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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 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






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






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






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






5. 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 _____ _






6. 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.

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7. 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.






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






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






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






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






12. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.

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

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






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






16. 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).






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






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






19. 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.






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






21. 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.






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






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






24. 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.






25. Metals have electronegativities less than ____






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






27. 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.






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






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






30. 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 _______.

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






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






34. 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.






35. When a system at equilibrium is disturbed by adding or removing one of hte substances - all the concentrations will change until a new equilibrium point is reached with the same value of Keq.

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36. 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.






37. Electronegativities _______ as you go down a group.






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






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






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






41. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).






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






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






44. 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






45. 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.






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






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






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






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






50. The vapor pressure increases with increasing _____.