Download Chemistry 11 Review Sheet

Chemistry 11 Review Sheet
Name: ______________
Part 1- Activities of Science, Matter and Significant figures
Review all your safety rules.
1.
2.
Change the following into scientific notation with round to two significant figures.
a) 0.0117853
b) 9985364
Change the following to the power in parenthesis.
a) 1.58 x 10 –7 (10-9)
3.
b) 1.89 x106 (109)
How many significant figures are in the following:
a) 0.003200 mm
b) 160km
4.
Convert the following units
5.
a) 160cm = ________ km
c) 16 cm2 = ________km2
Evaluate to correct sig figs.
a) 1.6 x 10 –2 cm/2.3 x103cm
b) (1.8x10-3 m) x(4.6x102m)
c) 16g/5.80x10-2g
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
c) 408.0 g
d) 9.00 mm
b) 12 L = __________ mL
d) 250mm3= _______ cm3
d) 16.1+2.314+0.62
e) 0.0005009+3
f) 250+12
g) 8.0012-0.09
Describe the difference between an inference and an observation?
What is the scientific method?
What is the difference between accuracy and precision?
Describe the procedure for heating materials on Bunsen burner?
How do solutions differ from mixtures?
What characteristics of pure substances distinguish them from mixtures?
What causes plateaus on cooling curves?
How do cooling curves differ between mixtures and pure substances?
Define chemical and physical change. Give examples.
Describe electrolysis and distillation and other methods that can be used to separate mixtures?
Draw the classification of matter chart and define and give examples of elements, compounds,
ions atoms, molecules and polyatomic atoms, diatomic atoms and metal and nonmetals.
Explain the law of definite composition, law of multiple proportions, and law of conservation of
mass.
What is an intensive and an extensive variable. Give examples of each?
Define density and calculate the density of an object that has mass of 4.562g. When the object is
placed in a graduated cylinder with 20.00mL of water, the level of the water rose to 21.53mL,
How is density determined from a graph?
19.A student measured a selection of jar lids and recorded the following data.
diameter (cm)
| 2.7 | 4.4 | 8.1 | 11.3 | 13.7
circumference (cm) | 8.5 | 14.2 | 25.4 | 35.0 | 44.0
a) On a separate piece of graph paper, plot the data using circumference as
the dependent variable. (5 marks)
b) Calculate the slope of the resulting graph and what does the slope represent. (3 marks)
c) What is the equation for the line? (1 mark)
21. Write the formulae for the following compounds.
a)
b)
c)
d)
e)
copper(II) chloride
calcium sulfate
diphophorus pentoxide
sulfuric acid
sodium hydroxide
Part 2 The Mole Concept
22. What is relative mass?
23. What is Avogadro’s hypothesis and what is its significance?
24. Mole conversions: Complete the table
Mass (g)
Moles
0.20 moles of CO2
3.50 moles of O2
Molecules
Volume
1.5 x 1023 molecules of
CH3COOH
1.8 molecules of N2
Not gas
35.0 g N2O
25.0 g AgI
3.46 L of H2 (g)
25. A 5.5g sample of a compound containing carbon and oxygen was analyzed. It was found to
contain 1.50g C. Determine the empirical formula of the compound.
26. Determine the percentage composition of C12H22O11
27. Determine the empirical formula of a compound that is 37.5% C, 12,5% H and 50% O.
28. If the empirical formula of a compound is CH3 and its molecular mass is 30.0g/mole, determine
its molecular formula?
29. What is the empirical formula of a compound that is 79.9% Cu and 20.1% S?
Part 3 Chemical Reactions
Complete and balance the following equations and
(12 marks)
30. Balance the following equations:
classify:
a)
b)
BaCl2 + H2SO4 ---->
C4H10 + O2 ---->
c)
Ca + O2 ---->
d)
e)
HgO ---->
Li2SO4 + BaCl2 ---->
f)
Zn + HCl ---->
31. Balance the following equations: (2 marks each)
a)
b)
Al + H2O ----> Al(OH)4 + H2
Na2CO3 + HCl ----> NaCl + H2O + CO2
c)
PbCO3 + HNO3 ----> Pb(NO3)2 + H2O + CO2
d)
CaCO3 + HC2H3O2 ----> Ca(C2H3O2)2 + H2O + CO2
K2CO3 + H3PO4 ----> K3PO4 + H2O + CO2
e)
Part 4: Stoichiometry
32. If 7.30 g N2 and 8.30 g O2 react in the reaction
N2(g) + O2(g) N2O(g)
a) what is the limiting reactant?
b) what is the mass of the reactant in excess?
c) How many grams of the product are produced?
