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






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






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






4. Electronegativities _______ as you go down a group.






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






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






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






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






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






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






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






12. Metals have electronegativities less than ____






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






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






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






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






17. *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.






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






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






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






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






22. 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.






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






25. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).






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






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






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






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






30. Cells that convert electrical energy into chemical energy.






31. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge






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






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






34. 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.






35. 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






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






37. 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.






38. Heat added to a system and work done by a system are considered _________ quantities.






39. 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).






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






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

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






43. The vapor pressure increases with increasing _____.






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






46. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.






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






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






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






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