Test your basic knowledge |

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






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






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






4. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.






5. 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.






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






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






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






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






10. Metals have electronegativities less than ____






11. 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.






12. The solubility of gases in liquid or solid solvents always increases with ________ pressure.






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


14. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.






15. *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.






16. 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.


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






18. *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.






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






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






21. 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.






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






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






24. **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.






25. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.






26. A hypothetical gas would follow Boyles law under all conditions and is called?






27. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.






28. 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.






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






30. Cells that convert electrical energy into chemical energy.






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






32. 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.






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






34. 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.


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






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






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






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






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






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






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






42. 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 _____ _






43. 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






44. 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






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






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






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






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






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






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