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






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






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






4. 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.






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






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






7. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.






8. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






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






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






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






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






13. 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.






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






15. *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.






16. 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






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






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






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






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






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






22. 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.






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






24. 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.






25. *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.






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






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






28. 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.






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






30. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.






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






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






33. Electronegativities _______ as you go down a group.






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






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






36. 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).






37. 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).






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






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






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






41. 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






42. 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.






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






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






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






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






47. 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.






48. 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 _____ _






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






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