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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 chemical reaction formed from the union of its elements.






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






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






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






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. Liquids with strong attractive forces have ______ boiling points.






7. 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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8. 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 _____ _






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






10. 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.






11. 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).






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






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






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






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






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

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






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






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






20. 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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21. Cells that convert electrical energy into chemical energy.






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






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






24. 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.






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






26. The vapor pressure increases with increasing _____.






27. 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.






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






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






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






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






33. 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






34. 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.






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






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






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

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






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






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






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






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






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






45. *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.






46. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.






47. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge






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






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






50. Electronegativities _______ as you go down a group.