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. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.






2. 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.






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






4. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






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






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






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






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






9. 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).






10. The vapor pressure increases with increasing _____.






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






12. Cells that convert electrical energy into chemical energy.






13. 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.






14. 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.






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






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






17. 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.






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






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






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






21. 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.






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






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






24. 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






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






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






27. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l






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






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






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






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






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






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






34. 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.

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


35. 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


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






37. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.






38. 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.






39. 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.

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


40. 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.






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






42. 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 _______.

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


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






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






45. 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).






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






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






48. 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.






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






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