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






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






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






4. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.






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. Electronegativities ________ from left to right in a period.






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






8. 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.






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






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






11. 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






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






13. 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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14. 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.






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






16. Electronegativities _______ as you go down a group.






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






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






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






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






21. 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.






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






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






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






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






26. 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.






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






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






29. *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.






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






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






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






33. 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.






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






35. 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.






36. 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.






37. 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.






38. *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






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






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






41. The vapor pressure increases with increasing _____.






42. 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.






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






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






45. 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.






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






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






50. *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.