Go through your notes and highlight the most important concepts based on what we have emphasized in this course.
Summarize your notes and clarify with your teather anything which you do not understand In the notes. Putting each units key ideas onto seperate study sheetys works.
Work through study sheets selecting questions that are emphasizing points of importance you highlighted.
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1. Define:
| element | compound | chemical change | mech. mixture |
| solvent | molecule | physical change | homogeneous |
| heterogeneous | solution | solute | pure substance |
| atom | isotope |
2. Give the names of the following: (do not look at a periodic table)
| K | Cl | Cu | Pb | Au | N | U | C | Ag | Mg | O |
3. List 5 characteristics of metals and non-metals. What are metalloids?
4. List four clues for recognizing a chemical change.
5. State whether each is a chemical property or a physical property.
| a)iron nails rust |
| b)nitrogen is a colourless gas |
| c)nitrogen liquifies (condenses) at -196 degrees celsius |
| d)wood burns |
| e)frost forms on car windows |
| f)rock is crushed into gravel |
| g)butter goes rancid if left out |
6. State whether each is a chemical change or a physical change,
| a)the burning of candle wax |
| b)the melting of naphthalene |
| c)the reaction of lead nitrate and potassum iodide to produce a bright yellow precipitate |
| d)the cutting of sodium metal |
| e)the glowing of a 1OOW light bulb |
| f)the souring of milk |
| g)the boiling of alcohol |
7. How would you separate a mixture of salt, sand and isopropyl alcohol?
8. Describe the Law of Conservation of Mass and the Law of Constant Composition
9. Indicate the contributions of the following scientists to the development of the concept of the atom: Dalton, Rutherford, Chadwick, Bohr.
10. Draw electron dot diagrams (Bohr-Rutherford Diagrams) for an atom whose atomic # is 16. and for Na.
Complete the following:
| Mass Number | Atomic Number | Number of Protons | Number of Neutrons | Number of Electrons | |
| . | 133 | 53 | . | . | . |
| . | . | 27 | . | 28 | . |
| Zn | . | . | . | 36 | . |
| Zn | . | . | . | . | . |
| K | . | . | . | . | . |
12. For each of the following, list
| a) how many elements in it |
| b) how many atoms of each element |
| c) how many atoms TOTAL in it |
Fe2O3 (NH4)2 CO3 Al2(S2O3)3
13. Identify the product of the following equations, and then write out the entire equation using symbols.
| a) sodium phosphate + potassium permanganate -- > ? + ? |
| b) lithium sulfide + barium chloride --- > ? + ? |
14. Element X has 5 naturally occurring isotopes. Find the average atomic mass of the following: 70 X = 20.5%, 72 X = 27,4%, 73 X = 7.80 %, 74 X = 36.5%, 76 X = 7.8%
15. 4.65 g of sodium and 15.98 g of bromine react to form 20.58 g of sodium bromide. How much sodium is required to react with 24.83 g of bromine? (SHOW WORK)
16. Iron and oxygen react together t0 form iron oxide according to the equation below. 4.7020 g of iron produces 8.7426 g of iron oxide the reaction.
iron + oxygen --- > iron oxide
| a) Determine the mass of oxygen needed for the reaction to take place. |
| b) Determine the % composition of iron oxide |
| c) What mass of iron will react with 1.00 g of oxygen? |
| d) What mass of oxygen will react with 17.8461 g of iron? |
| e) Find the mass of iron and the mass of oxygen in a 3.461 1 g sample of iron oxide. |
1 . Define:
| metalloid | alkali metal | electron affinity |
| covalent bond | isoelectronic | valence electron |
| halogen | ionization energy | period |
| Ionic bond | group | stable octet |
| noble gas |
2. List the trends in the periodic table of the following qualities:
| atomic radius electron affinity |
| ionization energy metallic characteristic |
3. What is the main differe.ce between an ionic and a covalent bond?
4. What types (or categories) of elements a,e involved in ionic bonding?
5. What causes elements in a covalent bond to stay together?
6. Draw Lewis Structures (electron dot diagrams) for each of the following:
| a) CO2 | b) H2Se | c) BCI3 | d) P2 | e) NF3 | f) Cl- |
7. List the following elements in order of decreasing atomic radius. As, F, Sn, S
1 8. List the elements neon (Ne), sodium (Na), chlorine (CI) and iodine (I) in order of increasing ionization energy.
