Chem 106 Comp Exam 2 PRACTICE
| 1. | The dots around an element symbol in a Lewis dot structure represent an atom’s | |
| isotope number | ||
| electrons that can be used to bond ionically | ||
| group number | ||
| valence electrons |
| 2. | To achieve a noble gas electronic configuration, a selenium (Se) atom would | |
| lose 2 electrons | ||
| lose 1 electron | ||
| gain 2 electrons | ||
| gain 1 electron |
| 3. | Which of the following has a noble gas electronic configuration? | |
| Ra2+ | ||
| Sc+ | ||
| S- | ||
| P2- | ||
| more than one choice is correct |
| 4. | What is the correct formula for the ionic compound that would form between Al and F? | |
| Al F | ||
| Al F2 | ||
| Al F3 | ||
| Al3F |
| 5. | What is the correct name for the ionic compound Cs2S? | |
| dicesium sulfide | ||
| cesium sulfide | ||
| dicesium monosulfide | ||
| cesium (II) sulfide |
| 6. | Mercury (Hg) can have a 1+ or 2+ charge.
What is the correct name for the ionic compound HgO? |
|
| mercury oxide | ||
| mercury (I) oxide | ||
| mercury (II) oxide | ||
| mercury monoxide |
|
|
| 7. | The Lewis structures for elements X and Y are shown above. What molecular formula would result if X and Y were to covalently bond? | |
| XY | ||
| XY2 | ||
| XY3 | ||
| XY4 |
| 8. | The correct formula of an ionic compound containing Fe3+ and HPO42- is | |
| Fe HPO4 | ||
| Fe (HPO4)2 | ||
| Fe2 HPO4 | ||
| Fe2 (HPO4)3 |
| 9. | What is the correct name for the ionic compound CuNO3?
(Cu can have a 1+ or 2+ charge) |
|
| copper (II) nitrate | ||
| copper (I) nitrate | ||
| copper nitrate | ||
| copper nitrotrioxide |
| 10. | Which of the following would exhibit the greatest amount of covalent bonding (have the lowest differences in electronegativities)? | |
| FeS | ||
| NO | ||
| Se F2 | ||
| Al N |
| 11. | Which element has the lowest electronegativity? | |
| F | ||
| At | ||
| Nb | ||
| Cs |
| 12. | What is the correct name for the covalently bonded H2O molecule? | |
| hydrogen oxide | ||
| hydrogen monoxide | ||
| dihydrogen monoxide | ||
| dihydrogen oxide |
| 13. | What interparticle forces would you expect to find in a sample of the element zirconium (Zr)? | |
| hydrogen bonding | ||
| ionic | ||
| dipolar covalent | ||
| metallic |
| 14. | Which of the following reactions is correctly balanced? | |
| N2 + H2 = 2NH3 | ||
| 2H2O + C = CO + 2H2 | ||
| Zn + 2HCl = H2 + ZnCl2 | ||
| CO + O2 = CO2 |
| 15. | Which of the following is a combination reaction? | |
| 2SO2 + O2 = 2SO3 | ||
| 2C2H2 + 5O2 = 4CO2 + 2H2O | ||
| 2H2O2 = 2H2O + O2 | ||
| AgNO3 + NaCl = AgCl + NaNO3 |
| 16. | CuO + H2 = Cu + H2O
The reaction above is an example of a ________ reaction |
|
| combination | ||
| decomposition | ||
| single replacement | ||
| double replaclement |
| 17. | NH3(g) + HCl(aq) = NH4Cl(aq)
Write the reaction above in total ionic form. The dissolved substances (designated by (aq)) are the only ones that dissociate completely into ions. What is (are) the spectator ion(s)? |
|
| H+ | ||
| Cl- | ||
| NH4+ | ||
| more than one choice is correct |
| 18. | When K2SO4 dissolves, what ions are formed? | |
| 2K+and SO42- | ||
| 2K+, 4O2- and S6+ | ||
| K2+ and SO4- | ||
| K2+, 2O2- and SO2 |
| 19. | 2H2O = 2H2 + O2
According to the reaction above, 2.0 mol of water will produce how many grams of O2? |
|
| 16 | ||
| 32 | ||
| 36 | ||
| 64 |
| 20. | Ca + 2H2O = Ca(OH)2 + H2
Using the equation above, how many molecules of H2 could be produced if 50 water molecules reacted with excess calcium? |
|
| 100 | ||
| 50 | ||
| 25 | ||
| 12.5 |
| 21. | CH4 + 2O2 = CO2 + 2H2O
If 5g of CH4 reacted with 5g of O2 according to the reaction above, what would be the limiting reagent? |
|
| CH4 | ||
| O2 | ||
| there will be no limiting reactant, both reactants will be entirely reacted |
| 22. | N2 + 3H2 = 2NH3
1.00 mole of N2 was reacted with 3.00 moles of H2 in the reaction above to produce 28.0g of NH3. What was the % yield of this reaction? |
|
| 122% | ||
| 100% | ||
| 93.7% | ||
| 82.2% |
| 23. | Small compressibility is a characteristic of which state of matter? | |
