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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. Rays made up of electrons in basic electron charges.






2. 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).






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






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. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.






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






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






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

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






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






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






12. *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.






13. 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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14. The vapor pressure increases with increasing _____.






15. 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 _____ _






16. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.






17. 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.






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






19. 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).






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






21. 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.






22. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.






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






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






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






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






27. 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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28. *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






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






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






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






32. 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.






33. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.






34. 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.






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






36. 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.

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

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






39. This process occurs when the system is thermally isolated so that no heat enters or leaves.






40. The energy required to remove an electron from an isolated atom in its ground state.






41. 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.






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






43. 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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44. 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.






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






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






47. 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.






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






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