9. What is efectronegativity?
10. List the following in order of in electronegativity. Cl, F, O, S
11. When an aluminum atom forms an Al3+ ion, the atom
| a) loses three electrons | b) gains three electrons |
| c) loses three proton | d) gains 3 protons |
12. Define atomic number.
13. Identify the type of bonding present in, each substance.
| H2 | NaCl | HCI | H2O | NH3 | MgO | Cl2 |
1. Define the following:
| -Dalton's Law | -Boyle's Law | -Charies'Law |
| -STP | -partial pressure | -mole |
| -Kinetic-Molecular theory | -ideal gas | -moiar volume |
| -ideal gas equation | -kelvin | -molar mass |
| -combined gas law equation | -vapour pressure | |
| -Avogadro's Hypothesis | -universal gas constant |
2. Explain how Gay-Lussac's observations led Avogadro to develop his hypothesis.
3. Use the Kinetic Molecular theory to explain:
| -Boyle's Law | -Charies'Law | -compressibility of gases | -partial pressures |
4. A bulb contains a gas mixture which is 10% O2, 35% SO2, and 55% SO3. If the total pressure in the bulb is 120 kPa, what is the partial pressure of each gas? (12/42/66)
5. What mass of gaseous ethane, C2H6 at 60.8 kPa pressure and -25 degrees celsius contains the same number of particles as 9.20 g of NO2 (g) at 101 .3 kPa and O degrees celsius (6.0 g)
6. Calculate the molar mass of a gas if 20.4 g occupy 11.4 L at 507 kPa and 273'C. (1 6 g)
7. How many molecules of oxygen gas (O2(g)) are present in 1.2 L of the gas at STP? (3.01 x 10 to the power 23)
8. The molar mass of hydrogen (H2) is 2.0 g/mol. What is the mass of 6.0 L of H2 at STP? (0.54 g)
9. For more practice, try problems at the back of chapters 1 3 & 14.
10. What volume will 12.9 g Of SO2 occupy at 30'C and 101.3 kPa pressure? (5.0 L)
11. A balloon contains 5.0 L of air at a pressure of 149 kPa. If the temperature remains constant, what will be the pressure in the balloon if the volume is decreased to 4.0 L (1 86 kPa)
12. A cylinder of volume 1.5 kL contains compressed air at a pressure of 10 MPa. What volume would the air occupy at the same temperature and a pressure of 101 kPa (149kL)
13. A balloon contains 125 L ot air at 35oC.What will be the new volume of the balloon if the temperature drops to -35 degrees celsius as the pressure is constant?
14. At constant volume a gas at 200 kPa and 40 degrees celsius is cooled to O degrees celsius. What will the pressure of the gas be at the new temperature? (174 kPa)
15. How many moles of glucose are there in 90 g of glucose (C6Hl2O6)? (0.5 mol) How many molecules? (3.01 X 1 023 ) How many atoms? (7.2 x10 to the power 24)
16. Find the mass of 100 L of methane (CH4) gas at STP. (71.6 g)
17. A gas occupies 2.0 L at 25 degrees celsius and 120 kPa. What volume will it occupy at STP? (2.2 L)
18. A balloon is filled with 2.2 L of gas at a pressure of 108 kPa and a temperature of 21 degrees celsius. It is then taken down to the bottom of the ocean where the pressure is 11.8 MPa and tile temperature is 6 degrees celsius. Find the new volun,e of the balloon (19 mL)
19. The major ingredient in solid air fresheners is a paradichlorobenzene. If a 9.87 9 block of air freshener is vapourized in a 1.5 L container at 125 degrees celsius, the resulting pressure is 148.2 kPa. Determine the molar mass of paradichlorobenzene. (1 47 g/mol)
1 . Predict the formula of the binary compound that is likely to b,a formed by each of the following pairs of metals and nonmetals, and give an acceptable name for each compound:
