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






2. *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.






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






4. 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.






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






6. 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.






7. 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.






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






9. *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.






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






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






12. 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 _______.


13. 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






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






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






16. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.






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






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






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






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






21. 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






22. 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).






23. 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.






24. Electronegativities _______ as you go down a group.






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






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






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






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






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






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






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






32. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.






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






34. 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.






35. 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.






36. *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.






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






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






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






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






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






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






43. 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.






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






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






46. The solubility of gases in liquid or solid solvents always increases with ________ pressure.






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






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






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






50. 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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