Unit 1 Introduction to Chemistry (12%) /12
Multiple Choice (6 marks)
1. Chemistry is the study of ______and ______
2. This chemist won the Nobel prize for chemistry in 1903 for discovering the electron?
a. Schrödinger
b. Marie Curie
c. Niels Bohr
d. J.J. Thomson
e. Robert Millikan
3. The number 0.30020 has how many sig figs?
a. 6
b. 5
c. 4
d. 3
e. 2
4. How many sig figs does the answer to the following question have?
8.1 + 2.234 + 0.23=
a. 1
b. 2
c. 3
d. 4
e. 5
5. Which diagram below represents inaccurate but precise results?
6. The piece of glass where shown to the right is called:
a. Erlenmeyer flask
b. Florence flask
c. Volumetric flask
d. Beaker
e. Burette
Short Answer: (6 marks)
7. List the 6 observable signs that a chemical change has occurred. (3 marks)
8. If 103mL = 1L, conver 250mL to litres. (Show your work using a conversion factor & Use Scientific Notation) (2 marks)
9. What contributions did Lavoisier make to chemistry? (1 mark)
Unit 2: Atoms & Elements (20%) /33
Multiple choice: (6 marks)
1. The mass of a neutron:
a. Is less than that of an electron
b. Is less than that of a proton
c. Is equal to that of a proton
d. Is greater than that of an electron
e. Is equal to that of an electron
2. The number of electrons an atom has helps to determine the:
a. Charge
b. Number of neutrons
c. Number of protons
d. Mass Number
e. Atomic Number
3. What is the full name of the p orbital?
a. Principal
b. Pair
c. Pure
d. Placement
e. Partial
Which d orbital does the following picture represent?
a. dz2
b. dx2-y2
c. dyz
d. dzx
e. dxy
4. The p orbital holds how many electrons?
a. 2
b. 3
c. 6
d. 10
e. 14
5. What does the P in VSEPR stand for?
a. Principal
b. Pair
c. Pure
d. Placement
e. Partial
Short answer: (27 marks)
6. Define the following terms: (4 marks)
Proton:
Neutron:
Electron:
Isotope:
7. What contributions did Schrödinger and Heisenberg make to the model of the atom? (1 mark)
8. Identify which chemist proposed the following model by placing the corresponding letter in the corresponding blank. (3 marks)
a. Everything is made up of 4 elements; air, water, earth and fire
b. Atoms are small indivisible particles
c. Atoms contain protons and neutrons
d. Atoms have empty space
e. Atoms have electrons
f. Electrons orbit the nucleaus in statistically predictable areas
______Thompson
______Aristotle
______Schrodinger & Heisenburg
______Bohr
______Rutherford
______Dalton
20. Fill in the following chart (4 marks).
Element / Charge / Element Symbol / Atomic # / # ofp+ / # of
e- / # of
n0 / Mass # / Isotope
Symbol
Carbon - 14 / 10
+1 / K
56
21. Calculate the average atomic mass of silicon using the data provided below for percent natural abundance and mass of each isotope (2 marks)
12C - 98.9 % (12.000000000amu), 13C - 1.1 % (13.0033548378amu), 14C - 0.1 %(14.003241989amu)
22. In class you were given 10 elements whose symbols were originated from their Latin name. List five of those elements and their Latin names. (1 mark)
23. Describe the trend of atomic radius as you go across the periods from left to right and down the groups from top to bottom (2 marks)
24. List the 7 diatomic elements? (2 marks)
25. What name do we give group 2 elements?(1 marks)
26. Write out the full electron configuration for Tin. Include labelled shell diagrams(2 marks)
27. Write out the abbreviated electron configuration for Lead. (2 marks)
28. When Nitrogen has a full valence shell, what charge does is have? Which orbitals are the valence electrons of Nitrogen located in (number and letter)? (2 marks)
29. Draw the Lewis Dot structure for a neutral atom of Sulfur. (1 mark)
Unit 3: Bonding (20%) /27
Multiple Choice: (4 marks)
1. What does the P in IUPAC stand for?
a. Principal
b. Pair
c. Pure
d. Placement
e. Partial
2. The type intramolecular force is found in a water molecule:
a. Covalent bond
b. Ionic bond
c. Hydrogen bond (H-Bonds)
d. Molecular force
e. Alkane bond
3. A cation ...
a. consists of two or more atoms with a charge
b. has a charge greater than +1
c. has a negative charge
d. has no charge
e. has a negative charge
4. Ammonium Ferrocyanide (NH4)4Fe(CN)6 is used as a colorant in some cosmetics. Which of the following statements is false?
a. Ammonium Ferrocyanide is a compound made up of five different elements.
b. Ammonium Ferrocyanide is made up of thirty three ( 33 ) atoms.
c. Ammonium Ferrocyanide is a compound, not an element.
