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






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






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






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






5. *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.






6. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.






7. 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.

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






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






10. Electronegativities _______ as you go down a group.






11. 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).






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






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






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






15. 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.






16. Metals have electronegativities less than ____






17. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.






18. 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.






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






21. 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.






22. The action of salts of weak acids or bases with water to form acidic or basic solutions.






23. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.






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






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






26. Heat added to a system and work done by a system are considered _________ quantities.






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






28. The most active nonmetals are found in what corner of the periodic table?






29. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.






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






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






32. 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






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






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






35. 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).






36. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.






37. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.

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38. 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.






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






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






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






42. 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.






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






44. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.

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






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






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






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






49. 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.






50. The change in enthalpy of an exothermic reaction is ________.