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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. *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.






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






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






4. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






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






6. 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.






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






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






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






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






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






12. The change in enthalpy of an exothermic reaction is ________.






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






14. 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.






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






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






18. 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






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






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






21. Cells that convert electrical energy into chemical energy.






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






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






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






25. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






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






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






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






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






31. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






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






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






34. 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






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






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






37. 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).






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






39. A process that occurs whent eh system is maintained at constant pressure.






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






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






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






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






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






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






46. 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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47. 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.






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






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






50. 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.