| a) magnesium and oxygen | d) potassium and oxygen |
| b) gallium and fluodne | e) zinc and sulfur |
| c) phosphorus and chlorine |
2. Name the following compounds:
| a) SnCl2 | b) CuBr | c) AGNO3 | d) Mg(NO3)2 | e) CuSO4 5H2O |
3. Write the formula for each of the following:
| a) boron trifluoride | d) lead (II) chloride |
| b) magnesium oxide | e) hydrochloric acid |
| c) sodium hydroxide |
4. Name each of the following compounds:
| a) SnSO4 | c) Ca (MnO4)2 | e) Pb(OH)4 | g) KOH |
| b) Ca3(PO4)2 | d) Sn3(PO3)2 | f) Fe2(SO4)3 | h) AgClO4 |
5. Write the formula for each of the following:
| a) tin (IV) sulfate | f) potassium nitrate |
| b) potassium peroxide | g) hydrogen gas |
| c) lead (IV) dichromate | h) zinc chlorate |
| d) iron (II) hydroxide | i) iron (III) sulfite |
| e) ammonium Perchlorate | j) hydrogen peroxide |
6. Find the molar masses of : glucose, water, nitric acid, dinitrogen pentoxide.
7. How many grams of H2O has the same amount of moles as 12 g of nitrogen gas? (7.7 g)
8. Find the mass of 2 molecules of C6H12O6 (130 u)
9. Find the percent composition of: P207H4
10. Find the empirical formulas for:
| a) 50.5% C, 5.26% H, 44.2% N (C4H5N3) |
| b) 45.3% Li, 53.7% 0 (Li2O) |
11. Find the molecular formula for the compound whose empirical formula is CNOH3 and has a molecular mass of 90 u.
12. How many moles of NAOH are required to react with 8.61 moles of H2SO4 according to:
2 NAOH + H2SO4 -- > Na2SO4 + 2 H20 (17.22)
13. How many grams of H2SO4 are necessary to produce 4.77 moles of Na2SO4? (467.5 g)
14. Identify the following reaction type and balance:
K3PO4 + mgso4 -- > Mg3(PO4)2 + K2SO4 BN + F2 -- > BF3 + N2 CuCO3 -- > cuO + CO2
15. Explain the terms limiting reagent and theoretical yield.
16. How many grams of HgO are required to produce 0.5 kg of Hg according to:
2 HgO (s) --- > 2 Hg (l) + O2 (g) ? (539.9 g HgO)
17. According to the equation: 3 H2 + N2 --- > 2 NH3
18. 35 g of FeCO3 burned in air produces 22.5 g of Fe2O3 according to:
4 FeCO3 + O2 --- > 2 Fe2O3 + 4 CO2
Find:
| a) the limiting reagent (FeCO3) |
| b) the theoretical yield (24 g Fe,03 : your other product is CO, gas) |
| c) the percent yield (93.7%) |
19. According to the equation SiO2 + 4 HF ---> SiF4 + 2 H2O, 12.2 g SiO2 and 50 g HF react.
| a) Find the limiting reagent (SiO2) |
| b) Find the theoretical yield of SiF4 (21 g) |
| c) If 3.2 g of SiF4 are produced, find the percent yield, (15.2 %) |
1 . Define the following:
| acid | solute | base |
| solvent | neutralization | solubility | strong electrolyte | weak electrolyte |
| non electrolyte | equivalence point | end point |
2. Explain the concept of "Like dissolves like" using at least two different examples.
3. What are the products of all neutrlization reactions?
4. Describe the characteristics of acids and bases.
5. Find the concentrations (M) of the following solutions.
| a) 20 g Ca(OH)2 in 300 mL aqueous solution. (0.90 M) |
| b) 65 g Pb(NO3)2 in 125 mL of aqueous solution. (1.6 M) |
| c) 92 g NH4CL in 760 mL of aqueous solution. (2.3 M) |
6. What volume of 0.028 M LiCl contains 0.15 g LiCl? (126ml)
7. Find the volume of 0.15 M K2Cr2O7 (potassium dichromate) ,which contains 80.0 g of K2Cr2O7. (1.8-1 L)
8. What volume of 5.0 M NAOH is required to make 2.0 L of 0.25 M NAOH? (1.0 X 102 mL)
9. What is the concentration ot OH- and H+ for the diluted solution above?
10. What is the pOH and pH of the above solution?
11. A 28 mL sample of KOH solution was titrated to an endpoint against 50 mL of HNO3. Find the concentration of the base if the acid is 0.60 M(l .07 M)
12. What mass of KOH is required to neutralize 20 mL of 0.20 moL/L HCl?
13. What mass of NAOH is required to neutralize 50 mL of 0. 1 0 mol/L H2SO4 solution?
14. What volume of 0. 1 5 mol/L Mg(OH)2 is required to neutralize 20 mL of 0. 20 mol/L H3PO4?
15. What volume of distilled water must be added to 50 mL of 0.40 mol/L HCI solution to make it 0. 1 0 mol/L?
16. Calculate pH and pOH for:
| a) H+ = 0.0123 M |
| b) OH- = 9.76 x 1O to the power -9 M |
| c) H+ = 5.22 x l0 to the power -3 M |
| d) OH- = 4.76 x 10 to the power -6 M |
17. Calculate the concentrations of H' and OH- for:
| a) pH = 7.814 | b) pOH= 10.05 |
| c) pH = 3.176 | d) POH = 9.561 |
16.
| a) pH = 1.91, pOH = 12.09 |
| b) pH = 6.99, pOH = 8.01 |
| c) pH = 2.28, pOH = 11.71 |
| d) pH = 8.68, pOH = 5.32 |
17.
| a) H' = 1.535 x 10" / OH- = 6.516 x 10 -7 |
| b) H' - 1.122 x IV I OK - 8.913 x 10 -11 |
| c) H' - 6.668 x 1 0'4 / OK - 1.6 x 1 0 -11 |
| d) H' = 3,639 x 107' / OH- = 2.748 x 1 0 -10 |
1 . Define the following:
| isomer | unsaturated | alkyne |
| structural formula | combustion reactions | saturated |
| alkene | alkane | substitution reactions |
2. Know the steps for nomenclature of alkanes, alkynes, and alkenes
3. Identify the following substances by their functional groups:
| alcohols | esters | amines | ethers |
| aldehydes | ketones | carboxylic acids |