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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 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.






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






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






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






5. 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






6. Metals have electronegativities less than ____






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






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






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






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






11. *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.






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






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






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






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


16. *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.






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






18. Electronegativities _______ as you go down a group.






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






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






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






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






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






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






25. Cells that convert electrical energy into chemical energy.






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






27. 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 _____ _






28. In an exothermic process - energy is released and ^E of reaction is ________.






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






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






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






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






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






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






35. 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.






36. The action of salts of weak acids or bases with water to form acidic or basic solutions.






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






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






40. The molecules in a gas are in constant - continueous - random - and straight-line motion.






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






42. The vapor pressure increases with increasing _____.






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






44. 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.


45. 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.






46. 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).






47. 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.


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






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






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.