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






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






3. 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.






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






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






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






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






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






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






10. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.






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






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






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






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






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






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






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






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






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






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






21. 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






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






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






24. Metals have electronegativities less than ____






25. 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.






26. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.






27. 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.






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






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






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






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






32. Liquids with strong attractive forces have ______ boiling points.






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






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






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






36. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.


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






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






39. The action of salts of weak acids or bases with water to form acidic or basic solutions.






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






41. 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).






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






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


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






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






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






47. 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.


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






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






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