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






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. 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.






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






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






7. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.






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






9. 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.






10. 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.

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11. 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.






12. 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






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






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






15. 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.

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

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






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






19. 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 _____ _






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






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






22. 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.






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






24. The most active nonmetals are found in what corner of the periodic table?






25. 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






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






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






28. 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.






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






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






32. 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.






33. *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.






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






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






36. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?






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






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






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






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






41. 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).






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






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






44. 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.






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






46. 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.

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






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






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






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