Test your basic knowledge |

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. Liquids with strong attractive forces have ______ boiling points.






2. 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.






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






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






5. Cells that convert electrical energy into chemical energy.






6. *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.






7. 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.

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


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






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






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






11. 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.






12. *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.






13. 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






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






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






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






17. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.






18. 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.






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






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






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






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






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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


24. 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






25. 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.

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


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






27. 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.






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






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






30. 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.






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






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






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






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






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






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






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






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






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






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






42. The change in enthalpy of an endothermic reaction is ________.






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






44. 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.






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






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






47. 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.






48. 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 _______.

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


49. 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.






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