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






2. The heat change during a process carried out at a constant pressure.






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






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






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






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






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






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






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






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






12. 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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13. 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.






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






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






16. Rays made up of positive electrodes in basic electron charges.






17. Cells that convert electrical energy into chemical energy.






18. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f






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






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






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






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






23. 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.






24. 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.






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






26. The most active nonmetals are found in what corner of the periodic table?






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






28. A chemical reaction formed from the union of its elements.






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






30. *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.






31. *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.






32. The vapor pressure increases with increasing _____.






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

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






36. 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.






37. 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.






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






39. 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 _____ _






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






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






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






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






44. 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.






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






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






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






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






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