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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. 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).






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






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






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






5. Electronegativities _______ as you go down a group.






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






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. *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






9. Cells that convert electrical energy into chemical energy.






10. 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.






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






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






13. *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.






14. 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.






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






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






18. 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.






19. 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 _____ _






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






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






22. 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.






23. 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.






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






25. 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






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






27. 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.






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






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






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






31. 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.






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






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






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






35. 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.






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






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






38. 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.






39. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.






40. 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.






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






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






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






44. The vapor pressure increases with increasing _____.






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






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






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






48. A solution in which solid solute is in equilibrium with dissolved solute.






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






50. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.