| solid | ||
| liquid | ||
| gas | ||
| both A and B are correct |
| 24. | As a substance changes from a liquid to a solid, the cohesive forces between particles ________ and the disruptive forces ________ | |
| increase, increase | ||
| decrease, decrease | ||
| increase, decrease | ||
| decrease, increase | ||
| remain the same, decrease |
| 25. | Disruptive forces in matter are related to the | |
| kinetic energy of particles | ||
| potential energy from particle attractions | ||
| electronegativities of particles | ||
| more than one choice is correct |
| 26. | Convert a temperature of 73K to oC | |
| –-200oC | ||
| –-147oC | ||
| 200oC | ||
| 346oC |
| 27. | A pressure is recorded as 860 torr. What is the pressure in atm? | |
| 1.26 | ||
| 1.13 | ||
| 0.884 | ||
| 0.531 |
| 28. | A gas sample has a volume of 500 mL at 20oC. At what Celsius temperature would the gas have a volume half as large? | |
| 10oC | ||
| 147oC | ||
| 0oC | ||
| –-127oC |
| 29. | 2500 liters of oxygen gas is produced at 1.00 atm of pressure. It is to be compressed and stored in a 20.0 liter cylinder. If the temperature is a constant, calculate the pressure of the oxygen in the cylinder. | |
| 125 atm | ||
| 4.00 atm | ||
| 80.0 atm | ||
| 8.00 atm |
| 30. | During a physical change of state, the particles of a substance slow down. This would be an example of | |
| evaporation | ||
| decreasing cohesive forces | ||
| an endothermic process | ||
| an exothermic process |
| 31. | In a closed container, a liquid will form a(n) _______ with the vapor above it. | |
| pressure | ||
| phase change | ||
| equilibirum | ||
| endothermic process |
| 32. | Moving water to a point 1500 meters higher than you are at now will have what effect on its boiling point? | |
| increase it | ||
| lower it | ||
| will have no effect | ||
| too little information to know |
| 33. | A change in chemical composition that results from heating is called | |
| decomposition | ||
| melting | ||
| sublimation | ||
| more than one choice is correct |
| 34. | How many dots representing electrons would be on a Lewis dot structure for bromine (element 35)? | |
| 35 | ||
| 7 | ||
| 5 | ||
| 1 |
| 35. | What is the correct formula for the ionic compound that forms when Ca and N combine? | |
| CaN | ||
| Ca2N3 | ||
| Ca2N3 | ||
| Ca3N2 |
| 36. | The covalent bond structure for CO2 involves _____ bonds. | |
| two single | ||
| two double | ||
| one double and one single | ||
| one single and one triple |
| 37. | The correct Lewis dot structure for a NO3- ion, where each O is bonded to the N, would have | |
| three single bonds | ||
| two single and one double bond | ||
| two double and one single bond | ||
| three double bonds |
| 38. | In the polar covalent HCl molecule, which atom would carry a partial negative charge? | |
| Edit this textH | ||
| Br | ||
| cannot be determined |
| 39. | KClO3 ---> KCl + O2 When the reaction above is correctly balanced, what coefficient precedes O2? |
|
| 1 | ||
| 2 | ||
| 3 | ||
| 4 |
| 40. | Ca + 2H2O ---> Ca(OH)2 + H2 How many grams of H2 can be produced if excess water is reacted with 160.32 g of calcium? |
|
| 160.32 | ||
| 112.30 | ||
| 8.064 | ||
| 4.032 |
| 41. | MnO2 + 4HCl ---> MnCl2 + Cl2 + 2H2O How many moles of H2O can be produced by the reaction above if excess MnO2 is reacted with 6.00 moles of HCl? |
|
| 1.00 | ||
| 2.00 | ||
| 3.00 | ||
| 6.00 |
| 42. | Which state of matter has the largest cohesive forces in comparison to its disruptive forces? | |
| solid | ||
| liquid | ||
| gas |
| 43. | A 6.00 L sample of gas at 0.00oC and 1.00 atm of pressure is compressed into a 1.00 L canister. If the temperature is increased to 30.00C, what is the pressure in atm inside the canister? | |
| 6.66 | ||
| 3.33 | ||
| 1.98 | ||
| 0.543 |
| 44. | What process has occurred when a solid changes directly to a gas without becoming a liquid? | |
| evaporation | ||
| condensation | ||
| melting | ||
| sublimation |
Answers:
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