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






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






3. 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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4. 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.






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






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. 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.






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






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






10. *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.






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






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






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






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






16. A hypothetical gas would follow Boyles law under all conditions and is called?






17. 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).






18. The vapor pressure increases with increasing _____.






19. 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.






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






21. 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.






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






23. Electronegativities _______ as you go down a group.






24. 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.






25. 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.






26. 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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27. 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






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






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






30. 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.






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






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






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






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






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






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






37. 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).






38. Rays made up of positive electrodes in basic electron charges.






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






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






41. *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.






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






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






44. 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.






45. When the rate of evaporation equals the rate of condensation - the system is in __________.






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






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






48. 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.






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






50. 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