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






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






3. 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.






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






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






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






7. 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 _______.


8. 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.


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






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






11. The pressure exerted by each gas in a mixture is called its _____ pressure.






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






13. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.






14. Cells that convert electrical energy into chemical energy.






15. 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.






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






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






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






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






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






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






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






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






25. 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.






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






27. 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.






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






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






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






31. Electronegativities _______ as you go down a group.






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






33. *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.






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






35. 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 _____ _






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






37. The solubility of gases in liquid or solid solvents always increases with ________ pressure.






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






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






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






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






42. The vapor pressure increases with increasing _____.






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






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






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






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






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






48. 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.






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






50. Metals have electronegativities less than ____