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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 pressure exerted by the gas molecules when they are in equilibrium with the liquid.






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






3. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.


4. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.






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






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






7. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.






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






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






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






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






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






13. 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.






14. 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 _____ _






15. 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 _______.


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






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






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






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






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






22. The _____ speed up the rate of a chemical reaction but do not change the equilibrium constant - it simply speeds up the rate of approach to equilibrium.






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






24. 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






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






26. 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.






27. 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.






28. 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.






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






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






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






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






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






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






35. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.






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






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






38. *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.






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






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


41. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






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






43. 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).






44. 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






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






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






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






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


49. 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






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