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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. 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.






2. 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.






3. 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.

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






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






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






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






8. 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.

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






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






11. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.






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






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






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






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






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






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






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






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






20. *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.






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






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






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






24. 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.






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

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26. 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 _____ _






27. *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.






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






29. **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.






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






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






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






33. 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.






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






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






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






37. Heat added to a system and work done by a system are considered _________ quantities.






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






39. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g






40. 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.






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






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






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






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






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






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






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






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






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

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50. 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