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


2. 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.


3. 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.






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






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






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






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






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






9. Metals have electronegativities less than ____






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






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






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






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






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






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






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






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






18. 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.


19. *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.






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






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


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






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






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






26. The vapor pressure increases with increasing _____.






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






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






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






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






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






32. 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.






33. 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.


34. 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.






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






36. 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).






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






38. 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.






39. *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.






40. 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.






41. 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.






42. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






43. 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.






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






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






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






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






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






49. 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.






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