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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 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.






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






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






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






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






6. *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.






7. Metals have electronegativities less than ____






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






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






10. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.






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






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






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






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






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






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






17. 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.


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






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






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






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






22. 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.






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






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


25. *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.






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






27. 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.






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






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






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






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






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






33. 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 _______.


34. 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.






35. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.






36. 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






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






38. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.






39. 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.


40. 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).






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






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






43. *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.






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






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






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






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






48. 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.


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






50. 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.