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






2. 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.






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






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






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






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






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






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






9. 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






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






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






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






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






14. 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.






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






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






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






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






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






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






21. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.

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






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






24. 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.






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






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






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






28. The vapor pressure increases with increasing _____.






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






30. 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.






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






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






33. 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.






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






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






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






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






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






39. 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.






40. The pressure exerted by each gas in a mixture is called its _____ pressure.






41. 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.






42. 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).






43. 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.

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






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






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






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






48. 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.






49. 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.






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