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






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






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


5. Metals have electronegativities less than ____






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






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






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






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






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






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






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






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






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






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






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






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






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






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






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






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






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






23. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g






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






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






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






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






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






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






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






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






32. 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.


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






34. 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.






35. 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.


36. **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.






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






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






39. 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.






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






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






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






43. *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.






44. 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.






45. 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.






46. Electronegativities _______ as you go down a group.






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






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






49. 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






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