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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. The law stating that in any spontaneous process there is an increase in the entropy of the universe.






2. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l






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






4. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.






5. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.






6. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.






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






8. The relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).






9. In an endothermic process - energy is absorbed and ^E is _______.






10. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.






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






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






13. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.






14. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.






15. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.






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.

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17. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.

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18. Real gases act in a less than ideal way - especially under conditions of increased pressure and/or decreased temperture. Real gas behavior approaches that of ideal gases as the gas pressure becomes very low. The ideal gas is thus considered a _____ _






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






20. **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.






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






22. Electronegativities _______ as you go down a group.






23. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.






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






25. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.






26. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.

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27. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.






28. *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.






29. The temperature at which a substance's solid and liquid phases are in equilibrium.






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






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






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






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






34. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?






35. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.






36. 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.






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






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






39. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.






40. 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 _______.

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






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






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






44. When a system at equilibrium is disturbed by adding or removing one of hte substances - all the concentrations will change until a new equilibrium point is reached with the same value of Keq.

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45. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge






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






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






48. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.






49. *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.






50. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f