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CLEP Chemistry 1

Subjects : clep, science, chemistry
Instructions:
  • Answer 50 questions in 15 minutes.
  • If you are not ready to take this test, you can study here.
  • Match each statement with the correct term.
  • Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.
1. In an endothermic process - energy is absorbed and ^E is _______.






2. In an exothermic process - energy is released and ^E of reaction is ________.






3. The heat required to change 1mole of solid completely to vapor.






4. The _____ speed up the rate of a chemical reaction but do not change the equilibrium constant - it simply speeds up the rate of approach to equilibrium.






5. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






6. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






7. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.






8. Metals have electronegativities less than ____






9. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.


10. **Proceeding across a period from left to right - the ionization energy _______.






11. A chemical reaction formed from the union of its elements.






12. A hypothetical gas would follow Boyles law under all conditions and is called?






13. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.






14. Deviations from Boyles law that occur with real gases represent _______ behavior.






15. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.






16. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.


17. *The nature of the reactants and products affect chemical reactions because some elements and compounds have bonds that when broken/formed - react more rapidly with each other than others.






18. Liquids with strong attractive forces have ______ boiling points.






19. The pressure exerted by each gas in a mixture is called its _____ pressure.






20. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.






21. When an electron moves from an excited state to the ground state - it _______ energy.






22. In titration - this is the point at which a particular indicator changes color.






23. The vapor pressure increases with increasing _____.






24. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.






25. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.


26. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.






27. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.






28. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






29. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.






30. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.






31. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.






32. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.






33. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.


34. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).






35. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.






36. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






37. When the rate of evaporation equals the rate of condensation - the system is in __________.






38. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?






39. The change in enthalpy of an endothermic reaction is ________.






40. When the electron moves from the ground state to an excited state - it ______ energy.






41. _____ bonds are present in molecules containing double or triple bonds.






42. Electronegativities ________ from left to right in a period.






43. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.






44. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






45. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.






46. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






47. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.






48. Cells that convert electrical energy into chemical energy.






49. This process occurs when the system is maintained at the same temperature throughout an experiment.






50. _______ has very little effect on the solubility of liquids or solids in liquid solvents.