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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. 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).






3. 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.






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






5. 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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6. In titration - this is the point at which a particular indicator changes color.






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






8. Cells that convert electrical energy into chemical energy.






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






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

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






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






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






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






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






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






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






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






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






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






23. 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.






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






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






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






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






28. 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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29. 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.






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






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






32. 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.






33. 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






34. 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.






35. 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.






36. Metals have electronegativities less than ____






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






38. 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.






39. 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.






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






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






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






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






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






45. 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.






46. 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 _____ _






47. A state function in which it is the heat content of a substance.






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






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






50. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.

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