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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 vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.






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






3. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.






4. This law states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases in mixture.






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






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






7. *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.






8. 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 _______.


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






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






11. 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.






12. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.






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






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






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






16. Electronegativities _______ as you go down a group.






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






18. The solubility of gases in liquid or solid solvents always increases with ________ pressure.






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






20. The molecules in a gas are in constant - continueous - random - and straight-line motion.






21. 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.






22. A solution in which solid solute is in equilibrium with dissolved solute.






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






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






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






26. The most active metals are found in what corner of the periodic table?






27. Cells that convert electrical energy into chemical energy.






28. 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.


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






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






31. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.






32. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____






33. 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.






34. 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.






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






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






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






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






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






40. 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






41. Rays made up of electrons in basic electron charges.






42. The vapor pressure increases with increasing _____.






43. A process that occurs whent eh system is maintained at constant pressure.






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






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






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






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






48. 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.


49. 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






50. *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.