d. Ammonium Ferrocyanide is an ionic compound
Short Answer: (23 marks)
5. How many atoms are in the molecule Cr(C2O4)2? (1 mark)
6. How many atoms of hydrogen will combine with sulfate to form sulfuric acid? (1 mark)
7. Use VSEPR to determine the shape and geometry of CH4 and XeF4. Draw the 3 Dimensional structure of this molecule. (6 marks)
8. Draw the dipole for the bond that forms between hydrogen and Fluorine. List all intermolecular forces involved in this molecule. (2 mark)
9. Determine the charge in the metal for the following compounds. ( 3 marks)
a. CrPO4 : ______
b. Pb(MnO4)2: ______
c. Cu3(BO3)2: ______
10. Write the formulas for the following: (5 marks)
a. Diphodphorus pentoxide ______
b. Chlorine gas ______
c. Aluminum phosphate ______
Iron (II) nitrate ______
d. Hydrobromic acid ______
11. Write names for the following: (5 marks)
a. HNO2 ______
b. CO2 ______
c. Sn(CrO4)2 ______
d. Mg(HSO4)2 ______
e. Mn2(SiO3)3 ______
Unit 4: Chemical Reactions (20%) /27
Multiple Choice (4 marks)
1. In all chemical reactions:
a. The number of elements is always conserved
b. The number of atoms is always conserved
c. The number the charge always conserved
d. All of the above are true
e. none of the above are true
2. When aqueous solutions of CaCl2 and AgNO3 are mixed, only AgCl precipitates. Which one of the following is the correct net ionic equation for this reaction?
a. Cl22-(aq) + Ag+(aq) à AgCl(s)
b. 2Cl-(aq) + Ag+(aq) à AgCl(s)
c. 2Cl-(aq) + 2Ag+(aq) à AgCl(s)
d. Cl-(aq) + Ag+(aq) à AgCl(s)
e. Cl-(aq) + Ag+(aq) àAg+Cl-(s)
3. 10.0 g of salt is stirred into water to make 25 mL of salty water solution. The solvent is
a. salty water
b. water
c. salt
d. salt and water
4. Which of the following combinations of reactants will produce no reaction?
a. Na + H2O
b. F2 + NaCl
c. Zn + HCl
d. Zn + Al2(SO4)3
e. Cu + AgNO3
Short Answer: (23 marks)
5. BALANCE the equations and classify the TYPE of reaction. (8 marks)
___Zn (s) +___ HCl (aq) ___ ZnCl2 (aq) + ___H2 (g)
____P4O10 + ____H2O à ____H3PO4
___FeCl3 (aq) +___ AgNO3 (aq) ___ AgCl (s) +___ Fe(NO3)3 (aq)
___KOH (aq) + ___H3PO4(aq) ___ K3PO4(aq) +___ H2O (l)
____C6H6 + ____O2 à ____CO2 + ____H2O
____KClO3 à ____KCl + ____KClO4
6. Complete each word equation. Then write a balanced formula equation. (4 marks)
a.) Octane + oxygen à
b) Sodium and water à
7. Complete the balanced equation below and write the net ionic equation. (3 marks)
Iron (II) nitrate + sodium hydroxide à
8. List 5 ways you can increase the rate of a reaction. (2 marks)
9. For the equations below, state whether they are exothermic or endothermic: (2 marks)
2H2O + energy à 2H2 + O2
2 H2 + O2 à 2H2O + heat
10. Write the balanced equation for the reaction that occurs when silver nitrate is mixed with sodium phosphate (include states). Is a precipitate formed? (2 marks)
11. Answer the questions below, based on the graph below: (2 marks)
a. State what the substance’s freezing point is:______
b. What state is the substance in at 2oC?______
Unit 5: Moles and Stoichiometry (20%) /25
Multiple choice: (2 marks)
1. This number represents one mole is equal to:
a. 22.4L of any gas
b. Average atomic mass
c. 6.022 x 1023
d. Concentration
e. All of the above
2. The number of moles of a substance CANNOT be calculated from which of the following sets of data?
a. 44.8 L of oxygen ( O2 ) at S.T.P.
b. 650 mL of 0.095 M H2S04 solution
c. 150 g of copper metal (Cu)
d. 3.0 x 1023 molecules of glucose
e. Number of moles can be calculated using all of these
Short Answer: (23 marks)
3. How many molecules of hydrogen are in 2.0 moles of hydrogen gas? (2 marks)
4. What is the molar mass of H2SO4? (1 mark)
5. How many moles of copper (II) chloride are in a 50.0g sample? (2 marks)
6. What volume would 3.4 moles of methane gas take up at STP? (2 marks)
7. What is the percent composition of iron in iron (III) oxide? (2 marks)
8. In the reaction below, what volume of hydrogen is produced (@ STP) from a reaction with 2.0g of zinc and an excess of water? (3 marks)
____Zn + _____HNO3 à __ZnNO3 + ____H2
9. For the equation below, 5.0g of sodium carbonate is mixed with 5.0g of calcium chloride.
a. Which of the reactants would be limiting and which one would be in excess? (show work) (4 marks)
____Na2CO3 + ____CaCl2 à ____NaCl + ____CaCO3
b. What mass of precipitate will form? (3 marks)
10. 3.00g of sodium hydroxide is added to water to make 2.5 L of solution. What is the molarity of this solution? (3 marks)
11. How many moles of K2Cr2O7 are dissolved in a 0.25L sample of a 1.50M solution? (1 marks)
Unit 6: Organic Chemistry (8%) /9
Multiple Choice: (3 marks)
1. Alkanes are primarily used for:
a. flavouring food
b. biological preservatives
c. nail polish remover
d. fuels
e. none of the above
2. Which of the following is an isomer of hexane?
3. Which of the following molecules is unsaturated?
a. Choice 1 only
b. Choice 2 and 3
c. Choice 2 only
d. Choice 1 and 4
Short Answer (6 marks)
4. What is the name of the organic molecules shown below (for the aromatic compound below, be sure to name it using the appropriate letter in place of numbers)? (6 marks)
______
______