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






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






3. 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.


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






5. *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.






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






7. 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.






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






10. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.






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






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






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






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






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






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






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






19. 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.






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






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






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






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






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






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






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






27. 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 _______.


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






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






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






31. 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.


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






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






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






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






36. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?






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






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






39. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






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






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






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






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






45. Cells that convert electrical energy into chemical energy.






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






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






48. 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.






49. 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.






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