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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 _____ 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.






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






3. Electronegativities _______ as you go down a group.






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






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






6. *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.






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






8. 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.






9. 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.






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






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






12. The vapor pressure increases with increasing _____.






13. 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.


14. 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.






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






16. 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






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






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






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






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






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


22. 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






23. 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.






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






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






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






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






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






29. *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






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






31. 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.






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






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






34. 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.






35. 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.






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






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


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






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






40. **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.






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






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






43. *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.






44. 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.






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






46. Cells that convert electrical energy into chemical energy.






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






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






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






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