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






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






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






4. 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.


5. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






6. 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.






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. 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).






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






10. 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.






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






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






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






14. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.






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






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






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






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






19. 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.






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






21. Cells that convert electrical energy into chemical energy.






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






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






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






25. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






26. 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.


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 is always lowered by addition of solute.






29. Metals have electronegativities less than ____






30. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.






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






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






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






34. 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.






35. 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.






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






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






38. The vapor pressure increases with increasing _____.






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






40. 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.






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






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






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






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






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






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






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






48. 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.






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






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