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Chem 11
Ms. Lee
Chemistry Test
Lab reporting skills, Atomic Theory, Periodic Table, Organic Chemistry
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1. How many significant figures are in the following numbers? (4 marks)
a. 504 ______
b. 1,000,101______
c. 2.1 x 106______
d. 0.00500______
2. Write the following into scientific notations with correct significant figures. (4 marks)
a. 763,000 __________________
b. 2,560,000__________________
c. 0.000066__________________
d. 0.00500__________________
3. Give measurements with uncertainties for Ruler A and Ruler B. (2 marks)
Ruler A:
Ruler B:
4. Alpha had a party and invited all the Summit 10’s. However, Astrid decided to bring
some non-Summit friends to the party (*gasp*). Alpha expected 28 guests but ended up
with 32. What was the percentage error of her party? (2 marks)
5. Calculate the following and give the final answer in correct significant figures (8 marks)
a. 106.7 g +0.25 g + 0.195 g
b. 35.25 mL – 30.5 mL
c. 50.5 cm x 12 cm
d. 103.37 g/20.5 mL
6. Give the number of protons, neutrons, and electrons of each of the following isotopes.
(6 marks)
a. 105𝐵
7. An element has the following natural abundances and isotopic masses: 90.92%
abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abundance
with 21.99 amu. Calculate the average atomic mass of this element. (2 marks)
8. Use complete subshell notations (no core notation) to predict the electron configuration
of the following atoms: (4 marks)
a. C
b. P
c. V
d. Sb
9. Use complete core notation to predict the electron configuration of the following
atoms: (2 marks)
a. Mo
b. Ca2+
10. Which atom has the electron configuration ending with 4d2? _________ (1 mark)
11. Which atom would be expected to have a half-filled 4s subshell? ____________ (1 mark)
12. Fill in the orbital diagram for Nickel. (3 marks)
13. Which of the following pairs of elements belong to the same period? (1 mark)
A. Na and Cl
B. Na and Li
C. Na and Cu
D. Na and Ne
14. Which of the following pairs belong to the same group? (1 mark)
A. H and He
B. Li and Be
C. C and Pb
D. Ga and Ge
15. How does an element’s period number relate to the number of the energy level of its
valence electrons? (1 mark)
16. Why do all the members of a group have similar properties? (1 mark)
17. The measure of the attraction that an atom has for electrons involved in chemical bonds is known
as: (1 mark)
A. Ionization energy
B. Electronegativity
C. Ionic bond
D. Covalent bond
18. As one moves from down ( ↓ ) a group on the periodic table, the ionization energy of
the elements encountered tends to: (1 mark)
A. Remain the same
B. Increase
C. Decrease
19. The elements with the largest atomic radii are found in the: (1 mark)
A. lower left-hand corner of the periodic table
B. upper right-hand corner of the periodic table
C. lower right-hand corner of the periodic table
D. upper left-hand corner of the periodic table
20. Which of the following elements would have the lowest ionization energy? __________
(1 mark)
21. Of the following elements, which one would have the smallest radius? (1 mark)
A. Iodine (I, atomic #53)
B. Bromine (Br, atomic #35)
C. Fluorine (F, atomic #9)
D. Chlorine (Cl, atomic #17)
22. What’s the relationship between electronegativity, atomic radius, and number of
protons? (3 marks)
23. Draw Lewis Dot structures of: (6 marks)
a. CCl4
b. NI3
c. MgO
24. Is it ionic or covalent? (4 marks)
a. The atoms of a molecule have an electronegativity difference of 0.3 ________
b. Diatomic molecule of oxygen __________
c. H2O ______
d. NH4OH _______
25. Is it non-polar or polar covalent? (4 marks)
a. HCl ________
b. H2O________
c. O2________
d. Diamond (C-C-C-C-C-C-…)________
26. Name the following organic structures: (8 marks)
b. (include cis- or trans-)
27. Identify the following functional groups: (2 marks)