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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. Electronegativities _______ as you go down a group.






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






4. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.






5. Cells that convert electrical energy into chemical energy.






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






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






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






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






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






11. 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.






12. 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.






13. 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.






14. 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.






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






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






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






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






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






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






21. 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.






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






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






24. 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 _______.


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






26. 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






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






28. 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.


29. 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.


30. 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.


31. 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.


32. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.






33. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






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






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


36. 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 _____ _






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






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






39. 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.






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






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






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






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






44. 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.






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






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






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






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






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


50. *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.