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






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






3. *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






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






5. Electronegativities _______ as you go down a group.






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






7. 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.






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






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






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






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






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






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






14. 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.






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






16. In an endothermic process - energy is absorbed and ^E is _______.






17. 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.






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






19. _______ has very little effect on the solubility of liquids or solids in liquid solvents.






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






21. 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.






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

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23. 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.






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






25. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.

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






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






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






30. 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.






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






32. *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.






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






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






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






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






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






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






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






40. 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).






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






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






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






44. Cells that convert electrical energy into chemical energy.






45. 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.






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






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






48. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.

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






50. 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.