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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 nature of the reactants and products affect chemical reactions because some elements and compounds have bonds that when broken/formed - react more rapidly with each other than others.






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

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3. 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.






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






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






6. Metals have electronegativities less than ____






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






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






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






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






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






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






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






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






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






16. 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.






17. 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.






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






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






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






21. 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 _____ _






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






23. Cells that convert electrical energy into chemical energy.






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






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






27. *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.






28. 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).






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






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






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






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






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






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






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






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






37. 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.






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






39. 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.






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






41. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






42. 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.






43. In an exothermic process - energy is released and ^E of reaction is ________.






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






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






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






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






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






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






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







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