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






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






3. The freezing point is always lowered by addition of solute.






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






5. Rays made up of positive electrodes in basic electron charges.






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






7. 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.






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






9. 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.






10. A valence theory that permits the geometric arrangement of atoms - or groups of atoms - about some central atom to be determined solely by considering the repulsions between the electron pairs present in the valence shell of the central atom.






11. The heat change during a process carried out at a constant pressure.






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






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






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






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






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






17. 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.






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






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






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






21. 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.

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22. 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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23. 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.






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






25. Cells that convert electrical energy into chemical energy.






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






27. *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.






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






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






30. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.






31. 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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32. 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.






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






34. 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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35. Metals have electronegativities less than ____






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






37. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g






38. 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.






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






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






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






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






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






44. 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).






45. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.






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






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






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






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






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