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






2. 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.






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






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






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






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






7. 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.






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






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. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.






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






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






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






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


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






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






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






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






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






20. 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.






21. *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






22. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.






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






24. *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.






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






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






27. 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 _____ _






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






29. 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.


30. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.






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






32. 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.


33. 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.






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






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






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






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






38. 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).






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






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






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






42. 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.


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






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






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






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






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






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






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






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