Test your basic knowledge |

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






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 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.






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






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






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






8. The law stating that in any spontaneous process there is an increase in the entropy of the universe.






9. 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.






10. 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.






11. 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.






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






13. 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).






14. The action of salts of weak acids or bases with water to form acidic or basic solutions.






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






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






17. 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.






18. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.






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






20. 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.






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






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






23. 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.

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


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






25. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.






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






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






28. **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.






29. 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






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






31. 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.






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






33. Metals have electronegativities less than ____






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






35. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






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






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






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






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






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






41. Electronegativities ________ from left to right in a period.






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






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






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






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






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






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






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






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






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