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






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






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






4. *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.






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






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






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






8. 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.






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






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






11. The vapor pressure increases with increasing _____.






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






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






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






15. 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.


16. The energy required to remove an electron from an isolated atom in its ground state.






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. 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.


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






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






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






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






23. 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.


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






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






26. 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).






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






28. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.






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






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






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






32. 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.






33. 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.






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






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






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






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






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






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






40. *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






41. 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.






42. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.






43. 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.






44. 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 _______.


45. 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.






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






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






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






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






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