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






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






3. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.






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






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






8. 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 _____ _






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






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






11. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f






12. 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.






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






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






15. 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.






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






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






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






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






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






21. The action of salts of weak acids or bases with water to form acidic or basic solutions.






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






23. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.






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






25. 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.






26. Cells that convert electrical energy into chemical energy.






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






28. 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.






29. 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.






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






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






32. 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






33. 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).






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






35. *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.






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






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






38. 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.


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






40. 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.






41. 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 _______.


42. *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.






43. 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).






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






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






46. 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.






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






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






49. 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.


50. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.