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






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






3. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.






4. **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.






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






6. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.






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






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






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






11. 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.






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






13. 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.






14. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.






15. 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.






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






17. The freezing point is always lowered by addition of solute.






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






19. *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.






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






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






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






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






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






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


26. 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.






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






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






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






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






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






32. 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.


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






34. Liquids with strong attractive forces have ______ boiling points.






35. 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.






36. 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






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






38. 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.






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






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


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






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






43. The vapor pressure increases with increasing _____.






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. 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.






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






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






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






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. Metals have electronegativities less than ____