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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. 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






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






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






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






5. 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.






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






7. 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 _____ _






8. 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.






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






10. The vapor pressure increases with increasing _____.






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






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






13. 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).






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






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






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






17. 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.






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






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






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






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






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






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






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






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






26. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.






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






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






29. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.






30. *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.






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






32. 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.






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






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






35. *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.






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






37. 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






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






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






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






42. 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.






43. 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.

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44. 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.






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

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






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






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






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






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






Can you answer 50 questions in 15 minutes?



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