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






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

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






5. Metals have electronegativities less than ____






6. 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






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






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






9. *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.






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






11. 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).






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

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






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






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






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






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






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






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






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






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






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






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






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






26. Electronegativities _______ as you go down a group.






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






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






29. Cells that convert electrical energy into chemical energy.






30. 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






31. 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.






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






33. 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 _______.

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






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






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






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






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






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






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






41. *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.






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






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






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






45. 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.






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






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






48. 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






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






50. 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.