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






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






3. 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.






4. Metals have electronegativities less than ____






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






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






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






8. 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.






9. **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.






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






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






12. 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.






13. 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.






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






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






16. 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.






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






18. Electronegativities _______ as you go down a group.






19. A process that occurs whent eh system is maintained at constant pressure.






20. 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.






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






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






23. 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.

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24. 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.






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






26. 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






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






28. 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.

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29. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.






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






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






32. 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






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






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






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






36. *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






37. 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.

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






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






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






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






42. 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).






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






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






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






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






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






48. 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.






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






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