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






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






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






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






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






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






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






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


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






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






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






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






13. 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.






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






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






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






17. 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.


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






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






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






21. Electronegativities _______ as you go down a group.






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






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






24. Cells that convert electrical energy into chemical energy.






25. 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






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






27. 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.






28. 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.


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






30. 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.


31. Metals have electronegativities less than ____






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






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






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






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






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






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






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






40. This process occurs when the system is thermally isolated so that no heat enters or leaves.






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






42. 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 _______.


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






44. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).






45. 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.


46. 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.


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






48. 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.






49. A state function in which it is the heat content of a substance.






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