it decomposes according to the equation:

CaCO3(s) → CaO(s) + CO2(g)
When 60 g of calcium carbonate is heated, 16.8 g of calcium oxide are formed. What is
the percentage yield?
A. 16.8% B. 25% C. 50% D. 60%