33. Propane (C3H8) burns in the presence of oxygen gas to produce carbon dioxide and water. If 600.0 L
of oxygen gas are available to burn 250.0 g of propane:
a) write and balance the equation for this reaction.
b) what volume (in liters) of oxygen will be used?
c) what mass of carbon dioxide would be produced?
Part 5: Gases
34.
35.
36.
37.
Explain what the molar volume of a gas represents? What is the molar volume of any gas at STP?
How degrees Celsius are in 373 Kelvin’s.
What is STP?
What is the Pressure of 7.85 g of Oxygen gas that has a volume of 19.8 L at 27.0 degrees Celsius.
Use the ideal gas law.
Part 6: Solutions and Solubility
38. How many grams of K2SO4 are contained in 100.0 mL of 1.50 M H2SO4 solution?
39. Calculate the volume of a 0.400 M BaCl2 stock solution required to prepare 500 mL of a 0.100 M
BaCl2 solution.
40. A solution of chromium (III) nitrate is mixed with a solution of potassium sulfide.
a) Write a balanced complete ionic equation. (2)
b) Write the net ionic equation.
41. The following data was collected when a 0.25 M solution of NaOH was titrated into 5.00 ml of an
HCl solution until the phenolphthalein just turned pink.
Final buret reading...............28.8 ml
Initial buret reading...............11.2 ml
a) Write the balanced equation for the reaction? (1)
b) What is the [HCl]? (3)
42. Two ions found in "hard water" (water with high mineral content) are Ca 2+ and Mg2+ . What ion
will precipitate only one of these ions?
43. A 100.0 mL sample of 0.600 M Ca(NO3)2 is diluted by adding 400.0mL of water. Calculate the
concentration of ions in the resulting solution.
44.
A 100.0 mL saturated solution of FeF2 contains 0.0787 g of solute. Determine [Fe2+] and [F-] in
the solution.
45. Write the dissociation equation for 0.50M BaCl2 and find each ion concentration.
Part 7: Atomic Theory
46. Describe the early models of the Atom, gold foil experiment?
47. Describe the organization of the periodic table?
48. Explain the following trends:
a) Electronegativity b) ionization energy c) atomic size
49. Calculate the average atomic mass, given the data for the naturally occurring isotopes. (\. marks)
Si-28............92.21%
Si-29............4.70%
Si-30............3.09%
50. If the following pairs of atoms were to form a bond, which would be the correct method of
representing the bond dipole?
<----->
--->
--->
<--1. O-Cl
2. Br-Br
3. N-I
4. C-O
5. S-Br
51. How many protons, neutrons and electrons are in Mg, Mg2+, F, F-, Na, Al, Br
52. Draw the electron dot structure and name the molecular shape of each of the following:
a) CH3OH b) CCl4 c) HCN d) HCOOH e) N2 f) H2O
53.
Draw the electron configuration for the following atoms: Mg, Cl -, Ne, Ca2+
54. Define a covalent bond ,ionic bond ? Give examples of each.
55. How do you determine whether a molecule is polar or nonpolar is H 20 polar or nonpolar?
Part 8 : Organic Chemistry
56. Draw the structural formula for 2,2-dimethylbutene.
57. Draw the structural formula for 3,4,5-trimethylhexyne.
58. Name the following compound:
59. Draw the structural formula for methanol.
60. Name the following structure:
61. Describe how you made an ester , name it and identify its smell.
62. What type of compound is the following:
63. Write down the names and isomers of C6H12.