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






2. 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.






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






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






5. 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.






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






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. 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.






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






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






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






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






13. Cells that convert electrical energy into chemical energy.






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






15. The vapor pressure increases with increasing _____.






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






17. 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).






18. 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.






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






20. 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






21. 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.






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






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






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






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






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






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






29. A hypothetical gas would follow Boyles law under all conditions and is called?






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






31. 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






32. 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.

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






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






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






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






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






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






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






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






41. 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.






42. *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.






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






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






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






46. **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.






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






48. Electronegativities _______ as you go down a group.






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

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