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






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






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






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






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






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






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






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






10. 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.






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






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






13. **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.






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






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






16. 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).






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






18. The most active metals are found in what corner of the periodic table?






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






20. Electronegativities _______ as you go down a group.






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






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






23. 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.






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

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






26. This law states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases in mixture.






27. 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.






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






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






30. The vapor pressure increases with increasing _____.






31. 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).






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






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






34. 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.






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






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






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






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






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






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






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






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






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






44. 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.






45. 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






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






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






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






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






50. 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.

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