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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. 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.






2. 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).






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






4. 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.






5. 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.


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






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


8. 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.






9. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.


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






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






12. 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.






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






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






15. **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.






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






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






18. 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.


19. 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).






20. Electronegativities _______ as you go down a group.






21. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.






22. The pressure exerted by each gas in a mixture is called its _____ pressure.






23. 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.






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






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






26. 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.






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






28. 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.






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






30. 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 _______.


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






32. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.






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






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






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






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






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






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






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






40. 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






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






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






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






44. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.






45. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l






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






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






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






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






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