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






2. Metals have electronegativities less than ____






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






4. Real gases act in a less than ideal way - especially under conditions of increased pressure and/or decreased temperture. Real gas behavior approaches that of ideal gases as the gas pressure becomes very low. The ideal gas is thus considered a _____ _






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






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






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






8. *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.






9. 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.






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






11. 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.






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






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






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






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






16. 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.


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






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






19. 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.






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






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






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






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






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






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






26. 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.


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






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






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






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


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






33. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.






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






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






36. 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.






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






38. 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.






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






40. **Proceeding across a period from left to right - the ionization energy _______.






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






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






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






44. 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.


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






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






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






48. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.






49. *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.






50. 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.