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






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






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






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






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






6. 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.






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






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






9. 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.






10. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____






11. The freezing point is always lowered by addition of solute.






12. 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.






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






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






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






16. 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.






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






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






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






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






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






22. 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.






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






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






25. 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.






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






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






28. 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.






29. A process that occurs whent eh system is maintained at constant pressure.






30. 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.






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






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






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 relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).






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






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






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






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






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






40. 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).






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






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






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






44. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.






45. 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.






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






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






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






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

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